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H+ is the chemical formula for hydron or hydrogen ion or cation. The hydrogen nucleus has general name called Hydron, which is used deprived of concerns to the nuclear mass of hydrogen. H+ ion has some synonyms like proton, hydrogen ion or cation. It comes under the members of atomic nucleus, i.e. a monovalent inorganic … Read more
HOF is the chemical formula for hypofluorous acid. Here we are discussing about HOF lewis structure, characteristics and some facts about it.
HOF (hypofluorous acid) can also be written as FHO. HOF has some synonyms like fluoranol, fluoroalcohol, hydroxyl fluoride and fluoridohydridooxygen. HOF (hypofluoro acid) or fluoranol is an fluorine oxyacid which is a conjugate acid of hypofluorite. HOF has molecular weight of 36.006. HOF consists of three elements mainly hydrogen, oxygen and fluorine.
How to draw HOF lewis structure?
The lewis structure of HOF can be drawn by considering the following steps:
Predict the group positions of hydrogen, oxygen and fluorine atoms on periodic table
Count overall valence electrons available on HOF lewis structure.
Selection of central atom which is most electronegative from all the atoms and the rest of the atoms are being bonding atoms.
Make bonding within all H, O and F atoms of HOF lewis structure.
Remaining valence electrons are put on the bonding atoms which are being non – bonding electrons.
Then count the lone pair electrons on HOF lewis structure.
Finally predict the shape, hybridization and bond angle of HOF lewis structure.
HOF lewis structure
HOF valence electrons
The HOF lewis structure composed of three elements i.e. hydrogen atom, oxygen atom and fluorine. Thus, the hydrogen atom belongs to 1st periodic table group, oxygen atom belongs to 16th periodic table group and the fluorine atom belongs to 17th (7A) periodic table group. Therefore, the H, O and F atoms contain one, six and seven valence electrons respectively, in their valence shell outer orbital.
The total valence electrons available on hydrogen, oxygen and fluorine atoms of HOF lewis structure is calculated as follows:
Hydrogen atom of HOF lewis structure has valence electrons is = 01
Oxygen atom of HOF lewis structure has valence electrons is = 06
Fluorine atom of HOF lewis structure has valence electrons is = 07
Hence, total valence electrons on HOF lewis structure is = 1 (H) + 6 (O) + 7 (F) = 14.
Therefore, the valence electrons on HOF lewis structure are fourteen.
If we see the total electrons pairs on HOF lewis structure, the HOF valence electrons get divided by two.
Thus, total electron pairs on HOF lewi structure = 14 / 2 = 7
Therefore, there are seven electron pairs in MOF lewis structure.
Valence electrons on HOF lewis structure
HOF lewis structure lone pairs
The HOF lewis structure has total 14 valence electrons, out of which four electrons are the bond pair electrons which forms two single sigma covalent bonds with hydrogen and oxygen (H-O) atom and oxygen and fluorine (O-F) atom. Hence, the remaining 10 valence electrons go to O and F atoms.
Thus, the oxygen atom has four non – bonding electrons and fluorine atom has six non – bonding electrons on HOF lewis structure. These 10 non-bonding electrons of HOF are being the five lone electron pairs. Hence, the HOF lewis structure has total five lone electron pairs available on it two on O atom and three on F atom.
HOF lewis structure octet rule
There is two lone pair electrons are on oxygen atom and three lone pair electrons are on fluorine atom of HOF lewis structure. Hence, the hydrogen atom of HOF lewis structure has two bonding electrons satisfied it’s valency as per it capacity. The O atom contains 4 bond pair electrons (creates H-O and O-F bonds) and 4 non-bonding electrons.
Hence O atom of HOF lewis structure has eight electrons and have complete octet. The fluorine atom of HOF lewis structure has two bonding electrons forming O-F bond and also it has six non – bonding electrons. Thus, F atom of HOF lewis structure has total eight electrons and its octet is also complete. So, in HOF lewis structure the O and F atoms has eighit electrons which shows complete octet.
HOF lewis structure formal charge
The presence of formal charge on any lewis structure makes it more stable structure. Evaluation of formal charge on any molecules is done with the help of below given formula:
The HOF lewis structure formal charge evaluation is done with the help of using above given formula. Here, first we have to evaluate the formal charge present on each hydrogen, oxygen and fluorine atoms of HOF lewis structure.
Hydrogen atom: Valence electrons on hydrogen atom of HOF = 01
Non- bonding electrons on hydrogen atom of HOF = 00
Bonding electrons on hydrogen atom of HOF = 02 (2e = one bond)
Thus, Formal charge on hydrogen atom of HOF lewis structure is = (01 – 00 – 2/2) = 00
So, the Hydrogen atom of HOF lewis structure contains zero formal charge.
Oxygen atom: Valence electrons on Oxygen atom of HOF = 06
Non – bonding electrons on Oxygen atom of HOF = 04
Bonding electrons on oxygen atom of HOF = 04 (2e = one bond)
HOF acid follows AX2E2 generic formula of VSEPR theory. Here, A is central atom, X is bonded atoms with central atom and X is lone electron pairs on central atom. According to which the HOF acid has bent molecular shape and tetrahedral electron geometry.
The HOF acid has the bent molecular shape and tetrahedral electrons geometry as the central O atom has two bonding atoms and two lone electron pairs. Therefore, as per the VSEPR theory the HOF acid should have 109.5 degree bond angle. But in HOF the H-O bond angle is less than O-F bond angle, thus the bond angle of HOF get decreases and have 97.2 degree bond angle.
HOF hybridization
With accord to VSEPR theory module HOF lewis structure belongs to AX2E2 generic formula, so HOF shows bent shape and tetrahedral geometry. Also it has H-O-F bond angle of 109.5 degree. Thus, HOF (hyprflorous acid) acid has sp3 hybridization.
Why HOF has sp3 hybridization?
In HOF molecule, the central O atom has two bonds with H and F atoms and also it has two lone electron pairs. Thus as per VSEPR theory HOF molecule has tetrahedral electron geometry and sp3 hybridization.
HOF solubility
HOF is an explosive substance and mostly insoluble in most of the organic solutions. Thus when HOF get added to water it behaves as an intermediate substance for oxidation of water by fluorine. Also it get decomposes as O2 and HF molecules. Hence, HOF is insoluble in nature and also unstable.
Is HOF soluble in water?
Yes, HOF is soluble in water. When HOF gets added to water it shows rapid explosive nature of reaction and thus HOF acts as an intermediate substance for water oxidation by fluorine molecule. Also the decomposition of HOF acid gets occurs and it get dissociates into HF and O2 in alkaline condition. Also on reaction with water of HOF it can produce peroxide and hydrogen fluoride in acidic medium.
Is HOF a monobasic acid?
No, HOF is not a monobasic acid it gets ionizes as fluorine and oxygen when added to water. Thus it cannot act as monobasic acid.
Why HOF is not a monobasic acid?
Monobasic acids are those acids which can have only one detachable hydrogen atom (H+ ion) per molecule in water. All the halogen atoms can produce monobasic oxyacids except the case of HOF. HOF is also an oxyacid but it is not monobasic in nature.
HOF is an oxyacid but it is exists in unstable form. As on dissolving in water it shows explosive behaviour and thus decomposed as fluorine (HF) and oxygen (O2). Hence, HOF does not act as a monobasic acid in nature.
Is HOF polar or non- polar?
HOF is a polar acid in nature as it has asymmetrical arrangement of all atoms and the dipole creates get cancel each other.
Why HOF is polar?
In HOF molecule, there is more electronegativity difference between hydrogen, oxygen and fluorine atoms. The electronegativity difference between H and O atoms are 1.24 and electronegativity difference between F and O atom is 0.54.
Thus it creates a dipole within the molecule and developed the partial negative charge on central O atoms and partial positive charge on bonding H and F atoms. There is no electron density present on H atom. But the F atom has more electron density which pulls the electron cloud towards itself and hence cancels the dipoles in HOF molecule. Hence, HOF is a polar molecule.
Is HOF stronger than HOCl?
Yes, HOF acid is stronger than HOCl acid. The fluorine atom is more electronegative in nature than chlorine and thus HOF can be stronger than chlorine.
Why HOF is stronger than HOCl?
In oxyacids, the weaker the O-H bond the stronger is the acid as the H+ ions can readily dissociates. In HOF the O-F bond is quite stronger as compared to O-Cl bond in HOCl.
The atomic size of F atom is less than Cl atom and also F is more electronegative than Cl. In HOF the O-F bond is stronger due to which the O-H bond becomes weaker and hence HOF is stronger than HOCl.
Is HOF ionic or covalent?
HOF is not ionic because it is an unstable covalent compound having two H-O and O-F covalent bonds within HOF molecule.
Why HOF is covalent?
HOF acid is strong acid and has single sigma covalent bonds within H and O atoms (H-O) and O and F atoms (O-F). The covalent bond is a strong bond which does not breaks easily. Hence, the HOF cannot ionize easily and so it is a covalent acid.
Is HOF ionic hydride?
No, HOF is not ionic hydride because it is an oxyacid. Oxyacids formed when the halogen reacts with water.
Why HOF is not ionic hydride?
When halogen like fluorine reacts with water gives the production of unstable oxyacid like HOF (hypoflurous acid). HOF is an intermediated of oxidation of water and fluorine.
F2 + H2O → HOF + HF
Thus, HOF is being an oxyacid, so it is not ionic hydride.
Is HOF isoelectronic?
No, HOF is not isoelectronic in nature. HOF is only one oxyacid of fluorine atom. Isoelectronic compounds are those two or more compounds which has similar structure and similar atoms position and bonding with same electronic configuration but different in properties. HOF does not have any similar molecule and hence it is not isoelectronic.
Is HOF ionic or molecular?
HOF is molecular because it cannot form ions. HOF is a triatomic molecule consisting of three atoms i.e. hydrogen, oxygen and fluorine atoms. Also it is only the oxyacid of fluorine and on decomposition it forms molecules like HF and O2. Hence, it is a molecular and not ionic.
Is HOF ion dipole?
Yes, HOF has a net dipole moment of 2.23. In HOF molecule fluorine atom is more electronegative than O and H atoms and hence the net dipole pulls towards the F atom. Thus HOF acid has dipoles.
Conclusion:
HOF is only one oxyacid of fluorine. HOF lewis structure has 14 valence electrons and has 7 electrons pairs from them two are bond pair electrons and five lone pair electrons. There is no formal charge on HOF molecule and has covalent bonds within H-O and O-F. The HOF lewis structure has bent shape and tetrahedral geometry also it has bond angle of 97.2 degree. Hof is a polar acid.
HgCl2 is the chemical formula of mercuric chloride. Here, we are discussing about HgCl2 lewis structure, characteristics and quick facts.
Mercuric chloride (HgCl2) is a white solid crystalline powder with no odour. It is a triatomic molecule consists of one mercury atom and two chlorine atoms linearly. HgCl2 is highly toxic in nature. It has some synonyms like sublimate, mercury (ii) chloride, mercury bichloride and Dichloro mercury. The molecular weight of HgCl2 is 271.50.
How to draw HgCl2 lewis structure?
Lewis structure can be drawn with the help of following points listed below:
Firstly note the positions of groups of Hg and Cl atoms in periodic table.
Then count the total valence electrons in available on Hg and Cl atoms.
Most electronegative atom will be the central atom and rather all are bonding to it by forming sigma covalent bond within Hg and two cl atoms.
After forming bonds within Hg and Cl left over valence electrons should get put on the bonding Cl atoms and they are being non – bonding electrons.
Note the number of lone electrons present on HgCl2 lewis structure.
Finally, predict the shape and geometry of HgCl2 lewis structure with its hybridization and bond angle.
HgCl2 lewis structure
HgCl2 valence electrons
In HgCl2 lewis structure, there are on Hg atom and two chlorine atoms are present in it structure. Here, the Hg atom belongs to 12th periodic table group and the chlorine atom belongs to 7th periodic table group.
Thus, the Hg atom has two valence electrons in its outer valence shell orbital and the chlorine atoms have seven valence electrons in its outer valence shell orbital. Hence, the overall valence electrons available on HgCl2 lewis structure are:
Valence electrons on mercury (Hg) = 2
Valence electrons on chlorine (Cl) = 7 x 2 (Cl)
Therefore, Valence electrons on HgCl2 lewis structure = 2 + 14 = 16
Hence, total sixteen valence electrons present on HgCl2 lewis structure.
Total electrons pairs on HgCl2 can be calculated by dividing 16 valence electrons by 2.
Thus, HgCl2 total electron pairs = 16 / 2 = 8
So, HgCl2 lewis structure has total eight electrons pairs.
HgCl2 lewis structure has total 16 valence electrons present on it. From these 16 valence electrons 4 valence electrons becomes bond pair electron as they are forming two Hg-Cl bonds within one mercury and two chlorine atoms.
Hence, the remaining 12 valence electrons of HgCl2 lewis structure goes on two chlorine atoms and being 12 non – bonding electrons on two chlorine atoms i.e. each chlorine atom has six non – bonding electron. Thus the two chlorine atoms of HgCl2 lewis structure has total eight electrons i.e. two bond pair electrons and six non – bonding electrons.
Therefore, the two chlorine atoms of HgCl2 lewis structure has complete octet. The central mercury (Hg) atom has for electrons i.e. four bond pair electrons. Thus, the mercury atom of HgCl2 lewis structure has incomplete octet. Hence, in HgCl2 lewis structure Hg has incomplete octet and two Cl atoms has complete octet.
Octet rule on HgCl2 lewis structure
HgCl2 lewis structure lone pairs
HgCl2 lewis structure has 16 total valence electrons. From them four electron are bond pair electrons forming two Hg-Cl bonds within central Hg atom and two bonding Cl atoms. The remaining 12 valence electrons are being non – bonding electrons on two Cl atoms of HgCl2 lewis structure.
Here, these 12 non – bonding electrons on two Cl atoms are being six lone electrons pair. Each chlorine atoms contains three lone electron pairs on HgCl2 lewis structure. Therefore, the HgCl2 lewis structure has total six lone pair electrons.
HgCl2 lewis structure formal charge
The stability of any lewis structure depends upon the formal charge present on it. If the formal charge is present on lewis structure, the lewis structure considered to be a stable lewis structure. There is a formula to evaluate the formal charge present on any lewis structure:
The evaluation of formal charge present on HgCl2 lewis structure can be done by evaluating the formal charge present on each Hg and Cl atoms present in HgCl2 lewis structure. Let us calculate the formal charge on HgCl2 lewis structure:
Mercury atom: Mercury atom has valence electrons in HgCl2 = 02
Mercury atom has non-bonding electrons in HgCl2 = 00
Mercury atom has bonding electrons in HgCl2 = 04 (one bond = 2 electrons)
Mercury atom of HgCl2 lewis structure contains formal charge = (02–00–4/2) = 0
Thus, in HgCl2 lewis structure the mercury atom has zero formal charge.
Chlorine atom: Chlorine atom has Valence electrons in HgCl2 = 07
Chlorine atom has Non- bonding electrons in HgCl2 = 06
Chlorine atom has Bonding electrons in HgCl2 = 02 (one bond = two electrons)
Chlorine atom of HgCl2 lewis structure has formal charge = (7–6–2/2) = 0
Thus, in HgCl2 lewis structure the chlorine atom has zero formal charge.
Therefore, the Mercury atom and Chlorine atoms in HgCl2 lewis structure has zero formal charge.
HgCl2 lewis structure resonance
In HgCl2 lewis structure all these conditions are not fulfilled. There are only two single sigma covalent bonds are present on HgCl2 lewis structure.
Chlorine atoms have lone electron pairs but sill movement of electrons are not possible to form double or triple bond and also there is no formal charge is available on HgCl2 lewis structure. Hence, the resonance structure of HgCl2 is not possible.
HgCl2 lewis structure shape
The HgCl2 lewis structure is a triatomic molecule, composed of one mercury and two chlorine atoms in which the central mercury atom connected with two chlorine atoms.
Thus, with accord to VSEPR theory, the HgCl2 lewis structure consists of AX2 generic formula in which A is central atom and X is bonding atoms connected to central atom. There is no lone pair electrons present on central Hg atom. Hence, as per the VSEPR theory, the HgCl2 lewis structure has linear molecular shape and linear electron geometry.
HgCl2 lewis structure angle
HgCl2 lewis structure comes under AX2 generic formula of VSEPR theory as the central Hg atom gets linked with two bonding Cl atoms. Thus, HgCl2 lewis structure has linear molecular shape and linear electron geometry.
Also the HgCl2 lewis structure has ‘sp’ hybridization. Hence, the bond angle of HgCl2 is 180 degree. Therefore, the HgCl2 lewis structure has Cl-Hg-Cl bond angle of 180 degree.
Bond angle of HgCl2 lewis structure
HgCl2 hybridization
As the HgCl2 lewis structure composed of three atoms i.e. one Hg and two cl atoms. They all are connected to each other with single covalent bonds and comes under AX2 generic formula of VSEPR theory.
Thus, the HgCl2 lewis structure has linear molecular shape and linear electron geometry. Therefore, according to VSEPR theory the HgCl2 lewis structure has ‘sp’ hybridization.
Why HgCl2 has ‘sp’ hybridization?
HgCl2 molecule consists of three atoms having one mercury atom and two chlorine atoms. The hybridization of any lewis structure can be predicted from its steric number. Here, the HgCl2 lewis structure hybridization can be recognized by the steric number of the central Hg atom.
Steric number is the addition of total bonded atoms joined to the central atom or element and lone electron pairs present on it.
Steric number of HgCl2 = No. of bonding atoms to Hg + lone electron pairs present on Hg atom
Therefore, Hg atom have steric number in HgCl2 lewis structure = 2 + 0 = 2
Hence the HgCl2 lewis structure has 2 steric number and thus the mercury (Hg) atom has ‘sp’ hybridization.
How HgCl2 has ‘sp’ hybridization?
In HgCl2 lewis structure, the Hg atom has electronic configuration at ground state is [Xe], 4f14, 5d10, 6s2. Therefore, the Hg (mercury) atom contains two valence electrons in its outer shell valence orbital.
Hence, the steric number of Hg atom in HgCl2 lewis structure is 2 + 0 = 2, as there are no lone electron pairs on central Hg atom. Even the HgCl2 molecule has linear molecular shape and electron geometry as per VSEPR theory. Thus, in the HgCl2 lewis structure, the Hg atom is ‘sp’ hybridized due to its geometry of two ‘sp’ hybrid orbitals.
HgCl2 solubility
Mercuric chloride (HgCl2) is soluble in:
Water (sparingly soluble)
Ether
Alkanol (R-OH)
Ethyl acetate
Acetone
Benzene (slightly soluble)
Carbon disulphide (CS2) (slightly soluble)
Pyridine (slightly soluble)
Why HgCl2 is soluble?
HgCl2 is an binary compound containing one metal atom i.e. Hg atoms and other halogen atom i.e. chlorine atom. Thus, it is considered that all the binary compounds containing halogen atoms and metals (except silver [Ag] metal) atoms are soluble in water and other polar solvents.
Is HgCl2 soluble in water?
Yes, HgCl2 is soluble in water, but it is sparingly soluble in water not completely soluble in water.
Why HgCl2 is soluble in water?
HgCl2 is an binary substance having one metal atom and halogen atom. These kinds of all binary compounds get soluble in water except silver metal. Even if we add the more chlorine to the water then the solubility of HgCl2 compound gets increases.
How HgCl2 is soluble in water?
HgCl2 is sparingly soluble in water, the solubility of HgCl2 increases in water after the addition of more chlorine to the solution and even if it gets heated or warm, the HgCl2 gets completely dissolved. HgCl2 forms a complex compound in water solution after the addition of more chlorine atoms.
HgCl2 + 2Cl− → [HgCl4]2−
Is HgCl2 polar or nonpolar?
HgCl2 is a non – polar compound. In HgCl2 there are two dipole moments on two chlorine atoms which get cancel out each other, hence HgCl2 is non – polar in nature.
Why HgCl2 is non – polar?
The HgCl2 is a non – polar substance because there is the formation of two dipole moments on two chlorine atoms of HgCl2 molecule. Both the chlorine atoms of HgCl2 pull the electron density towards them away from the centrally placed mercury atom.
Thus, the two dipoles on two chlorine atoms have similar strength and both on opposite direction of central Hg atom. Hence, both the dipole moments get cancel out each other being a HgCl2 is non – polar in nature.
How HgCl2 is non – polar?
The HgCl2 molecule has symmetrical arrangement of in its structure, as it has linear molecular shape and electron geometry. So, the electron cloud generates on two chlorine atoms which stretch this electron cloud in opposite direction of central Hg atom. Hence, HgCl2 is a non – polar molecule.
Is HgCl2 an acid or base?
HgCl2 is behaved as lewis acid, as it is capable of accept electron pairs from other lewis bases or chemical compounds.
Why HgCl2 is a lewis acid?
Lewis acids are the substance which contains empty orbitals and are able to accept electron pairs from other lewis bases. Here, the HgCl2 has the incomplete octet of central Hg atom. Thus it has empty orbitals to accept electrons and hence HgCl2 can behave as lewis acid.
How HgCl2 is a lewis acid?
HgCl2 has pKa value of 3.2 thus it shows more acidity in its character. Also it behaves as a lewis acid when it reacts with a base like ammonia it accepts electron pair from ammonia solution and form Hg-NH2 bond to form HgNH2Cl.
HgCl2 is an white solid crystalline compound and not an aqueous solution. But it can sparingly soluble in water and form aqueous solution. At pH 2 and 4.5 it can form an aqueous solution with HgCl2 when mixed in water. Also its solubility increases by adding chlorine solution to it.
Is HgCl2 ionic?
HgCl2 is not ionic compound rather it is a covalent compound. There are two covalent bonds between Hg and Cl atoms and there is no any positive or negative formal charge is present on HgCl2 molecule. Thus, it is a covalent compound and not ionic.
Is HgCl2 a precipitate?
HgCl2 when reacts with compounds like SnCl2 (stannous chloride) or KI (potassium iodide). When HgCl2 reacts with stannous chloride (SnCl2), the HgCl2 gets reduced as Hg and form Hg2Cl2.
No, HgCl2 is not a strong electrolyte because it is a weak electrolyte as it cannot form more ions when dissolved in water.
Why HgCl2 is weak electrolyte?
Electrolytes are those substance which when get mixed in water can dissociate and form ions to conduct electricity. The HgCl2 is a weak electrolyte, when it mixed in water it can form very less ions as it is sparingly soluble in water. Thus it is not a strong electrolyte but a weak electrolyte.
Conclusion:
Mercuric chloride (HgCl2) has total 16 valence electrons from the 4 are bonding electrons and remaining 12 electrons are non- bonding electrons. Thus it has two Hg-Cl covalent bonds and have total six lone electron pairs. It has zero formal charge. It has linear shape and geometry and sp hybridization and 180 degree bond angle.
Formic acid (HCOOH) has a central carbon (C) atom double-bonded to one oxygen (O) atom and single-bonded to a hydroxyl group (-OH) and a hydrogen (H) atom. The Lewis structure includes a C=O double bond, a C-O single bond, and an O-H single bond. Carbon contributes 4 valence electrons, each oxygen 6, and hydrogen 1, totaling 18 electrons. The molecule exhibits a trigonal planar geometry at the carbon with the C=O bond and a bent structure at the hydroxyl group. The molecule is polar, with significant electronegativity differences (C: 2.55, O: 3.44, H: 2.20), influencing its acidity and reactivity in organic chemistry.
Formic acid, also known as HCOOH, is a crucial compound in various chemical processes. Understanding the Lewis structure of HCOOH is essential for comprehending its molecular geometry, electron pair arrangement, and chemical bonding. In this article, we will delve into the intricacies of HCOOH’s Lewis structure, exploring its resonance structures, valence electrons, and molecular formula. By the end, you will have a comprehensive understanding of HCOOH’s molecular structure and its significance in the world of chemistry.
Definition of HCOOH (Formic Acid)
Formic acid, with the chemical formula HCOOH, is a colorless liquid with a pungent odor. It is the simplest carboxylic acid and is naturally found in the venom of certain ants and bees. Formic acid is widely used in various industries, including agriculture, textiles, and pharmaceuticals. It serves as a precursor for the production of other chemicals and is also utilized as a preservative and antibacterial agent.
Importance of Understanding HCOOH Lewis Structure
The Lewis structure of HCOOH provides valuable insights into its molecular properties and behavior. By examining the arrangement of valence electrons in the molecule, we can determine its molecular geometry, polarity, and reactivity. This knowledge is crucial for predicting the chemical reactions that formic acid can undergo and understanding its role in different chemical processes.
Overview of the Article Content
In this article, we will explore the Lewis structure of HCOOH in detail. We will begin by discussing the concept of valence electrons and their significance in determining the Lewis structure. Next, we will examine the steps involved in drawing the Lewis dot structure of HCOOH, highlighting the distribution of electrons and the formation of chemical bonds. We will also explore the resonance structures of formic acid and their implications. Finally, we will conclude by summarizing the key points discussed and emphasizing the importance of understanding HCOOH’s Lewis structure in the broader context of chemistry.
Now that we have set the stage, let’s dive into the fascinating world of HCOOH’s Lewis structure and unravel the mysteries of this compound’s molecular makeup.
HCOOH Lewis Structure: Polar or Nonpolar
The Lewis structure of a molecule provides valuable insights into its molecular geometry, electron distribution, and overall polarity. In the case of HCOOH, also known as formic acid, understanding its Lewis structure is crucial in determining whether it is a polar or nonpolar molecule.
Explanation of the concept of polarity
Before delving into the specifics of HCOOH’s Lewis structure, let’s first understand the concept of polarity. Polarity refers to the distribution of electrons within a molecule, which can result in regions of partial positive and partial negative charges. This distribution arises due to differences in electronegativity, the ability of an atom to attract electrons towards itself.
When two atoms with significantly different electronegativities bond together, the shared electrons are more likely to be found closer to the atom with the higher electronegativity. This creates an uneven distribution of charge, with the more electronegative atom acquiring a partial negative charge (δ-) and the less electronegative atom acquiring a partial positive charge (δ+). Such a molecule is said to be polar.
On the other hand, if the electronegativity difference between the atoms is negligible or non-existent, the shared electrons are equally distributed, resulting in a symmetrical electron cloud. In this case, the molecule is nonpolar, as there are no regions of partial positive or negative charges.
Analysis of the HCOOH molecule’s electron distribution
To determine the Lewis structure of HCOOH, we need to consider its molecular formula and the arrangement of its atoms. HCOOH consists of one carbon atom (C), one oxygen atom (O), and two hydrogen atoms (H). The molecular formula gives us a hint about the number of valence electrons each atom contributes to the molecule.
Carbon has four valence electrons, oxygen has six, and hydrogen has one each. Adding up the valence electrons, we get a total of 12 electrons for HCOOH. However, we need to account for the negative charge on the oxygen atom, which adds an additional electron.
To distribute the electrons, we start by connecting the atoms with single bonds. Carbon forms single bonds with both hydrogen atoms, leaving eight electrons remaining. We then place the remaining electrons around the oxygen atom, ensuring it satisfies the octet rule (having eight electrons in its valence shell).
Determination of whether HCOOH is polar or nonpolar
Now that we have determined the Lewis structure of HCOOH, we can analyze its electron distribution to determine its polarity. In the case of HCOOH, the oxygen atom is more electronegative than both carbon and hydrogen. As a result, the oxygen atom attracts the shared electrons towards itself, creating a partial negative charge (δ-) on the oxygen atom.
On the other hand, the carbon and hydrogen atoms have a partial positive charge (δ+) due to the electron density being pulled towards the oxygen atom. This uneven distribution of charge indicates that HCOOH is a polar molecule.
The polarity of HCOOH is further reinforced by the presence of the carbonyl group (-C=O), which contributes to the overall dipole moment of the molecule. The dipole moment is a measure of the separation of positive and negative charges within a molecule.
In conclusion, the Lewis structure of HCOOH reveals that it is a polar molecule due to the electronegativity difference between the oxygen and carbon/hydrogen atoms. The presence of a dipole moment further confirms its polarity. Understanding the polarity of HCOOH is essential in various chemical processes, as it influences its interactions with other molecules and its behavior in different environments.
Lewis Diagram for HCOOH
Lewis diagrams, also known as Lewis structures or Lewis dot structures, are graphical representations that show the arrangement of atoms and valence electrons in a molecule. They are named after the American chemistGilbert N. Lewis, who introduced this notation in 1916. Lewis diagrams are useful tools in understanding the chemical bonding and molecular geometry of a compound.
Explanation of Lewis diagrams and their purpose
Lewis diagrams are used to depict the valence electrons of atoms in a molecule and how they are shared or transferred between atoms to form chemical bonds. Valence electrons are the outermost electrons in an atom’s electron cloud and are responsible for the atom‘s chemical behavior. By representing these electrons as dots around the atomic symbol, Lewis diagrams provide a visual representation of how atoms interact with each other.
The purpose of Lewis diagrams is to provide a simplified representation of a molecule’s structure and bonding. They help chemists predict the shape and properties of molecules, as well as understand the types of chemical bonds present. Lewis diagrams also aid in determining the presence of lone pairs of electrons, which play a crucial role in molecular reactivity.
Step-by-step process for drawing the Lewis diagram for HCOOH
Drawing the Lewis diagram for HCOOH, which is the molecular formula for formic acid, involves several steps. Let’s go through them one by one:
Determine the total number of valence electrons: In formic acid (HCOOH), hydrogen (H) has one valence electron, carbon (C) has four valence electrons, and oxygen (O) has six valence electrons. Since there are two hydrogen atoms, one carbon atom, and two oxygen atoms in formic acid, the total number of valence electrons is calculated as follows:
Hydrogen (H): 2 atoms x 1 valence electron = 2 valence electrons
Carbon (C): 1 atom x 4 valence electrons = 4 valence electrons
Identify the central atom: In formic acid, carbon (C) is the central atom since it is less electronegative than oxygen (O) and can form multiple bonds.
Connect the atoms with single bonds: Place a single bond between the central carbon atom and each of the surrounding atoms (hydrogen and oxygen). Each bond consists of two electrons.
Distribute the remaining valence electrons: After connecting the atoms with single bonds, distribute the remaining valence electrons around the atoms to satisfy the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons (except for hydrogen, which only needs two valence electrons).
Start by placing lone pairs of electrons around the outer atoms (hydrogen and oxygen) until they each have a complete octet (two valence electrons for hydrogen).
Place any remaining valence electrons on the central atom (carbon) to complete its octet.
Check for octet rule compliance: Ensure that all atoms (except hydrogen) have eight valence electrons or a complete octet. If not, you may need to form multiple bonds or expand the octet of the central atom.
Description of the resulting Lewis diagram for HCOOH
The Lewis diagram for formic acid (HCOOH) shows the arrangement of atoms and valence electrons in the molecule. Here is the resulting Lewis diagram for HCOOH:
Atom
Valence Electrons
H
2
C
4
O
6
H: . C: . O: .
H – C – O – O – H
In the Lewis diagram, the dots represent the valence electrons of each atom. The single bonds between the atoms are represented by lines (-). The central carbon atom is bonded to two oxygen atoms and two hydrogen atoms. The oxygen atoms each have two lone pairs of electrons, while the hydrogen atoms have no lone pairs.
The Lewis diagram for formic acid provides a visual representation of the molecule’s structure and bonding. It helps us understand how the atoms are connected and how the valence electrons are distributed. This information is essential in predicting the molecule’s shape, polarity, and reactivity.
Resonance in HCOOH Lewis Structure
Resonance is a fundamental concept in chemistry that helps us understand the behavior of molecules and their bonding patterns. In the case of the HCOOH molecule, also known as formic acid, resonance plays a crucial role in determining its structure and properties.
Definition of Resonance in Chemical Structures
Resonance refers to the phenomenon where a molecule can have multiple valid Lewis structures that differ only in the placement of electrons. These structures, called resonance structures, are not separate entities but rather contribute to the overall description of the molecule. Resonance allows us to represent the delocalization of electrons within a molecule, leading to enhanced stability.
Explanation of How Resonance Applies to the HCOOH Molecule
To understand how resonance applies to the HCOOH molecule, let’s first examine its Lewis dot structure. HCOOH consists of a carbon atom (C) bonded to two oxygen atoms (O) and one hydrogen atom (H). The carbon atom is double-bonded to one of the oxygen atoms and single-bonded to the other oxygen atom. The hydrogen atom is attached to the carbon atom.
In the Lewis dot structure, we represent the valence electrons of each atom as dots. Carbon has four valence electrons, oxygen has six, and hydrogen has one. By following the octet rule, we can distribute the electrons around the atoms to form the initial structure.
However, the Lewis dot structure alone does not fully capture the electronic distribution in the molecule. This is where resonance comes into play.
Description of the Different Resonance Structures of HCOOH
In the case of HCOOH, there are two resonance structures that contribute to its overall description. These structures arise from the movement of electrons within the molecule.
In the first resonance structure, the double bond between the carbon and oxygen atoms can be shifted to the other oxygen atom. This results in a negative charge on the oxygen atom that gained the double bond and a positive charge on the carbon atom. The hydrogen atom remains bonded to the carbon atom.
In the second resonance structure, the double bond can be shifted to the other oxygen atom, similar to the first structure. However, in this case, the hydrogen atom is attached to the oxygen atom that gained the double bond. The carbon atom carries a positive charge.
The actual electronic distribution in the HCOOH molecule is a combination, or hybrid, of these two resonance structures. The electrons are delocalized, meaning they are not confined to a specific bond but are spread out over the molecule. This delocalization enhances the stability of the molecule.
To summarize, resonance in the HCOOH molecule allows for the delocalization of electrons, resulting in multiple valid Lewis structures. The actual electronic distribution is a hybrid of these structures, leading to enhanced stability. Understanding resonance is crucial in comprehending the behavior and properties of molecules, and it plays a significant role in the study of chemical bonding.
HCOOH Lewis Structure and Formal Charge
Formic acid, with the chemical formula HCOOH, is a simple organic compound commonly found in nature. Understanding its Lewis structure and formal charge is crucial in comprehending its chemical properties and behavior. In this section, we will delve into the definition of formal charge in Lewis structures, calculate the formal charge for each atom in the HCOOH molecule, and analyze the formal charges in the HCOOH Lewis structure.
Definition of Formal Charge in Lewis Structures
In Lewis structures, formal charge is a concept used to determine the distribution of electrons within a molecule. It helps us understand the stability and reactivity of a compound by evaluating the charge on individual atoms. Formal charge is calculated by comparing the number of valence electrons an atom possesses in its neutral state with the number of electrons it actually has in the Lewis structure.
Calculation of Formal Charge for Each Atom in the HCOOH Molecule
To calculate the formal charge for each atom in the HCOOH molecule, we need to follow a simple formula. The formal charge of an atom is determined by subtracting half the number of bonding electrons from the total number of valence electrons. Mathematically, the formula can be represented as:
Analysis of the Formal Charges in the HCOOH Lewis Structure
From the calculated formal charges, we can analyze the distribution of electrons in the HCOOH Lewis structure. The Lewis structure of HCOOH can be represented as follows:
H
|
C=O
|
H
In this structure, the carbon atom (C) has a formal charge of +1, while both oxygen atoms (O) have a formal charge of -1. The hydrogen atoms (H) have a formal charge of 0. The formal charges indicate that the carbon atom is electron-deficient, while the oxygen atoms carry a negative charge.
The distribution of formal charges in the HCOOH molecule suggests that the carbon atom tends to attract electron density, making it a positively charged center. On the other hand, the oxygen atoms have an excess of electron density, making them negatively charged centers. This charge distribution influences the chemical bonding and reactivity of formic acid.
Understanding the formal charges in the HCOOH Lewis structure is essential for predicting the molecule’s behavior in various chemical reactions. It helps us comprehend the stability and reactivity of formic acid, enabling us to make informed decisions in the field of organic chemistry.
In the next section, we will explore the molecular geometry and resonance structures of HCOOH, further enhancing our understanding of this fascinating compound.
HCOOH Lewis Structure and Bond Angle
The Lewis structure of HCOOH, also known as formic acid, provides valuable insights into its molecular geometry and bond angles. Understanding the arrangement of atoms and the bond angles in a molecule is crucial in predicting its chemical behavior and properties.
Explanation of Bond Angles and Their Significance
Bond angles refer to the angle formed between two adjacent bonds in a molecule. They play a vital role in determining the overall shape of a molecule, which, in turn, affects its reactivity and physical properties. The bond angle is influenced by several factors, including the number of electron pairs surrounding the central atom and the repulsion between these electron pairs.
Determination of Bond Angles in the HCOOH Molecule
To determine the bond angles in the HCOOH molecule, we need to examine its Lewis structure. The Lewis structure of HCOOH consists of one carbon atom (C), one oxygen atom (O), and two hydrogen atoms (H). The carbon atom is the central atom, bonded to both the oxygen and hydrogen atoms.
In the Lewis structure, we represent the valence electrons of each atom using dots. Carbon has four valence electrons, oxygen has six, and hydrogen has one. The carbon atom forms a double bond with the oxygen atom, and each hydrogen atom forms a single bond with the carbon atom.
Description of the Bond Angles in the HCOOH Lewis Structure
In the HCOOH Lewis structure, the carbon atom is surrounded by three regions of electron density: the double bond with oxygen and the two single bonds with hydrogen. These regions of electron density repel each other, causing the molecule to adopt a bent or V-shaped geometry.
The bond angle between the two hydrogen atoms (H-C-H) in HCOOH is approximately 109.5 degrees. This angle is slightly less than the ideal tetrahedral angle of 109.5 degrees due to the repulsion between the electron pairs in the molecule. The bond angle between the carbon and oxygen atoms (C=O) is approximately 120 degrees, reflecting the presence of a double bond.
It is important to note that the Lewis structure of HCOOH does not accurately represent the actual distribution of electrons in the molecule. The molecule exhibits resonance, meaning that the double bond can shift between the carbon and oxygen atoms. This resonance structure influences the bond angles and contributes to the stability of the molecule.
In conclusion, understanding the Lewis structure and bond angles of HCOOH provides valuable insights into its molecular geometry and chemical behavior. The bent shape of the molecule, along with the bond angles, influences its reactivity and physical properties. By studying the Lewis structure, we can gain a deeper understanding of the structure-function relationship in organic molecules.
HCOOH Lewis Structure and Hybridization
The Lewis structure of a molecule provides valuable insights into its molecular geometry and bonding patterns. In the case of HCOOH, also known as formic acid, understanding its Lewis structure and hybridization is crucial to comprehend its chemical properties and behavior.
Definition of Hybridization in Chemical Bonding
Before delving into the hybridization of the carbon atom in the HCOOH molecule, let’s first understand the concept of hybridization in chemical bonding. Hybridization refers to the mixing of atomic orbitals to form new hybrid orbitals that participate in bonding. This process occurs when atoms form covalent bonds by sharing electron pairs.
Hybridization allows for the formation of stronger and more stable bonds, leading to the creation of unique molecular structures. By combining different types of atomic orbitals, such as s, p, and d orbitals, hybrid orbitals are formed, which have specific shapes and orientations.
Analysis of the Hybridization of the Carbon Atom in the HCOOH Molecule
In the HCOOH molecule, the carbon atom is bonded to two hydrogen atoms (H) and one oxygen atom (O). To determine the hybridization of the carbon atom, we need to consider its valence electrons and the number of electron pairs around it.
Carbon has four valence electrons, and in the HCOOH molecule, it forms two single bonds with two hydrogen atoms and a double bond with the oxygen atom. This results in a total of three electron pairs around the carbon atom.
To accommodate these three electron pairs, the carbon atom undergoes sp2 hybridization. In sp2 hybridization, one s orbital and two p orbitals from the carbon atom combine to form three sp2 hybrid orbitals. These hybrid orbitals are arranged in a trigonal planar geometry, with bond angles of approximately 120 degrees.
Description of the Hybridization in the HCOOH Lewis Structure
Now that we understand the hybridization of the carbon atom in the HCOOH molecule, let’s examine its Lewis structure. The Lewis structure of HCOOH represents the arrangement of atoms and valence electrons in the molecule.
To draw the Lewis structure of HCOOH, we start by placing the carbon atom in the center, surrounded by the hydrogen and oxygen atoms. The carbon atom is connected to the two hydrogen atoms through single bonds and to the oxygen atom through a double bond.
The Lewis structure of HCOOH can be represented as follows:
H H
| |
H-C=O-H
|
H
In this structure, the carbon atom is sp2 hybridized, with three sp2 hybrid orbitals forming sigma bonds with the hydrogen and oxygen atoms. The remaining p orbital on the carbon atom forms a pi bond with the oxygen atom, resulting in the double bond.
It’s important to note that the Lewis structure of HCOOH is a simplified representation, and the molecule exhibits resonance structures due to the delocalization of electrons. This resonance contributes to the stability and reactivity of formic acid.
Understanding the hybridization and Lewis structure of HCOOH provides a foundation for comprehending its molecular geometry, electron distribution, and chemical behavior. By analyzing these aspects, scientists can gain insights into the properties and reactions of formic acid, contributing to various fields such as organic chemistry, biochemistry, and materials science. Conclusion
In conclusion, understanding the Lewis structure of HCOOH is crucial for comprehending its chemical properties and reactions. By examining the arrangement of atoms and electrons in this molecule, we can gain insights into its polarity, acidity, and reactivity. The Lewis structure of HCOOH reveals that it consists of a central carbon atom bonded to two oxygen atoms and two hydrogen atoms. The carbon atom forms a double bond with one oxygen atom and a single bond with the other oxygen atom. The hydrogen atoms are attached to the carbon atom. This structure helps us understand why formic acid is a polar molecule, with the oxygen atoms exerting a stronger pull on electrons than the hydrogen atoms. Additionally, the presence of the carboxylic acid functional group in HCOOH contributes to its acidic nature. The Lewis structure also provides a foundation for predicting and understanding the chemical reactions that formic acid can undergo. Overall, the Lewis structure of HCOOH serves as a valuable tool in studying and understanding the properties and behavior of this important organic compound.
Frequently Asked Questions
1. What is the Lewis structure for formic acid (HCOOH)?
The Lewis structure for formic acid (HCOOH) consists of a carbon atom bonded to two oxygen atoms and two hydrogen atoms. The carbon atom is double bonded to one oxygen atom and single bonded to the other oxygen atom. The hydrogen atoms are single bonded to the carbon atom.
2. Is the Lewis structure of formic acid (HCOOH) polar or nonpolar?
The Lewis structure of formic acid (HCOOH) is polar. This is because the oxygen atom, which is more electronegative than carbon and hydrogen, pulls the electron density towards itself, creating a partial negative charge on the oxygen atom and a partial positive charge on the hydrogen atoms.
3. What is the molecular geometry of formic acid (HCOOH)?
The molecular geometry of formic acid (HCOOH) is bent or V-shaped. The carbon atom is the central atom, and the two oxygen atoms and two hydrogen atoms are bonded to it. The presence of two lone pairs of electrons on the oxygen atom causes the molecule to adopt a bent shape.
4. How many valence electrons are there in formic acid (HCOOH)?
Formic acid (HCOOH) contains a total of 12 valence electrons. The carbon atom contributes 4 valence electrons, each oxygen atom contributes 6 valence electrons, and each hydrogen atom contributes 1 valence electron.
5. What is the resonance structure of formic acid (HCOOH)?
Formic acid (HCOOH) exhibits resonance, meaning that the double bond can be delocalized between the carbon and oxygen atoms. This results in two resonance structures, where the double bond alternates between the two oxygen atoms.
6. What is the molecular formula of formic acid?
The molecular formula of formic acid is HCOOH. It represents the composition of the molecule, indicating that it contains one carbon atom, one oxygen atom, and two hydrogen atoms.
7. What is the Lewis dot structure for formic acid (HCOOH)?
The Lewis dot structure for formic acid (HCOOH) shows the arrangement of atoms and valence electrons. It consists of a carbon atom in the center, with two oxygen atoms and two hydrogen atoms bonded to it. The valence electrons are represented as dots around the atomic symbols.
8. How does chemical bonding occur in formic acid (HCOOH)?
In formic acid (HCOOH), chemical bonding occurs through the sharing of electrons between atoms. The carbon atom forms covalent bonds with the two oxygen atoms and the two hydrogen atoms, resulting in a stable molecule.
9. What breaks when CH3COOH(l) is dissolved in water?
When CH3COOH(l) (acetic acid) is dissolved in water, the covalent bonds between the carbon, hydrogen, and oxygen atoms do not break. However, the hydrogen bonding occurs between the acetic acid molecules and water molecules, leading to the formation of a solution.
10. Why is the blogul lui Atanase not about pizza?
The blogul lui Atanase is not about pizza because it focuses on a different topic or subject matter. The specific reasons for this can vary, but it is likely that the author has chosen to write about something other than pizza.
HCl is the chemical formula of hydrochloric acid. Here we are discussing about HCl lewis structure, characteristics and some quick facts.
Hydrochloric acid (HCl) is a liquid and hydrogen chloride (HCl) is a gas. Hydrochloric acid is in watery liquid form with no colour and having pungent smell. Hydrogen chloride is a yellowish inflammable gas and corrosive in nature. HCl is mainly consists of one hydrogen atom and one chlorine atom in its structure. It has synonyms like muriatic acid and chloro – hydric acid.
How to draw HCl lewis structure?
Lewis structure can be draw with the help of following steps:
Predict the group position of H and Cl atoms in periodic table.
Evaluate total valence electrons of HCl lewis structure by adding valence electrons of H and Cl atoms.
More electronegative atom is being central atom but in HCl it is diatomic so it gets placed besides each other.
Form single covalent bond between H and Cl atoms.
Remaining valence electrons goes to chlorine atom and being non- bonding electrons.
Check the complete octet of atoms and mark lone electron pairs.
Recognize the shape, hybridization and bond angle of the HCl lewis structure.
HCl lewis structure
HCl valence electrons
In HCl lewis structure, the hydrogen atom comes under 1st periodic table group and chlorine atom comes under 17th periodic table group. Hence, the H and Cl atoms of HCl lewis structure have 1 and 7 valence electrons in its outermost valence shell. Let first calculate the total valence electrons present on HCl lewis structure.
Hydrogen atom of HCl has valence electrons = 01
Chlorine atom of HCl has valence electrons = 07
Total valence electrons of HCl lewis structure = 01 (H) + 07 (Cl) = 08
Therefore the total valence electrons on HCl lewis structure are eight.
Total electron pairs on HCl lewis structure can be predict by dividing all valence electrons by two.
Total electron pairs on HCl = 8 / 2 = 4
Hence, total electron pairs on HCl are four.
Eight Valnce electrons on HCl lewis
HCl lewis structure octet rule
HCl lewis structure there are eight total valence electrons are present out of which two electrons are bond pairs creating a covalent bond between hydrogen and chlorine atoms. So, now we have left more six valence electrons for further bonding or sharing.
H atom cannot contain more than two electrons as it already had two bond pair electrons so the hydrogen has complete octet with two electrons as per its capacity. The remaining six electrons now get place on chlorine atom as non- bonding electrons.
Therefore chlorine atom now have total eight electrons surrounding it i.e. two bonding electrons and six non- bonding electrons. Hence the chlorine atom also have complete octet. Thus both H and Cl atoms of HCl lewis structure has complete octets.
HCl lewis structure comprises of eight valence electrons in its molecule. From them two electrons are bond pair electrons and on chlorine atom non- bonding electrons are six. If we pair these non- bonding electrons they are being three lone pair electrons. Thus, the HCl lewis structure contains three lone electrons pairs present on chlorine atom of HCl molecule.
Lone electron pairs on HCl lewis structure
HCl lewis structure formal charge
If any lewis structure has some formal charge then that lewis structure is considered to be a stable structure. Formal charge evaluation is done with the following formula.
Resonance structure of HCl lewis structure of molecule is not possible, as there is no multiple bonds in its structure. HCl lewis structure has only one single covalent bond and there is no formation of double or triple bond in the structure.
Also HCl lewis structure has zero formal charge, no negative or positive formal charge is present on it. So there is no movement of electrons is possible in HCl lewis structure to form multiple bonds. Thus no resonance structure of HCl molecule is possible.
HCl lewis structure shape
HCl lewis structure is composed of two elements i.e. H and Cl attached with single covalent bond and having three lone electron pairs on Cl atom. To accord with VSEPR theory HCl lewis structure belongs to AXE3 generic formula.
Here, A represents central atom, x represents bonding atoms with central atom and E represents lone pair electrons on bonding neighbouring atoms. Thus the HCl lewis structure contains molecular shape linear and electron geometry tetrahedral.
HCl hybridization
As the HCl lewis structure belongs to VSEPR theory’s AXE3 generic formula, by which it has molecular shape linear and electron geometry tetrahedral. Therefore, HCl lewis structure contains sp3 hybridization.
HCl lewis structure angle
As the HCl lewis structure has linear shape (molecular shape) and tetrahedral geometry (electron geometry) as it has AXE3 generic formula of VSEPR theory. Hence HCl lewis structure is sp3 hybridised and has bond angle of 109.5 degree.
HCl solubility
HCl (hydrochloric acid) is soluble in:
Water
Ethanol
Methanol
Is HCl soluble in water?
Yes, HCl is soluble in water. When HCl get mixed with water it get dissociates as H+ and Cl- ions and hence forming hydronium ions.
Why HCl soluble in water?
When HCl (hydrochloric acid) dissolved into water it forms an exothermic reaction and evolves some heat. HCl gets dissociates into water as H+ (hydrogen ion or proton) and Cl- ions and hence there is increase of concentration of H+ ions in water and thus forma hydronium ion (H3O+).
How HCl soluble in water?
If we mixed HCl in water (not water in HCl as it can burst the beaker), the H atom present in HCl acid forms an hydrogen bond with oxygen atom of H2O (water) molecule. Hence, HCl on miscible with water it get ionizes as H+ and C- ions to form H3O+ (hydronium) ion.
HCl → H+ + Cl-
HCl + H2O → H3O+ + Cl-
Hydrogen bond formation between HCl and H2O
Is HCl an electrolyte?
Yes, HCl (hydrochloric acid) is an electrolyte, instead it is an strong electrolyte as it is a strong acid and when mixed with water it can ionizes as H+ and Cl- ions in water aqueous solution.
Why HCl is electrolyte?
Hydrochloric acid is an strong electrolyte. Electrolyte is an compound on mixing with water produce ions and conducts electricity. HCl can behaves as electrolyte as when it get mixed in water it get dissociates into positively charge H+ ion (cation) and negatively charged Cl- ion (anion) and hence conducts electricity in the solution.
How HCl is electrolyte?
When HCl (hydrochloric acid) on mixing with h2O (water) it get ionizes as cation H+ ion and anion Cl- ion. When the outer electric current is applied on electrolytic solution of HCl and H2O, the hydrogen ions and chlorine ions produced into the solution. So, the H+ ions (cations) going towards cathode (positively charges) and the Cl- ions (anions) going towards anode (negatively charged).
Is HCl a strong electrolyte?
Yes, HCl is an strong electrolyte. The compounds on dissolving in water produc ions and conduct electricity are electrolytes. Strong electrolytes are the substance which can produce more ions into solution when dissolved into water to conduct electricity. The HCl (hydrochloric acid) when dissolved in water produce more H+ and Cl- ions and also forms H3O+ ions and on applying electricity it can conduct electricity.
Is HCl acidic or basic?
Yes, HCl is an acidic compound. HCl behaves as an acid, when it get mixed with H2O, HCl get dissociates as H+ and Cl- ions. The compounds which can release or donates H+ ions on mixing with water are known to be acids.
Why HCl is acidic?
When HCl added in water it get dissociates into water as H+ and Cl- ions. So, there is increase of H+ (hydrogen) ions in the water HCl solution and hence it can act as an acidic compound. It can dissociated mostly in water thus act as a strong acid.
How HCl is acidic?
HCl on adding in water get ionized as H+ and Cl- ions and further the H+ ions joins with H2O molecule to form H3O+ (hydronium) ion and therefore HCl can act as acid
HCl + H2O → H3O+ + Cl-
Is HCl a strong acid?
Yes, HCl is a strong acid. When HCl (hydrochloric acid) get mixed in water, which is then ionises or dissociates in H+ and Cl- ions. It forms more number of H+ ions in water solution and forming hydrogen bonds. It forms exothermic reaction producing heat. Hence, HCl is a strong acid.
Is HCl polyprotic acid?
No, HCl is not an polytprotic acid instead it is an mono- protic acid. Monoprotic acids are those which contain only one hydrogen (proton or H+) atom in the molecule. Polyprotic acids are those acids which has more than one hydrogen (proton or H+) atoms in the molecule.
In HCl (hydrochloric acid) has only one hydrogen atom and one chlorine atom present in it. Hence, HCl acid when reacting with water will release or ionize its one proton i.e. hydrogen atom. Hence, HCl is monoprotic and not polyprotic.
Is HCl a lewis acid?
Yes, HCl is an lewis acid. The acids which have ability to accept lone pair electrons are lewis acids. Lewis acids are the substances which have at least an empty valence shell orbital in its atoms. HCl can act as lewis acid as it is capable of gaining protons from water when mixed in water.
Why HCl is a lewis acid?
HCl can act as lewis acid as it is capable to gain or accept lone pair of electrons.
Is HCl an arrhenius acid?
Yes, HCl is an Arrhenius acid. The acids which can increase the H+ ion concentration are considered as Arrhenius acids.
Why HCl an Arrhenius acid?
HCl when added to water, the bond of HCl molecule gets break and forms H+ and Cl- ions in that aqueous solution. Hence, HCl acid can increase the H+ ions concentration in water by liberating H+ ions in it.
HCl → H+ + Cl-
How HCl an Arrhenius acid?
Hydrochloric acid on mixing with water breaks down as H+ and Cl- ions and hence the H+ ion concentration increases in water. Thus, these H+ ions get added to H2O to form H3O+ and Cl- ions.
HCl + H2O → H3O+ + Cl-
Is HCl polar or nonpolar?
Hydrochloric acid (HCl) is polar in nature. HCl is polar molecule as there is more electronegativity difference within hydrogen and chlorine atoms.
Why HCl is polar?
The electronegativity value of hydrogen and chlorine atoms is 2.20 and 3.16 respectively. Hence, the H and Cl atom has electronegativity difference of 0.96. This value is much greater than prescribed value by Paulings of 0.4.
As the HCl acid has more electronegativity difference value of 0.4 so it is polar in nature. Even the Chlorine atom is more electronegative than hydrogen atom, therefore the electron cloud pulls towards chlorine atom.
Therefore, HCl acid consists of electron distribution which is not equal on both Hydrogen and Chlorine atoms and thus it has whole dipole moment on HCl molecule causing partial positive charge on Hydrogen atom and partial negative charge on Chlorine atoms in HCl molecule.
How HCl is polar?
HCl acid has uneven electrons distribution thus it has asymmetrical arrangement of atoms in its structure. So, the HCl molecule represents molecular shape which is linear and electron geometry which is tetrahedral due to irregular distribution of electrons in it and therefore, HCl acid is polar.
Is HCl linear?
Of course, HCl is linear in shape. Accordance to VSEPR theory’s AXE3 generic formula, the HCl acid contains linear molecular shape. The HCl lewis structure is an diatomic molecule consists of H and Cl atoms which are attached with a single covalent bond in straight single line. Know more about Uric Acid Structure
So, the one electron of hydrogen atom shared with chlorine atom and creates single covalent bond in HCl structure and thus it has linear structure.
Is HCl paramagnetic or diamagnetic?
Hydrochloric acid (HCl) is a diamagnetic molecule as it has all paired electrons in its structure.
Why HCl is diamagnetic?
HCl has eight total valence electrons from which one is bond pair electron within H and Cl atoms by sharing one electron of H and one electron of Cl atom. Hence, HCl acid has one bond pairs and three lone electron pairs. As the HCl acid has all paired electrons so it is diamagnetic in nature.
How HCl is diamagnetic?
Diamagnetic molecules have negative value of magnetic susceptibility. The HCl acid has negative value of magnetic susceptibility so it is diamagnetic in nature. Also when magnetic field is applied externally on HCl acid it can repel in opposite direction of magnetic field and hence it is diamagnetic in nature.
HCl boiling point
Hydrochloric acid (HCl) has 110 degree Celsius boiling point. The temperatures at which the liquid substances get converted into gases are known as boiling point of that substance. HCl acid has the higher boiling point of 110 degree Celsius as it is polarised in nature and have large size.
Why HCl has higher boiling point?
Hydrochloric acid on reaction with water forms hydrogen bonds with H2O molecules. So, there are strong intermolecular forces forming with hydrogen and chlorine atoms of HCl acid.
These intermolecular forces are hydrogen bonds within HCl and H2O molecules and which is not easy to break down this bonds. HCl is polar molecule and thus it has dispersion forces with greater degree which can operates HCl acid and hence having higher boiling point.
Is HCl diprotic?
No, HCl is not an diprotic acid as it is a mono- protic acid. Diprotic acids are those which contains two hydrogen (H+) atoms, they are also known to be polyprotic acids. Monoprotic acids contains only one hydrogen aton in its structure. In HCl acid, it has only one hydrogen atom present in its structure. So, they are not considered to be diprotic as it is a mon- protic acid.
Is HCl ionic or covalent?
Hydrochloric acid (HCl) is covalent in nature also it can behaves as polar covalent in naure.
Why HCl is polar covalent molecule?
Hydrochloric acid (HCl) contains hydrogen and chlorine atoms having 2.2 and 3.16 electronegativity values. So, the electronegativity difference between H and Cl atoms is 0.9. This value is comes under the prescribed value of electronegativity difference for bonding within atoms from 2.0 to 0.5.
Hence, as per this consideration the HCl acid is a polar covalent, as it has 0.9 electronegativity difference value which comes under polar covalent prescribed value of 2.0 to 0.5. Thus, HCl is a polar covalent acid and not ionic in nature.
How HCl is covalent or polar covalent molecule?
The HCl acid contains H and Cl atoms in its molecule. The H atoms have one valence electron and Cl atom has 7 valence electrons in their outermost valence shell orbitals. Here, in HCl both H and Cl atoms are sharing one – one electron to each other to make a single covalent bond which is not a pure covalent bond.
This covalent bond is an strong bond but showing polar nature. HCl is being an polar covalent acid as it has uneven electron sharing within H and Cl atoms. Further the Cl is more electronegative than hydrogen atom and thus the electron density creates on chlorine atom of HCl acid. Therefore, HCl is polar covalent acid.
Is HCl amphiprotic?
No, HCl is not amphiprotic acid. The compound which can act both as acid or bases are known to be amphoteric or amphiprotic compounds.
Why HCl is amphiprotic?
HCl is an strong acid and do not behave both as acid and a base. If the HCl acid get reacts with a base it will donate proton and produce a conjugate acid. HCl acid cannot gain or accept proton on reaction with base. Thus HCl do not show any basic nature and it is not amphiprotic acid.
How HCl is amphiprotic?
According to acid – base theory of Bronstead – Lowry, the compounds which can release protons to base and form conjugate acids are known as acids. Similarly the compounds which can gain protons to produce conjugate base are known as base.
If HCl added to base like H2O (water) or NH3 (ammonia), it can donate proton to basic substance (NH3 or H2O) and produce conjugate acids such as hydronium ion or ammonium ion. But HCl do not accept protons from other basic substances. Thus, HCl is not amphiprotic.
Is HCl binary or ternary?
HCl is an binary acid. The compounds or molecules which have to non – metallic atoms present in its structure are known as binary compounds. In HCl, the non-metal H forms a bond with another non-metal Cl to form HCl molecule.
Why HCl is binary?
HCl acid contains two atoms mainly which are non-metals. So, the HCl molecule has one H and one Cl atoms and both are non-metals. Thus, the HCl acid is an binary molecule.
How HCl is binary?
Binary acids are the acids in which the hydrogen which are non-metal is linked with another non-metal atom. Thus in HCl, the H atom is linked with Cl which is also non-metal atom. Here, Bi meaning two, thus two non-metals are available on HCl and therefore, it is binary acid.
Is HCl balanced?
No, basically HCl is not balanced equation. To balance the HCl reaction equation we have to adjust same number of elements on both sides of reaction. HCl acid is produced by reaction between hydrogen gas (H2) and chlorine (Cl2). Here, H2 is an reducing agent and Cl2 is an oxidising agent.
H2 (g) + Cl2 (aq) → HCl
The reaction seen above is not balanced equation as the atoms on reactant side (H2 + Cl2) are not equal to the atoms on product side (HCl). Hence we have to add 2 above HCl of product side to make equal number of atoms on both sides.
H2 + Cl2 → 2HCl
Therefore, now the above HCl formation reaction is balanced equation.
Is HCl conductive?
Yes, HCl is conductive acid. HCl on mixing with water produced ions and hence conducts electricity. Thus HCl is conductive molecule.
Why HCl is conductive?
Hydrochloric acid (HCl) when mixed with water, it donates H+ ions in H2O solution and creates hydrogen bonds with water molecules. Hence, HCl acid is able to produce ion on mixing with water and thus can conduct electricity.
How HCl is conductive?
Hydrochloric acid (HCl) composed of two non-metal atoms i.e hydrogen atom and chlorine atom. So, the hydrochloric acid acts as an acid by losing H+ ions in water solution. Also it creates h+ and Cl- ions in wate(aqueous solution).
As the hydrogen(H+) ions joined to H2O molecule to produce hydronium (H3O+) ions. These ions are flowing or moving towards cathods and anode to conduct electricity in the aqueous solution. Therefore, HCl can acts as strong acid or strong electrolyte which can conduct electricity.
HCl + H2O → H3O+ + Cl-
Is HCl conjugate base?
HCl is an produce conjugate base on reaction with lewis base. Generally HCl whne reacts with base to form acid-base reaction to produce a conjugate base.
Why HCl is conjugate base?
Hydrochloric acid can easily donates its protons (H+ ions) when reacts with base. As the basic substance can accept H+ ions and thus, it can form higher products with positive charge. Hence HCl can produce conjugate base.
How HCl is conjugate base?
HCl on reaction with ammonia (NH3) which is an lewis base, the HCl acid can lose H+ ions to ammonia molecule. Hence, it can form ammonium ion (NH4+) and Cl- ions as a product in this acid-base reaction. In this reaction, Cl- ions are formed which is a conjugate base.
HCl + NH3 → NH4+ + Cl- (Cl- = conjugate base)
Is HCl corrosive?
Yes, HCl is corrosive acid. Hydrochloric acid on mixing with water forms H3O+ ions and thus on contact with water it is being corrosive.
Why HCl is corrosive?
HCl acid on reaction with H2O get dissociates as H+ and Cl- ions. HCl is an strong acid which are able to form more H+ ions in H2O solution. So, because of the increasing H+ ions in the aqueous solution the HCl acid has lesser pH value (less than 4 or 7 pH). Therefore, the pH value of HCl acid is 3.5 and thus it is corrosive an acid.
How HCl is corrosive?
When strong acids like hydrochloric acid (HCl) on mixing with H2O and it ionize as H+ and Cl- ions and thus there is increase in H+ ion concentration in aqueous solution. Hence, HCl acid will form H3O+ ions in aqueous solution.
These H3O+ ions get reduced on contact with metal surface and thus create corrosion.The corrosive nature of acids can measure the acids capacity to donate H+ ions by acid dissociation constant (pKa). The HCl acid has -5.9 pKa value and thus HCl is corrosive.
Is HCl concentrated?
Yes, hydrochloric acid is a concentrated acid. The acids which are in pure form or the acids have more concentration in water or the acids which can increase the H+ ion concentration in water are known as concentrated acids.
HCl acid on mixing with water ionizes as H+ and Cl- ions and also form H3O+ ion. Hence, HCl acid can increase concentration of H+ ions in water that is why it is an concentrated acid.
Is HCl solid liquid or gas?
HCl is present both in gaseous and liquid form. HCl in pure form is a gas known as hydrogen chloride. Hydrogen chloride only forms H+ and Cl- ions on ionization. When hydrogen chloride (HCl) gas bubbled in H2O, it forms aqueous HCl solution known as hydrochloric acid.
The hydrochloric acid on further reaction with water forms H3O+ ions. Thus, HCl (hydrochloric acid) is an liquid. So, HCl (hydrogen chloride) is gas and HCl (hydrochloric acid) is a liquid.
Is HCl hygroscopic?
Yes, HCl acid is hygroscopic acid. The molecules or acids which can absorbs moisture from atmosphere or air are known as hygroscopic compounds. The hygroscopic nature of any compound can change its physical properties like boiling point, melting point, etc. Thus, HCl acid also absorbs moisture from atmosphere and hence it is hygroscopic in nature.
Is HCl hydrogen bonding?
HCl (hydrochloric acid) forms hydrogen bond on added to water (H2O). If HCl mixed with H2O it ionizes as h+ and Cl- to produce H3O+ ions in aqueous solution. Here,H atom of HCl forms hydrogen bond with more electronegative O atom of H2O molecule.
HCl + H2O → H3O+ + Cl-
Is HCl metal or non-metal?
HCl is an non – metallic acid. In HCl aicd there are two non – metallic atoms are present i.e. hydrogen and chlorine atoms. Thus HCl is non – metallic acid due to presence of two non – metals. Also pure form of HCl gas on adding to water forms aqueous solution hydrochloric acid. Hence, Hcl is non – metallic acid.
Is HCl neutral?
No HCl is not neutral substance. HCl is an acid thus it is an acidic substance. HCl can form H+ ions on mixing with water. It also has polar covalent bonds due to which the electron cloud creates on more electronegative chlorine atom. Hence there is rise of some partial posistive charge on H atom and partial negative charge on Cl atom. Thus, HCl is and acidic compound and not neutral.
Is HCl a nucleophile?
No, hCl is not an nucleophile. Nucleophilic substances are those which are electron rich and able to donate electron pairs. They are basically lewis base and neutral compounds or negatively charged species. Rather, HCl is an electrophile which can gain electrons.
Why HCl is not a nucleophile?
HCl is an electrophile due to its capacity to gain electrons and lose protons. Thus, they are electron loving compounds which can gain or accepts electrons from other species. Generally electrophiles are lewis acids, positively charged compounds or neutralmolecules.
How HCl is not a nucleophile?
HCl is basically electrophile in nature which can give its hydrogen atoms to make new bond with other molecules by gaining electrons from them. Ex: If ethane reacts with hydrochloric acid (HCl) it gives the production of chloro ethane.
CH2=CH2 + HCl → CH3-CH2Cl
In the above reaction, HCl (hydrochloric acid) acts as an electrophile as it is accepting electron pairs from ethane molecule and losing its hydrogen atom. Here, there is the formation of new C-H bond as the H atom of HCl get added on it and Cl ion also joined with second C atom of ethane.
Is HCl organic or inorganic?
Hydrogen chloride or hydrochloric acid (HCl) is an inorganic acid. The compounds which has carbon atom in its molecule are the organic compounds. The hydrocarbon chain generally present in organic compounds. HCl acid does not contain any carbon atom in it and hence it is an inorganic acid.
Is HCl oxidizing agent?
HCl acid is not oxidizing agent instead it is an reducing agent or basically a strong reducing agent. Hydrogen chloride has high dissociation energy because of which HCl can ionize or dissociate easily on mixing with water. HCl can ionize as H+ and Cl- ions in H2O, thus it is a reducing agent.
Is HCl polyatomic?
Yes, HCl is an polyatomic substance. It is composed of two non – metallic elements like H and Cl atoms. Due to the presence of two atoms in HCl it is a diatomic acid i.e polyatomic. Hence, HCl acid is an polyatomic acid.
Is HCl unstable?
HCl is an unstable acid. Stability of any molecule is determined by atoms electronegativity, formal charge present on it and the size of its atoms. The molecule is more stable in nature if it has the small size of the atoms or halogen atoms which should be more electronegative. Therefore, HCl is an unstable acid as it has small size and more electronegative halogen atom as compared to hydrogen atom.
Why HCl is unstable?
Molecules stability depends on gaining or losing of electrons by it. The species is more stable if it loose or gains electrons as it has complete octet. As more the stable is compound less reacts it is.
HCl is dissociates on dissolving in H2O but it does not dissociates readily in H2O. Some of HCl molecules are still exists in H2O. So, the HCl acid is an unstable acid. It can be stable at some recognized storage situation.
Is HCl volatile?
HCl is an volatile acid. Any compounds volatile nature can be measured with the presence of intermolecular force in it. The compound gains its molecular weight though its Wander walls forces also increases. It can easily evaporate into the atmosphere.
Why HCl is Volatile?
Hydrochloric acid (HCl) liquid is a volatile acid as it has weak intermolecular force of attraction i.e. hydrogen bonds. It also get ionizes readily and get eveporised easily in atmosphere at room temperature. Hence HCl is an volatile acid.
Is HCl viscous?
Hydrochloric acid (HCl) liquid form is volatile in nature as it has capacity to form hydrogen bond. The measure of fluids or liquids resistant to flow or move is known as viscosity.
HCl molecules do not form hydrogen bonds with other HCl molecules but they can form hydrogen bonds when mixed with water. As the HCl is liquid or fluid substance it can form hydrogen bonds with water as it forms intermolecular forces and hence the hydrochloric acid is viscous acid.
Conclusion:
HCl is present in both gaseous and liquid form. It is has total 8 valence electrons in its lewis structure. HCl lewis structure has one bond pair and three lone pair electrons. It has no formal charge and no resonance structure. Cl atom has complete octet in HCl lewis structure. HCl lewis structure has linear molecular shape, tetrahedral electron geometry, sp3 hybridization and 109.5 degree bond angle.
HBr is the chemical formula of hydrogen bromide. We are learning here about HBr lewis structure, characterizations and quick facts.
Hydrogen bromide is an anhydrous gas with no colour having strong irritating smell. It is corrosive in nature and heavier than air. HBr molecule contains one hydrogen atom and one bromine atom in its structure. The molecular weight of HBr is 80.91. HBr has synonyms like bromane, hydrobromic acid, hydrobromide, etc.
How to draw HBr lewis structure?
Steps to draw HBr lewis structure as follows:
Determine the H and Br position in periodic table group and evaluate total valence electrons on HBr molecule.
Most electronegative atom is at central position and makes bonding within H and Br atoms.
After bonding remaining electrons put on bonding atoms and mark lone electron pairs.
Check the octet of H and Br complete or incomplete.
In HBr lewis structure, H atom and Br atom belongs to 1st and 7th periodic table group respectively. Thus, both H and Br having 1 and 7 valence electrons in its valence shell. So, the total valence electrons in HBr lewis structure are:
Valence electrons of hydrogen atom = 1
Valence electrons of bromine atom = 7
Total valence electrons of HBr lewis structure = 1 (H) + 7 (Br) = 8
Therefore, HBr lewis structure has total eight valence electrons.
To fine total electron pairs on HBr lewis structure just divide total HBr valence electrons by 2.
HBr lewis structure has one valence electron on H atom and seven valence electrons on Br atom, thus having total eight valence electrons. The one valence electron of H atom gets shared with one electron of Br atom forming single covalent bonds.
The remaining six valence electrons go to the Br atom. Therefore, H atom gets satisfied its valency of two max electrons and Br atom has complete octet due to the presence of eight electrons in HBr lewis structure.
The HBr lewis structure has total eight valence electrons from them two electrons are being bond pairs and six electrons are non- bonding electrons on bromine atom. These six non- bonding electrons are being three lone electron pairs on bromine atom of HBr lewis structure. Thus, the HBr lewis structure has three lone electron pairs.
On any lewis structure is being stable if there is minimum formal charge is present on it. There is a formula to evaluate the formal charge of any lewis structure.
HBr lewis structure cannot form any resonance structure as it does not obey the rule of resonance structure. HBr lewis structure has do not have any multiple bonds and formal charge but it has three lone electron pairs. So, there is no possible movement of electrons in HBr lewis structure to form multiple bonds.
HBr lewis structure shape
According to VSEPR theory the HBr lewis structure has AXE3 generic formula where, A = central atom, X = bonding atom to central atom, X = lone electron pairs on bonding atoms. So, the HBr lewis structure has one central H atom, one bonding Br atom and three lone electron pairs on Br atom. Thus, HBr lewis structure has linear molecular shape and tetrahedral electron geometry.
HBr lewis structure shape
HBr hybridization
As the HBr lewis structure follows the AXE3 generic formula of VSEPR theory, so it has linear molecular shape and tetrahedral electron geometry. Because the HBr lewis structure has one hydrogen atom bonding with one bromine atom and Br atom has three lone electron pairs. Thus the HBr lewis structure has sp3 hybridization.
HBr lewis structure angle
The HBr lewsis structure comes under AXE3 generic formula of VSEPR theory. According to which it has linear molecular shape and tetrahedral electron geometry with sp3 hybridization. Thus, the HBr lewis structure has 109.5 degree bond angle.
HBr solubility
Hydrogen bromide (HBr) is soluble in:
Water
Acetic acid
Some other organic solvents
Is HBr soluble in water?
Yes, HBr is soluble in water. It gets dissociated in water as ions i.e. H+ and Br- ions.
Why HBr soluble in water?
When HBr gas added in water it get ionises as H+ (hydrogen ion or proton) and Br- ions. Hence it increases the H+ ions concentration in water and forms H3O+ (hydronium) ion in water.
How HBr soluble in water?
HBr (hydrogen bromide) gas reacts with water and forms HBr (hydrobromic acid) liquid. The hydrogen atom of HBr molecule forms hydrogen bonds with electronegative oxygen atom of water (H2O) molecule. Thus, HBr on mixing with H2O get dissociates as H+ and Br- ions and forms H3O+ ions.
HBr → H+ + Br-
HBr + H2O → H3O+ + Br-
Hydrogen bonding in HBr and water
Is HBr an electrolyte?
Yes, HBr (hydrogen bromide) is an electrolyte, rather HBr is a strong electrolyte. HBr when mixed with water it gets completely dissociated into water.
Why HBr is electrolyte?
HBr is an strong electrolyte. Electrolyte is a substance which when dissolve in water get ionizes and conduct electricity. HBr is an strong electrolyte because when it dissolve in water it get ionizes as positively charged cations H+ ions and negatively charged Br- anions and it can conduct electricity.
How HBr is a electrolyte?
When HBr (hydrogen bromide) get mixed with water it get dissociates into H+ (cation) and Br- (anion). When the electric current applied into the electrolytic solution like HBr + H2O, the H+ and Br- ions get formed and the positively charged H+ ions moves towards cathode and Br- ions moves towards anode.
Is HBr a strong electrolyte?
Yes, HBr is a strong electrolyte. Electrolytes are the compounds which get dissolved in water and forms ions to conduct electricity. Strong electrolytes are the compounds which get completely ionized into water to conduct electricity. In HBr (hydrogen bromide) when mixed with water get ionised into H+ and Br- ions i.e. completely ionizes and conduct electricity.
Is HBr acidic or basic?
Yes HBr is acidic in nature. HBr behaves as acid as when it dissolved in water it get ionizes a s H+ and Br- ions. Acids are the compounds which liberates H+ ions (protons) into water solution.
Why HBr is acidic?
When HBr gas mixed in water it get completely dissociated into H+ and Br- ions and thus it is behaves as strong acids. It get completely dissociates into water thus considered as strong acid.
How HBr is acidic?
HBr on mixing with H2O get dissociated into H+ and Br- ions and then the H+ ions further reacts with water molecules to form H3O+ ions. Hence, HBr is behaves as acid.
HBr + H2O → H3O+ + Br-
Is HBr a strong acid?
Yes, HBr is a strong acid. When HBr (hydrogen bromide) dissolved in water which gets completely dissociates or ionizes as H+ and Br- ions. As HBr molecule get completely ionizes into water hence it is a strong acids. The compounds or substance produce H+ ions into water by ionizing completely are strong acids.
Is HBr polyprotic acid?
No, HBr is not a polyprotic acid rather it is a mono- protic acid in nature. Monoprotic are the acids which contain only one hydrogen atoms or H+ ions or protons in its molecule. Polyprotic are the acids which contain more than one hydrogen atoms or H+ ions or protons in its molecule.
The HBr (hydrogen bromide) compound consists of one hydrogen atom and one bromine atoms only. Thus, HBr molecule on reaction with water can produce or release or dissociated only its one hydrogen atom or H+ ion or protons. Hence, HBr is monoprotic molecule.
Is HBr a lewis acid?
Yes, HBr is a lewis aicd. Lewis acids are those which have capability to accept a lone electron pairs. In lews acids the molecule should has at least one empty orbital in their valence shell in its atoms. The HBr is an lewis acid, because it has the capability to accept protons from water molecules when dissolve in water.
Why HBr is a lewis acid?
HBr is behaves as a lewis acid because it has the capacity to accept a pair of electrons.
How HBr is a lewis acid?
HBr when reacts with water can accepts a pair of proton (H+) from water molecules and hence HBr can acts as a lewis acid.
Is HBr an arrhenius acid?
Yes, HBr is an Arrhenius acid. Arrhenius acids are the species or compounds which can increases the concentration of H+ ions (protons) in the solution.
Why HBr an Arrhenius acid?
The HBr when mixed with water, the bond get breaks between the H and Br atoms and thus forms H+ ions and Br- ions in the aqueous solution. Thus, HBr is increasing the H+ ion concentration in water by releasing H+ ions in it.
HBr → H+ + Br-
How HBr an Arrhenius acid?
When HBr get mixed in water it get breaks as H+ and Br- ions and thus the H+ ions get increases into water solution. So, the H3O+ (hydronium) ion gets formed in HBr and H2O reaction with the breakdown of Br- ion.
HBr + H2O → H3O+ + Br-
Is HBr polar or nonpolar?
Hydrogen bromide (HBr) is a polar molecule. HBr is polar molecule because the H and Br atoms have much difference in their electronegativity values.
Why HBr is polar?
The H atom has electronegativity value 2.20 and the Br atom has electronegativity value 2.96.Thus the electronegativity difference between H and Br atoms of HBr molecule is 0.7 which is greater value than 0.4 prescribed in Paulings rules. It states that any compound which has electronegativity difference between the atoms if more than 0.4 then it is a polar molecule.
Also the H atom is less electronegative than Br atom, thus the Br atom pulls the electron density towards itself. So, there is unequal sharing of electrons on H and Br atoms the net dipole moment arises in HBr molecule causing partial positive charge on H atom and partial negative charge on Br atom of HBr molecule.
How HBr is polar?
The HBr molecule has asymmetrical arrangement of atoms due to unequal or unsymmetrical distribution of electrons in HBr structure. So, the HBr molecule has linear molecular shape and tetrahedral electron geometry as it has unequal distribution of electrons in HBr. Hence, the HBr molecule is polar in nature.
Is HBr linear?
Yes, HBr is a linear molecule. As per the VSEPR theory the HBr lewis structure has AXE3 generic formula so it has linear structure.
Why HBr is linear?
According to VSEPR theory the HBr lewis structure has AXE3 generic formula and hence the molecular shape of HBr molecule is linear. Thus, HBr is linear in shape.
How HBr is linear?
In HBr lewis structure, it is a diatomic molecule containing only two atoms H and Br which are linked with each other with a single covalent bond in a straight line. The H atom shared its one electron with Br atom and form single covalent bond forming a straight line of the structure and hence HBr is a linear molecule.
Is HBr paramagnetic or diamagnetic?
Hydrogen bromide (HBr) is diamagnetic in nature, due to the presence of all paired electrons in the molecule.
Why HBr is diamagnetic?
Hydrogen bromide has total eight valence electrons, out of which it forms one single covalent bond within H and Br atoms by sharing their one – one valence electrons with each other. So, the HBr molecule has one bond pair electrons and three lone pair electrons on HBr molecule. Hence, all the electrons are paired in HBr thus it behaves as a diamagnetic molecule.
How HBr is diamagnetic?
The magnetic susceptibility values of diamagnetic molecules are negative always. Hence the HBr molecule has negative value of magnetic susceptibility. When the external magnetic field is applied on HBr solution it repels with the magnetic field and moves in opposite direction of magnetic field. Thus, HBr is diamagnetic in nature.
HBr boiling point
Hydrogen bromide (HBr) molecule (gas or liquid) has 122 degree Celsius boiling point. Boiling point of liquid is the temperature at which the liquid substance boils and hopefully converts to vapours or gas. HBr has higher boiling point of 122 degree Celsius due to the larger size of HBr also it is more polarised molecule.
Why HBr has higher boiling point?
Hydrogen bromide gas when reacts with water it forms aqueous or liquid HBr solution i.e. hydrobromic acid. While forming liquid hydrobromic acid the HBr (hydrogen bromide) gas can form hydrogen bonds with water molecules.
Hence, there is the formation of strong intermolecular forces between H and Br atoms of HBr molecules i.e. hydrogen bonds and it is quite difficult to break these bonds. Also it is more polar in nature and having greater degree of dispersion forces within the molecule, which operates the HBr molecule and hence HBr has higher boiling points.
HBr bond angle
As per the VSEPR theory, the HBr molecule has followed the AXE3 generic formula. According to which the HBr molecule has linear molecular shape and tetrahedral electron geometry. Also HBr has sp3 hybridization and hence the HBr molecule has 109.5 degree bond angle.
Is HBr diprotic?
No, HBr is not a diprotic molecule rather it is a mono – protic molecule. Di – protic is a molecule having two protons or two hydrogen atoms also known to be poly – protic. Mono – protic is a molecule having one proton or one hydrogen atom. In HBr molecule, there is only one proton or one hydrogen atom is present so it cannot be di – protic molecule rather it is being a mono – protic molecule.
Is HBr ionic or covalent?
Hydrogen bromide (HBr) is a covalent molecule in nature rather it behaves as polar covalent molecule.
Why HBr is covalent or polar covalent molecule?
The HBr molecule composed of H and Br atoms which have 2.2 and 2.9 electronegativity values. So, it has 0.7 electronegativity difference between H and Br molecule. As per the prescribed values of bonding within the molecules having particular electronegativity difference between its atoms, the molecule should be ionic, covalent and polar covalent in nature.
The ionic molecules are those which have electronegativity difference value of 2.0 within its atoms. The polar covalent molecules are those which have electronegativity difference value of 2.0 to 0.5 between its atoms. Covalent molecules are those which have electronegativity difference value of less than 0.5.
Hence, the HBr molecule has 0.7 electronegativity difference value between H and Br atoms, which comes under the prescribed value range of 2.0 to 0.5. Hence it has a polar covalent bonds. Thus, the HBr molecule is polar covalent in nature and not ionic molecule.
How HBr is covalent or polar covalent molecule?
The HBr (hydrogen bromide) molecule consists of hydrogen and bromine atoms. The hydrogen atom has one valence electron in its valence shell and the bromine atom has seven valence electrons in its valence shell. Both H and Br atoms thus share one – one electron with each other to form a single covalent bond.
This single covalent bond is quite strong bond which is not easily gets break. But the HBr molecule is being polar in nature. The HBr molecule is being polar covalent bond due to the unequal sharing of electrons between H and Br atoms. Br atom is more electronegative than H atom and hence the electron cloud is pulls towards Br atom. Hence, HBr is polar covalent in nature.
Is HBr amphiprotic?
No, HBr (hydrobromic acid) is not an amphiprotic in nature. Amphiprotic or amphoteric compounds or molecules are those compounds which can behave both as an acid or base.
Why HBr is amphiprotic?
HBr (hydrobromic acid) cannot show both acidic and basic nature. When HBr acid reacts with base it can donate its proton and forms conjugate acid. But HBr (hydrobromic acid) cannot accept protons when reacts with base. HBr does not show any basic character so it is not amphiprotic in nature.
How HBr is amphiprotic?
As per the Bronstead and Lowery theory of acids and base, the acids are those compounds which can donate H+ ions or protons to base to form conjugate acid and the base are those compounds which can accepts H+ ions or protons to form conjugate base.
When hydrobromic acid (HBr) reacts with base like water (H2O) or ammonia (NH3) it will release or donate its proton to base (H2O or NH3) to form conjugate acids like H3O+ (hydronium) ions or NH4+ (ammonium) ions. But HBr (hydrobromic acid) cannot accept protons from other chemical compounds or basic compounds and hence it is not amphiprotic.
Is HBr binary or ternary?
HBr (hydrobromic acid) is a binary compound. Binary compounds are those compounds which have two non – metallic elements present in it. Especially the hydrogen atom (non – metal) gets combined or reacts with another non – metallic element.
Why HBr is binary?
HBr (hydrobrmoc acid) composed of two elements which are non – metallic in nature. That is the HBr molecule composed of one hydrogen atom and one bromine atom they both are non – metals and hence the HBr molecule is binary compound.
How HBr is binary?
Binary acids are those in which hydrogen atom is get connected with other non – metallic atom. Here, in HBr the hydrogen atom get attached with other non – metallic element like bromine. Bi means two, so two elements (non – metallic) are present in HBr and hence it is binary acid. HBr is a strong acid with pKa value of -9.0.
Is HBr balanced?
No, HBr is not a balanced equation basically, we have to balance the reaction by arranging same number of atoms on both reactant and product side. HBr aqueous or liquid i.e. acidic HBr (hydrobromic acid) it formed with the reaction of H2 (hydrogen) gas and Br2 (bromine) liquid. H2 which act as reducing agent and Br2 is act as oxidising agent.
H2 (g) + Br2 (aq) → HBr
The above reaction is not balanced as the atoms present on reactant side (H2 + Br2) is not equivalent with the product side (HBr), so we have to add 2 in front of HBr of product side to equalise the reaction equation.
H2 + Br2 → 2HBr
Hence the above HBr formation reaction is now balanced.
Is HBr conductive?
Yes, HBr is conductive in nature. HBr produces ions when mixed with water and conduct electricity and thus it is conductive in nature.
Why HBr is conductive?
HBr gas in pure form, it cannot conduct electricity. But when the hydrogen bromide gas (HBr) get bubbled in water (H2O) it forms a chemical reaction with water and form HBr liquid form i.e. hydrobromic acid.
This hydrobromic acid (HBr) on mixing with water release or donates H+ ions in water molecule and forms hydrogen bonding with water. Thus, HBr acid produces ions in water solution and conduct electricity.
How HBr is conductive?
HBr (hydrobromic acid) consists of two non – metallic elements like H and Br atoms. Hence, Hydrobromic acid (HBr) behaves as acid by donating H+ ions into water. It forms H+ and Br- ions in water solution i.e. it completely ionizes in water.
Also this H+ ions get attached with H2O (water) molecule to form H3O+ ions. These ions get moved towards the anode and cathode and conduct electricity in that solution. Hence, HBr behaves as strong acid and strong electrolyte and conduct electricity.
HBr + H2O → H3O+ + Br-
Is HBr conjugate base?
HBr (hydrobromic acid) can form conjugate base when reacts with a lewis base. Basically when HBr form acid base reaction it produces a conjugate base.
Why HBr is conjugate base?
Hydrobromic acid (HBr) donates or release a proton or H+ ions when reacts with base. Hence the base accepts the H+ ion or proton and form higher molecule with positive charge more protons and producing conjugate base as by – product.
How HBr is conjugate base?
HBr (hydrobromic acid) when reacts with lewis base like ammonia (NH3), the HBr acid donates H+ ion or proton to ammonia (NH3) molecule. Thus there is the formation of NH4+ (ammonium) ion and Br- ion as product of this acid – base reaction. Here, the Br- ion is formed in the reaction which acts as conjugate base.
HBr + NH3 → NH4+ + Br- (Br- = conjugate base)
Is HBr corrosive?
Yes, HBr is corrosive in nature. Hydrobromic acid on reaction with water produce H3O+ ion and when comes in contact with water and it forms corrosion.
Why HBr is corrosive?
HBr (hydrobromic acid) when reacts with water it gets ionizes completely and form H+ and Br- ions in water. HBr is a strong acid which forms more H+ ions in water or release more protons.
Hence due to the presence of more H+ ions in the solution, its pH value is less than 7 or less than 4. The pH value of hydrobromic acid is 3.01 and hence it is more corrosive in nature.
How HBr is corrosive?
When strong acidic compounds like HBr gets mixed with water it forms H+ and Br- ions in the solution and hence H+ ion concentration increases in water solution. Thus, the HBr acid can produce H3O+ ions in the solution. These H3O+ ions can reduce when comes in contact with metallic surface and form corrosion.
Also the acids corrosive nature can be measure capacity of acid to release H+ ions with the ‘acid dissociation constant’ pKa value. The HBr acid has -0.9 pKa value and hence more corrosive in nature. Therefore, HBr acid shows corrosive nature.
Is HBr concentrated?
Yes, hydrobromic acid (HBr) is a concentrated acid. Concentrated acids are those acids which are in pure forms or having its more concentration in water or produce more H+ ion concentration of water.
The HBr acid when mixed with water get completely dissociates into water as H+ and Br- ions. Hence there is the production of more H+ ions in water due to addition of HBr. Also it produces H3O+ ions so more concentration of H+ ion increases. Therefore, HBr is an concentrated acid.
Is HBr solid liquid or gas?
Yes, HBr is present in both a gas and a liquid. Pure form of HBr (hydrogen bromide) is present in gaseous form. It can produce only H+ and Br- ions when dissociates. But when this HBr gas gets bubbled into water.
There is the formation of aqueous hydrobromic acid (HBr aq). When this hydrobromic acid further reacts with water it forms hydrogen bonds with water and form H3O+ ions. Hence, HBr can show both gaseous and liquid nature.
Is HBr hygroscopic?
Yes, HBr is hygroscopic in nature. Hygroscopic substances are those substance or compounds which can absorb moisture from air or atmosphere and hence the physical properties (melting point, boiling point, etc) of that substance get changed. HBr can also absorb moisture from air and hence behaves as hygroscopic molecule.
Is HBr hydrogen bonding?
Yes HBr (hydrobromic acid) can form hydrogen bonding when mixed with water (H2O). When HBr acid get added to water it get dissociates into H+ and Br- ions, also it forms H3O+ (hydronium) ions in the solution as the H+ ion form hydrogen bond with H2O molecule.
HBr + H2O → H3O+ + Br-
Is HBr metal or non-metal?
HBr is non – metallic. HBr is composed of hydrogen (H) atom and bromine (Br) atom. Both H and Br atoms are comes under non – metals in the periodic table. Hence the hBr is non – metallic in nature.
Also the HBr in pure form is a gas (hydrogen bromide) and when it reacts with water it forms an aqueous or liquid HBr solution (hydrbromic acid). Therefore, HBr is non- metal in nature.
Is HBr neutral?
No, HBr is not neutral molecule. HBr is an acidic compound as it produces H+ ions when dissolved in water. It can form H+ and Br- ions in water solution.
Also the HBr molecule has polar covalent bond as the electron density goes to more electronegative bromine atom. Thus it creates partial positive charge on H atom and partial negative charge on Br atom. Therefore HBr is not neutral rather it is acidic in nature.
Is HBr a nucleophile?
No, HBr is not a nucleophile. Nucleophile is a substance which can donates its electrons i.e. it is electron rich. Nucleophiles are generally lewis base and a negative charge or neutral species. But HBr is an electrophile i.e. electron loving. It can accept electrons.
Why HBr is not a nucleophile?
HBr is an electrophile which can accepts electrons from other chemical compounds and donates its proton. Hence it is electron loving which accepts electrons from other atoms. Mostly electrophiles are lewis acids in nature and positively charged or neutral species.
How HBr is not a nucleophile?
HBr (hydrobromic acid) is generally a electrophile as it release or give up its hydrogen atom or proton or H+ ion to from new bond with other compounds by accepting electron from them. For Example: When ethene reacts with hydrogen bromide (HBr) it produces bromo ethane.
CH2=CH2 + HBr → CH3-CH2Br
Here, HBr behaves a s electrophile because it can accepts electron pair from ethane and donated its hydrogen atom or proton and creates a C-H bond with ethane molecule and the Br ion also attached with another carbon atom of ethane.
Is HBr organic or inorganic?
HBr (hydrogen bromide or hydrobromic acid) is an inorganic compound. Organic compounds are the compounds which contains carbon atom in its molecule or structure.
Mostly it contains hydrocarbon chain in its structure. In HBr molecule there is no carbon atom is present in its structure or chemical formula. Hence, HBr is an inorganic compound.
Is HBr oxidizing agent?
HBr is not an oxidizing agent rather is it a reducing agent or strong reducing agent. HBr (hydrogen bromide) has quite well dissociation energy due to which it can easily dissociates or ionizes completely into water when mixed with water.
HBr can ionize or dissociates into H+ and Br- ions when mixed with water. Hence, HBr is an reducing agent and not oxidizing agent.
Is HBr polyatomic?
Yes, HBr (hydrobromic acid) or hydrogen bromide is an polyatomic molecule. HBr is composed of two elements i.e. hydrogen atom and bromine atom. So, there are two atoms are present in HBr molecule i.e. HBr is diatomic or polyatomic. Therefore, HBr is considered as polyatomic molecule.
Is HBr unstable?
The HBr is quite unstable compound. The stability of any compound is depends upon its electronegativity or charges present on atoms and its size.
The compound is more stable when it has small size or halogen atom and more electronegative in nature. Hence HBr is unstable in nature as it has the bromine atom which has small size and more electronegative than hydrogen atom.
Why HBr is unstable?
Stability of any compound is also depends on the loss or gains of electrons by the compound. When the compound gain or lose electrons being more stable by completing its octet. If the compound is more stable it can reacts less.
HBr is decomposed when dissolved in water but it cannot ionize easily or completely in water. Some of the HBr molecules are remains in water, so the HBr acid is unstable in nature. It can be stable under some recommended storage condition.
Is HBr volatile?
Yes, HBr is a volatile acid. Volatility can be predicted from the intermolecular forces within the molecule. As the molecular weight of the compound increases so the Vander walls forces also increases. It can vaporize easily into the atmosphere.
Why HBr is Volatile?
HBr (hydrobromic acid) is volatile in nature, due to the weak intermolecular forces or hydrogen bonding. It can ionize easily and vaporised or evaporate into the atmosphere at room temperature. Hence, HBr is a volatile acid.
Is HBr viscous?
Yes, HBr is quite viscous in nature as it can form hydrogen bonds. Viscosity is the measure of liquid resistant to move or flow. HBr cannot form hydrogen bonding with each other but it can form hydrogen bonds with water molecules.
As the HBr (hydrobromic acid) is fluid or liquid in nature. Thus due to intermolecular forces like hydrogen bonds with water hydrobromic acid is viscous in nature.
Conclusion:
HBr can be available in both gas and liquid forms. HBr lewis structure has total eight valence electrons. Out for which one is bond pair and three is lone pair electron. There is no resonance structure of HBr. Also no formal charge is present on HBr lewis structure. Br atom of HBr has complete octet. The HBr has linear shape and tetrahedral geometry with sp3 hybridization and 109.5 degree bond angle.
H2O’s Lewis structure features an oxygen atom with two lone pairs and two single bonds connecting to hydrogen atoms, forming a bent molecular geometry. The oxygen atom has six valence electrons, sharing two with hydrogens (each contributing one electron) to complete its octet, resulting in a bond angle of 104.5°, slightly less than the tetrahedral angle due to lone pair repulsion, following the VSEPR theory for its AX2E2 configuration.
How to Draw Lewis Structure of H2O
Water (H2O) is a molecule composed of two hydrogen atoms bonded to a central oxygen atom. The Lewis structure helps us understand the bonding and electron distribution in water, which is essential for understanding its chemical properties.
Steps to Draw the Lewis Structure of H2O
Follow these steps to draw the Lewis structure of H2O:
Step 1: Count the Total Valence Electrons
Valence electrons are the electrons in the outermost shell of an atom. To determine the total number of valence electrons in H2O, add up the valence electrons of each atom.
O Valence Electron
Hydrogen (H) has 1 valence electron.
Oxygen (O) has 6 valence electrons.
Since there are two hydrogen atoms and one oxygen atom in H2O, the total number of valence electrons is 2(1) + 6 = 8.
Step 2: Identify the Central Atom
In H2O, the oxygen atom is more electronegative than hydrogen, so it will be the central atom. The hydrogens will be the outer atoms.
Step 3: Connect the Atoms with Electron Pairs
Draw a single bond between the oxygen atom and each hydrogen atom to represent the sharing of electrons. Each bond consists of a pair of electrons.
Step 4: Distribute the Remaining Electrons
In H2O, we have used 2 electrons for the bonds, leaving us with 8 – 2 = 6 valence electrons. These remaining electrons will be placed on the central oxygen atom.
Step 5: Check the Octet Rule
The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with 8 electrons in their outermost shell.
In the Lewis structure of H2O, the oxygen atom has 6 valence electrons from step 1, plus the 6 non-bonding electrons from step 4, giving it a total of 12 electrons.
Since oxygen can accommodate a maximum of 8 valence electrons, we need to move a lone pair of electrons from the oxygen atom to form a double bond between the oxygen and hydrogen atoms.
Step 6: Finalize the Lewis Structure
After moving one of the lone pairs, the oxygen atom will have a total of 8 valence electrons, and each hydrogen atom will have 2 valence electrons.
The final Lewis structure of H2O is as follows:
Drawing the Lewis structure of H2O helps us visualize the arrangement of atoms and valence electrons in the molecule. It allows us to understand the bonding and electron distribution, which are crucial for understanding the chemical behavior of water.
Remember, the Lewis structure is a simplified representation, and the actual electron distribution may differ. However, the Lewis structure provides a useful framework for understanding chemical bonding.
Glycerol is the poly compound or polyol means it consists of one or more hydroxyl groups in it. Here, we are learning about Glycerol structure and its characterization.
Glycerol has empirical or chemical formula C3H8O3. The structural formula for glycerol is C3H5(OH)3. It can also be written as CH2OH-CHOH-CH2OH. Glycerol has the synonyms like glycerine and 1,2,3-propanetriol. Glycerol is a viscous liquid with no colour and odour, but it is quite sweet in taste. It is a non- toxic compound at low concentrations.
The glycerol structure is composed of mainly three elements i.e. carbon, hydrogen and oxygen. It has a hydrocarbon chain of three carbon atoms i.e. propane in which the three hydrogen atoms get replaced with three hydroxyl groups. All the three central C atoms have sp3 conformation and hence the glycerol molecule has free rotation over all bonds.
Glycerol is a triol compound that means it has three hydroxyl groups. It is much hygroscopic in nature and also soluble in water. It is capable of forming hydrogen bonds in water. The hygroscopic and water soluble nature of glycerol is due to presence of these three hydroxyl groups.
What is structure of glycerol?
Glycerol structure is mainly composed of three elements i.e. three carbon atoms, three hydrogen atoms and three hydroxyl groups. Due to the presence of three hydroxyl groups it is known as triols. In glycerol there is hydrocarbon long chain consists of three carbon atoms in a straight line.
The middle carbon atom has one hydrogen atom and one hydroxyl group, another two carbon atoms has two hydrogen atoms and one hydroxyl group. Basically it is consists of a propane molecule in which the three hydrogen atoms get replaced by three hydroxyl groups.
Glycerol structure
How to draw Glycerol lewis structure?
Lewis structure drawing is done by following some rules. Firstly check the periodic group positions of all C, H and O atoms present in the glycerol structure, as they are present in 14th, 1st and 16th groups of the periodic table. Then count the total valence electrons present in the glycerol structure by adding the valence electrons of all the elements.
Place the atom at central position of the structure which has lowest electronegativity. Hydrogen cannot take central position due to low valence, so carbon is less electronegative (2.55) than oxygen (3.44). Thus three carbon atoms are at the central position of the glycerol structure. Now, as per the total valence electrons make the bonding with all the outer bonding atoms i.e. hydrogen atoms and hydroxyl groups.
The valence electrons which form bonds are being bond pair electrons and the remaining electrons get put on the outer bonding H and OH groups. Now, count the lone electron present on each bonding atoms, also check whether the octet is complete or not of all the atoms. Finally count the formal charge present on the glycerol molecule and also verify its structure, hybridization and bond angle.
Glycerol structure consists of three elements i.e. C, H and O which belong to the 14th, 1st and 16th group of periodic table. Thus, C atom has 4 valence electrons, H atom has 1 valence electrons and O atom has 6 valence electrons in their outer shell orbital. Let us calculate the valence electrons of glycerol structure.
Valence electrons of C atom of glycerol = 04 x 03 (C) = 12
Valence electrons of H atom of glycerol = 01 x 08 (H) = 8
Valence electrons on O atoms of glycerol = 06 x 03 (O) = 18
Total valence electrons on glycerol structure = 12 (c) + 08 (H) + 18 (O) = 38
Thus, glycerol structure has total thirty eight valence electrons present in it.
Let us calculate the total electron pairs present on glycerol molecule, for that we have to divide total valence electrons by 2.
Total electron pairs on glycerol structure = 38 / 2 = 19
Therefore, total 19 electron pairs present on glycerol structure.
Valence electrons in Glycerol structure
Glycerol lewis structure octet rule
In glycerol structure, there are single covalent bonds between three carbon and hydrogen atoms (C-H) forming three C-H covalent bonds. Similarly, there is formation of covalent bonds between three C and three OH groups. Here, hydrogen atom cannot take more than two electrons in its valence shell orbital as it is belongs to 1st group having one valence electron.
Three central Carbon atoms has four valence electrons which they get shared with five hydrogen atoms and three oxygen atoms of three OH groups which has six valence electrons.Thus, all the three central carbon atoms of glycerol structure has complete octet as they have eight electrons which are four bond pair electrons forming C-H and C-OH bonds.
Similarly, each hydrogen atom also has satisfied its valency by having two bonding electrons forming C-H and O-H single covalent bonds. At last, the three oxygen atoms of glycerol also has complete octet as they have eight electrons present on it i.e. two C-H and O-H bond pairs and two non- bonding electron pairs. Hence, all the three C and O atoms of glycerol structure has complete octet.
Glycerol structure showing complete octet of C and O atoms
Glycerol lewis structure lone pairs
Out of total thirty eight valence electrons of glycerol structure, twenty six electrons are engaged in bonding. Now, we are left with more twelve valence electrons. These remaining twelve valence electrons should put on three oxygen atoms. Each oxygen atom can occupy more four electrons, which are being non- bonding electrons.
Therefore, the glycerol structure has total twelve non- bonding electrons on three oxygen atoms of glycerol. These twelve non- bonding electrons are being lone electron pairs of glycerol structure. However, there are total six lone electron pairs are present on three oxygen atoms of glycerol and thus the glycerol structure has total six lone electron pairs present on it.
Lone electron pairs on glycerol structure
Glycerol lewis structure formal charge
Any lewis structure is being much stable when there is quite little formal charge is present on the atoms of structure. Formal charge calculation can be done with the given following formula.
While calculating the formal charge on glycerol structure, we have to calculate the formal charge formed on each atom or element of the glycerol structure. So, first we have to calculate the formal charge present on C, H and O atoms.
Carbon atom: Valence electrons on C atom of glycerol = 04
Non- bonding electrons on C atom of glycerol = 00
Bonding electrons on C atoms of glycerol = 08
Formal charge on C atom of glycerol structure is = (4 – 0 – 8/2) = 0
Thus, formal charge present on carbon atom of glycerol structure is zero.
Hydrogen atom:Valence electrons on H atom of glycerol = 01
Non- bonding electrons on H atom of glycerol = 00
Bonding electrons on H atom of glycerol = 02
Formal charge on H atom of glycerol structure is = (01 – 00 – 2/2) = 0
Thus, formal charge present on hydrogen atom of glycerol structure is zero.
Oxygen atom: Valence electrons on O atom of glycerol = 06
Non- bonding electrons on O atom of glycerol is = 04
Bonding electrons on O atom of glycerol is = 04
Formal charge on oxygen atom of glycerol structure is = (6 – 4 – 4/2) = 0
Thus, formal charge present on oxygen atom of glycerol structure is zero.
Therefore, the glycerol structure has complete formal charge present on C, H and O atoms are zero.
Formal charge on glycerol structure
Glycerol lewis structure resonance
In glycerol structure, there is only single covalent bonds are present all over the structure. Also the formal charge on glycerol structure is zero. Just two lone electron pairs are present on O atoms of glycerol molecule but they are not movable to form more multiple bonds in the structure as all the atoms have complete octet with sufficient electrons. Thus, resonance structure of glycerol molecule is not possible as it is not satisfied all the conditions of forming resonance structure.
Glycerol lewis structure shape
Glycerol structure has three central carbon atoms; the middle carbon atom gets attached with two carbon atoms, one oxygen atom and one hydrogen atoms. The other two side carbon atoms get attached with one carbon atom, one oxygen atoms and two hydrogen atoms. Thus all the three central carbon atoms get attached with four bonding atoms.
The glycerol structure also follows AX4 generic formula as all the three C atoms joined with four bonding atoms. Here, A = central atom and X = bonding atoms attached to central atom. So, the glycerol structure has tetrahedral molecular shape and electron geometry.
Tetrahedral shape of Glycerol structure
Glycerol hybridization
According to VSEPR theory the glycerol molecule has AX4 generic formula, as all the three central C atoms get attached with four bonding atoms. Thus glycerol structure has tetrahedral molecular shape and electron geometry. Hence, as per the VSEPR theory all the central carbon atoms are sp3 hybridized. Therefore, the glycerol molecule has sp3 hybridization as per VSEPR theory.
Glycerol lewis structure angle
The middle C atom has C-C-O and C-C-H bond angle of 109.5 degree. Also, the other two carbon atoms have H-C-H bond angles of 109.5 degree. But the H-C-O bonds of both the side carbon atoms could be bent due to repulsion causing by presence of lone electron pairs on O atoms.
Thus, H-C-O bond angle of glycerol molecule could be bent and may be having 103.5 degree bond angles. Hence, glycerol structure has 109.5 degree and 103.5 degree bond angles.
Yes, glycerol is easily soluble in water. The solubility rule ‘Like dissolves like’ could apply on glycerol water solubility. Because both water and glycerol containing hydroxyl (OH) groups so they can easily soluble or miscible with each other.
Why glycerol is soluble in water?
Glycerol contains three hydroxyl (OH) groups due to which it becomes much viscous in nature. Also it is quite hygroscopic in nature as it can absorb moisture from atmosphere or air. As more it absorbs the moisture from atmosphere, glycerol becomes less viscous in nature. As the glycerol is more viscous less it soluble in water and as glycerol is less viscous more it soluble in water.
Also the glycerol contains polyol groups i.e. glycerol contains more hydroxyl groups than water. The glycerol contains three hydroxyl groups and the water contains one hydroxyl group thus glycerol can form more hydrogen bonds with water and hence it is easily soluble in water.
How glycerol is soluble in water?
When glycerol is added to water, it first get settle down at the bottom of the container because the glycerol is much denser in nature than water and having specific gravity1.26. But as the glycerol get more soluble over time in water by stirring or heating the solution. So, all the undissolved glycerol gets soluble in water.
Also glycerine or glycerol is a trihydric quite big alkanol molecule. Glycerol has three hydroxyl (OH) groups joined to three carbon atoms. These three hydroxyl groups are hydrophilic regions and are polarized in nature. Thus these three hydroxyl groups of glycerol makes the solubility process easy with water molecules which also contains polarized hydroxyl (OH) group.
Hydrogen bonding between glycerol and water
Is Glycerol a strong electrolyte?
Glycerol is not a strong electrolyte. Glycerol is basically a non- electrolyte. Electrolyte is a substance which when dissolves in water can generate mobile ions which permit the water for electricity conduction. The compounds which cannot generate mobile ions when mixed in water and cannot permit the water to conduct electricity are non- electrolytes. Here, glycerol play a role of non- electrolyte.
Why glycerol is non- electrolyte?
In terms of covalent compounds, the covalent compounds get reacts with water in another way to work as electrolyte. When covalent acids react with water it donates the protons (H+) ions to water to produces ions in water. Similarly when covalent bases react with water it accepts protons from water to produce ions in water.
The glycerol compound is also a covalent compound as it has the single covalent bonds all over its structure. Still glycerol is non- electrolyte because when glycerol mixed with water it cannot form ions in water solution. But it can form hydrogen bonds with water molecules and being a neutral or non- electrolytic in nature. Thus, Glycerol is non- electrolyte.
How glycerol is non- electrolyte?
There are three kinds of electrolytes i.e. strong electrolyte, weak electrolytes and non- electrolytes. Strong electrolytes are those compounds which are strong conductors of electricity as they can form huge number of mobile ions. Rather, weak electrolytes are those compounds which are weak conductors of electricity as they can form small number of mobile ions.
Non- electrolytes are those compounds which are non- conductors of electricity as they cannot form mobile ions in water solution. Thus the glycerol is the compound which is not a good conductor of electricity and cannot produce mobile ions when mixed with water. Hence, glycerol is a non- electrolytic in nature.
Is Glycerol acidic or basic?
Glycerol is nor acidic neither basic in nature. Rather basically it is a neutral compound. But the glycerol in pure form behaves as a weak acid. Glycerol is an alkanol (R-OH) containing hydroxyl (-OH) group. The glycerol molecule has pH value nearly 7.3 which shows the neutrality of glycerol. Hence, glycerol is considered as a neutral compound.
Why glycerol is neutral?
Glycerol is an hydrocarbon containing hydroxyl (OH) groups which cannot get separated into ions. Pure form of glycerol when reacts with water it quite acts as a weak acid like methanol. But even if glycerol contains three hydroxyl (OH-) ions, still it is not acts like a base.
Glycerol molecule contains three hydroxyl (OH) groups in its structure, still this three hydroxyl (OH) groups cannot divides as ions. It is basically an alkanol (R-OH) to which three OH groups joined to three C atoms.
Even at higher pH values like 12 or 13 the hydrogen atom of hydroxyl ion of glycerol can somewhat dissociates forming a charged ion or species. This can somewhat increases the solubility but still the uncharged compounds solubility is infinite and no change formed in its solubility.
How glycerol is neutral?
Glycerol cannot form salts when reacts with acids but it can form esters known as triglycerides. In water solution it depends on concentration of water and glycerol which is slightly less than 7. Pure form of glycerol has pH value more than 7. pH is generally determines the H+ ions (hydrogen cations) concentration in water solution but not for pure form of compounds.
Pure form of glycerol can behaves as a very weak acid because it is quite difficult to separate hydrogen from OH groups. Even difficult to separate H+ ion from water too. Thus H+ ions cannot be stable with water and pure glycerol reaction. Thus H+ ion concentration is very less in pure glycerol. Hence it is a neutral or very weak acid in nature.
Is Glycerol polar or nonpolar?
Yes glycerol is a polar molecule. As we seen it is easily soluble in water which is a polar molecule. Thus polar polar molecules get dissolves with each other. Hence, glycerol molecule is also polar in nature.
Why Glycerol is polar?
Glycerol is polar molecule. Even the polarity of glycerol molecule cancel out somewhat, still it is polar molecule because of the presence of three carbon oxygen (C-O) bonds. These three C-O bonds of glycerol are polar bonds. Hence, glycerol molecule behaves as polar in nature.
How Glycerol is polar?
Glycerol molecule contains three OH groups, thus polar in nature. In polar molecules there is a separation of electric charge, also it contains a polar bond. The polar molecule which contains more than one polar bond have asymmetric geometry, thus the bond dipoles cancels out each other.
Also the polar bonds are caused due to the electronegativity difference between the bonded atoms. Polar molecule reacts with each other by hydrogen bonds and dipole- dipole intermolecular forces. The net dipoles are present on polar molecules due to the presence of opposite charged ions. Hence, there are three C-O polar bonds in glycerol due to which it becomes polar in nature.
Is Glycerol paramagnetic or diamagnetic?
Yes, glycerol is diamagnetic in nature. All the electrons are paired in the structure of glycerol molecule, so it should be considered as diamagnetic molecule. The magnetic susceptibility value of glycerol is -57.06·10−6 cm3/mol.
Why glycerol is diamagnetic?
Glycerol is diamagnetic in nature. The magnetic compounds which are aligning opposite way to magnetic field are known as diamagnetic compounds. Magnetic susceptibility value for diamagnetic compounds is always a negative value and which is less than zero (x<0).
These compounds are repelled with magnetic field and moves from stronger magnetic field to a weak magnetic field. They are temperature independent. As these compounds magnetized in opposite way, they have very tiny amount of magnetic intensity. These compounds have persistent relative permeability.
How glycerol is diamagnetic?
The magnetism is determined by presence of paired and unpaired electrons in the compound, and also determined with the application of outer magnetic field and movement of the compound towards or opposite direction of magnetic field. Also it is determined by calculating magnetic susceptibility value of that compound.
If the compound has paired electrons then it is diamagnetic. So, the glycerol structure has all the paired electrons in its structure. Hence glycerol is a diamagnetic compound. Also it get moves in opposite direction of magnetic field i.e. moves towards weak magnetic field. Glycerol has negative susceptibility value -57.06·10−6 cm3/mol which is less than zero. Thus glycerol is a diamagnetic compound.
Glycerol viscosity
Glycerol is highly viscous in nature. The ability of the liquid to move or flow is known as viscosity of that compound. The highly viscous fluids or liquids like glycerol can move or flow very slowly.
Why glycerol is viscous?
Viscosity is the ability of the liquid substance to flow. Glycerol is a highly viscous compound as it consists of three hydroxyl (OH) groups and thus it can form more hydrogen bonds. Due to this reason glycerol molecules are highly connected, so glycerol is highly viscous in nature.
How glycerol is viscous?
Glycerol molecule is highly viscous as it has three hydroxyl groups. So, they have greater intermolecular forces due to formation of more hydrogen bonds. Viscosity is also determined by intermolecular forces strength and the shape of the liquid compounds. The polar liquids which can form hydrogen bonds are generally highly viscous.
Also the long chain liquid compounds are more viscous. Glycerol is three carbon chain containing compound CH2OH-CHOH-CH2OH thus it is partly viscous as the length of C chain is not so long but can more viscous due to it ability of forming hydrogen bonds.
Is glycerol a lipid?
Glycerol is not a lipid but it is an alkoxy (R-OH) compound as it contains OH groups in it. Lipids are the substance which comes under macromolecules including steroids, fats and phospholipids. Glycerol is an an alcoholic compound having three OH groups attached to three carbon atoms.
Why glycerol is not a lipid?
Lipids are very long chain macromolecule compounds. Glycerol molecule contains a small carbon chain having only three C atoms in its structure. Glycerol can produce lipids by dehydration reaction with fatty acids but originally glycerol is not a lipid rather it is an alkoxy compound.
How glycerol is not lipid?
Glycerol is a triol containing three OH groups. It is a sugar alkanol so it can consider as carbohydrates also. But glycerol is not a lipid rather glycerol is the main constituent or backbone in the formation of lipids. It can form easter bonds with glycerol and fatty acids known as glycerides. Many complex lipids are produced with combining hydrophobic and hydrophilic compounds like glycerol and fatty acids.
Is glycerol lipid soluble?
No, glycerol and lipids are not soluble with each other as they both have opposite properties. Glycerol is a polar molecule and lipids are non- polar in nature. Thus they both are insoluble with each other.
Why glycerol is not lipid soluble?
Glycerol is the important constituent in lipid formation. But glycerol is unable to soluble in lipids. Lipids are long carbon chain compounds and glycerol is short chain carbon compounds. Hence, they both are not soluble with each other due to difference in carbon chain lengths of both compounds. As glycerol is polar molecule it is being soluble in polar compounds only.
How glycerol is not lipid soluble?
Generally glycerol is a polar compound and soluble only in polar molecules only. Lipids are non- polar compounds but some lipids like phospholipids shows both polar and non- polar nature due to presence of phosphate ion it is partially water soluble too. But triglycerides are totally non- polar. So the polar glycerol is not soluble in non-polar triglycerides.
Is glycerol hydrophobic?
No, glycerol is not hydrophobic rather it is hydrophilic in nature as it is soluble in water. Hydrophilic means water loving, due to solubility in water it is hydrophilic and not hydrophobic.
Why glycerol is hydrophilic?
Glycerol molecule contains three OH groups in its structure. Thus when it gets mixed with water it is able to form more hydrogen bonds with water molecules and hence it is hydrophilic.
How glycerol is hydrophilic?
The glycerol has three OH groups and showing polar nature, water is also polar molecule thus they both are soluble with each other. O atom of glycerol has lone pair electrons which it get shared with hydrogen atom of water to form hydrogen bond within them. So, glycerol is water loving and thus hydrophilic molecule.
Is glycerol glycerine?
Glycerol and glycerine is quite different compounds as they are being used in different ways. Still they are considered to be same generally.
Why glycerol and glycerine is different?
Production of glycerol needed glycerine. Glycerin is commercial compound and used as a main component to form glycerol. Glycerol and glycerine is generally used in similar ways. Glycerin is an polyol compound which is used as sweetner and preservative. Also it is a thick gummy substance on being frozen. Hence, both are different.
How glycerol and glycerine is different?
Glycerol is fats component which is colourless and add sweet taste as used as wine making process. It is a natural sweetner and used as solvent, preservative and thickening agent. It is used as cough syrups and body creams while glycerine used in toothpaste. Thus both are different.
Is glycerol soluble in hexane?
No, glycerol and hexane is not miscible with each other. Both are opposite solutions in nature i.e. polar and non- polar and thus are not possible to mix with each other.
Why glycerol is not soluble in hexane?
Glycerol is a polar molecule having three OH groups present on three C atoms and hexane is a non-polar molecule having long carbon chain of six carbon atoms and no OH group is present in it. Thus they both are insoluble with each other.
How glycerol is not soluble in hexane?
Polar compounds with small C chain can dissolve with the polar compounds only, as the C chain increases the compound being non polar in nature. Thus, hexane having long carbon chain and glycerol has small carbon chain with only three C atoms and there is no exchange of ions and thus they are not soluble with each other.
Conclusion:
Glycerol is a alkanol compound with three OH groups attached to three C atoms. It has no odour, no colour but sweet in taste. It has 38 valence electrons and forming single covalent bonds and have no formal charge and six lone electron pairs are present on it. It is polar molecule, soluble in water and viscous in nature. It has tetrahedral shape, sp3 hybridization and 109.5 and 103.5 degree bond angles.
FeO is the chemical formula for ferrous oxide. It has the synonyms like iron (ii) oxide or oxoiron. Here we are discussing about the FeO structure, its characteristics and some facts.
FeO (ferrous oxide) or iron (ii) oxide is composed of two elements i.e. iron and oxygen atoms. In FeO structure the Fe ion is in +2 oxidation state. It is totally different from Fe2O3 ion in structure and characteristics. FeO is a mineral form which is known as Wustite. This compound is black in colour. It resembles the structure of NaCl.
The symmetry of the structure changes to rhombohedral and the FeO compound becomes antiferromagnetic. Hence the antiferromagnetic arrangement is in [1, 1, 1] direction necessitating the selection of cell which contains at least two different Fe atoms in this direction.
The rhombhohedral centred hexagonal site or cell is the lowest or smallest cell which fulfils this condition. FeO has the lattice in this condition has parameters a = b = c = 5. 260 and angles of α = β = γ = 33. 557. Thus, the iron atoms (Fe) are located at fractional coordinates of (0, 0, 0) and (0.5, 0.5, 0.5), and oxygen atom (O) are located at (0.25, 0.25, 0.25) and (0.75, 0.75, 0.75).
FeO structure in general form
Some facts about FeO structure
The FeO ferrous oxide or iron (ii) oxide is prepared by the iron (ii) oxalate thermal decomposition.
Here, Ferrous oxide or iron (ii) oxide cones under the group of non- stoichiometric compounds, which are especially deficient of iron compositions from the range of Fe0.84O to Fe0.95O. FeO (iron (ii) oxide) have the similar structure like NaCl (rock salt). In FeO crystalline structure, the FeO crystals are iron deficient and always show non- stoichiometric.
There are some vacant cationic sites and some site contains Fe3+ ions in it, but its combination makes the structure quite electrically neutral. The approximate formula of FeO is Fe0.95O. FeO molecule has the structure like rock salt and also has the density of 5.073 g/cm3.
What is FeO structure?
The FeO structure is like the rock salt (NaCl) structure. It is a non- stoichiometric structure as there are some vacant sites or holes in the structure or some of the Fe3+ ions are present in the structure in place of Fe2+ ions. Here, each iron (Fe2+) ion gets surrounded by six neighbouring oxygen (O2-) ions or each oxygen (O2-) ion gets surrounded by six neighbouring iron (Fe2+) ion i.e. vice versa.
FeO (iron (ii) oxide) has the cubic structure or face centred cubic (FCC) rock salt structure and each edge of FeO unit cell is 5.0 A0. Therefore there are four Fe2+ ions and four O2- ions are present in each edge of the unit cell of the crystal structure. In this structure, the iron atom is coordinated to oxygen atoms octahedrally and in similar way, the oxygen atoms get coordinated to iron atoms octahedrally (vice- versa).
The structure is non- stoichiometric as there is the comfort of oxidation of Fe2 to become Fe3 ion get disturbed by replacing small section of Fe2+ ions with two 3rd number of Fe3+ ions which takes the tetrahedral position in closed packed lattice of FeO structure. In compare to the crystalline solid, in the melted state iron atoms are coordinated by four or five oxygen atoms predominantly. There is a quite small transformation in the structure below 200 kelvin temperature.
FeO structure FCC (faced centred cubic structure)
Is FeO ionic or covalent?
Yes, FeO is polar covalent compound. In FeO structure, the iron atom has an electronegativity of 1.83 and the oxygen atom has electronegativity of 3.44. The difference between both electronegativities are 3.44 (O) – 1.83 (Fe) = 1.61. The nature of bond in FeO is polar covalent thus the difference is very near to that of ionic bonds. So iron (ii) oxide is a polar covalent compound with ionic characterizations.
Why FeO is ionic?
In FeO molecule, the iron (Fe) and oxygen (O) atoms are present and having 1.61 electronegativity difference. This electronegativity difference is below the given standard value 1.71. Due to low value as compared to 1.7 the FeO molecule is being polar covalent molecule.
If the electronegativity value is above 1.7 then any compound will be an ionic compound. But still there is a predominant ionic character in FeO molecule due to the presence or two oppositely charged ions i.e. Fe2+ and O2-.
How FeO is ionic?
According to Fuzan Rule, the compound with bigger cation in size and smaller anion in size favours the ionic characteristic while bond formation within cation and anion. Thus, FeO is quite more ionic but can show covalent character too.
Generally ionic bonds can formed between the two oppositely charged ions i.e. positive charge and negatively charged ions. Hence, ionic bonds are formed by the electrostatic attraction within oppositely charged ions. The anion is which gains electrons and the cation is which donates electrons.
Is FeO soluble in water?
FeO (iron (ii) oxide) or ferrous oxide is not soluble in water. The iron oxides which occurs naturally are mostly insoluble in water. Thus FeO ferrous oxide also insoluble in water as it is a naturally occurring compound. Also it is ionic in nature thus it cannot form ions in water when it reacts with water.
Why FeO is insoluble in water?
FeO is an ionic compound as it consists of two opposite charged ions. FeO molecule has Fe2+ ion (cation) and O2- ion (anion). Hence when FeO (ferrous oxide) when mixed or reacts with water it cannot form ions into water. Thus, FeO cannot dissociates or completely not dissociates in water. Therefore, FeO (iron (ii) oxide) is not soluble or insoluble in water.
How FeO is insoluble in water?
Generally iron in elemental form (elementary iron) is soluble in water at normal room condition. But according to solubility rule the oxides of iron is not soluble in water. The solubility of iron containing molecules or compounds are increases with the lower pH value.
The solubility of iron compounds can be increased with lower positive charge compounds. As the Fe2+ ion has lower charge than Fe3+ ion hence the Fe2+ containing compounds are quite soluble than other compounds but cannot dissociated in water thus they considered as insoluble compounds. Hence, FeO is insoluble in water.
Is FeO a solid?
Yes, FeO is a solid compound as it has a crystalline rock salt structure like NaCl. Even the FeO powder is a black solid powder form of compound. The crystal structure of FeO ion is non – stoichiometric.
Why FeO is solid?
FeO (ferrous oxide) is a solid compound as it has crystalline rock salt structure like NaCl. Also the crystalline structure of FeO has face centred cubic structure (FCC) in which each Fe2+ atom is surrounded by neighbouring O2- ions. Thus the ions of the structure are closely packed in a cube and hence it is a solid compound.
How FeO is solid?
In FeO crystal structure, all the Fe2+ and O2- ions are closely packed in face centred cubic structure. In any solid compound the atoms or ions are closely packed and have a particular shape. Thus FeO ion has face centred cubic shape and ions are closely packed. Thus it is a solid compound.
Conclusion:
FeO is known as ferrous oxide or iron (ii) oxide. In FeO structure, the Fe ion is in +2 oxidation state and O atom is in -2 oxidation state. It is a non – stoichiometric structure as the FeO structure has some vacant places or some Fe2+ ions get replaced with Fe3+ ions. The FeO structure is face centred cubic structure. It has polar covalent bond but shows ionic characters. It is ionic, insoluble in water and a solid compound.
Read more about following Structure & Characteristics
Oxides formed with the reaction of metal atoms with oxygen atom. Here, at this juncture, we are learning about acidic oxide example and some facts about it. When oxide gets reacted with water it gives acid and known as acidic oxides. Also oxides can behaves as neither acid nor bas and remain as a neutral.
CO2 + H2O → H2CO3
SiO2 + 2H2O → Si(OH)4
P4O6 + 6 H2O → 4 H3PO3
P4O10 + 6 H2O → 4 H3PO4
P2O3 + 3H2O → 2H3PO3
P2O5 + 3H2O → 2H3PO4
SO2 + H2O → H2SO3
SO3 + H2O → H2SO4
Cl2O +H2O ↔ 2HOCl
Cl2O7 + H2O → 2 HClO4
CrO3 + H2O → H2CrO4
N2O5 + 3H2O → 2HNO3
B2O3 + 3H2O → 2H3BO3
2NO2 + H2O → HNO3 + HNO2
Cr2O3 + H2O → H2Cr2O4
Mn2O7 + H2O → 2 HMnO4
3NO2 + H2O → 2HNO3 + NO
N2O3 +H2O → 2HNO2
N2O5 + H2O → 2HNO3
SeO2 + H2O → H2SeO3
Acidic oxide Example is listed as follows:
The acidic oxides formed especially with the non- metals elements and oxygen. The non- metal elements of group 14 to 17 can from acid oxides and this is the form of acid anhydrides which form acid and water. Acid oxides and also known to be acidic anhydrides. The non- metal elements and oxygen atom have a covalent bond between them.
Mostly acid anhydrides have low boiling point and melting points except the oxides like boron oxide (B2O3) and silicon oxide (SiO2) as they have high boiling point and melting point and can form giant compounds. Most of the oxides which are covalent are highly acidic cation which exhibits acidic properties.
CO2 + H2O → H2CO3
When Carbon dioxide reacts with water it gives carbonic acid. Here, carbon dioxide (CO2) is the acidic oxide example.
SiO2 + 2H2O → Si(OH)4
When silicon oxide reacts with eater it produces ortho silicic acid. Here, silicon dioxide (SiO2) is the acidic oxide example.
P4O6 + 6 H2O → 4 H3PO3
When phosphorous trioxide reacts with water, it produced phosphorous acid. Here, phosphorous trioxide (P4O6) is the acidic oxide example.
P4O10 + 6 H2O → 4 H3PO4
When phosphorous pentaoxide reacts with water it gives phosphoric acid. Here, phosphorous pentaoxide (P4O10) is the acidic oxide example.
P2O3 + 3H2O → 2H3PO3
When di- phosphorous trioxide reacts with water, it gives phosphorous acid. Here, di- phosphorous trioxide (P2O3) is the acidic oxide example.
P2O5 + 3H2O → 2H3PO4
When di- phosphorous pentaoxide reacts with water it gives phosphoric acid. Here, di- phosphorous pentaoxide (P2O5) is the acidic oxide example.
SO2 + H2O → H2SO3
When sulphur dioxide reacts with water it produced sulphurous acid. Here, sulphur dioxide (SO2) is the acidic oxide example.
SO3 + H2O → H2SO4
When sulphur trioxide reacts with water it forms sulphuric acid. Here, sulphur trioxide (SO3) is the acidic oxide example.
Cl2O + H2O ↔ 2HOCl
When di- chlorine mono- oxide reacts with water it gives hypochlorous acid. Here, di- chlorine mono- oxide (Cl2O) is the acidic oxide example.
Cl2O7 + H2O → 2 HClO4
When chlorine heptoxide reacts with water it gives perchloric acid. Here, chlorine heptoxide (Cl2O7) is the acidic oxide example.
CrO3 + H2O → H2CrO4
When chromium trioxide reacts with water, it produces chromic acid. Here, chromium trioxide (CrO3) is the acidic oxide example.
N2O5 + 3H2O → 2HNO3
When di- nitrogen pentaoxide reacts with water it gives nitric acid. Here, di- nitrogen pentaoxide (N2O5) is the acidic oxide example.
B2O3 + 3H2O → 2H3BO3
When di- boron tri- oxide reacts with water it gives boric acid. Here, di- boron tri- oxide (B2O3) is the acidic oxide example.
2NO2 + H2O → HNO3 + HNO2
When nitrogen dioxide reacts with water it gives nitric acid and nitrous acid. Here, notrigen dioxide (NO2) is the acidic oxide example.
Cr2O3 + H2O → H2Cr2O4
When di- chromium trioxide reacts with water it gives Dihydroxy (dioxo) dichromium. Here, di- chromium trioxide (Cr2O3) is the acidic oxide example.
Mn2O7 + H2O → 2 HMnO4
When tri- oxo manganese reacts with water, it gives permanganic oxide. Here, tri- oxo manganese (Mn2O7) is the acidic oxide example.
3NO2 + H2O → 2HNO3 + NO
When nitrogen dioxide reacts with water it gives nitric acid with liberation of nitrogen mono- oxide. Here, nitrogen dioxide (NO2) is the acidic oxide example.
N2O3 + H2O → 2HNO2
When di- nitrogen tri- oxide reacts with water it gives nitrous acid. Here, di- nitrogen tri- oxide (N2O3) is the acidic oxide example.
N2O5 + H2O → 2HNO3
When di- nitrogen penta- oxide reacts with water it gives nitric acid.Here, di- nitrogen penta- oxide (N2O5) is the acidic oxide example.
SeO2 + H2O → H2SeO3
When selenium oxide reacts with water it gives selenious acid. Here, selenium oxide( SeO2) is the acidic oxide example.
When these oxides get mixed in water they produce oxo anion. Hence, the elements of oxo anion have equal oxidation number as the oxides have. When the oxides get mixed with water if they formed strong or highly strong acids then the oxides consider being soluble in water, as these acids completely ionized and the equilibrium get shifted towards dissolution.
Acid formation due to reaction between acidic oxides and water
If the oxides get mixed in water and gives moderate acidic oxoacids, thus the oxides should not be completely soluble in water. In this case, the produces oxoacid is weak acids in nature. Hence, the oxides generally soluble, but not always dissolve in water. The acidic oxides of sulphur atom (SO3) and nitrogen atom (NO2) are considered as air pollutants.
These SO3 and NO2 oxides get reacts with moisture present in atmosphere and produces the acid rain. Some oxides like ClO2 and NO2, in which the oxidation state of central atom does not matches with the oxidation state of the elements of the known or stable oxo acids. This kind of oxides by disproportionation produces a mixture of anions or oxo acids.
Conclusion:
Acidic oxides are formed with the reaction of non- metal elements and oxygen. When these acidic oxides get dissolved or miscible in water it gives acids. Non- metals of the group 14th to 17th are the participants of acidic oxides. Acidic oxides are also known as acid anhydrides. The most common acidic oxide examples are CO2, NO2, SO2, SO3, N2O5, Cl2O7, Cl2O, P2O3, P2O5, etc.
