Cu2+ Lewis structure is highly motivating fact to illustrate the chemical overview on the element cupper. There is some knowledgeable facts supports sketch of Lewis structure rather electronic configuration of Copper.
The facts that would be discussed in this article are:
Drawing of Lewis structure involves few steps for every element in the periodic table. Those steps make the sketch of elements intense and specified with internal matters happens through electronic configuration of the element.
While demonstrating the first step of identifying the number of valence electron in Copper this can be recognised from the electronic configuration that is for Cu is 1s22s22p63s23p64s23d104s1. It means the number valence electron in Copper is 9.
Next step is to put dots as the notation of electrons around Cu that is 9 dots. This step completes the simple Lewis structure of Copper that is significantly comparative in accordance with the Lewis structure of Cu2+.
Drawing Cu2+ Lewis structure
Studying about a strong cation Cu2+ in chemistry and its significance can be initiated with the preliminary drawing of Lewis structure of this ion. Cu2+ is named as cupric ion in chemical study.
Inputting valence electron as dots around copper after leaving two electron from its valence shell is the main perspective shared by Lewis structure of Cu2+. Lewis structure of cupric ion refers to the fact of electron deficiency in Copper.
Cu2+ Lewis structure resonance
Resonance means altering of bonds by electrons. Resonance is a mechanism which elaborates the significance of having pi bond in the structure. In resonance the pi bond is replaced by negative charge of any one atom of respective elements. Therefore, it is obvious that having a pi bond is the most required feature of resonance.
Cu2+ is definitely a positively charged ion but it denotes the deficiency of two electrons in its electronic structure. Therefore, after creating bon d with other elements it cannot initiates resonance. Resonance is irrelevant mechanism to proceed for cupric ion.
In Cu2+ the number of electron changes and it is formed in the shape of distorted octahedral or square-pyramidal for cupric ion. Lewis structure plays a significant role in determining this change in shape for this ion with chemical demonstration.
Cu2+ Lewis structure formal charge
Formal charge of can be determined fie any compound by calculating the number of bonding and non-binding electrons in each of the elements participate in the formation of the compound.
In the case of a specific element of an ion it becomes important to observe the number of electrons it is releasing from its valence shell which identifies the entire formal charge of the ion. For cupric ion the formal charge is very precisely 2+.
Cu2+ Lewis structure angle
Lewis structure is responsible for expressing the angular dimensions of compounds which creates covalent of ionic bond by electron sharing. Angle of the compounds depends of several features such as types of bond and the presence of lone pairs.
Cu2+ is a ion which has no bond and it is formed from an angle periodic element that is copper. Therefore, the angle of this element is undefined.
Cu2+ Lewis structure octet rule
Octet rule refers to the chemical rules, which drives the periodic elements to reach out with eight electrons in its valence shell to get ultimate stability. It is the rules which initiates the process of bonding in chemistry to make the elements stable by getting similar electronic configuration like its nearest noble gas.
Electronic configuration of CU2 and Cu2+ to Identify Cu2+ Lewis structure from Wikipedia
For Cu, its nearest noble gas in periodic table is Argon that has electronic configuration as 3s23p6. Cupric ion has a tendency to gain two electrons to get back the structure of Copper. It reduces its oxidation state and this is how it gets stability without prioritising octet rule much.
Otherwise, Cu can get eight electrons in its last energy level to fulfil octet rule but Cu3+ is not possible due to the extreme stability gain by fulfilling g d orbital. 3d10 orbital of Copper makes its different from octet stabilisation.
Cu2+ Lewis structure lone pairs
Presence of lobe pairs is detected by the Leis electronic structure of the elements. Presence lone pairs and its number are important to know its impact on electron exchange process.
Cu2+ is a complex ion and complex ions use to possess active number of lone pairs at its outermost energy level. When Cu2+ combines with other elements having negative changes, it highlights its coordination number instead of presenting lone pairs. However, the ion holds one unpaired electron in 4s orbital.
Cu2+ valence electrons
Valence electron identification is the most important job to do before sketching Lewis structure of any element, the number of valence electrons can be obtained in Copper as 2.
After eliminating two electrons the element becomes a complex ion which exceeds two valence electrons as well. The ions named as cupric ion holds 1 valence electron in its last energy shell.
Cu2+ hybridization
Hybridisation is another simple fact about the elements that is determined from the existence of electrons in the orbitals. After creating binds with other elements these orbitals over loops and electronic shift amid orbitals, takes place, which is denoted by Lewis structure.
Cu2+ has 9 electrons in d orbitals which is almost filled with the deficiency of 1 electron. However, the ion is noticed to form sp3 hybridisation after bonding with NH3 that donates a lone pair to cupric ion.
Cu2+ solubility
Solubility is water or other solutions depends on the charge of elements. Strong ionic elements of compounds have lower dissolving power in water.
Cupric ion is insoluble in water but it gets dissolved in strong hydrochloric acid. in hydrochloric acid the formation of complex ion becomes easier.
Cu2+ ionic
The power holding charges is the definite fact regarding identification of a element as ionic or covalent.
Cu2+ is the ionic state of metal Copper. After releasing two electrons from valence shell, the metal forms positively charged cupric ion.
Cu2+ acidic or basic
Lewis acid refers to those elements, which accepts electron with feasible nature, and Lewis base is those elements which donates electrons superiorly to the needy elements.
Cu2+ has ben identified as a strong electron acceptor. Therefore, this element is considered as a powerful Lewis acid is the series.
Cu2+ polar or nonpolar
Polarity depends on the bonding ability of the elements. Carrying charges giving rise to polarity in the periodic elements.
Cu2+ is positively charged ion, the charge give its topographical polar surface area. The value of this type of polarity in Cu2+ is 0 Ų.
Cu2+ tetrahedral
Tetrahedral shape is common is sp3 hybridised element of compounds.
Cu2+ has distorted octahedral shape with deficiency of two electrons. Otherwise the shape of Cu2+can be defined as square pyramidal as well. Octahedral geometry papers due to the presence of unpaired electrons. As Cu2+ has, one unpaired electron in its electronic geometry possesses this kind of shape.
Cu2+ linear
Octahedral shapes refers to the non-linear structure of compounds, extremely complex structure signifies the present on non-linear orbitals.
Cu2+ is complex ion that is holding distorted octahedral shape. Therefore, it is clarified that it has no linear structure. However, the element is non-linear in chemistry.
Cu2+ symmetrical or asymmetrical
Symmetric structure is held by the elements, which are identical by every side whereas asymmetric structure denotes that the elements are not looking same from each side.
Cu2+ is holding a symmetric geometry as its structure is argued as a square planner structure.
Cu2+ paramagnetic or diamagnetic
The presence of unpaired electrons in an element defines the magnetic structure of that element as paramagnetic. The definition of diamagnetic is vice versa that is when all the electrons in an element is paired then it is called diamagnetic.
Cupric ion has one unpaired elections therefore specifically it is a paramagnetic element. It is obvious that it cannot be called diamagnetic at all.
Cu2+ colour
Transition of electrons from one energy level to another energy level is the main mechanism that indicts the change in colour of elements. Besides, the presence of unpaired electrons is also influential factor to represent the colour of elements.
After releasing one electron Cu becomes Cu+ with filled d orbital that is d10 therefore; it is colourless. When Cu+ releases one mire electron, it becomes coloured due to presence of one unpaired electron that makes the transition feasible. Cu2+ is blue in colour.
Cu2+ a reducing agent
Reducing agent refers to those elements that can donate electrons to otgher needy elements. Therefore, reduction is possible only among thme who have excess electrons in valence shell.
It is clear that cupric ion has deficiency of two electrons therefore; it cannot be an electron donor. Besides, this ion can adopt electrons easily with string bonding with other elements such as Ammonia.
Cu2+ an oxidizing agent
Oxidation state of cupric ion is notable fact, which describes its stability. After reducing two electrons from valence shell Copper gives rise to this complex ion which impose a relevant oxidation state to create coordination with other periodic elements.
Oxidation and reduction state of Copper from Wikipedia
Cu2+ is one of the strongest oxidising agents. Aluminium is another strong oxidising agent but not stronger than cupric ion. Therefore cupric ion can oxide Al but Al cannot oxidise it. The 2+ oxidation state held by the ion is more stable in chemical matters than 1+. Therefore, Cu2+ is considered as a stable and powerful oxidising agent.
Stability of Cu2+
Stability of ions can be identified by examining the ability of making binds with water molecules. In a simpler language, hydration energy of the ions determines the stability of the ions.
Cupric ion is a strong ion with high charge density that releases a huge amount of energy and makes string binds with other elements. Therefore, this ion is considered as a stable ion in chemistry.
Conclusion
This article has illustrated the more than enough facts regarding the complex ion Cu2+ which has been found to be named as cupric ion in chemistry. After eliminating two electrons from valence shell, Copper emphasises the formation of this ion.
In this article we will discuss about GaH3 Lewis structure , characteristics : 17 Fact to Know
Gallium hydride is a molecule in which gallium (Ga) is attached to three hydrogen atoms. Its molecular weight is 72.74. it is also called trihydridogallium (GaH3) or gallane, which is an inorganic compound photosensitive colorless gas.
How to draw GaH3 lewis structure ?
In the GaH3 Lewis structure, Gallium (Ga) is a metal and Hydrogen (H) is a gas. So, the hydrogen atom in the gallium hydroxide has 1 valence electron while the gallium atom in the gallium hydroxide has three valence electrons Considering there are 3 hydrogen atoms in the gallane (GaH3) molecule hence total, 3 valence electrons of a hydrogen atom. So, in total, we have 3+3 = 6 valence electrons.
out of the two atoms, gallium is the least electronegative atom (1.81), so while drawing Lewis’s structure of gallium hydride we can put gallium (Ga) in the center and three hydrogen atoms around it. Then connect the gallium (Ga) and three hydrogen atoms with single bonds. We’ve used six electrons so far (one bond = two electrons). Each hydrogen atom and gallium atom to fulfilling the octet rule, Gallium donates three electrons to three hydrogen atoms and completes their octet.
The gallium hydroxide molecule does not show resonance because this molecule does not contain a double bond for the delocalization of electrons, also there is no movement of electrons in the molecule hence GaH3 does not exhibit resonance and also there is no resonating structure for GaH3.
GaH3 Lewis structure shape
Trihydridogallium or gallane (GaH3) has trigonal planer geometry. With the three Sp3 hybrid orbitals.
The Lewis structure formal charges of GaH3 can be calculated by the following formula FC = V – N – B/2 Where V = no. of valence electrons , N = no. of non–bonding electrons , B = no. of bonding electrons
FC of H in GaH3 Lewis structure = 1-0-1/2 = 0 In the gallane (GaH3) molecule the Gallane and hydrogen have zero formal charges.
GaH3 Lewis structure bond angle
The gallium hydride is trigonal planer geometry with a bond angle of 120o
GaH3 Lewis structure octet rule
In the gallium hydroxide (GaH3) molecule gallium (Ga) requires to donate its outermost three electrons to the hydrogen atom and complete its outermost orbitals octet, while the hydrogen (H) atom has only one electron in its outermost shell therefore it accepts one electron from the gallium atom and completes its duplet, in this way three hydrogen atom accepts three electrons from gallium atom and complete their octet and become stable.
The octet rule itself states that the molecule is said to be stable when all the atoms in the molecule complete their octet by sharing electrons with each other.
GaH3 lewis structure lone pairs
Gallium hydride (GaH3) has no lone pairs. The lone pair on the atom is denoted by a dot. Lone pairs are the pair of electrons which are not participating in bond formation in the molecule, generally, lone pairs are present on the central atom.
The lone pair represents many significant properties of a molecule like the shape of that molecule, Gallane (GaH3) does not contain lone pair of electrons, it contains all bond pairs of electrons.
GaH3 valence electrons
In the GaH3 Lewis structure, Gallium (Ga) is a metal and Hydrogen (H) is a gas. So, the hydrogen atom in the gallium hydroxide has 1 valence electron while the gallium atom in the gallium hydroxide has three valence electrons Considering there are 3 hydrogen atoms in the gallane (GaH3) molecule hence total, 3 valence electrons of a hydrogen atom. So, in total, we have 3+3 = 6 valence electrons.
GaH3 hybridization
In Gallane (GaH3) molecule gallium atom undergoes sp3 hybridization as,
Ga = [Ar] 3d10 4s2 4p1
H = 1s1
The gallium atom contains three p unpaired electrons and the hydrogen atom has 1s unpaired electron hence gallium atom donates three electrons to the three hydrogen atoms and forms three-sigma Ga – H bond. Which form three sp3 hybrid orbitals. And undergo sp3 hybridization due to sp3 hybridization GaH3 has trigonal planer geometry.
GaH3 solubility
Gallane (GaH3) is a nonpolar molecule which is soluble in tetramethyl ethylenediamine polar solvent. And insoluble in a nonpolar solvent.
Is GaH3 soluble in water
Gallium hydride (GaH3) is in gaseous form and insoluble in water it is a nonpolar molecule, which dissolves in polar solvent only.
Is Gah3 a strong electrolyte?
Gallium hydride (GaH3) is not a strong electrolyte because it is not easily dissociated into ions it is not soluble in water. it acts as an electrolyte in tetramethyl ethylenediamine polar solvent because GaH3 dissolve in that polar solvent and dissociates into ions in that solvent.
Is Gah3 acidic or basic ?
Gallium hydride is Bronsted acidic in nature.
Is Gah3 polar or nonpolar ?
Gallium hydride (GaH3) is formed by combining one gallium and three hydrogen atoms the electronegativity of the gallium atom is 1.81 and that of electronegativity of the hydrogen atom is 2.20 the difference between the electronegativity of hydrogen and gallium is 0.39.
This much electronegativity difference between gallium and hydrogen indicates that the electron pairs are weekly attracted to the hydrogen atom hence Ga-H bond in the GaH3 molecule is non-polar. The electronegativity difference between gallium and a hydrogen atom is very less hence the hydrogen and gallium atoms are weekly attracted to each other hence Ga-H bond is highly non-polar.
Is GaH3 linear ?
Gallium hydride is not a linear molecule it is trigonal planer geometry.
Is Gah3 paramagnetic or diamagnetic ?
Gallium hydride (GaH3) shows diamagnetic nature because gallane (GaH3) contains all paired electrons which are 10 in number hence it is strongly attracted by the applied magnetic field and forms an induced magnetic field in the opposite direction.
Also, those atoms, ions or molecule which contain lone pair electrons or vacant outermost orbital has a paramagnetic nature while that atom, ion or molecule containing all paired electrons are diamagnetic in nature.
GaH3 boilingpoint
The boiling point of gallium is very high which is 22040C while the gallium hydride (GaH3) boiling point cannot be determined. The gallium hydride (GaH3) is in the viscous liquid form its melting point is -15oC.
Conclusion
In the above article we will discuss the Lewis structure of GaH3 and its 19 facts which includes Lewis structure, lone pair, the shape of the molecule, hybridization, resonance, octet rule, formal charges, solubility, Acid or basic nature, polar or non-polar, bond angle, paramagnetic or diamagnetic nature, boiling point etc.
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.
In this article we going to discuss about cobr2 lewis structure including its characteristics and structure and 13 most important facts regarding this.
Cobr2 which is commonly known as bromophosgene in analogy with phosgene. It is produced in fire extinguishers, when halon compounds are decomposed. It is a colourless liquid with a molar mass of 187.818 gm/mol. It starts boiling at 64.50c, when it decomposes. Even at low temperature, it slowly decomposes to poisonous co and elemental br.
Cobr2 Lewis Structure Drawing
In cobr2 the central atom is C atom in which O and 2 Br atoms are attached. In cobr2, central c atom uses sp2 hybrid orbital. In the ground state, C atom has 4 valance electron but only 2 remains unpaired. To form cobr2, 4 unpaired electrons is required.
When some energy is applied, one 2s electron of c atom becomes unpaired and total 4 unpaired electron is present now. Hence 2 br atoms form 2 sigma bonds and o atom forms 1 sigma as well as 1 pi bond with central c atom. All these are covalent bonds. This is because all these are formed by sharing of electrons between 2 atoms.
From VSEPR theory we can assume that the shape of cobr2 is trigonal planner. In this structure central carbon atom is surrounded by 2 br atoms and 1 o atom in trigonal planner manner.
The structure of cobr2 does not contain any lone pair of electron on central c atom; hence distortion of ideal trigonal planner structure does not occur. In cobr2, central C atom uses sp2 hybrid orbital to form 2 c-br bonds and 1 c=o bond. As cobr2 has planner structure all the atoms in cobr2 lie in the same plane.
Cobr2 Lewis Structure Formal Charges
The formula we used to calculate the formal charge is -Formal Charge (f.c) on each atom= (Total No of valance electrons of the atom)-(Total no of bonding electron formed by that atom)/2- (total no of nonbonding electrons on that atom).
Hence formal charge on the central c atom in bromophosgene =4-8/2-0=0.
Formal charge on oxygen atom in cobr2=6-4/2-4=0.
Formal charge on 2 terminal br atoms in cobr2=7-2/2-6=0.
Hence formal charge on central C atom in cobr2 is 0 and each bromine atoms and also O atom has formal charge of 0, making the overall compound is electrically neutral.
Cobr2 lewis Structure Lone Pairs
Total No of unshared pair of electron exist on any atom= the valance electrons present on the atom-total no of bonds formed by that particular atom.
In cobr2 lone pair present on central c atom= 4-4=0 i.e. No lone pair of electron on c atom.
Lone pair present on oxygen atom in cobr2=6-2=4 i.e. 2 lone pair of electron.
Lone pair present on br atoms in cobr2= 7-1=6 i.e.3 unshared pair of electron.
These unshared pair of electrons on o and terminal br atoms is shown in the cobr2 lewis structure as electron dots.
Cobr2 Hybridization
Hybridization is a process in which central c atom in cobr2 mixes its atomic orbital to form hybrid orbitals because higher energy atomic orbitals does not take part in bonding. In the ground phase, C has 4 valance electrons out of which only 2 electrons are unpaired. But this is not enough electrons to form cobr2.
Hence when C absorbs hybridization energy, its 2s electron becomes unpaired and requirement of 4 unpaired electron becomes fulfilled. By using this electron C atom forms Cobr2 with the help of 3 sigma bonds and 1 pi bond. In cobr2, c uses sp2 hybrid orbital to make c-br and c=o bonds. According to sp2 hybridization, the structure of cobr2 is trigonal planner.
Cobr2 Hybridization
Cobr2 solubility
Cobr2 is soluble in polar solvents because of the fact that as cobr2 is polar in nature, it like to dissolve in polar solvents like water, ethanol, methanol etc. In 100 ml of water, approx 66.7 gm cobr2 dissolved at about 590c.
Cobr2 valance electrons
To calculate the total no of valance electron in cobr2, it is required to know the valance electron of c,o and br atoms. The valance electron present in c atom is 4. The valance electron present in O and Br atom is 6 and 7 respectively. The total no of valance electron present in cobr2 is sum of valance electron of c,o and br atoms i.e. (4*1+6*1+7*2)=24.
Cobr2 lewis structure angle
In cobr2, central c atom is sp2 hybridized and the structure of cobr2 is trigonal planner. According to VSEPR theory, the angle prsent in trigonal planner shape is 1200. Hence the angle between br-C-br and br-C-O is exactly 1200.
Cobr2 lewis Structure Resonance
In Cobr2 resonance occurs and in resonance process nonbonding electron pair shifts from one atom into another atom through conjugation. The structure we get through delocalization is called resonating structure.
When resonance takes place in cobr2, we get 3 equivalent resonating structure and delocalization occurs through conjugation of nonbonding electron pair with carbonyl group in its ∏* orbital.
Cobr2 Resonance
Cobr2 lewis structure Octet Rule
When we see the lewis structure of cobr2 we find that each bromine atom has 8 electrons in the outermost shell and satisfy octet rule. In cobr2 compound central carbon atom forms 2 C-Br bonds and 1 C=O bond making a total of 4 electron pair i.e. 8 electrons around central C atom.
O atom forms 2 bond with central C atom and also contain 2 lone pairs making a total of 8 electrons around O atom. 2 Br atoms form 1 sigma bond each with C atom and both contains 3 lone pair of electron i.e. octet rule is also satisfied for Br atom.
Cobr2 Polar Or Nonpolar?
SOCl2 is a non-polar compound. In cobr2, c=o bond moment lies towards more electronegative o atom. 2 c-br bond moments lie towards Br atom, as br is more electronegative than c atom. All these bond moments cancel each other and hence making the dipole moment of this compound is 0 Debye.
Is cobr2 ionic?
Cobr2 is an ionic compound. This is due to the fact that the electronegativity difference between the C-Br bonds and C=O bond. Cobr2 is soluble in water like ionic compounds do. It has also high melting as well as boiling point similar to that of ionic compound. It also conducts electricity in molten as well as in solution state.
Is cobr2 acidic or basic?
Cobr2 is amphoteric in nature i.e. it is act as an acid or as a base. When cobr2 reacts with acid, it accepts H+ ion through the donation of O atom and act like a like base. When it reacts with base, OH- donates its lone pair of electron and cobr2 accepts this electron and act as a lewis base.
Is cobr2 tetrahedral?
Cobr2 attains trigonal planner geometry in which c atom act as the central atom. It has no tetrahedral geometry, because central c atom is not sp3 hybridized.
Is cobr2 linear?
Cobr2 is not linear because central c atom is not sp hybridized. As the central c atom in cobr2 acquires sp2 and does not attain 1800 hence, question of cobr2 has linear geometry does not arises.
Is cobr2 symmetrical or asymmetrical?
Cobr2 is symmetrical in nature. This is because of the fact that a mirror plane i.e. sigma plane cut the cobr2 compound into 2 symmetrical halves. The sigma plane passes through the carbonyl group. It also contains c2 axis which passes through C=O group, after this operation br is superimposable with another br group.
Conclusion
Cobr2 is a stable compound in which central C atom is sp2 hybridized and due to absence of lone pair of electron the structure is real trigonal planner. In this compound all the atoms satisfied their octet.
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.
This article should contain the HNO3 lewis structure and its different important facts. Let’s discuss the HNO3 lewis structure.
In the HNO3 lewis structure, the molecule is consist of N, H, and three O atoms. All the atoms in the HNO3 lewis structure make a covalent bond. The N is the HNO3 lewis structure is sp2 hybridized while O is sp3 hybridized. There is one -OH group and two ketonic groups are present. Due to the presence of that -the OH group makes the molecule acidic. The electronegativity of O and N is so high that make that H is more acidic.
HNO3 or Nitric acid is one of the strongest inorganic acids. The aqua regia is made from this acid. The structure of the HNO3 is different because here two central are different hybridization. Around the N it is trigonal planar and around the O it is tetrahedral.
Some important facts about HNO3
The physical state of nitric acid is liquid. The color of the nitric acid is colorless but when it is stored for a long time its color changed to yellowish due to the decomposition of oxide of nitrogen. The boiling point and the melting point of Nitric acid are 356 K and 231 K respectively. The molar mass of this acid is 63.012 g/mol. The odor of nitric acid is acidic and very suffocating. The density of this acid is 1.51 g/cm3. Fuming nitric acid has vapor pressure and the value is 48 mmHg at 200C.
It can be produced by the reaction of water and nitrogen dioxide.
4 NO2 + 2 H2O → 2 HNO3 + NO + NO2 + H2O
The net reaction is,
3 NO2 + H2O → 2 HNO3 + NO
Nitrogen dioxide bubble goes through the hydrogen peroxide improving the yield of the product.
2 NO2 + H2O2 → 2 HNO3
In the laboratory, nitric acid can be prepared by the thermal decomposition of copper nitrate to produce nitrogen dioxide and that nitrogen dioxide then reacted to water to get nitric acid.
2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2
2 NO2 + H2O → HNO2 + HNO3
The above process is called the Ostwald process.
Nitric acid can behave as a strong oxidizing agent. To incorporate the nitro group in any organic synthesis nitric acid is used widely.
1. How to draw the HNO3 lewis structure?
The HNO3 lewis structure is quite different from the other covalent molecule because it has two central atoms one is N and the other is an O atom. N and O both are p block elements, so they have to follow the octet rule in the drawing of the HNO3 lewis structure. Let us consider the HNO3 lewis structure.
Step 1 – In the first step of the HNO3 lewis structure, we should count the valence electrons for every atom present in it. The electronic configuration of H is 1s1. So it has only one electron and this electron is used for its valence electron and via this single electron, H can form a bond. We know O is the group 6thelement and p block element so its last orbital should be p orbital and the electronic configuration of O is [He]2s22p4. So it has six electrons in its valence shell which can be used for bond formation.
Now for N, the electronic configuration is [He]2s22p3, so it has five electrons in its valence shell and the maximum number of bonds N can form is four. Now we add all the valence electrons in the HNO3 lewis structure and the total valence electrons for the HNO3 lewis structure is, 1+5+(6*3) = 24 electrons. There are three O atoms present and each O contains six valence electrons.
Step 2 – Now it is a most confusing step, that here we select the central atom, here N and O both are present at the central position and the electronegativity difference between both is very less. In the HNO3 lewis structure, all the atoms are not connected through N or O atoms, but the central atom should connect all the atoms.
That’s why here N and one O are considered central atoms and for this reason, we have to calculate the hybridization for two atoms separately and the values of hybridization of two atoms are different. Two atoms are experiences different environments.
Step 3 – In the HNO3 lewis structure, all the atoms are from the s and p block, so they should follow the octet rule. For the s block element, they try to complete only their s orbital because s is their valence orbital. the total number of electrons accumulated by the s orbital is 2. For p orbital, the total electrons accumulated is 6.
Now, according to the octet rule, the electrons needed for the HNO3 lewis structure are 2+(4*8) = 34 electrons. But the valence electrons in the HNO3 lewis structure is, 24, so the shortage of electrons is 34-24 = 10 electrons. These 10 electrons should be accumulated in the number of suitable bonds. So the bonds needed 10/2 = 5 bonds. So there is a minimum of five bonds are needed. To assign the five bonds we need to add a double bond between N and O.
Step 4 – In this step, we should connect every atom in the HNO3 lewis structure via the required number of bonds. There is one bond between terminal H and O, one bond between O of -OH group and N. then other three bonds are used between N and two O atoms, and there is a double bond between one O and N atoms.
Step 5 – In this last step, we add lone pairs and multiple bonds to complete the valency of atoms. O has six electrons in its valence shell and it forms two bonds, one with H and one with N, so it has four unpaired electrons which exist as two pairs of lone pairs. Other O atoms which form a double bond with N, it has the same four electrons in their valence shell and they exist as two pairs of lone pairs. The last O which makes a single bond with N forms a dative bond and six electrons exist after one bond formation so it gets a negative charge and two pairs of lone pairs.
2. HNO3 lewis structure shape
The shape of the molecule is dependent on the electron count and based on the central atom, but in the HNO3 lewis structure, there are two central atoms one is N and the other is O. for N the shape of the molecule is planar but concerning O the shape of the molecule is tetrahedral. The electron density is different for two atoms and the shape of the HNO3 lewis structure.
HNO3 Shape
The HNO3 lewis structure in the gaseous form is planar. The same structure is also for a solid-state. The N-O bond distance in the nitro group is equal. The third N-O bond distance is longer and corresponds to a single bond. We know Nitro is a variable structure and there is a double bond character shown between two O and N atoms. The nitro group is tilted away from the H atoms by 20.
If we consider the VSEPR(Valence Shell Electrons Pair Theory), then we should count the electrons and consider the structure. But here the structure is different for different atoms. For the -OH oxygen their electron count is 8 including two lone pairs, so according to the VSEPR, it adopts a tetrahedral shape. But for the nitro group electron count is 6 so it adopts trigonal planar structure, where three o atoms are present in three vertices.
3. HNO3 valence electrons
For calculating the total valence electrons for the HNO3 lewis structure, we should count individual valence electrons for each atom. There are three O atoms, one N and one h atom are present. The environment of three N atoms is different and therefore their valence electrons are also different.
HNO3 Valence Electrons
From the electronic configuration of N it is evident that there are five electrons are present at the valence shell in N. O is group 6thelement so it has six electrons in its valence shell which are ready for bond formation. But O forms only one bond with N and the rest of the two electrons exist as lone pairs. H has only one electron and this one electron is the valence electron for the H atom.
So the total number of valence electrons of the HNO3 lewis structure is 1+5+(6*3) = 24 electrons.
4. HNO3 lewis structure lone pairs
In the HNO3 lewis structure, only lone pairs are available on the O atoms, N forms a dative bond with O in the nitro group then it has lone pairs otherwise not.
For counting the lone pairs, we have to check the available electrons in the valence shell of every atom after bond formation. H has only one electron, so H can’t contain lone pair. Now O has six electrons in its valence shell and after two sigma bond formation, it has the remaining four electrons. These four electrons exist as two pairs of lone pairs over O in the -OH groups.
HNO3 Lone Pairs
For the nitro groups, there are two O atoms present in the HNO3 lewis structure, One O is formed a double bond with N to complete the octet, so it has four electrons and again the same case arises. This O atom has two pairs of lone pairs. Now the other O atoms form a variable bond with N, there is not possible for two double bonds for N, because N cannot show pentavalent, so there is only one possible way that O makes a single bond with N or forms a dative bond.
A dative bond is a coordination covalent bond. The electron density is reside more towards the O site. That O also carries a negative charge and contains three pairs of lone pairs. Accounting for N is contain a positive charge.
So the total number of lone pairs over the HNO3 lewis structure is 2+2+3=7 pairs of lone pairs, otherwise, six pairs of lone pairs if they do not form a dative bond.
5. HNO3 lewis structure formal charge
From the HNO3 lewis structure, we can say that there is a charge present over N and O in the nitro group. By calculating the formal charge, the charge over every atom should be predicted. It is a hypothetical concept accounting for the same electronegativity of each atom in the HNO3 lewis structure.
The formula we can use to calculate the formal charge, F.C. = Nv – Nl.p. -1/2 Nb.p.
Where Nv is the number of electrons in the valence shell or outermost orbital, Nl.p is the number of electrons in the lone pair, and Nb.p is the total number of electrons that are involved in the bond formation only.
The environment of three O atoms should be different so, we have to calculate the formal charge individually for all the atoms.
The formal charge over the H atom is, 1-0-(2/2) = 0
The formal charge over the O atom in -OH group = 6-4-(4/2) = 0
The formal charge over the N atom is, 5-1-(8/2) = 0
The formal charge over the O in the nitro group is, 6-4-(4/2) = 0
From the formal charge calculation, we cannot say that there is a dative bond between N and O in the nitro group. Overall the molecule is neutral.
6. HNO3 lewis structure angle
The bond angle of the HNO3 lewis structure is different due to two different central atoms and two shapes of the molecule being present. The hybridization of two atoms is different and the environment is also different. So, in the HNO3 lewis structure, there is two bond angles are observed concerning N and O atoms.
HNO3 Bond Angle
For the Nitro group in the HNO3 lewis structure, there is only three atoms are present surrounding the central N atom, and there are no lone pairs over the N atom. According to the VSEPR theory, if the molecule AX3 is without lone pair over the central atom, then the bond angle should be 1200. But here the lone pairs of three O atoms are present.
So if the bond angle goes 1200, then there is massive lone pairs-lone pair repulsion occurs. So to minimize this kind of repulsion, N changed its bond angle to 1120. This value is also for the presence of three electronegative atoms and the s character of the hybridization value increases.
Now for the other O atom, there is one H and one N atom are present surrounding that O atom. There are also two pairs of lone pairs present. So this shape is similar to a water molecule, like a V shape, so the bond angle is nearly 1040, because of lone pairs repulsion and the presence of one electronegative atom N.
7. HNO3 lewis structure octet rule
In the HNO3 lewis structure, there are s and p block elements present, so they have to follow the octet rule. The octet rule for s block elements is completing the s orbital via two electrons and for p block elements they complete their octet via eight electrons. Because p orbital can accumulate a maximum number of six electrons.
HNO3 Octet
In the HNO3 lewis structure, we should check each atom to complete its octet. The H atom has only one electron in its s orbital and it needs one more electron to complete its octet. Via the bond formation with the O atom, H and O share one electron each, and therefore H can complete its octet via the one electron from the O site.
Now for the O of -OH group, it has six electrons in its valence shell, as it is the group 6th element. So it required two more electrons in its valence shell to complete its octet. Now this O makes a bond with H and N atoms sharing two electrons. So it completes its octet by gaining two electrons from N and O, which are shared in the bond formation.
Now N has five electrons in its valence shell and it needs three more electrons in its valence shell to complete its octet. So it makes a bond with three O atoms and shares three electrons with them. Now N can complete its octet too via gaining those three electrons from three O atoms which are shared in the bond formation.
Two O atoms of the nitro group make a double bond at a time with the N atom and hence they can complete their octet too, via sharing two-electron in the double bond.
8. HNO3 lewis structure resonance
In the HNO3 lewis structure resonance will be observed because there more electron clouds are present within the molecule, which can be delocalized over the different skeleton forms of the HNO3 lewis structure. The molecule shows a positive and negative charge within it and there is more number of lone pairs present, so they can be delocalized, because the octet of the N and ketonic O is not complete somehow.
HNO3 Resonating Structure
all the above three structures are different skeleton forms of HNO3 lewis structure or we can say that they area resonating structure. Among the three, structure I and structure II are similar, the negative charge dispersed over the two O atoms in the nitro group. These two structure is most contributing because all three structure contains the same number of covalent bond, but in these two structure the most electronegative atom O gets a negative charge and the less electronegative atom N gets a positive charge.
In structure III, the number of covalent bonds is the same but here N gets a positive charge is ok but O also gets a positive charge which is a destabilization factor. O is a more electronegative atom and the positive charge over it is a destabilization factor.
9. HNO3 hybridization
The hybridization of the HNO3 lewis structure is different because it has two central atoms and we should predict the hybridization of two central atoms individually. The energy of 1s orbital of H and 2p orbital of O is not equivalent so they undergo hybridization to form equivalent orbital. Similarly, the N atom also undergoes hybridization from a hybrid orbital with three O atoms.
We calculate the hybridization of the HNO3 lewis structure by using the following formula,
H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.
When we find the hybridization of N in the HNO3 lewis structure, there are three electrons for N and three O atoms are present at the surrounding position.
So, the hybridization of central N in the HNO3 lewis structure is ½(3+3+0+0) = 3 (sp2)
For the O atoms, the valence electrons are 6 and one N and one H atom are present.
So the hybridization of O in the HNO3 lewis structure is, ½(6+2+0+0) =4 (sp3)
Structure
Hybridization value
State of hybridization of central atom
Bond angle
Linear
2
sp /sd / pd
1800
Planner trigonal
3
sp2
1200
Tetrahedral
4
sd3/ sp3
109.50
Trigonal bipyramidal
5
sp3d/dsp3
900 (axial), 1200(equatorial)
Octahedral
6
sp3d2/ d2sp3
900
Pentagonal bipyramidal
7
sp3d3/d3sp3
900,720
From the above table of hybridization, we can conclude that if the hybridization value is 4 then the central atoms is sp3 hybridized and if the number of orbitals are involved in hybridization is three then the atoms is sp2 hybridized.
Let’s understand the hybridization of N and O atoms separately.
Hybridization of N
It is evident from the hybridization diagram that we cannot consider the π bond in the hybridization. We consider only the sigma bond with O atoms, N forms a three-sigma bond with three O atoms undergoing sp2 hybridization. S orbital cannot participate in multiple bond formation, so we consider p orbital electron for forming a double bond.
Hybridization of O
From the hybridization diagram, we can tell that the lone pairs over the O atoms are also involved in the hybridization. For this reason, the shape around that O atom is tetrahedral and this also interns the value of the bond angle is near 109.50.
10. HNO3 solubility
In the HNO3 lewis structure, we can say that there is charge separation observed and this makes the molecule slightly polar and ionic, so it can soluble in a different polar solvent. HNO3 is a very good solvent for different metals. It forms aqua regia, which is a good solvent for the soluble gold metal. HNO3 is soluble in the following solvents,
Benzene
Ethanol
Water
CCl4
11. Is HNO3 soluble in water?
In the HNO3 lewis structure, we see some polarity in this molecule, so it is soluble in a polar solvent. HNO3 is not soluble in water directly, it is miscible in water, the density of water and HNO3 is different but it has a polar character and is ionized in water and gets miscible in an aqueous solution.
12. Is HNO3 polar or nonpolar?
The presence of different atoms and the shape of the HNO3 lewis structure make the molecule polar. Although the electronegativity of N and O is almost close the electronegativity of ketonic Oxygen and alcoholic Oh is different. The shape of the molecule concerning N is planar but concerning O it is tetrahedral and due to its unsymmetric shape it makes the molecule polar. Due to the unsymmetric structure, the dipole moment of the molecule is not canceled out and the molecule has some resultant dipole moment.
HNO3 Dipole-Moment
The direction of the dipole moment is from N to O, as N gets a positive charge and the electropositivity is increased here and O gets a negative charge, and the electronegativity increases, and for this reason, the difference between electronegativity is higher and dipole moment works. from the structure, we can say the dipole moment is not canceled out or not exactly opposite to each other. So it has a valid dipole-moment value and makes the HNO3 lewis structure polar.
13. Is HNO3 an electrolyte?
Yes HNO3 is an electrolyte it dissolves in water and makes the aqueous solution ionic.
14. Is HNO3 a strong electrolyte?
HNO3 is a strong electrolyte, cause when it gets solvated in an aqueous solution is it ionized in H+ and nitrates ions. The mobility of the H+ ion is very high and for this reason, the HNO3 lewis structure is a strong electrolyte.
15. is HNO3 acidic or basic?
HNO3 is strongly acidic, when it is dissolved in water it released H+ ions easily and makes a stronger acidic.
16. Is HNO3 a strong acid?
HNO3 is a strong acid, it can release H+ ion easily because there is an electronegative O atom is present and for the electronegativity, it pulls electron density toward itself and making O-H bonds weaker and H+ easily cleaved, if a molecule release H+ easily then the acidic nature of this molecule is very high and making a stronger acid.
17. Is HNO3 an arrhenius acid?
If a molecule gives H+ ion then it is called Arrhenius acid and HNO3 easily releases an H+ ion, so HNO3 is an Arrhenius acid.
18. Is HNO3 a lewis acid?
HNO3 can acts as lewis acid because it can accept electron density in N atom because it is positively charged.
19. Is HNO3 stronger than HNO2?
HNO3 is a stronger acid than HNO2 because the conjugate base of HNO3 is NO3- which is more stabilized due to conjugation as compared to the conjugate base of HNO2, which is NO2-. So more stable the conjugate base stronger the acid is.
20. Is HNO3 stronger than H2SO4?
HNO3 is less strong than H2SO4, as H2SO4 is dibasic acid and also the conjugate base of H2SO4 is SO42-, which is a more stable conjugate base due to better overlap between O and S as compared to the conjugate base of HNO3, which is NO3-. SO HNO3 is a weaker acid than H2SO4.
21. Is HNO3 a conjugate acid?
No HNO3 is itself an acid and it is not a conjugate acid of another molecule.
22. Is HNO3 a conjugate base?
HNO3 is an acid, so it has a conjugate base and the conjugate base of HNO3 is NO3-, which is more stable and makes the HNO3 stronger acid.
23. Is HNO3 diprotic?
There is one hydrogen atom present and it can be donated, so HNO3 is monoprotic, not diprotic.
24. Is HNO3 binary or ternary?
HNO3 is a ternary oxoacid.
25. Is HNO3 a buffer?
When HNO3 reacts with a weak base then it can form a buffer of strong acid, otherwise, it is an acid.
26. Is HNO3 a salt?
HNO3 is an acid and when it reacts with a strong base then it forms salt and water molecule.
27. Is HNO3 conductive?
HNO3 is a conductive agent when it is soluble in water it can carry electricity.
28. Is HNO3 corrosive?
HNO3 is highly corrosive.
29. Is HNO3 hydrogen bonding?
There is no H bonding observed in the HNO3 structure.
30. Is HNO3 linear?
HNO3 is not linear it is planar and tetrahedral in shape.
31. Is HNO3 paramagnetic or diamagnetic?
HNO3 has only one unpaired electron over the N atom and it is paramagnetic.
32. Is HNO3 amphoteric?
HNO3 is a strong acid and donates H+ ions only so it is not amphoteric.
33. Is HNO3 a dehydrating agent?
HNO3 is a dehydrating agent, it can remove water molecules.
34. Is HNO3 gas?
The physical state of HNO3 is liquid.
35. Is HNO3 electrophile?
The nitronium ion in HNO3 acts as an electrophile.
36. Is HNO3 hygroscopic?
The dilute HNO3 is hygroscopic but the concentrated form is not.
37. Does HNO3 have a charge?
HNO3 is not a charged molecule but there is a negative charge dispersed between ketonic groups in HNO3.
38. Is HNO3 heavier than air?
The density of HNO3 is much higher than in air.
39. Is HNO3 liquid or aqueous?
The physical state of HNO3 is liquid.
40. Is HNO3 monobasic?
HNO3 has one replacable H+ ion is present so it is monobasic acid.
41. Is HNO3 acid metal?
No HNO3 is not a metallic compound.
42. Is HNO3 an oxidizing agent?
In HNO3 the oxidation number of N is high and it can be decreased so it behaves as a stronger oxidizing agent.
43. Is HNO3 radical
No, HNO3 is not radical, it can be ionized.
44. Is HNO3 a reagent?
Yes in organic synthesis it uses as a nitro group incorporated reagent.
45. Is HNO3 triatomic?
Yes HNO3 is triatomic as it contains N, O, and H atoms.
46. Is HNO3 volatile?
Yes, it is more volatile than H2SO4.
47. why HNO3 is yellow?
When HNO3 lasted for a long time, then oxide of N is deposited and for this reason, the color of HNO3 is yellow.
Conclusion
HNO3 is a monobasic strong acid in liquid form. It is used as a reagent in different chemical syntheses.
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.
In this article we will discuss about the Fe3+ Lewis structure , characteristics 15 facts we should know.
A Ferric ion or Fe3+ is a trivalent metal cation and a monoatomic trication. It is the oxidized form of iron (Fe) metal.
How to draw Fe3+Lewis structure ?
While drawing the Lewis structure of any molecule or ion the number of electrons that take part in bond formation plays an important role. In order to draw the Lewis structure of an ion or molecule, the number of valence electrons is considered for the Lewis dot structure and other electrons which participate in bond formation also play an important in Fe3+ Lewis structure.
When three electrons are lost from an iron atom it forms a ferric ion or Fe3+. The electronic configuration is as follows,
Fe = 1s2 2s2 2p6 3s2 3p6 3d6 4s2. and Fe3+ = 1s2 2s2 2p63s2 3p6 3d5
Ferric ion (Fe3+) has only one resonating structure is same as that of its Lewis structure. because ferric ion (Fe3+) does not contribute in delocalization of electrons or delocalization of double bonds in its chemical structure . Hence (ferric ion) Fe3+ Lewis structure shows only one resonance structure.
Resonance structure of Fe3+
Fe3+ Lewis structure shape
Ferric ion (Fe3+) does not undergo any hybridization as it is in the ionic form, it does not show any specific shape. When it is combined with another metal or undergoes complex ion formation then it shows some shape according to its hybridization.
Fe3+ Lewis structure formal charge
In the (Ferric ion) Fe3+ Lewis structure number of actual charges corresponds to total formal charges. The formal charges are calculated by the Fe3+ Lewis structure which is calculated by the following formula,
The formal charge on Fe3+ ion = valence electron of Fe3+ – lone pair of Fe3+ -1/2 (bond pair of electrons)
According to the formal charge calculation formula, Fe3+is not a molecule and it’s an ion. It doesn’t take part in any chemical bond hence it has no formal charges on itself.
Fe3+ Lewis structure angle
The bond angle is the angle which is formed by the bonds present in the molecule, In (Ferric ion) Fe3+ Lewis structure does not show a bond angle, because it is an ion which does not form a bond in them when this ferric ion forms any molecule or complex then it shows some bond angle.
Fe3+ Lewis structure octet rule
In the case of the Fe3+ ion, its octet is fulfilled. When a ferric ion loses three electrons then its outermost shell completes its octet and becomes stable. The outermost electronic configuration of Fe is [Ar] 3d6 4s2 and Fe3+ is [Ar] 3d5so Fe 3+ is stable by completing its octet.
Fe3+ lewis structure lone pairs
Lone pair of electrons are those pair of electrons which does not take part in a chemical reaction , The lone pair of an electron in an atom can be calculated by subtracting no. of electrons shared by the atom from the valence electrons and divided by two. There is no lone pair of electrons in the Fe3+ Lewis structure.
Fe3+ valence electrons
Valence electrons are the electrons which are present in the outermost orbital of an atom, ion or molecule. These valence electrons take part in chemical bond formation. In ferric ion (Fe3+) outermost shell contains 5 valence electrons that is Fe3+ = [Ar] 5d5
Fe3+ hybridization
Hybridization is a process in which the atomic orbital of molecules combines to form a new hybrid orbital. In ferric ion, it does not have atomic orbitals hence it does not undergo Since Fe3+ is an ionic compound. So Fe3+Lewis structure does not show any hybridization.
Fe3+ solubility
Generally, the salt of Fe+3 is insoluble and Fe+2 soluble because Fe+3 salt is more covalent in nature than Fe+2 salt. covalent compounds are more soluble than ionic compounds.
Is Fe3+ acidic or basic?
A compound or an ionic species has a capacity to accept an electron which means the compound or an ion has a vacant orbital in their outermost orbital. Electron configuration for Fe3+ is 1s2 2s2 2p6 3s2 3p6 4s0 3d5. Here Fe3+ ion has 4s and 5d vacant orbital so the ferric ion can accept three electrons for completing its outermost shell It makes Fe3+ Acidic in nature.
Is Fe3+ polar or nonpolar ?
If the molecule is symmetrical or unsymmetrical structure the charge distribution among themselves is uneven or even, so their dipole moments become zero or non-zero. A Ferric ion is an ionic compound so we cannot determine the polarity of that Fe3+ ion.
Is Fe3+ a lewis acid or base?
A compound or an ionic species has a capacity to accept an electron which means the compound or an ion has a vacant orbital in their outermost orbital. Electron configuration for Fe3+ is 1s2 2s2 2p6 3s2 3p6 4s0 3d5. Here Fe3+ ion has 4s and 5d vacant orbital so the ferric ion can accept three electrons for completing its outermost shell It makes Fe3+ a Lewis Acid.
Is Fe3+ paramagnetic or diamagnetic ?
Ferric ion (Fe3+) shows paramagnetic nature . because ferric ion contain more unpaired electrons which are 5 in number hence it is weekly attracted by external magnetic field and form internal induced magnetic field in opposite direction.
while ferrous ion (Fe2+) contain less unpaired electrons hence less paramagnetic in nature. Also those atoms , ions or molecule which contain lone pair electrons or vacant outermost orbital has a paramagnetic in nature while those atom, ion or molecule contain all paired electrons are diamagnetic in nature .
Is Fe3+ reduced or oxidized ?
Ferric ions (Fe3+) is the oxidized form of iron (Fe). When the element or atom loses or gain its electrons and form a reduced or oxidized form of an element or an atom. Iron oxidizes to ferric ions. When iron loses three electrons from its outermost orbital it forms a ferric ion (Fe3+).
Conclusion
In the above article we will discuss the Lewis structure of Fe3+ ion also we will discuss the Lewis structure shape, hybridization, bond angle , lone pair , valence electrons , paramagnetic nature, Lewis acid property , oxidation property, non polar nature , solubility octet rule of ferric ion (Fe3+).
f2 lewis structure and all other details are going to be discussed in this article.
Fluorine is a chemical element, which is present in the P block of the periodic table. It is present in the second period and the seventeenth group of the periodic table. It exists in the atmosphere as difluorine gas and, is a halogen. It is denoted by the symbol F. Fluorine has an atomic number of 9 and atomic mass of 18.99g/mol. It is the lightest of all the halogens and is highly electronegative. It is also highly toxic in nature and highly reactive. It reacts with every element expect for Ar, Ne, He.
It exists as both solid and gas. In it’s solid form it has a bright yellow colour, it acquires a pale yellow colour when in gaseous nature. It’s solid form is has two types: Alpha and beta form. Alpha is opaque in nature and beta is transparent in nature. It has a melting point and boiling point of -219.67°C and -188.11°C respectively.
Its density is found to be 1.696 g/L (STP). It’s crystalline structure is cubic. It is prepared through different methods. Hydrogen fluoride or hydro fluoric acid is the precursor of fluorine.
Applications
1) Production of nuclear material for nuclear power plants. 2) Insulation of electric towers. 3) Hydrogen Fluoride is used to etch glasses. 4) Fluorine is used to make Teflon. Teflon in turn, is used to make a special type of plastic called PTFE which is flexible and has high heat resistance. This is possible because Fluorine has high boiling point.
Teflon is also used in dental health. 5) Fluorine is used as refrigerants. 6) Enrichment of Uranium by UF6 gas.
Lewis Structure of F2
Lewis structure of a compound denotes the electronic arrangements or representation of the combining atoms. Lewis structure can be drawn for any molecules. There are certain rules to draw the Lewis structure of F2. They are as follows
Calculate the total number of electrons. Fluorine has seven electrons in its valence shell. So F2 has total 14 electrons.
Write the symbol of two fluorine atoms surrounded with their seven valence electrons.
Valence Electrons in F2
Make a bond with the two Fluorine atoms and calculate their formal charge. It is found to be zero for both the Fluorine atoms. So this will be the most stable Lewis structure of difluorine molecule.
Resonance is the movement of electrons within the molecule to make more than one structure. While doing resonance the stability of the molecule wouldn’t change.
Here in the case of difluorine when its lone pairs gets involved in resonance then the formal charge of the molecule tends to increase. So that can’t be a stable structure. So there is no resonance structure found for difluorine. Mostly resonance is seen in compounds with either double bond or lone pair of electrons.
Formal Charge in F2
The equation for finding the formal charge of a compound is
Formal charge = Valence electrons – No. of lone pairs of electrons – No. of Bonds
The formal charge of both the Fluorine atoms is = 7 – 6 – 1 = 0
So the formal charge of difluorine is zero.
Valence electrons in F2
The total number of electrons seen in the outer shell of an atom is its valence electrons. The sum total of electrons in difluorine is 14 electrons.
Octet Rule in F2
According to octet rule there should be eight electrons in the valence shell of an atom after bond construction. When we look into difluorine there are total eight electrons in their outermost shell. Each fluorine has six electrons as lone pairs and two in bond making. So in total there is eight electrons in the outer shell.
Octet Rule in F2
Lone Pairs in F2
The electrons which don’t participate in bond making procedure is found to be the non – bonding or lone pair of electrons of an atom. Here each fluorine has three pairs. So in total difluorine has six lone pairs or twelve electrons as lone pairs.
Shape and Bond Angle of F2
The shape of the molecule is linear with 1800 bond angle. Here both the Fluorine atoms are joined by a single bond surrounded with its lone pairs. It can also have tetrahedral geometry with one fluorine in the tetrahedral with corners having three lone pairs.
Shape and Angle of F2
Hybridisation in F2
Hybridisation of difluorine is sp3 hybridization. The electronic configuration of fluorine is 1s2 2s2 2px2 2py2 2pz1. All the 2p orbitals except 2pz is filled. So the 2pz orbitals of two Fluorine atoms shares their electrons each other to form a single bond. Another way of finding hybridization is through finding the steric number. Steric number is the sum of Sigma bonds and lone pairs in a molecule. Here there is one Sigma bond and three lone pairs. So four is its steric number.
When a molecule’s steric number is four then it follows sp3 hybridization. According to this concept it may have tetrahedral geometry with bond angle 1090
Solubility of F2
Fluorine is found to be very soluble in water. It reacts with water to form hydrogen fluoride gas or hydrofluoric acid.
Is F2 Ionic or not ?
Difluorine is a covalent compound with one single bond between the two Fluorine atoms.
Is F2 Acidic or not ?
Difluorine is a Lewis acid. Due to the electronegative nature of fluorine it accepts electron pairs and acts as Lewis acid.
Is F2 is Polar or not ?
Difluorine is non- polar in nature. We all know that fluorine is an electronegative element and it should be polar in nature. But the arrangement of fluorine atoms in difluorine is symmetrical. So the polarity of each element got cancelled and as a result it exist as non- polar molecule.
Is F2 is Tetrahedral or Linear ?
The arrangement of two fluorine atoms in difluorine is symmetrical. So it’s a molecule with linear structure.
Is F2 Paramagnetic or diamagnetic ?
Difluorine is a diamagnetic substance. Magnetic properties of an atom or a molecule can be understood by checking whether it has paired or unpaired electrons. If a molecule has paired electrons it is diamagnetic and with unpaired electrons paramagnetic. Here difluorine doesn’t have any unpaired electrons. So it is diamagnetic is nature.
Is Cu2+ is Paramagnetic or diamagnetic ?
Cu2+ is paramagnetic substance. The general electronic configuration of Cu is 3d9 4s2. For attaining more stability one of the electron from 4s level get promoted to 3d. So now it’s electronic configuration is 3d10 4s1 . Cu2+ is copper atom lost with two electrons. When copper losses it’s two electrons the configuration changes to 3d9 4s0 . Here there is one unpaired electron. So it is paramagnetic in nature.
Electronic Configuration in Cu2+
Is F2 Oxidising or Reducing Agent ?
Difluorine is a strong oxidising agent. Because it can accepts electrons from other compounds due to its high electronegativity. Since it is used to oxidise another substance we can consider difluorine as a strong oxidising agent.
Conclusion
This article briefly explains all the facts regarding difluorine molecule. Fluorine exits as difluorine gas with pale yellow color. It has six lone pairs with sp3 hybridisation. It is non polar due to linear or symmetrical shape with angle 1800. It has varoius applications in many fields.
H2S is a colorless gas, carries pungent smell like rotten egg, mainly used for producing Sulfuric acid, Sulfur, creating pesticides also used in nuclear power plant.
The article describes the H2S lewis structure with other properties it has which can be describe from the hybridization of the structure and the ‘d’ orbital that Sulfur carries.
How to draw H2s lewis structure?
With the atomic symbols of Sulfur (S) and Hydrogen (H), the H2S lewis structure shows the outer orbit electrons distribution, spreading around the particular atom and sharing electron cloud with neighbor atom in GeCl4 molecule.
Count the total valence electrons:
In modern Periodic table the Sulfur atom is in group 16 with electronic distribution in 3s and 3p orbital, that is [Ne] 3s2 3p4 and Hydrogen atom contains only one electron its outer orbital as a group 1 element, so total eight loosely bonded valence electrons are there to form covalent bond.
Draw the skeletal of H2S lewis structure:
As Hydrogen atom can’t coordinate with more than one atom so Sulfur become central atom and two Hydrogen atoms are written on the opposite sides. This H2S lewis structure follows the Octet rule with electron sharing and also has zero formal charge.
H2S lewis structure
H2s lewis structure resonance
H2S lewis structure can’t form resonating structure as the ligand has no ‘d’ orbital for delocalization of electrons and also ligand atom has no unshared electron which can delocalize to the vacant 3d orbital of central atom Sulfur.
In spite of having 3d vacant orbital as a 3rd period element canonical structure can’t form as the only one electron of Hydrogen atom is already involved in the covalent bonding.
H2s lewis structure shape
According to VBT theory molecular geometry and shape are two slightly different things if the central atom has unshared electrons, which can be clearly understood by the hybridization of orbital of the central atom of a covalent molecule.
From the intermixing of orbital of the Sulfur atom in the H2S lewis structure generate hybrid orbital which is sp3, the geometry of the molecule should be tetrahedral type as for the AX2E2 where X stands for Hydrogen atom and E for electron lone pair.
But for the steric repulsion between lone pairs in the structure which Sulfur carries make the geometry disturbed from its original form and the angle between the bonding orbitals decreases forms a bent ‘V’ like shape.
H2S lewis acid structure shape
H2s lewis structure formal charge
Formal charge of H2S lewis structure is zero, calculated to check stability of the canonical form with help of total outer shell electron, bonding electron cloud and unshared electron and assuming that the bonding electron are distributed equally.
In the molecule only Sulfur atom has four electrons that not take part in bonding, so formal charge for the central atom Sulfur is = {6- 4- (4/2)} = 0 and without any nonbonding electron formal charge for the each Hydrogen atom is = {1- 0- (2/2)} = 0.
As both the constituent atom has zero formal charge, this particular canonical form of H2S also has zero formal charge which makes the structure energetically stable one.
H2s lewis structure angle
In the H2S lewis structure, the intermixing 3s, 3p orbital form sp3 hybridized orbital, so the covalent bond angle should be 109.5̊ but it is lowered to 92.1̊ by the steric repulsion between dense two non bonding electron pair of ‘S’.
For decreasing the bond angle (angle between the overlapping bonding orbital), the angle between the two nonbonding electron pairs increases for stabilizing the electron dot structure from the repulsion of dense lone electron pairs.
The angle between the bonding electron pair and non bonding electron pair is also decreased to adjust the new ‘V’ like bent structure.
H2s lewis structure octet rule
Last filled orbit, specific energy wave function must have eight electrons for satisfy the energy of stability of the particular canonical form, known as Octet rule which naturally can be seen in inactive inert gas molecules.
From the Periodic table we can say Sulfur needs two more electrons to cover the 3p orbital where Hydrogen needs only one electron to stabilize its configuration like Helium, so both shares electron cloud and cover up their last filled shells.
H2s lewis structure lone pairs
Lone pair are those valence electron pair with higher electronic concentration which does not take part in the bond formation and causes steric repulsion with bonding electron cloud and disturbs the geometry of a molecule.
From the hybridization we see the Sulfur has two electrons in 3s and another two in 3p which don’t take part in bond formation with Hydrogen, remaining as lone pairs over Sulfur atom where the one electron of Hydrogen involves in bonding, so no lone pair over Hydrogen.
H2s valence electrons
The last filled shell containing electrons are valence electrons which are far apart from nucleus so loosely bound by nuclear attraction and if ‘d’ orbital is there they become more energetically available for excitation in the chemical reaction.
Being a ‘p’ block element of group 16 in 3rd Period, Sulfur contains two electrons in 3s and four in 3p whereas each of the two Hydrogen atoms has one electron in their 1s orbital, so total eight loosely bounded electrons are energetically available for bonding.
H2s hybridization
Hybridization is the concept where not equivalent atomic orbitals intermix to give same energy hybrid orbital, the concept is used for central atom of covalent molecule for understanding the better orbital overlapping in the molecule.
As a ‘p’ block atom the central atom Sulfur has six outer shell electrons in 3s and 3p, the orbitals mixes up, creates new hybrid orbital ‘sp3’ with new shape and energy than previous, which carry 25% ‘s’ character and 75% ‘p’ character and overlap with H2 1s orbital.
From this hybridization we can say that the covalent nature is greater in the molecule as it contains more ‘p’ character and electro-negativity of Sulfur is also not much because the greater the hybrid orbital carry the ‘S’ character greater its electro- negative nature become.
H2s solubility
Solubility of H2S in solvent is determined by the concentration of H2s at the equilibrium of the reaction, as a covalent compound of weak dipole- dipole interaction it is gas at room temperature making low solubility in water.
H2S solubility in water is 4 g/dm at 20̊ C so it is slightly soluble in water which can be described by the dipole moment present in the molecule.
In spite of having non polar bonding for low difference in electro-negativity H2S lewis structure is polar for presence of the dipole moment which causes delta charge separation and as a result H2S slightly soluble in polar solvent like H2O.
Is H2s an electrolyte?
Electrolytes are the compound generally made by metal and non-metal or semiconductor as they can fully ionized in solution to carry the electronic charge make them good electrolytes.
As both Sulfur and Hydrogen are non- metal so they can’t fully oxidized so can’t be goof electrolyte, it only slightly dissociates in water.
Is H2s acidic or basic?
H2S acts as a bronsted acid as it forms (HS-) by donating a hydrogen ion (H+) when it slightly soluble in water, hence it is weak acid in nature by donating one proton, another proton releasing is quite energy requiring process.
With pKa 7.0 it can turns a blue litmus paper in red color by the formation of bisulfide (HS-) indicates its acidic nature as (SH-) can be stabilized for the bulky size of the Sulfur which accelerate the (H+) ion releasing process.
Is h2s a strong acid?
An acid which completely dissociates in its components ions are known as strong acid but after one proton donation H2S forms (HS-) ion and the dissociation constant for 2nd step of the reaction is too small, makes it a weak acid.
Is H2s polar or nonpolar?
In the H2S lewis structure, electro-negativity of ‘S’ is 2.58 and that of ‘H’ is 2.20 on the basis of Pauling scale, makes bond electron cloud pulling capability difference by 0.38, which is quietly less, results a non-polar bond but creates some charge separation denoted as delta (δ).
The delta charge separation creates a dipole moment with certain direction in the structure. The structure also contains lone pairs which also have some vector direction of polarity and overall for bent structure both can’t cancel out and H2S become a polar molecule.
polarity of H2S lewis structure
Is H2s a lewis acid or base?
H2S lewis structure contains sulfur atom which has vacant 3d orbital to accept electron pair from donor to act as lewis acid and also the structure contains nonbonding electron pairs can do nucleophilic attack to act as lewis base.
In water it accept electron in its vacant 3d orbital to form hydronium ion (H3O+), becomes a lewis acid (accept electron pair from donor).
In presence of strong acid like H2SO4 it donate electron to form new S-H bond results in H3S+ formation which indicates the lewis base (can transfer electron pair to acceptor) character of H2S lewis structure.
Is H2s linear?
H2S can’t be linear although it can form a linear H-S-H configuration but this is distorted as Central atom Sulfur contains nonbonding two electrons in 3s and two in 3p which causes steric repulsion and according to VSEPR theory causes bent form.
According to this theory as lone pairs only concentrate over parent atom, having more electronic density it causes greater inter lone pair repulsion than lone pair- bond pair and the bond angle decreases causes bent molecule.
Is H2s paramagnetic or diamagnetic?
The magnetic property of H2S lewis structure can be explained by the electronic arrangement of the central atom Sulfur, after bonding with Hydrogen 1s electron there is no unpaired electron remains in the sp3 orbital of ‘S’.
As all the electrons are paired up so the electrons with opposite spin can cancel out each other’s magnetic field, so H2S lewis structure become diamagnetic in nature but for paramagnetic there will be at least one unpaired electron.
H2s boiling point
Boiling point is dependent on the environment pressure, in a constant pressure at which temperature the vapour pressure of liquid and atmospheric pressure of the environment of liquid come in equilibrium that is called boiling point of that temp.
The measuring boiling point of H2S lewis structure is (-60̊ C), the low value is because of the covalent nature of the molecule so the attraction between the atoms are lesser than ionic compounds, results in easily bond breaking, also there is no Hydrogen bonding.
H2s bond angle
The angle between covalent bonding which is formed by hybridized orbital overlapping, is 92.1 which is measured depending on hybridization of outer orbital of central atom, Sulfur has four such electrons which not participate in bonding.
In the H2S lewis structure, the 4s and 4p orbital of Sulfur atom intermixes, form sp3 hybridized orbital, so the bond angle should be 109.5̊ but it is lowered by the steric repulsion between non bonding electron pair of ‘S’ as they have more electronic density.
Is h2s corrosive?
H2S is corrosive in nature but it alone with water can’t cause much damage. H2S can react with water and gives (H+) ion as a weak acid, so it the source of (H+) ions and act as a catalyst in absorption of (H+) ion on steel causes cracking in steel.
In the reaction Sulfide is formed so the corrosion can cause discolor of the copper or silver as it can form a thin black cover, in case of silver it produces Silver sulfide (black).
Does H2S have conductivity?
H2S lewis structure become metallic conductor type which can transfer electricity above a pressure of 90 giga-pascal, if it is cooled down and set the temperature below the critical temperature the high pressure state of H2S shows super conductivity.
Is h2s coloured?
H2S is a colorless gas compound but for its reducing agent nature the color can be changed with long time.
Normally the compound with transition metal element which contains ‘d’ orbital shows color for as there electronic transition can be took part and the color it shows is the complementary color related to the energy which releases in the electron emission process.
Is h2s odorless?
H2S has a specific rotten egg type smell where compounds with Sulfur have some pungent smell but only it has specific characteristic odor, smelling which is not harmful for human but causes some uneasiness in health.
Is h2s capable of dipole dipole interactions?
Dipole moment of a covalent bond has magnitude with a specific vector direction which causes a charge separation between delta positive and delta negative which can be seen in the H2S lewis structure, for the electro negativity difference of atoms.
When two molecules of H2S approach each other there dipole- dipole interaction occurs between the delta positive Hydrogen atom of one molecule and delta negative Sulfur of another molecule which is a weak interaction but stronger than London interaction.
Is h2s permanent dipole?
The dipole moment which is produced in the H2S lewis structure is permanent as it is based on the difference of the electron pulling capacity of its constituent atoms, not by induced effect from the environment.
If the dipole moment of the molecule is produced by the induction effect of environment then it can be normalized by controlling the environment but here in H2S lewis structure the dipole moment is permanent with value of 0.97 D.
Is h2s electron deficient?
Hydrides of Sulfur is not electron deficient as central atom Sulfur belongs from group 16 which makes proper covalent bonding with Hydrogen atoms by sharing the electron cloud, following the Octet rule properly.
Generally group 13 elements produces the covalent hydride compounds where the central atom outer shell is not filled up with eight electrons so they become electron deficient molecules.
Is h2s oxidizing agent?
H2S can’t act as an oxidizing agent as (-2) is the oxidation state of H2S lewis structure and H2S can’t produce lower oxidation state by accepting electron from a donor atom.
The Sulfur atom of other molecule which has (+) oxidation state in a molecule and can lower the oxidation state by accepting electron from donor can act as an oxidizing agent like H2SO4 where the oxidation state of Sulfur is (+6).
Is h2s fully oxidized?
Fully oxidized means here the releasing of (H+) ion in highest amount, but being a weak acid one H2S lewis structure can’t release two of its hydrogen atoms freely (high 2nd dissociation constant) though it is a diprotic acid.
It slightly dissociates in water to give (SH-) as a conjugate base as (H+) ion so H2S lewis structure is not fully oxidized always.
Is h2s reducing agent?
For having ‘d’ orbital Sulfur atom of H2S molecule can shows different oxidation states and can forms molecules with various coordination number where in H2S it has (-2) oxidation state.
This Oxidation state (hypothetical charge of an atom in a molecule) of Sulfur is lowest among all other Oxidation states so it can’t be lowered more so H2S act as a reducing agent as it can donate electron pair in redox reaction.
Does h2s form hydrogen bonds?
In spite of having dipole- dipole interaction there Hydrogen bonding can’t be formed between the H2S lewis structures, which can be seen only molecule having high electro negativity atom like ‘F’, ‘O’ or ‘N’ attached with any electro-positive atom.
Sulfur is quite less electro-negative (2.58) with respect to these electro- negative atoms so H-X bond (X=S) will not be that much polar that the Sulfur can induce dipole moment to Hydrogen atom of another H2S molecule and form any Hydrogen bonding.
Is h2s heavier than air?
H2S is slightly heavier than air as it is 1.19 times denser than air, so we can find that H2S gas gathers in the low lying spaces for the property.
Is h2s london dispersion?
As a hetero atomic molecule, with electro negativity difference between the constituent atom the H2S lewis structure possess some permanent dipole moment in the covalent bond of the molecule so have dipole-dipole interaction present.
For non polar symmetric molecules where is no dipole moment, there can be seen the London dispersion force between the molecules which is the weakest attraction force causes temporary dipole moment in molecules which is not for polar asymmetric H2S.
Is h2s monoprotic diprotic or triprotic?
H2S is a diprotic acid as it can release two Hydrogen ions (H+) in the solution though the 2nd dissociation constant is two low making the 2nd step slow.
In the 1st step of reaction (H+) is released with (HS-) where from one more (H+) ion can be released with precipitation of (S2-) ion, where the 1st dissociation constant is relatively higher.
Is h2s more acidic than h2o?
H2S is more acidic than water (H2O) which can be explained by two following reasons, one is the size of Sulfur which has ‘d’ orbital to accept electron pair and other reason is the strength of O-H bond is greater than S-H bond strength.
Being a group 16 member in period 3 makes Sulfur molecule more bulky than Oxygen which is in period 2 makes the conjugate base (SH-) more stable than (OH-), also ‘S’ has the diffused ‘d’ orbital which can bear nucleophilic attack and release (H+) ion in solvent.
In X-H (X= O / S) bond breaking the dissociation energy of bond plays an important role which is lower in case of H2S than H2O as the electro-negativity of Oxygen is greater to pull bonding electron cloud towards itself to fast and can release hydrogen ion.
But for higher electro-negativity the Oxygen of water (H2O) make intermolecular bond with Hydrogen atom of one molecule to Oxygen atom of another molecule which is very strong, requires more energy to dissociates result H2S stronger acid than H2O.
Is h2s more acidic than hbr?
No, H2S is less acidic (pKa = 7) than HBr (pKa = (-9)) which can be explained by electro-negativity difference between Bromine (Br) that is 2.96 and Sulfur (S) that is 2.58.
With greater electro negativity of an atom it can pull the bond electron cloud towards itself more easily so there will be a shift in electron cloud density makes easy for bond dissociation which not required energy too much.
Electronegative halogen atom Bromine can pull the Br-H electron cloud greater than in case of Sulfur in S-H bond and also Bromine is not as electro-negative as Oxyhen so the intermolecular hydrogen bonding is not so strong like H2O make HBr stronger acid than H2S.
Is h2s metal or nonmetal?
From Periodic table we know H2S lewis structure contains non metal elements like Sulfur and Hydrogen form group 16 and group 1 respectively, results in the forming of non metal molecule with combination between them.
As non metal molecule the boiling point of H2S is very low even it is in gas form at room temperature as there is no strong electrostatic attraction between atoms of the molecule, in spite they have weak dipole- dipole interaction between molecules.
Is h2s positive or negative?
To satisfy the octet rule the atoms of H2S lewis structure shares their valence electron cloud makes the molecule covalent in nature so it is neutral in nature without any positive or negative charge.
But as Sulfur and Hydrogen has some difference in electro-negativity (capacity of pulling the electron pair), dipole moment arise in the covalent bond which is 0.97 D, for this a slightly partial charge separation occurs in the molecule that is ‘S’ (δ+) and ‘H’ (δ-).
Is h2s pyramidal?
As per the Hybridization of the central Sulfur atom which occupying two non bonding electrons makes the geometry disturbed and form bent ‘V’ like not pyramidal which can be seen in AX3E type molecule with one lone pair.
The geometry of this type molecule should be tetrahedral but the bonding skeletal looks like pyramidal as the lone pair posses over one bonding direction in the tetrahedral geometry.
Is h2s symmetrical or asymmetrical?
H2S is a asymmetric molecule for which we can see that the dipole moments are not cancel out each other and the H2S lewis structure overall has a net dipole moment which causes polarity of the molecule in spite of having non polar bonds.
If this was a symmetrical molecule the vector directions of dipole moment can cancel out each other and H2S become non polar in nature which is not possible the electron pairs that Sulfur has which not participate in bonding with Hydrogen atoms.
Is h2s volatile?
H2S is much volatile than Sulfur’s upper periodic element Oxygen’s Hydride (water, H2O), even H2S lewis structure is in gas form in normal room temperature but water is in liquid form in room temperature.
This phenomenon can be described by the electro negativity of central atom and Hydrogen bond formation as a consequence of it. As there is no possibility for H2S lewis structure to form Hydrogen bonding they can be easily energized and stay in gas form.
If inter molecular Hydrogen bonding will there the molecules are tightly bonded with each other and for transfer them in gas form, high temperature will be required causes high boiling point.
Conclusion:
Being a covalent and slightly polar molecule it shows its properties sometimes different as central atom of H2S lewis structure has the vacant 3d orbital which can easily accept electron pairs from donor atom.
