AsF5 is an inorganic metalloid halide containing arsenic and five fluorine atoms in which the metalloid is the arsenic atom and the halide is the fluorine atom.
In asf5 Lewis structure Arsenic atom is bonded to five fluorine atoms in a trigonal bipyramidal shape by sharing the five electrons present in its valence shell to each of the five fluorine atoms attaining the sp3d hybridization. They are Lewis’s acid and are non-polar in nature.
Asf5 valence electrons
AsF5 compound has a total of 40 valence electrons in its valence shell (5 from arsenic and 35 valence electrons from five fluorine atoms).
From the periodic table, we can see that Arsenic atom belongs to the p block and comes under the group 15 (pnictogen). We know that from group 13 to 18 the valence electron number will be 10 minus the group number
As for fluorine atom it comes under the group 17th (Halogens)
Valence electrons of arsenic atom = 15- 10 = 5 valence electrons
Valence electrons of fluorine atom =17- 10 = 7 valence electrons
Then the total valence electrons number in AsF5 will be sum of the valence electrons of arsenic and 5 fluorine atoms.
5 +(7) 5 =40
The total valence electrons of AsF5 = 40 valence electrons.
Asf5 Lewis structure lone pairs
In AsF5 has no lone pair of electrons because all the 5 valence electrons of Arsenic atom are used to form five single bonds with five fluorine atoms.
The lone pair of an electron is an electron pair not shared with the other atoms in the bond formation.
Out of the 40 valence electrons in AsF5 10 electrons are used for bond formation and the remaining 30 valence electrons does not take part in bond formation. The 30 valence electrons are present in the valence shell of 5 fluorine atoms each taking 6 electrons (3 lone pairs).
So, the total lone pairs present in 5 fluorine atoms will be =30/2 =15 lone pairs
Each lone pair contains 2 electrons.
How to draw Asf5 Lewis structure?
Lewis structure of AsF5 is drawn by using the valence electrons of arsenic and fluorine atoms and following few steps.
Few steps to follow are;
1)Know the total number of valence electrons present in arsenic pentafluoride compound.
Arsenic atom has 5 valence electrons and fluorine atom has 7 valence electrons in its outer shell making the total valence electrons of AsF5 to be 40.
2)Select the central atom and place it at the center and the remaining atoms surrounding it.
The least electronegative atom is selected as the central atom to draw a Lewis structure it is because the least electronegative atom tends to share more of its electrons to the surrounding atoms
We know that the fluorine atom is considered the most electronegative atom. So, in AsF5 Arsenic atom is considered the central atom the 5 fluorine atoms are placed around the central atom arsenic.
3)The central atom and its surroundings undergo a chemical combination by pairing its valence electrons, forming a single (sigma) bond.
The 5 valence electrons of arsenic atoms pair with each electron of 5 fluorine atoms, and a single bond is formed.
Thus, 10 valence electrons take part in bond formation i.e. 5 from arsenic and 1 each from 5 fluorine atoms. So, there are 10 bonding electrons (5 bond pairs) and 30 non-bonded (15 lone pairs) electrons in AsF5.
4)In order to complete the remaining valence, electrons should be placed around the surrounding atoms.
The 5 valence electrons of arsenic atoms are used up, so the remaining 30 electrons belong to 5 fluorine atoms, and each fluorine atom requires 8 electrons to complete its octet.
The total number of non-bonded electrons present = 30
Number of surrounding atoms (Fluorine) present = 5
So, the number of atoms required by each surrounding atom =30/5 =6
Each 6 electrons are shared between the 5 fluorine atoms from 30 electrons and thus, each fluorine atom completes its octet (6 electrons from non-bonded electrons and 2 electrons from single bond with arsenic atom).
An arsenic atom will have a total of 10 electrons after bond formation (5 electrons from its valence shell and the other 5 electrons from 5 fluorine atoms shared during bond formation).
These are the steps to be followed, and that is how the AsF5 Lewis structure is drawn.
AsF5Lewis structure does not obey the octet rule because the arsenic atom has more than 8 electrons in its valence shell.
According to the octet rule, the atoms of various elements enter into chemical combinations in order to attain the eight-electron configuration in their outermost shell.
In AsF5 compound, Arsenic atom has a total of 10 electrons in its valence shell (arsenic forms 5 single bonds with 5 fluorine atoms) and more than 8 electrons with the expanded octet.
The reason is because the arsenic atom has a principal quantum number n = 4. Therefore, it has an empty 4d orbital in its shell which can take part in hybridization and thus have an expanded octet.
Asf5 Lewis structure formal charge
The formal charge of arsenic atom and the 5 fluorine atoms in Arsenic Pentafluoride Lewis structure is zero.
Formal charge on an atom in a Lewis structure = total number of valence electrons in the free atom -the total number of non-bonding (lone pair) electrons -half the total number of bonding electrons.
Formal charge on Arsenic atom
Total number of valence electrons in Arsenic atom = 5
Total number of non-bonding electrons in Arsenic = 0
Total number of bonding electrons in Arsenic atom =10
Formal charge = 5-0-10/2 =5-5 =0
Therefore, the formal charge of arsenic atom is = 0
Formal charge on fluorine atom
Total number of valence electrons in fluorine atom = 7
Total number of non-bonding electrons in fluorine = 6
Total number of bonding electrons in fluorine atom =2
Formal charge = 7-6-2/2 =7-6-1 =0
Therefore, the formal charge of fluorine atom is = 0
Thus, the total formal charge of the atoms in AsF5 will be = 0
Resonance is the movement of pi electrons or lone pair of electrons that are conjugated to the pi bonds within the compounds.
The reason for Arsenic Pentafluoride Lewis structure to not exhibit resonance is because it does not have pi electrons in its structure to resonate and also the lone pair electrons present in the fluorine atom does not take part in resonance.
Asf5 Lewis structure shape
AsF5 Lewis structure has trigonal bipyramidal shape containing 5 bond pair of electrons and 15 non-bonding (lone pair) pair of electrons.
Trigonal bipyramidal shape of AsF5
The shape of the AsF5 Lewis structure is determined according to the VSEPR theory. The central atom arsenic shares its 5 valence electrons with the 5 fluorine atoms. The 2 fluorine atoms are present in the axial position and 3 fluorine atoms are in the equatorial position.
Asf5 Lewis structure angle
AsF5 Lewis structure forms 2 bond angles 120o and 90o degree having trigonal bipyramidal geometry.
AsF5 bond angle
In AsF5 structure 3 fluorine atoms are present in the equatorial position and the bond angle formed between the 3 fluorine atom is 120o. The bond angle formed between the remaining 2 fluorine atoms present in the axial position is 90o.
The electronic configuration of As is [Ar] 3d10 4s2 4p3.
Electronic configuration box diagram of AsF5
Thus, AsF5 acquire sp3d hybridisation and have trigonal bipyramidal geometry.
Asf5 solubility
AsF5 is soluble in benzene, ethanol, dimethyl ether. They are easily hydrolysed by water and humid air to form arsenic and hydrogen fluoride. It forms white clouds in moist air.
Is Asf5 acidic or basic?
It is a strong Lewis acid fluoride. They act as a strong fluorine ion acceptor.
When arsenic pentafluoride reacts with Sulphur tetrafluoride, it readily accepts fluorine and becomes AsF6–.
AsF5 +SF4 –> SF3 +SF6–
Is Asf5 ionic?
AsF5 is a monomeric covalent compound.
The bond formed between the arsenic and 5 fluorine atoms is by sharing of electrons and not by the transferring of electrons completely between the atoms.
Is Asf5 polar or nonpolar?
Arsenic Pentafluoride is a non-polar compound.
According to the Pauling scale it should be polar because of the electronegativity difference between As and F atom.
But the compound has a symmetrical geometry due to its triagonal bipyramidal structure, the charge induced by all As-F bond will be cancelled out making the net dipole moment to become zero.
Conclusion
Lewis structure of AsF5 helped us to study about its geometry, formal charge, hybridization, bond angle and its polarity and some other facts related to it.
CO Lewis structure: Triple bond between C (sp hybridized) and O (sp^2 hybridized), 10 valence electrons total. C: 4e^-, O: 6e^-. Triple bond accounts for 6 shared electrons, O retains a lone pair (2e^-), fulfilling octet rule. Bond length approx. 112.8 pm, bond energy around 1072 kJ/mol.
How to draw CO Lewis structure ?
1.Basis on the periodic table, Lewis structure has 4 for carbon and 6 for oxygen. CO formed by adding carbon and oxygen. Oxygen is present in group 16. It is also called chalcogens. Carbon is present in group 14. The electronic configuration of both ,O = 1s2 2s2 2p4 (6 valence electrons) C = 1s2 2s2 2p2 (4 valence electrons).
C Valence ElectronO Valence Electron
2. Determine the Skeleton Structure
For CO, deciding the skeleton is straightforward because we only have two atoms. Typically, the less electronegative atom is in the center, but since hydrogen is the exception (and not part of CO), we don’t worry about that here. Between carbon and oxygen, carbon is less electronegative, so it will be our central atom.
3. Draw the Initial Bond
Connect the carbon and oxygen with a single line, which represents a pair of shared electrons, or a single bond. This uses up 2 of our 10 valence electrons, leaving us 8 more to distribute.
4. Distribute Remaining Electrons to Fulfill the Octet Rule
Now, we aim to fulfill the octet rule, where each atom prefers to have 8 electrons in its valence shell. Start with the more electronegative atom, which is oxygen. After placing the single bond, oxygen needs 6 more electrons to complete its octet. These can be placed as three pairs of dots around the oxygen atom.
At this point, carbon is only bonded to oxygen with a single bond, giving it just 2 electrons. Carbon needs 6 more electrons to satisfy its octet.
5. Adjust for the Octet Rule
Since a single bond leaves both carbon and oxygen short of completing their octet, we need to introduce multiple bonds between them. A triple bond solves this issue. This means we draw two more lines (for a total of three) between carbon and oxygen, indicating three pairs of shared electrons (or six electrons). This bonding scenario allows both carbon and oxygen to achieve their octet with the total of 10 valence electrons we started with.
6. Add Lone Pairs
After forming the triple bond, place any remaining electrons as lone pairs. Oxygen will end up with one lone pair (two electrons) since it shares six electrons with carbon through the triple bond. Carbon’s octet is fulfilled entirely by its bonding with oxygen, so it doesn’t have lone pairs in this structure.
The Lewis structure for CO ends up showing carbon and oxygen connected by a triple bond, with oxygen also having a lone pair of electrons. This structure accounts for all 10 valence electrons, adheres to the octet rule for both atoms, and illustrates the strong triple bond that characterizes the carbon monoxide molecule.
CO Lewis structure shape:
Carbon monoxide lewis structure is a linear molecule. The shape is linear, having triple bond between carbon and oxygen. Carbon as well as Oxygen contained one pair of lone electrons in their structure. Carbon and oxygen combined with triple bond, means here 1 sigma and two pi bonds will present. Carbon monoxide mainly produced by the partial combustion of fossil fuels.
It can cause acute illness and worst case scenario is the death.In the periodic table carbon is less electronegative value than oxygen. Carbon having E.N value 2.5 and oxygen having E.N value 3.5. The shape will be confirmed linear because the bond angle is 180°.
If we take another probability , Four electrons are involved in chemical bond. Here the formal charge of carbon will be zero. So we get Formal charge of oxygen in CO is 6-4-2 = 6-6= 0. So it can be the best lewis structure having formal charges zero. The percentages of abundance are 40%.
Another probability is carbon and oxygen singly boded with each other. Here carbon having 1 lone pair and oxygen having 3 lone pairs.In the periodic table, carbon has 4 valence electrons. The percentages of abundance of this lewis structure is 10%.
CO Lewis structure lone pairs:
Basis on the best lewis Structure of CO. Two lone pair of electrons is present on the carbon atom and one oxygen atom. Geometry of CO should be linear in this because there are 2 lone pairs and the bonds are straight. Here we should know that to detect the shape of the molecule the lone pair will not be counted. The molecule is considered is linear molecule by nature.
Hybridization of CO:
The hybridization of carbon and oxygen in the carbon monoxide Lewis structure is sp. Carbon and oxygen have triple bond in between it. One unshared pair of electron in carbon and oxygen present in both.
Carbon carries negative charge and oxygen carries positive charge here. Two sp hybridized orbitals of the carbon atom overlap with two p orbitals of oxygen to form 2 Sigma bonds. Other 2 electrons of carbon are involved in pi-pi bonding.
CO Lewis structure is consist of two atom .One is oxygen and other one is carbon. CO is carbon monoxide, bonded by triple bond. It has no odor.
CO Lewis structure resonance:
Resonance is the Latin word come from the word “Resonatia”. It is otherwise known as mesmerism. This is the way to draw different bonding to describe the structure. Certain molecules are several type of contributing structure called resonance hybrid or canonical structure. The different delocalization can be showed through it. There are 3 type of resonating structure: 1. Resonating structure-1 2. Resonating structure-2 3. Resonating structure-3
1. Resonating structure-1 In this case carbon is bonded with oxygen by triple bond. Carbon and oxygen both have one pair of lone pair electrons in it. Oxygen shared one lone pair of electron with carbon to complete their octet .The resonate structure is found in 50% of abundance. 2. Resonating structure-2 We can draw 2nd resonating structure by making double bond in between carbon and oxygen. Carbon has four valence electrons.The formal charge is zero here. So it is the best resonating structure we can say. This resonating structure is found in 40% of abundance. 3. Resonating structure -3 It is found where carbon and oxygen is singly bonded with each other. Carbon has 4 valence electrons, 2 dots and 1bond present in it. So formal charge of carbon is, 4-2-1= +1. Oxygen has 6 valence electrons, 6 dots and 1bond, so the formal charge is 6-6-1= -1.The resonating structure is found only in 10% of abundance.
CO Lewis structure octet rule:
Octet rule is used to build a compound in stable form. In CO Lewis structure, the octet rule is fulfilled when carbon bonded with oxygen by triple bond. One pair of lone pair shared by oxygen to carbon to form a dative bond. By this the carbon and oxygen both obey the octet rule.
CO Lewis structure is polar in nature. It is produced by the incomplete burning of fossil fuels. CO is most toxic gas. It can cause acute illness and in worst case scenarios that is death. It is most common type of fatal poisoning in the whole world.
Conclusion:
Carbon monoxide molecules consist of carbon atom covalently boned with oxygen atom. In CO molecule C-O Length is 112.8 pm. It is toxic gas. The shape is linear. Each of the atom contain one lone pairs.
SO2 Lewis structure shows various chemical properties of the compound. There are so many facts about the internal structure obtained from drawing of lewis structure.
By using the lewis concept we can draw the best resonate structure for sulfur dioxide. We can understand the boding between atoms in a SO2 molecule. So we are going to study how the best structure we can determined by knowing shape , hybridization etc.
How to draw lewis structure for SO2 ?
Sulfur dioxide lewis structure of SO2 , first we require the total valence electrons of both sulfur and oxygen. There are 6 valence electrons of sulfur and oxygen. This bonded with single bond than sulfur didn’t obey the octet rule.This lewis structure is unstable. If one electron pair of oxygen is bonded with sulfur than another lewis structure is found. In this way ,sulfur and oxygen both obey the octet rule .Similarly if another electron from other oxygen bonded with sulfur than double bond will created. Here sulfur didn’t obey the octet rule. Sulfur contain 10 electrons. This is best lewis structure theoretically. But practically this is not really found.
SO2 lewis structure consists of Sulphur and oxygen. The chemical formula of sulfur dioxide is SO2. This is color less gas. Smell of SO2 is very much pungent odor. The smell is very much similar to the burnt matchsticks Sulfur dioxide released while volcanic eruptions.
SO2 lewis structure shape:
The shape of the SO2 is in bent shape.We can found the molecular geometry of SO2 in 2 ways. From 1st lewis structure of SO2 , where the unbounded electrons are spread up in three dimensions. This is because electron are repel to each other.
The lewis structure doesn’t tell us directly but if we visual the atoms in unbonded electron of central atom, repelling each other. Where the oxygen is move away from each other , give the molecule in bent shape.
That is by the valence shellelectron pair repulsion theory that is VSEPR theory. In the second way, the geometry of SO2 is trigonal planner. The three pairs of bonding electron is in 109° angel.
SO2 lewis structure of total valence electrons 18.Sulfur and oxygen has six electrons. sulfur has six valence electrons, 2 non bonding and 6 bonding electrons. Six bonding electrons divided by 2 , we get 3 electrons. So the Formal charge of sulfur is 6-2-3 =+1. One of the oxygen having formal charge +1. The formal charge of another oxygen will be 6-4-2= 0.
Take 2 electrons from another oxygen to sulfur make double bond in sulfur and oxygen. Sulfur has 6 valence electrons, 2 non bonding electrons and 8 bonding electrons. This bonding electrons divided by 2 , we get 4. By putting formula ,6-2-4=0. The formal charge of sulfur is 0.
Oxygen contain 6 valence electron,2 non bonding electrons and 2 bonds So we get 6-4-2=0. The formal charge of oxygen is zero. similarly other oxygen also has 0 formal charge. This is the most reasonable structure for SO2.
SO2 lewis structure lone pairs :
In the best reasonable structure ,the lone pairs of sulfur atom is one . The lone pairs of oxygen atom in each of SO2 lewis structure is two.There are total five lone pairs on SO2 atom.
It is the measure component of green house effect. This causes global warming.Scientists also have proved , that the SO2 is found in Venus and in other bodies of solar system also. SO2 is manufactured in industrial area byburning sulfur and its components in the presence of oxygen.
SO2 hybridization:
The hybridization takes place in SO2 is sp2 type . For formation of SO2 ,we need 2 double bond outside the sulfur atom, while sulfur is in the middle or central. During formation of SO2 , the hybridization used is SP2. There are 2 sigma, 2 pi and one lone pair of electrons. The SO2 is in bent shape.
It is the measure component of green house effect. This causes global warming. Scientists also have proved , that the SO2 is found in Venus and in other bodies of solar system also. SO2 is manufactured in industrial area by burning sulfur and its components in the presence of oxygen.
SO2 Lewis structure resonance:
There are two resonating structure in laboratory side. The least electronegative atom in the middle that is Sulphur and oxygen beside it. So contribution of the electron gives the best resonate structure.
This contribution of the electron gives the best resonate structure. This contribution equally to the overall hybrid structure of molecule. While the third one is best one only in theory. It doesn’t quite match with experimental data.
SO2 Lewis structure octet rule:
The sulfur doesn’t obey the octet rule is SO2 Lewis structure. Sulfur can carry more than 8 electrons. In SO2 sulfur carry 10 electrons. While oxygen obey the octet rule, SO2 emission are a precursor to acid rain and atmospheric particulates.
Conclusion:
To wrap with the post we can say that SO2 is an compound having V-shaped or bent. The bond angle between the atoms is 109 degree. The hybridization type is sp2 with bond order 1.5. The bond dissociation enthalpy is 297kj/mole. It forming three hybrid orbitals in their structure.
BaSO4 is the chemical formula for Barium sulphate. It is the sulphate salts of barium metal which is alkaline and a divalent metal.
BaSO4 (barium sulphate) is the whitish or yellow small crystalline powder which has no odour. It is not soluble in water, R-OH groups and dilute acids, but soluble in hot concentrated H2SO4 (sulphuric acid). Its IUPAC name is barium (2+) sulphate. Molecular weight of barium sulphate is 233.39.
How to draw BaSO4 lewis structure?
To draw the barium sulphate i.e. BaSO4 lewis structure, we have to recognize that the barium is a metal and the SO4 (sulphate ion) is a non- metal also consider as a polyatomic ion. Metals and non- metals forms an ionic compound together. So, the metals get transfer their electrons to the non- metal part of the compound. Thus, the barium metal gets transfer their electrons to the sulphate ion.
So, to write the BaSO4 lewis structure, we have to write first Barium which is a metal and then we have to add the sulphate ion group next to which is a non- metal to the structure. The barium metal get transfer its electron to the sulphate ion non- metal. Barium metal belongs to the group two of the periodic table, thus it has two valence electrons in its valence shell. So, Barium transfers its 2 valence electrons to SO4 ion.
The electrons are negatively charged, so Ba transfers its two negative charges to SO4 ion. Due to which the two positive (2+) charge creates on Ba metal and the SO4 ion accepts the two electrons from Ba metal creates a two negative (2-) charge on SO4 ion. We have the brackets around SO4 ion to show the electron transfer from Ba to SO4 i.e. the Ba lost electrons and sulphate gain them, so they are not sharing electrons like we do in a covalent bond.
Barium metal belongs to the second group of the periodic table, so it has two valence electrons in its valence shell. Sulphur atom belongs to the 16th group of the periodic table so it has six electrons in its valence shell. Oxygen atom also belongs to the 16th group of the periodic table so it also has six valence electrons.
In SO4 ion, sulphur atom attached to the four oxygen atoms and also there is a 2- charge on SO4 ion, so the valence electrons for SO4 ion are:
Ba metal has 2+ formal charges as it donates its two valence electrons to SO4 ion in BaSO4 lewis structure.
Also SO4 ion has 2- formal charge as it accepts two electrons from Ba metal in BaSO4 lewis structure.
In SO4 ion, central sulphur atom gets attached with four oxygen atoms with covalent bonds. So the formal charge for SO4 ion is as follows:
Formal charge for S atom = ( 6 – 0 – 8/2 ) = +2
Formal charge for O atom = ( 6 – 6 – 2/2 ) = -1
Formal charges on SO4 ion
BaSO4 lewis structure octet rule
Octet rule tells us about the presence of eight electrons in outer shell of any atom. Barium metal belongs to the 2nd group of the periodic table so it has two valence electrons in its outer valence shell orbital, as there are not eight electrons present in Ba atom so it has incomplete octet.
In SO4 ion, generally sulphur and oxygen atoms has complete octet as they both has eight – eight electrons, but with complete octet the SO4 ion has more formal charge on sulphur and oxygen atoms i.e. 2+ on S and -1 on each O atoms. By minimizing charge on two O atoms two double bonds creates on S atom making zero charge on S and two O atoms.
In that case S atom has 12 electrons, so it has extended octet and two O atoms has incomplete octet with six electrons while other two atoms has complete octet with -1 charge on it.
BaSO4 lewis structure consists of both metal and non- metal compounds i.e. barium metal and SO4 ion is a non- metal which is a polyatomic ion. In BaSO4 lewis structure, there are only two electrons present on Ba metal as it belongs to the 2nd group of the periodic table. So, only lone electron pairs are present on Ba metal of BaSO4 lewis structure which it get shared with SO4 ion and creates 2+ charges on Ba metal and 2- charge on SO4 ion. The sharing of electrons is shown by the bracket around SO4 ion.
BaSO4 lewis structure shape
BaSO4 is an ionic compound as it contains SO4 polyatomic ion in it. Basically BaSO4 molecule does not have its own original shape as it is only and ionic compound and there is no bonding between Ba and SO4 ion, there is just sharing of electrons within the molecule. Thus BaSO4 lewis structure does not have any shape. Rather than SO4 ion has is basic shape as tetrahedral as central sulphur atom attached with four oxygen atoms.
BaSO4 lewis structure angle
BaSO4 molecule does not have any bond angle as there is no bond present within the molecule as it is originally an ionic compound with the presence of metal and non-metal moieties. But the SO4 ion has a bond angle of 109.50 degree within each S-O bonds due to the presence of double bonds repulsion creates between the ion and making the bond angle of 109.50 degree in SO4 ion.
BaSO4 lewis structure resonance
BaSO4 lewis structure does not show any resonance structure as there is not bonding between the BaSO4 molecules. Even it is an ionic molecule containing metal (Ba) and non- metal (SO4) compounds in it. But the SO4 ion can show various resonance structures, as it has double bonds and single bonds within S and O atoms and also it has lone electron pairs present on it. So, the resonance structure of BaSO4 ion is not possible but the resonance structure of only SO4 ion can possible.
BaSO4 hybridization
BaSO4 lewis structure does not show any hybridization as there is no mixing and recasting of atomic orbitals within the molecule, there is only sharing of electrons between Ba metal and SO4 ion creating 2+ charge on Ba and 2- charge on SO4 ion. But the only SO4 ion can have the sp3 hybridization as the central sulphur atom attached to the four oxygen atoms in SO4 ion.
BaSO4 solubility
BaSO4 (barium sulphate) is soluble in:
Hot sulphuric acid (H2SO4)
BaSO4 (barium sulphate) is insoluble in:
Water ( or hardly soluble)
R-OH group compounds
Dilute acids
Is BaSO4 ionic?
Yes, Barium sulphate (BaSO4) is an ionic compound. As there is no presence of covalent or pi bonds within the molecule. There is only presence of charges on Ba metal and SO4 ion which makes the BaSO4 an ionic compound.
Why BaSO4 ionic? As the Ba metal belongs to 2nd group of periodic table it contains only two valence electrons, which it get shared with the SO4 ion creating 2+ charge on Ba and 2- charge on SO4 ion as it accepts electrons from Ba. Due to the presence of charges on BaSO4 molecule it is ionic in nature.
How BaSO4 ionic? BaSO4 is an ionic compound and due to which it is insoluble in water due to presence of bigger ions. Ba2+ and SO42- both are bigger ions i.e. the bigger cation (Ba2+) stabilizes the bigger polyatomic anion (SO42-). Due to the sharing of electrons the BaSO4 being an ionic compound as cation and anion both present in it.
Is BaSO4 polar or nonpolar?
BaSO4 (barium sulphate) compound is polar in nature. Due to the presence of polar bonds with Ba and SO4 ion it is polar in nature, also the SO4 ion is also polar molecule and they cannot cancel out each other. Still BaSO4 is not soluble in polar solvent like water, due to the presence of strong crystals in BaSO4 molecule as water has weak dipole strength as compared to BaSO4.
Why BaSO4 polar? As BaSO4 is an ionic compound containing positively charged cation and negatively charged anion on it, which creates a dipole within the BaSO4 molecule which makes it polar.
How BaSO4 polar? Due to the presence of polar bon within positively charged Ba cation and negatively charged SO4 anion in BaSO4 molecule, there is the formation of polar bond within Ba and SO4 ion, makes it a polar compound.
Is BaSO4 acidic or basic?
BaSO4 is an salt and consider as neutral molecule generally. The salts are produced by the reaction between acids and bases. Thus, BaSO4 does not consider as acid or a base as it does not creates H+ and OH- ions in the water and even does not dissolve in it. But BaSO4 consists of both acidic part (Ba2+) and basic part (SO42-).
Why BaSO4 not acidic or basic? As BaSO4 is prepared with strong acid (H2SO4) and strong base (Ba(OH)2), so it have the Ba2+ acidic ion an SO42- basic ion, but it is neutral in nature as it is originally a salt in nature.
How BaSO4 is not acidic or basic? BaSO4 is polar in nature still is is not soluble in polar solvent like water and also does not creates H+ and OH- ions so it is a neutral molecule as BaSO4 is made up of strong acid and base.
Conclusion:
BaSO4 consists of two ions i.e. Ba2+ cation and SO42- anion. It is an ionic compound and has polar nature. BaSO4 is soluble in hot concentrated H2SO4. It is a neutral molecule.
In this article, we should learn about the Ba2+ lewis structure and its characteristics detailed fact.
Ba2+ lewis structure will be included in its valence electrons, a number of available lone pairs, and also its chemical nature. Ba2+ is the dication of barium which is a s block element. It is an alkaline earth metal, it can form a strong base with hydroxide.
Barium metal has a 6s orbital so it shows relativistic contraction and for this phenomenon, the chemical, as well as physical behavior, will differ from other alkaline metals. It can form different salts with halogen anions.
The electronic configuration of Ba is [Xe]6s2, but for Ba2+ there will be two electrons less from Ba metal, and the valence shell will be 6s, so two electrons are removed from the 6s orbital. So, the electronic configuration of Ba2+ is 1s22s22p63s23p63d104s24p64d105s25p65d10. Ba2+ has 54 electrons and its gain nearest noble gas configuration similar to Xe. The ionic radius of Ba2+ is 135 pm and it is the largest alkaline earth metal dication.
1. How to draw Ba2+ lewis structure?
By the drawing Ba2+ lewis structure, we can predict the lone pairs of its, and the number of electrons available for bond formation.
First of all, it is a single dication so no need to add electrons, we should consider its electrons only. As it is a dication so an equal number of electrons should be removed from its configuration and no need to add a bond because there is no molecule here. After that, the lone pair is assigned if available.
2. Ba2+ lewis structure formal charge
The formal charge is generally assigned for a molecule taking into consideration all atoms should same electronegativity.
Ba2+ Formal Charge
But in the Ba2+ lewis structure, there are no other atoms present. So, we consider only the charge over the Ba2+ that is +2. So, the formal charge of Ba2+ is +2 as it is a cationic species so the formal charge is equal to the charge assigned to it.
3. Ba2+ lewis structure octet rule
The octet rule is for an atom that gives or takes electrons from other species to complete its valence shell and gain the nearest noble gas configuration.
The electronic configuration of Ba is [Xe]6s2 but the electronic configuration of Ba2+ is [Xe], which means two electrons should be removed from the 6s orbital as Ba is s block element so the valence shell should be one s orbital. In the Ba2+ lewis structure, ba2+ is already completing its octet donating its two electrons and gaining the nearest noble gas configuration.
4. Ba2+ lewis structure lone pairs
The concept of lone pairs comes after the bond pairs involved in bond formation and the remaining electrons consider lone pairs.
Ba2+ Lone Pairs
From the Ba2+ lewis structure, we can see all the 54 electrons are available and they do not participate in any bonding, as ba2+ is a single dication. So here we can’t predict the lone pairs of Ba2+.
5. Ba2+ valence electrons
Valence electrons are those electrons that are present in the valence shell or outermost shell of an atom.
From the Ba2+ lewis structure, the electronic configuration of Ba2+ is 1s22s22p63s23p63d104s24p64d105s25p65d10. So, the outer most shell will be 5d orbital and there are 10 electrons present so the shell in fully completed and those are the valence electrons for Ba2+.
6. Ba2+ solubility
The solubility of any atom or ion is represented as the how extent they can be soluble in a giver solution.
Ba2+ lewis structure is a dication ionic species so it must be soluble in water. Even Ba2+ can be soluble in any other polar solvent and in an organic solvent, the solubility will be low.
7. Is Ba2+ ionic?
A molecule or atom should be ionic by how many % of ionic character it has.
From the lewis structure of Ba2+, the ionic potential of Ba2+ is moderately high. The size of the cation is large and the charge density is also high. So Ba2+ is ionic.
8. Is Ba2+ polar or nonpolar?
The polarity of a molecule or atoms should be described that the molecule or atoms should have some resultant dipole moment.
The dipole moment always works from a more electronegative site to a less electronegative site. But in the Ba2+ lewis structure there is no such other atom present but the molecule has some dipole moment due to its cationic nature.
9. Is Ba2+ acidic or basic?
Acidity or basicity depends on the nature of cation and anions also.
From the HSAB (HARD SOFT ACID-BASE) principle, we can say that every cation having a larger size and less electron potential are soft acid. They have a low tendency to polarize any larger anion. They can form stable molecules by forming bonds with soft bases. Although Ba2+ is an alkaline earth metal so can form strong acid with hydroxide.
Conclusion-
From the above discussion of Ba2+ lewis structure, we can say that a dication is less important although they can form a stable form with dianion. The acidity and solubility are the physical and independent nature of a dication.
Nitrogen dioxide (NO2) is a chemical compound composed of nitrogen and oxygen atoms. It is a reddish-brown gas with a pungent odor and is commonly found in urban areas as a result of air pollution. Understanding the Lewis structure of NO2 is important in determining its chemical properties and reactivity. The Lewis structure provides a visual representation of the arrangement of atoms and electrons in a molecule, helping us understand how the molecule interacts with other substances. In this article, we will explore the NO2 Lewis structure in detail, discussing its electron arrangement, bond formation, and overall molecular shape. So, let’s dive in and unravel the mysteries of NO2!
Key Takeaways
The NO2 Lewis structure consists of a nitrogen atom bonded to two oxygen atoms.
The nitrogen atom has a lone pair of electrons, while the oxygen atoms have three lone pairs each.
The nitrogen-oxygen bonds are represented by single bonds, and the nitrogen-oxygen double bond is represented by a double bond.
The formal charges on the atoms in the NO2 Lewis structure are: nitrogen (-1), one oxygen (+1), and the other oxygen (0).
The NO2 molecule has a bent shape due to the repulsion between the lone pairs of electrons on the nitrogen and oxygen atoms.
The Lewis structure is a way to represent the bonding and electron distribution in a molecule. In the case of NO2, which stands for nitrogen dioxide, we can draw its Lewis structure to understand its molecular geometry and electron arrangement.
To draw the Lewis structure of NO2, we need to follow a few steps:
Determine the total number of valence electrons: In NO2, nitrogen (N) is in Group 5A of the periodic table, so it has 5 valence electrons. Oxygen (O) is in Group 6A, so each oxygen atom has 6 valence electrons. Since there are two oxygen atoms in NO2, we have a total of 5 + 2(6) = 17 valence electrons.
Identify the central atom: In NO2, nitrogen is the central atom as it is less electronegative than oxygen.
Connect the atoms: Place the nitrogen atom in the center and connect it to the two oxygen atoms using single bonds.
Distribute the remaining electrons: Distribute the remaining electrons around the atoms to satisfy the octet rule. Start by placing lone pairs on the outer atoms (oxygen) and then distribute the remaining electrons on the central atom (nitrogen).
Check for octet rule and formal charges: Make sure all atoms have an octet of electrons (except hydrogen, which only needs 2 electrons). If necessary, move lone pairs to form double or triple bonds to satisfy the octet rule. Also, check for any formal charges to minimize their presence.
Explanation of NO2 Lewis structure
The Lewis structure of NO2 shows that nitrogen is bonded to two oxygen atoms. The nitrogen atom has one lone pair of electrons, while each oxygen atom has two lone pairs. The double bond between nitrogen and one oxygen atom is represented by two dots or a double line, indicating the sharing of two pairs of electrons. The single bond between nitrogen and the other oxygen atom is represented by a single dot or a single line, indicating the sharing of one pair of electrons.
The Lewis structure helps us understand the arrangement of electrons in a molecule and predict its molecular geometry. In the case of NO2, the molecule has a bent or V-shaped geometry due to the repulsion between the lone pairs of electrons on the oxygen atoms. This bent shape gives NO2 a polar nature, with the oxygen atoms being slightly negative and the nitrogen atom being slightly positive.
Valence electrons in NO2 Lewis structure
Valence electrons are the electrons in the outermost energy level of an atom. In the Lewis structure of NO2, we consider the valence electrons of nitrogen and oxygen to determine the total number of electrons available for bonding.
Nitrogen, being in Group 5A, has 5 valence electrons. Oxygen, being in Group 6A, has 6 valence electrons. Since there are two oxygen atoms in NO2, we multiply the number of valence electrons of oxygen by 2. Therefore, the total number of valence electrons in NO2 is 5 + 2(6) = 17.
Valence electrons play a crucial role in determining the chemical properties and reactivity of a molecule. They are involved in forming chemical bonds and determining the electron distribution in a molecule.
Octet rule in NO2 Lewis structure
The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with 8 electrons in their outermost energy level. This rule helps us understand the formation of chemical bonds and the stability of molecules.
In the Lewis structure of NO2, we can see that nitrogen has 5 valence electrons and each oxygen atom has 6 valence electrons. By sharing electrons through single and double bonds, nitrogen and oxygen can achieve an octet of electrons in their outermost energy level.
The double bond between nitrogen and one oxygen atom satisfies the octet rule for both nitrogen and oxygen. However, the other oxygen atom only has 7 electrons around it. To satisfy the octet rule, one lone pair from the nitrogen atom is moved to form a double bond with the second oxygen atom. This redistribution of electrons allows all atoms in NO2 to have an octet of electrons, fulfilling the octet rule.
Understanding the NO2 Lewis structure and the application of the octet rule helps us predict the stability and reactivity of molecules. It provides insights into the chemical behavior and properties of compounds like nitrogen dioxide.
Hybridization in NO2 Lewis Structure
The Lewis structure of NO2, also known as nitrogen dioxide, is a representation of the molecule’s bonding and electron arrangement. In order to understand the Lewis structure of NO2, it is important to first grasp the concept of hybridization.
Definition of Hybridization
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals have different shapes and energies compared to the original atomic orbitals. Hybridization occurs when atoms bond together to form molecules.
Hybridization in NO2
In the case of NO2, the central nitrogen atom is bonded to two oxygen atoms. To determine the hybridization of the nitrogen atom in NO2, we need to consider the number of electron groups around it. An electron group can be a lone pair or a bond.
In NO2, there are two oxygen atoms bonded to the nitrogen atom, resulting in two electron groups. Additionally, there is one lone pair of electrons on the nitrogen atom. Therefore, the total number of electron groups around the nitrogen atom is three.
Explanation of sp2 Hybridization in NO2
The hybridization of the nitrogen atom in NO2 is sp2. This means that the nitrogen atom in NO2 undergoes hybridization by mixing one 2s orbital and two 2p orbitals to form three sp2 hybrid orbitals. These sp2 hybrid orbitals are arranged in a trigonal planar geometry around the nitrogen atom.
The three sp2 hybrid orbitals in NO2 are used to form sigma bonds with the two oxygen atoms and accommodate the lone pair of electrons. The remaining p orbital on the nitrogen atom contains one electron, which is involved in pi bonding with one of the oxygen atoms.
To summarize, the sp2 hybridization in NO2 allows the nitrogen atom to form three sigma bonds and one pi bond, resulting in a trigonal planarmolecular geometry.
In conclusion, understanding the hybridization in the NO2 Lewis structure is crucial for comprehending the molecule’s bonding and shape. The sp2 hybridization of the nitrogen atom in NO2 enables it to form three sigma bonds and one pi bond, leading to a trigonal planarmolecular geometry.
Formal Charges in NO2 Lewis Structure
The formal charges in a NO2 Lewis structure play a crucial role in understanding the distribution of electrons within the molecule. By assigning formal charges, we can determine the most stable arrangement of electrons and gain insights into the molecule’s reactivity and properties.
Definition of Formal Charges
Formal charges are hypothetical charges assigned to each atom in a molecule or ion. These charges help us understand the distribution of electrons and determine the stability of different resonance structures. The formal charge of an atom is calculated by comparing the number of valence electrons it should have with the number it actually possesses in the Lewis structure.
Calculation of Formal Charges in NO2
To calculate the formal charges in a NO2 molecule, we need to follow a step-by-step process:
Determine the total number of valence electrons in the molecule. For NO2, nitrogen (N) contributes 5 valence electrons, and each oxygen (O) contributes 6 valence electrons, giving us a total of 5 + 2(6) = 17 valence electrons.
Assign lone pairs of electrons to each atom. Nitrogen requires 3 lone pairs to complete its octet, while each oxygen atom requires 2 lone pairs.
Connect the atoms using single bonds. In the case of NO2, nitrogen forms a double bond with one oxygen atom, and a single bond with the other oxygen atom.
Distribute the remaining electrons as lone pairs to satisfy the octet rule for each atom. In NO2, the remaining 3 electrons are placed as a lone pair on the nitrogen atom.
Calculate the formal charge for each atom. The formula for formal charge is:
For example, for the nitrogen atom in NO2, the formal charge is:
Formal Charge = 5 – 3 – 0.5 * 4 = 0
For each oxygen atom, the formal charge is:
Formal Charge = 6 – 2 – 0.5 * 4 = 0
Formal Charges in NO2 Lewis Structure
In the NO2 Lewis structure, the nitrogen atom has a formal charge of 0, while each oxygen atom also has a formal charge of 0. This distribution of formal charges indicates that the Lewis structure is stable and represents the most favorable arrangement of electrons for NO2.
By analyzing the formal charges, we can conclude that the nitrogen atom in NO2 does not carry any excess or deficient electrons. Similarly, each oxygen atom also has the appropriate number of electrons to maintain stability.
Understanding the formal charges in the NO2 Lewis structure provides valuable insights into the molecule’s behavior and reactivity. It helps us predict how NO2 interacts with other molecules and how it participates in chemical reactions.
In the next section, we will explore the molecular geometry and bond angles in the NO2 molecule, further enhancing our understanding of its structure and properties.
Resonance in NO2 Lewis Structure
Resonance is an important concept in chemistry that helps us understand the behavior of molecules. In the case of the NO2 Lewis structure, resonance plays a significant role in determining its structure and properties.
Definition of Resonance
Resonance refers to the delocalization of electrons within a molecule. It occurs when there are multiple valid Lewis structures that can be drawn for a molecule, and the actual structure is a combination or average of these resonance structures. In other words, resonance structures are different ways of arranging the same atoms, but with different electron distributions.
Resonance in NO2 Lewis Structure
When we consider the NO2 molecule, we can draw multiple resonance structures. NO2, also known as nitrogen dioxide, consists of a nitrogen atom bonded to two oxygen atoms. The central nitrogen atom has a lone pair of electrons and forms a double bond with one of the oxygen atoms, while the other oxygen atom is bonded by a single bond.
To represent the resonance in the NO2 Lewis structure, we can draw two resonance structures. In the first resonance structure, the double bond is between the nitrogen and the oxygen on the left, while in the second resonance structure, the double bond is between the nitrogen and the oxygen on the right. These resonance structures can be interconverted by moving the double bond and the lone pair of electrons.
Explanation of Resonating Structures in NO2
The presence of resonance in the NO2 Lewis structure affects the overall structure and properties of the molecule. Due to resonance, the actual structure of NO2 is a hybrid of the two resonance structures. This means that the double bond character is shared between the two oxygen atoms, resulting in a more stable molecule.
The resonance in NO2 also affects the bond lengths and bond angles within the molecule. In the resonance structures, the nitrogen-oxygen bond lengths are equal, and the nitrogen-oxygen-nitrogen bond angle is approximately 134 degrees. However, in the actual structure, the bond lengths are intermediate between single and double bonds, and the bond angle is slightly less than 134 degrees.
The presence of resonance also influences the polarity of the NO2 molecule. Each resonance structure has a partial positive charge on the nitrogen atom and a partial negative charge on the oxygen atoms. In the actual structure, the polarity is distributed over the molecule, resulting in a polar molecule.
In conclusion, resonance in the NO2 Lewis structure is a fascinating phenomenon that arises due to the delocalization of electrons. It leads to the formation of multiple resonance structures, which contribute to the overall stability, structure, and properties of the NO2 molecule. By understanding resonance, we can gain valuable insights into the behavior of molecules and their chemical reactions.
Bond Angle in NO2 Lewis Structure
The bond angle in the NO2 Lewis structure plays a crucial role in determining the shape and properties of the molecule. Understanding the bond angle is essential for predicting the molecule’s behavior and its interactions with other molecules. In this section, we will explore the definition of bond angle, discuss the bond angle in the NO2 Lewis structure, and explain the bent shape of NO2.
Definition of Bond Angle
The bond angle is the angle formed between two adjacent bonds in a molecule. It is measured in degrees and provides valuable information about the molecular geometry and the arrangement of atoms in a compound. The bond angle is influenced by various factors, including the number of electron pairs around the central atom and the repulsion between these electron pairs.
Bond Angle in NO2 Lewis Structure
To understand the bond angle in the NO2 Lewis structure, let’s first take a look at its molecular geometry. NO2, also known as nitrogen dioxide, consists of a central nitrogen atom bonded to two oxygen atoms. The Lewis structure for NO2 shows that nitrogen has one lone pair and two single bonds with oxygen.
In the NO2 Lewis structure, the central nitrogen atom is surrounded by three electron pairs – two from the oxygen atoms and one lone pair. These electron pairs repel each other, causing the molecule to adopt a bent shape. The bond angle in the NO2 Lewis structure is approximately 134 degrees.
Explanation of Bent Shape in NO2
The bent shape of NO2 can be explained by considering the repulsion between electron pairs. The lone pair on the central nitrogen atom exerts a greater repulsive force compared to the bonding pairs. As a result, the bonding pairs are pushed closer together, leading to a decrease in the bond angle.
The repulsion between the lone pair and the bonding pairs causes the NO2 molecule to bend, resulting in a bond angle less than the ideal 180 degrees. This bent shape is also influenced by the electronegativity difference between nitrogen and oxygen, which leads to a polar molecule.
In summary, the bond angle in the NO2 Lewis structure is approximately 134 degrees, indicating a bent shape. This bent shape is a result of the repulsion between the lone pair and the bonding pairs, as well as the electronegativity difference between nitrogen and oxygen. Understanding the bond angle and molecular geometry of NO2 is crucial for comprehending its chemical behavior and interactions with other substances.
Lone Pairs in NO2 Lewis Structure
In the Lewis structure of NO2, lone pairs play a crucial role in determining the molecule’s geometry and properties. Let’s explore the definition of lone pairs, the number of lone pairs in NO2, and the impact they have on the molecule’s geometry.
Definition of Lone Pairs
Lone pairs, also known as non-bonding pairs, are pairs of electrons that are not involved in bonding with other atoms. In a Lewis structure, these electrons are represented as dots around the atom. The presence of lone pairs affects the overall shape and polarity of a molecule.
Number of Lone Pairs in NO2
In the NO2 molecule, there are two oxygen atoms bonded to a central nitrogen atom. To determine the number of lone pairs in NO2, we need to consider the valence electrons of each atom. Nitrogen has five valence electrons, while oxygen has six. Therefore, the total number of valence electrons in NO2 is:
(1 × 5) + (2 × 6) = 17
To distribute these electrons, we first form single bonds between the nitrogen atom and each oxygen atom. This accounts for four electrons (two from each oxygen). The remaining 13 electrons are then placed as lone pairs around the atoms.
Impact of Lone Pairs on NO2 Geometry
The presence of lone pairs in NO2 affects its geometry and bond angles. In NO2, the nitrogen atom is surrounded by two oxygen atoms and one lone pair. This arrangement gives rise to a bent or V-shaped molecular geometry.
The repulsion between the lone pair and the bonding pairs causes a distortion in the molecule’s shape. The bond angle between the nitrogen-oxygen bonds is less than the ideal 120 degrees due to this repulsion. In the case of NO2, the bond angle is approximately 134 degrees.
The presence of lone pairs also influences the polarity of the molecule. The electronegativity of oxygen is higher than that of nitrogen, resulting in a polar covalent bond between nitrogen and oxygen. The lone pair on nitrogen further enhances the polarity of the molecule, making NO2 a polar molecule.
To summarize, the NO2 molecule has one lone pair on the central nitrogen atom, which affects its geometry, bond angle, and polarity. The presence of the lone pair causes a bent molecular shape and a bond angle of approximately 134 degrees. Additionally, the lone pair contributes to the overall polarity of the molecule.
In the next section, we will delve into the resonance structure of NO2 and its implications on the molecule’s stability and reactivity.
Polar or Nonpolar Nature of NO2 Lewis Structure
Definition of Polar and Nonpolar Molecules
Before we delve into the polar or nonpolar nature of the NO2 Lewis structure, let’s first understand what it means for a molecule to be polar or nonpolar.
In chemistry, polarity refers to the distribution of electrons in a molecule. A polar molecule has an uneven distribution of electron density, resulting in a separation of positive and negative charges. On the other hand, a nonpolar molecule has an even distribution of electron density, with no separation of charges.
The polarity of a molecule is determined by the difference in electronegativity between the atoms involved in the chemical bond. Electronegativity is a measure of an atom’s ability to attract electrons towards itself. When two atoms with different electronegativities form a bond, the more electronegative atom pulls the shared electrons closer to itself, creating a polar bond.
Determining Polarity of NO2 Lewis Structure
Now, let’s apply this knowledge to the NO2 Lewis structure to determine its polarity.
The NO2 molecule, also known as nitrogen dioxide, consists of one nitrogen atom (N) and two oxygen atoms (O). To draw the Lewis structure of NO2, we start by counting the total number of valence electrons in the molecule. Nitrogen contributes 5 valence electrons, while each oxygen contributes 6 valence electrons, giving us a total of 5 + 2(6) = 17 valence electrons.
Next, we arrange the atoms in the structure, placing the nitrogen atom in the center and the oxygen atoms on either side. We then connect the atoms using single bonds, which account for 2 electrons each. After connecting the atoms, we distribute the remaining electrons as lone pairs around the atoms to satisfy the octet rule.
In the NO2 Lewis structure, the nitrogen atom is double-bonded to one of the oxygen atoms, while the other oxygen atom has a lone pair. This arrangement gives nitrogen a formal charge of +1 and the oxygen atoms a formal charge of -1 each. The Lewis structure can be represented as follows:
O
╱
N = O
╲
O
Now, let’s analyze the polarity of the NO2 molecule based on its Lewis structure. The nitrogen-oxygen double bond is a polar bond due to the difference in electronegativity between nitrogen and oxygen. Oxygen is more electronegative than nitrogen, so it pulls the shared electrons closer to itself, creating a partial negative charge on the oxygen atom and a partial positive charge on the nitrogen atom.
Additionally, the lone pair on the oxygen atom also contributes to the polarity of the molecule. The presence of the lone pair creates an uneven distribution of electron density, further enhancing the polarity of the NO2 molecule.
Therefore, based on the arrangement of atoms and the polarity of the bonds and lone pairs, we can conclude that the NO2 molecule is polar in nature.
In summary, the NO2 Lewis structure exhibits polarity due to the polar nitrogen-oxygen double bond and the presence of a lone pair on one of the oxygen atoms. Understanding the polarity of molecules is crucial in various chemical reactions and interactions, as it influences the behavior and properties of substances.
VSEPR Model and NO2 Lewis Structure
The VSEPR (Valence Shell Electron Pair Repulsion) model is a useful tool in predicting the shape and geometry of molecules. By considering the repulsion between electron pairs, we can determine the arrangement of atoms in a molecule. In this section, we will explore the application of the VSEPR model to the NO2 Lewis structure and discuss the electron geometry of NO2.
Overview of VSEPR Model
The VSEPR model is based on the principle that electron pairs in the valence shell of an atom repel each other. This repulsion leads to a specific arrangement of atoms in a molecule, which determines its shape and geometry. The VSEPR model is widely used to predict molecular geometries and understand the behavior of molecules.
To apply the VSEPR model, we start by drawing the Lewis structure of the molecule. The Lewis structure shows the arrangement of atoms and valence electrons in a molecule. By counting the number of valence electrons and considering the octet rule, we can determine the Lewis structure of a molecule.
Application of VSEPR Model to NO2 Lewis Structure
Now let’s apply the VSEPR model to the NO2 molecule. NO2, also known as nitrogen dioxide, consists of one nitrogen atom (N) and two oxygen atoms (O).
To determine the Lewis structure of NO2, we first calculate the total number of valence electrons. Nitrogen has 5 valence electrons, and each oxygen atom has 6 valence electrons. Therefore, the total number of valence electrons in NO2 is:
5 (from nitrogen) + 2 * 6 (from oxygen) = 17
Next, we arrange the atoms in the molecule and connect them with single bonds. In the case of NO2, nitrogen is the central atom, and the two oxygen atoms are bonded to it.
To distribute the valence electrons, we place them around the atoms, starting with the outer atoms and then the central atom. In NO2, each oxygen atom needs 2 electrons to complete its octet, while nitrogen needs 3 electrons. This leaves us with 17 – 4 = 13 electrons to distribute.
We place the remaining electrons as lone pairs on the oxygen atoms. Each oxygen atom will have one lone pair, and nitrogen will have one lone pair as well.
Electron Geometry of NO2
The electron geometry of a molecule is determined by the arrangement of electron pairs around the central atom. In the case of NO2, nitrogen is the central atom, and it has one lone pair and two bonding pairs.
According to the VSEPR model, the presence of one lone pair and two bonding pairs gives NO2 an electron pair geometry of trigonal planar. This means that the electron pairs are arranged in a flat, triangular shape around the nitrogen atom.
The bond angle in NO2 is approximately 134 degrees. This angle is slightly less than the ideal bond angle of 120 degrees due to the repulsion between the lone pair and the bonding pairs.
In summary, the VSEPR model can be used to determine the electron geometry of NO2, which is trigonal planar. The presence of one lone pair and two bonding pairs results in a bond angle of approximately 134 degrees. Understanding the electron geometry of molecules like NO2 is crucial in predicting their physical and chemical properties.
Uses of NO2
Nitrogen dioxide (NO2) is a highly reactive and toxic gas that is commonly used in various industrial processes and applications. Its unique properties make it valuable for a range of purposes. Let’s explore some of the key uses of NO2.
Industrial production of Nitric acid
One of the primary uses of NO2 is in the industrial production of nitric acid. Nitric acid is a vital chemical compound used in the manufacturing of fertilizers, explosives, dyes, and pharmaceuticals. NO2 is a key intermediate in the Ostwald process, which involves the oxidation of ammonia to produce nitric acid. In this process, NO2 reacts with water to form nitric acid and nitrogen monoxide (NO). The production of nitric acid is crucial for various industries, making NO2 an essential component in its synthesis.
Catalyst in chemical reactions
NO2 also serves as a catalyst in several chemical reactions. A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. NO2 acts as a catalyst in the oxidation of sulfur dioxide (SO2) to form sulfur trioxide (SO3). This reaction is a crucial step in the production of sulfuric acid, which is widely used in the manufacturing of fertilizers, detergents, and other chemical processes. The presence of NO2 enhances the efficiency of the reaction, making it an important catalyst in the sulfuric acid production process.
Regulation of sulfuric acid production
In addition to its role as a catalyst, NO2 also plays a significant role in the regulation of sulfuric acid production. The concentration of NO2 in the reaction mixture affects the rate of the oxidation reaction. By controlling the amount of NO2 present, manufacturers can regulate the production of sulfuric acid and ensure optimal efficiency. This regulation is crucial for maintaining the quality and quantity of sulfuric acid produced, as well as minimizing the environmental impact of the process.
Use as an oxidizer in rocket fuels
NO2 finds application as an oxidizer in rocket fuels. In rocket propulsion systems, an oxidizer is required to support the combustion of the fuel. NO2 is a powerful oxidizer that provides the necessary oxygen for the combustion process. It is commonly used in combination with fuels such as hydrazine to create highly energetic propulsion systems. The use of NO2 as an oxidizer allows rockets to achieve high speeds and propel payloads into space.
Manufacture of oxidized cellulose compounds
NO2 is also utilized in the manufacture of oxidized cellulose compounds. Oxidized cellulose is a material derived from cellulose fibers that have been chemically modified to enhance their properties. NO2 is used in the oxidation process, which introduces functional groups onto the cellulose structure, resulting in improved strength, stability, and absorbency. Oxidized cellulose compounds find applications in various industries, including healthcare, textiles, and paper manufacturing.
In conclusion, NO2 has a wide range of uses in various industries and applications. From its role in the production of nitric acid and regulation of sulfuric acid production to its use as a catalyst and oxidizer, NO2 plays a crucial role in numerous chemical processes. Its unique properties make it a valuable resource for enhancing the efficiency and performance of various industrial applications. Conclusion
In conclusion, understanding the NO2 Lewis structure is crucial for comprehending the chemical properties and behavior of nitrogen dioxide. By examining the arrangement of atoms and electrons within the molecule, we can gain insights into its polarity, reactivity, and overall stability. The Lewis structure of NO2 reveals that it consists of a central nitrogen atom bonded to two oxygen atoms, with one of the oxygen atoms carrying an unshared electron pair. This arrangement gives rise to a bent molecular geometry, resulting in a polar molecule with a partial positive charge on the nitrogen atom and partial negative charges on the oxygen atoms. The presence of a lone pair on one of the oxygen atoms makes NO2 highly reactive, particularly in terms of its involvement in atmospheric chemistry and air pollution. By studying the NO2 Lewis structure, scientists can better understand the behavior of this important compound and its impact on the environment and human health.
Frequently Asked Questions
1. How do you determine the Lewis structure of NO2?
To determine the Lewis structure of NO2 (nitrogen dioxide), you need to count the valence electrons and follow the octet rule. The Lewis structure for NO2 consists of a nitrogen atom bonded to two oxygen atoms, with a double bond between nitrogen and one oxygen atom, and a single bond between nitrogen and the other oxygen atom.
2. What is the hybridization of NO2?
The hybridization of NO2 (nitrogen dioxide) is sp2. In the Lewis structure of NO2, the nitrogen atom forms three sigma bonds with the two oxygen atoms and has one lone pair. This arrangement requires the nitrogen atom to undergo sp2 hybridization.
3. How many valence electrons are in the Lewis structure of NO2-?
In the Lewis structure of NO2- (nitrite ion), there are 18 valence electrons. The nitrogen atom contributes 5 valence electrons, and each oxygen atom contributes 6 valence electrons. The negative charge on the nitrite ion adds an additional electron, totaling 18 valence electrons.
4. Does the Lewis structure of NO2 follow the octet rule?
Yes, the Lewis structure of NO2 (nitrogen dioxide) follows the octet rule. The nitrogen atom has a double bond with one oxygen atom and a single bond with the other oxygen atom, resulting in a total of 8 valence electrons around the nitrogen atom.
5. Why does NO2 have a double bond?
NO2 (nitrogen dioxide) has a double bond because it allows the nitrogen atom to achieve a stable octet configuration. By forming a double bond with one of the oxygen atoms, the nitrogen atom can share two pairs of electrons, satisfying the octet rule.
6. What is the bond order in the Lewis structure of NO2+?
The bond order in the Lewis structure of NO2+ (nitronium ion) is 2. The nitrogen atom forms a double bond with one of the oxygen atoms and a coordinate covalent bond with the other oxygen atom, resulting in a bond order of 2.
7. How do you draw the Lewis structure of NO2?
To draw the Lewis structure of NO2 (nitrogen dioxide), start by placing the nitrogen atom in the center. Connect the nitrogen atom to two oxygen atoms using single bonds. Then, add a double bond between the nitrogen atom and one of the oxygen atoms. Finally, distribute any remaining valence electrons as lone pairs.
8. Does the Lewis structure of NO2 exhibit resonance?
Yes, the Lewis structure of NO2 (nitrogen dioxide) exhibits resonance. The double bond in the structure can be delocalized between the nitrogen atom and either of the oxygen atoms, resulting in resonance structures.
9. What is the bond angle in the Lewis structure of NO2?
The bond angle in the Lewis structure of NO2 (nitrogen dioxide) is approximately 134 degrees. The oxygen atoms are arranged in a bent shape around the nitrogen atom, resulting in a bond angle slightly less than 180 degrees.
10. Is the Lewis structure of NO2 polar or nonpolar?
The Lewis structure of NO2 (nitrogen dioxide) is polar. The presence of a bent molecular geometry and the unequal distribution of electrons due to the double bond result in a polar molecule.
In this article, we are going to study the Bas lewis structure and the important facts associated with it.
By using the lewis concept (bas Lewis structure) we can understand the bonding between atoms in a molecule. So we are going to apply this concept to barium sulfide and study the molecule in detail.
How to draw Bas lewis structure?
So in order to understand the bas Lewis structure we must know the number and types of atoms present in the molecule. There is one barium atom and one sulfur atom.
As we can see the bond formation is taking place between a metal (barium) and a non metal(sulfur). So the resultant compound will be of the ionic type. So in this type of bonding what will happen is valence electrons will be transferred to the non metal from the metal ( barium to sulfur). Valence electrons that are contributed by Ba is 2 and S is 6.
Hence the sum of all the Valence Electrons is 8 electrons. So in order to satisfy the octet of sulfur, barium will give 2 of its electrons to sulfur. In this way it will lead to the formation of ionic bond of barium sulfide.
Bas lewis structure resonance?
What we understand by resonating structure of a molecule are the structures(lewis) through which we can understand electrons delocalization in molecule or an ion(polyatomic).
The important condition for a molecule to resonate is it should possess at least one double bond and at least one pair of electrons that are available for donation.
So a lewis structure is of great help in studying the molecule.
Bas lewis structure shape
Barium sulfide is observed to be a colorless(crystalline type of solid). Having a density of around 4.25 g/cm3.
The observed melting point of this particular compound is around 2235 degrees Celsius and talking about its boiling point it decomposes very soon. So the shape of barium sulfide molecule is octahedral type. Where the cation has anions surrounding it.
We can carry out the calculation of formal charge by making use of the formula given below.
V symbolizes all the valence electrons that are present
N symbolizes all the non-bonding type of electrons(valence).
B symbolizes all the electrons that are shared in the bonds.
Hence the formal charge on the barium sulfide molecule is zero.
Bas lewis structure angle
We can that there are 2 atoms that participate in the formation of barium sulfide.
Out of which on is a barium element atom and the other is sulfur atom. As the compound is an example of ionic and the structure will be having octahedral type geometry. The bond angle of octahedral type of geometry is around 180 degrees.
In concept of octet rule, the atoms forming a molecule give away or accept electrons to satisfy their octet.
Meaning the outermost shell of an atom should be filled completely. This is called obtaining of a completely filled octet. So in the molecule of barium sulfide, barium gives away 2 of its available valence electrons to the sulfur atom (which has 6 valence electrons).
In this way an ionic bond is formed and the octet of barium sulfide is satisfied.
Bas lewis structure lone pairs
We know that a barium molecule has octahedral type of geometry. So contribution of valence type of electrons is 8. Presence of lone pairs has got very importance as it is responsible for predicting the structure of that particular molecule.
Bas valence electrons
The total valence electrons in the barium element are 2.
The total valence electrons in sulfur atoms are 6. So the total valence electrons present in the molecule will be 2+6=8. Hence two valence electrons of barium are donated to sulfur and its octet is satisfied.
Bas hybridization
Hybridization is the process where orbitals (atomic) are mixed so as to form new set of orbitals. This newly formed orbitals have totally different kind of shape, energy. If the s and p character is 50% each the it leads to sp hybridization.
Bas solubility
Coming to the solubility of barium sulfide, it will differ as we change the temperature.
When the temperature is zero degrees Celsius (less) the solubility is 2.8 g/100mL. When the temperature is 20 degrees Celsius (moderate) solubility is 7.68 g/100mL. When the temperature is 100 degrees Celsius (high) the solubility is 60.3 g/100mL.
It has been observed that barium sulfide will not dissolve in methanol and ethanol.
Is Bas ionic
A compound is said to be ionic when the bond formation occurs between a metal and a non metal. In the example of barium sulfide barium being a metal, sulfur (non metal), the bond is occurring between them. Thus the barium sulfide is an ionic type of compound.
Is Bas polar or non polar
A compound will be polar if there is at least some amount of difference in the electronegativity of atoms being involved for bond formation.
A non polar type of compound will not have any kind of difference w.r.t electronegativity. Meaning there is equal sharing of charge. The electronegativity of barium is 0.9 and the electronegativity of sulfur is 2.6. The electronegativity difference for the compound Bas is hence 1.77.
So yes there is some amount of difference in the electronegativity, hence the barium sulfide compound is polar.
Is Bas acidic or basic
Bas is an inorganic type of compound. So we can say barium sulfide is a source of sulfate and it is (moderately) soluble in acids and H2O.
Conclusion
To wrap with the post we can say that barium sulfide is an inorganic type of compound which has octahedral kind of geometry. The bond formation in the molecule takes place by the metal giving 2 electrons to the non metal and the resulting is an ionic kind of compound.
Al3+ is a cation of aluminium which has fewer electrons than normal real aluminium metal.
In article we are learning about Al3+ lewis structure. Aluminium is the metal belongs to the 13th group of the periodic table. It means Al has three electrons in its outer valence shell. Al3+ ion is produced by the reduction of three electrons from Al metal. Let us discuss the detailed Al3+ structure, geometry and its various facts.
How to draw Al3+ lewis structure?
The aluminium metal is belongs to the thirteenth group of periodic table, which confirms the presence of three valence electrons in its outer valence shell. Aluminium metal has atomic number 13. Thus the aluminium metal has 13 electrons. The electronic configuration for Al metal is as follows:
Al (13) – 1s2, 2s2, 2p6, 3s2, 3p1 or [Ne]10 3s2 3p1
The Al3+ ion is produced by the decrease in electrons in aluminium metal, so Al3+ ion consists of only ten electrons in it and its outer shell being similar to neon. Thus, it has total 10 valence electrons in Al3+ ion. So, the electronic configuration of Al3+ ion is as follows:
Due to the loss or donation of three electrons by Al metal, the tripositive (3+) charge gets creates on Al metal. So the Al metal shows under the square bracket with the 3+ charge on it. Actually Al3+ is just only shows the lewis symbol but Al3+ lewis structure is not possible to draw because Al is just only an atom.
Al3+ valence electrons
The Al3+ ion has total eight valence electrons.Al atom has total 13 valence electrons from which it donates 3 electrons to form Al3+ tripositive ion. As, the Al atom belongs to 13th group of periodic table so it has 3 valence electrons in its valence shell. But in Al3+ ion it has three fewer electrons, so it has total ten electrons in Al3+ ion as shown in following figure:
Valence electrons in Al3+
Al3+ lewis structure formal charge
To calculate formal charge on any element of lewsi structure we have a formula:
Al3+ ion formal charge calculation is a s follows:
Aluminium atom: Valence electrons on aluminium atom = 08
Non-bonding electrons on aluminium atom = 03
Bonding electrons with aluminium atom =00
Formal charge on aluminium Al atom is = (08 – 08 – 0/2)
Thus, aluminium atom has zero formal charge on it.
Actually, it is not possible to calculate formal charge of any single atom anion or cation as there is no bonding and non-bonding electrons are present on it.
Al3+ lewis structure octet rule
As aluminium atom has total 13 electrons present on it and so having 3 valence electrons. So the Al metal which has only 3 electrons in its last shell having incomplete octet. Similarly, Al3+ ion has total 10 electrons present on it, so having 8 valence electrons. As the Al3+ ions have eight valence electrons in its valence shell orbital, so the Al3+ ion has a complete octet.
Al3+ lewis structure lone pairs
The Al3+ ion has total 10 electrons and having 8 electrons in its valence shell. Means it has total eight non- bonding electrons present on it i.e. eight electrons are available on Al3+ ion for sharing or bonding with other elements or atoms.
So, if we pair up two electrons to make them electron pair for bonding and sharing with other elements or atoms. We will get total four pairs of non- bonding electrons present on it. Thus, the Al3+ lewis structure or ion has total four lone pair electrons present on it.
Is Al3+ an ion?
Yes Al3+ is an ion i.e. cation in nature. As the Al atom belongs to 13th group of periodic table and has total thirteen electrons present on it with three valence electrons. So, the three valence electrons are available for sharing or bonding with other atoms or elements. If the Al atom donates its three outer shell valence electrons to other atoms, it will remain with only ten electrons.
As the Al atom losses it three electron, there will be a tri- positive charge creates on it, converting the Al atom into Al3+ ion. As there is the positive charge creates on Al atom due to loss of electrons, so Al3+ ion is a cation.
Al3+ as an cation
Al3+ lewis structure resonance
The resonance structure of Al3+ ion is not possible as there is no other atom or element is attached to it. Al3+ ion is a single element ion which has tri- positive charge present on it with complete octet as it has eight valence electrons in its outer valence shell. So, Al3+ ion can not show any resonance structure of it.
Comparative structure of Al and Al3+
Al3+ lewis structure shape
Al3+ ion has no shape. As the Al3+ ion is a single atom cation with tri- positive charge on it and it has four lone electron pairs for bonding with other atoms. But as the Al3+ is just an ion it is not attached with other atoms so it doesn’t becomes a molecule.
Even it doesn’t have any bonds or bonding electrons, so it can’t bent or linear or do not orient towards anywhere. As it has not attached with other elements, there is no electron cloud density present on it and no comparisons of electronegativity of two or more than two elements.
Al3+ lewis structure angle
Al3+ is the single element ion and don’t have any other elements attached with it. Even it doesn’t have any kind of deviation towards electron cloud density of other atoms. Also there is no comparison of electronegativities between two or more atoms or elements. So, there is no any angle present in Al3+ lewis structure or Al3+ ion.
Al3+ hybridization
Al3+ ion originally don’t have any hybridization as it is just a single element ion. Hybridization occurs with the mixing and recasting of atomic orbitals of any molecule consists of two or more atoms in it. But in case of Al3+ ion there is no other elements are present rather than aluminium and also there is no bonding form within the ion.
So, alone Al3+ ion can’t show any kind of hybridization. But Al3+ ion can form complex compounds when AlCl3 reacted with aqueous acids forms a complex compound like [Al(H2O)6]3+. In complex compounds like this, Al3+ ion has sp3d2 hybridization.
Al3+ solubility
Al3+ ion is soluble in following list:
Bromides (Br–)
Chlorides (Cl–)
Chlorates (ClO3–)
Nitrates (NO3–)
Sulphates (SO42-)
Al3+ ion is insoluble in following list:
Carbonates (CO32-)
Hydroxides (OH–)
Oxides (O2-)
Phosphates (PO43-)
Dichromates (Cr2O72-)
Is Al3+ polyatomic?
No, Al3+ is not a polyatomic ion as it is consists of only one atom or element. Polyatomic means the compound which contains two or more than two atoms in its compound. But Al3+ ion doesn’t have any other atom in its Al3+ lewis structure. So, it is not a polyatomic ion. As forming compound with other atoms Al3+ ion can form polyatomic molecules.
Is Al3+ acidic or basic?
Al3+ ion is a high charge containing small ion, so it has the density of very high charge and great polarising power. When reacts with water it will take OH- ions from water and creating More H+ ions in the solution.
Al3+ metal ions acidity strength is related to its capability to attract the electron towards itself i.e. behaves as oxidising agent. The metal ion acidity strength is as in the order Al3+ > Mg2+ > Na+.
So, it acts as a lewis acid in water and also can produce aqua complex ions in it. Also Al3+ ion can act as a lewis base as it can accepts pair of electrons from water to form aqua complex.
Is al3+ paramagnetic or diamagnetic?
Compounds or atoms containing unpaired electrons in its valence shell are considered as a paramagnetic compound and the compounds or atoms which have completely paired electrons are considered as diamagnetic compounds. Magnetic field affects paramagnetic compounds but the magnetic field doesn’t affect diamagnetic compounds.
In aluminium metal there is a loss of three electrons from its valence shell, so there are remaining ten electrons forming Al3+ ion. So, the electronic configuration of Al3+ ion is:
Al3+ = 1s2, 2s2, 2p6
Electronic configuration of Al3+ ion
From the above electronic configuration of Al3+ ion we can see that there are all completely paired electrons are present in 2p6 orbital of Al3+ ion, so it is diamagnetic in nature.
Is Al3+ isoelectronic with neon?
Isoelectronic means the molecule or atom or ions having equal or same number of electrons are isoelectronic with each other.
The electronic configuration of neon and Al3+ ion are as follows:
Ne = 1s2, 2s2, 2p6 or [He] 2s2, 2p6
Al3+ = 1s2, 2s2, 2p6 or [Ne] 2s2, 2p6
As we can see from the above electronic configuration of Neon and Al3+ ion both have same number of electrons present in their outer valence orbitals i.e. ten electrons are present in both neon and Al3+ ion so they are isoelectronic with each other.
Conclusion:
Al3+ ions have 3 less electrons than original Al metal and have a tri- positive charge on it having 8 valence electrons in its outer shell. It has complete octet with four lone electron pair. It is a cation and isoelectronic with neon atom. It also shows diamagnetic nature as it has completely paired electrons.
According to this rule, atoms try to fill eight electrons in their valence shell to achieve noble gas configuration and stability.
This can be achieved by either sharing valence electrons(as in the case of covalent bonding) or by the transfer of electrons(as seen in ionic bonding).Hydrogen, helium, lithium, sulfur, and phosphorous are some examples of atoms that do not obey the octet rule.
How to draw Li2O lewis structure?
Lewis structure is a diagram in which valence electrons are arranged around all the atoms in a molecule in a way that it fills the valence shell of all the atoms present.
STEP 1: First, we have to recognize the central atom; it is usually the atom that is least in number or the atom that can form the most bonds.
Here, oxygen is the central atom with six electrons in its valence shell(2s2 2p6). It needs two more electrons to fill its valence shell, which it gets from the two lithium atoms.
Each lithium atom has one electron in its valence shell(2s1) that it donates to oxygen to attain a helium-like configuration(1s2). The valence electrons are shown by drawing dots around the atoms.
STEP 2: We will draw eight dots around oxygen(six valence electrons and two gained from lithium).
STEP 3: Lithium, after transferring its valence electron, will get a positive charge, and oxygen will get a 2- charge as it has gained two electrons.
The li20 structure forms an fcc crystal lattice. The li2O crystal lattice has an antifluorite structure.In this structure, the oxide anions occupy the face-centered lattice points, whereas lithium ions occupy the tetrahedral voids.The cations and anions ratio in this structure is 4:8. The shape of covalent compounds is determined by VSEPR theory. Since Li20 is ionic, only the structure of its crystal lattice is determined.
Li2O lewis structure resonance
Molecules that form double(or triple) bonds can have multiple lewis structures. These are resonating structures of lewis diagrams. In Li2O, there are no double bonds, and we can only draw one lewis structure of it as no resonance is present.
Li2O lewis structure lone pairs
In Li2O, each lithium atom has one valence electron with no lone pair, and oxygen has six valence electrons with two lone pair electrons. The total number of valence electrons present in Li2O is eight.
Li2O hybridization
The hybridization concept is used to describe the bonding in covalent compounds only. Li2O is an ionic compound, and therefore, it does not participate in hybridization.
Li2O lewis structure formal charge
A formal charge is a hypothetical charge we get when we assume that electrons in a bond are shared equally(assuming equal electronegativities of all atoms). The formal charge is calculated for a covalent bond. Since Li2O is an ionic compound, we cannot calculate its formal charge.
Li2O uses
Lithium oxide is used as a flux-it lowers the high melting point of glass, therefore used in the ceramic and glass industry. It promotes liquefaction.
It is an important material for lithium-ion batteries.
It is used to absorb carbon dioxide and water from the air.
It is used to produce lithium metal and lithium hydroxide by electrolysis of lithium oxide.
It produces blue and pink colors with copper and cobalt metal, respectively, and is used to color ceramics.
Is Li2O stable?
Li2O has high lattice energy and is thermodynamically stable.
Lattice energy depends on the charge of metal(lithium in this case) and decreases as the size of the anion increases. Since oxide is a small anion, lithium oxide will have high lattice energy, making it stable(Thermodynamic stability depends on the lattice energy).
CONCLUSION
Lithium oxide is an ionic compound. We explained the lewis diagram, stability, hybridization, use, and other important aspects related to lithium oxide.
Arsenic pentachloride (AsCl5) features a central arsenic (As) atom with 5 valence electrons, each forming a single bond with five chlorine (Cl) atoms, contributing 7 valence electrons each. The Lewis structure shows five single As-Cl bonds, using 40 valence electrons, with no lone pairs on arsenic. AsCl5 adopts a trigonal bipyramidal geometry, with three Cl atoms in equatorial positions and two in axial positions, resulting in 90° and 120° bond angles. The molecule’s symmetry makes it nonpolar, despite the polar As-Cl bonds due to the electronegativity difference (As: 2.18, Cl: 3.16). This structure influences its reactivity and use in research, though it’s less stable and common than AsCl3.
Arsenic pentachloride,AsCl5 is a chemical compound formed by arsenic and chlorine. Arsenic chloride has similiar structure like phosphurus pentachloride but has no stable existence.
Ascl5 Lewis Structure
How to draw AsCl5 Lewis structure ?
The Lewis dot structures are drawn to get facts related with the bonding in molecules and ions. This mainly deals with the shared pairs of electrons between the atom and the octet rule. While drawing lewis structure only the valence electrons are considered. The valence electrons are denoted as dots in lewis structures. So the structures drawn with the help of this concept is called lewis dot structures.
The lewis structure of Arsenic pentachloride or AsCl5 can be drawn easily. Before that it is important to understand how the compound is formed. The atomic number of arsenic is 33 and chlorine is 17. The valence electrons present in the outer shell of arsenic is 5.
The electrons present in the valence shell of chlorine is 7. Here there are 5 chlorine atoms so the total number of valence electrons of five chlorine atoms is 35. Arsenic pentachloride is a covalent compound formed by the mutual sharing of atoms between one arsenic and five chlorine atoms. So the lewis structure of Arsenic pentachloride can be drawn like this
Resonance is the movement of electrons delocalised in an atom of a molecule. This is mainly depicted through some contributing structures. Such structures or figures are called as its resonance structures. The resonance structure of arsenic pentachloride is same as its shape. There is no delocalistion of electrons takes place here in this case.
Shape of AsCl5
AsCl5 Shape
Arsenic pentachloride is formed by the sharing of five valence electrons of arsenic with five chlorine atoms. The shape of the compound is found to be triagonal bipyramidal structure. There are five bonds between arsenic and chlorine.
The two bonds are axial bonds and the remaining three is equatorial bonds. The bond length of axial bonds are greater than the equatorial bonds. The bond length of axial and equatorial bonds are 220.7 pm and 210.6 pm respectively.
Structure of AsCl5
AsCl5 Formal charge
Formal charge is a charge assigned to an atom when all of its valence electrons are perfectly shared with other atoms to form a chemical bond.
Formal charge of a molecule can be given as,
Formal charge of an atom = [No. of valence electrons –( No. of electrons + No.of bonds formed)].
The total number of valence electrons present in Arsenic is 5, the lone pair of electron in As is 0, the number of bonds formed by arsenic with five chlorine atoms is 5. So the formal charge of As can be
Formal charge of Arsenic = 5-0-5
= 0
The number of valence electrons present in Chlorine is 7, the electrons available as lone pairs in Cl is 6, the number of bonds formed with one arsenic is 1. So the formal charge of Cl will be
Formal charge of Chlorine = 7-6-1
= 0
The formal charge present in Arsenic and chlorine in AsCl5 is 0.
AsCl5 Bond Angle
The Bond angle in a molecule is the angle between the bonds of atoms when different or same atoms combine together to form a compound. AsCl5 is a compound with five bonds between arsenic and five chlorine atoms with triagonal bipyramidal structure. The bond angle of equitorial bonds in AsCl5 is 1200 and axial bond is 900 respectively.
Bond angle of AsCl5
AsCl5 Octet rule
The octet rule explains that the atoms are found to be very stable when their valence shell or outermost shell are filled with eight electrons. In the case of arsenic penta chloride there is one arsenic atom and five chlorine atoms are present.
The valence shells of each chlorine atom has 7 electrons when it forms five bond with arsenic then the valence shell of each of chlorine atom has eight electrons. So the octet of chlorine atoms in AsCl5 is completely satisfied hence it obeys octet rule. While in arsenic its valence shell contains five electrons and need three more to satisfy the octet rule.
But when it forms five bonds with chlorine atoms its valence shell is now filled with ten that is more than eight electrons. So arsenic shows deviation from octet rule. Hence arsenic is considered as a hypervalent molecule.
A hypervalent molecule is a molecule with one or more elements which has more than eight electrons in its valence shell due to bond formation with other atoms.
Bond formation in AsCl5
AsCl5 Lone pair of electrons
Lone pair of electrons are the electron pair present in the outermost shell of an atom that is not shared or get bonded to another atom. It can be also called as non bonding electron since it doesn’t took part in a bond formation.
The lone pair of electron in a molecule can be found out through the following equation.
Lone pair of electron in an atom = ( No. of valence electrons – No. of electrons shared by the atom) /2
Lone pair of electron in As = (5 – 5)/2
= 0
There is no lone pair in Arsenic atom in Arsenic pentachloride
Lone pair of electron in Cl = (7-1)/2
= 3
The lone pair of electrons in Chlorine is 3. Here there are five chlorine atoms each with three lone pair of electrons.
AsCl5 Valence electrons
Valence electrons are the electrons present in the outermost shell of an atom. Valence electrons participate in a chemical reaction by sharing the electrons to form stable compounds. Before bond formation arsenic has five and chlorine has seven valence electrons in the outermost shell.
After the bond formation arsenic has ten electrons in its valance shell and each chlorine atoms has eight valence electrons in its outermost shell. So the total number of valence electrons present in arsenic chloride is 40.
AsCl5 Hybridisation
The intermixing of atomic orbital with slightly different energy to form a set of new orbitals with same energy and shape is called Hybridisation. This concept gives a good picture about the bond formation in covalent compounds. The number of hybrid orbitals formed will be equal to the number of atomic orbitals got hybridised.
The freshly formed those orbitals are called as hybrid orbitals.
The ground state electronic configuration of Arsenic is 3d10 4s2 4p3. In its excited state electronic configuration is 4s1 4p3 4d1. One of electron in the 4s is excited to 4d level.
One 4s, three 4p and one 4d orbitals hybridise together to form five sp3d hybrid orbitals with same energy. The five chlorine atoms shares one electron present in its 3p orbital to form five covalent bonds. So the hybridisation in AsCl5 is sp3d hybridisation.
Hybridisation of AsCl5
AsCl5 Solubility
Since AsCl5 is unstable compound its solubility is not found out.
Is AsCl5 is Acidic or Basic ?
The acidic or basic character of arsenic pentachloride is doesn’t determined due to its unstable nature.
Is AsCl5 Ionic or Covalent ?
A covalent bond is formed by the mutual sharing of electrons between the bonded atoms. Arsenic pentachloride is formed by through sharing of electrons between arsenic and five chlorine atoms. Therefore Arsenic pentachloride AsCl5 is a covalent compound.
Is AsCl5 Polar or Non polar ?
Arsenic pentachloride is a covalent compound with non – polar nature.
Is AsCl5 triagonal bipyramidal ?
Arsenic pentachloride is a compound with triagonal bipyramidal geometry with two axial and three equatorial bonds.
Why is AsCl5 Unstable ?
Arsenic pentachloride is unstable. It due to the incomplete shielding of the 4p orbitals seen in between the nucleus and 4s orbital. Because of this reason electrons of 4s orbital are less available for bonding. Therefore it is unstable in its nature.
Conclusion
This article explains about full details regarding Arsenic pentachloride, a chemical compound. Its lewis structure, valence electrons, lone pairs, octet rule were discussed here. Inaddition to this its shape,solubility and polar nature are explained. Arsenic pentachloride is a compound with sp3d hybridisation with least stability.
