Chlorite or chlorite ion or chlorine dioxide anion is consisted of of one chlorine and also two oxygen atom v a negative charge having actually the chemistry formula ClO2-. It is also known as salts the chlorous acid. Chlorite is one of the the strongest oxidizers that chlorine oxyanions.
You are watching: Lewis dot structure for clo2-
In this article, us will research Chlorite ion(ClO2-) lewis structure, molecule geometry, hybridization, polar or nonpolar, link angle, etc.
Chlorite has actually a +3 oxidation state and is component of the chlorine oxides family. Chlorite is provided in the paper, pulp, and bleaching that textiles.
Properties the Chlorite ion
It has actually a molar fixed of 67.452 g.The conjugate mountain of chlorite ion is chlorous acid.It is a solid oxidizer.It is a salt that chlorous acid.| Name the Molecule | Chlorite ion |
| Chemical formula | ClO2- |
| Molecular geometry that ClO2- | Bent or V-shaped |
| Electron geometry the ClO2- | Tetrahedral |
| Hybridization | Sp³ |
| Bond angle | Less than 109.5º |
| Total Valence electron for ClO2- | 20 |
Page Contents present
1 just how to draw lewis structure for ClO2-(Chlorite)
2 monitor some steps for illustration the lewis dot framework of ClO2-
3 What is the molecular geometry the ClO2-?
4 Hybridization the ClO2-
5 The bond angle of ClO2-
6 Chlorite ion polarity: is ClO2- polar or nonpolar?
7 FAQ
8 summary
How to draw lewis framework for ClO2-(Chlorite)
ClO2- lewis structure consists of one single bond and one twin bond. Two lone pairs present on the central atom that the ClO2- Lewis structure. Lewis diagram is a depiction of the valence electron within a molecule.
To draw the lewis diagram of any type of molecule, we have to follow 5 or 6 an easy steps depending upon the intricacy of the molecule.
Here’s in this article, we will attract the ClO2- lewis framework with some simple steps consisting of all explanations.
Follow some measures for drawing the lewis dot framework of ClO2-
1. Count full valence electron in ClO2-
Counting valence electron is constantly the first step we need to follow for drawing the lewis diagram of any kind of molecule. To counting the valence electron the a molecule, simply watch the periodic group number of an atom.
In the case of the ClO2- molecule, chlorine belongs come the 17th routine group and oxygen 16th. Hence, the valence electron because that chlorine is 7 and for oxygen, that is 6.
⇒ Total variety of the valence electrons in chlorine = 7
⇒ Total variety of the valence electron in oxygen = 6
∴ Total variety of valence electron obtainable for drawing the lewis structure of ClO2- = 7 + 6(2) + 1 = 20 valence electrons <∴two oxygen atoms, one chlorine and one an unfavorable charge that count as a one valence electron>
2. Uncover the the very least electronegative atom and placed it at center
Now we have to discover the outer and main atom of the ClO2- molecule. Generally, less electronegative holds the location of the central atom, and also the remainder are spread evenly roughly it.
So, indigenous chlorine and also oxygen, chlorine(3.16) is much less electronegative 보다 oxygen(3.44). Hence, placed the chlorine in ~ the center, and oxygen atoms spread about it.
3. Connect outer atom to central atom with a solitary bond
Here’s in this step, us will attach outer atoms(oxygen) to the main atom(chlorine) v the aid of a single bond for further illustration the lewis framework of ClO2-. Simply place one-one single bonds between oxygen and chlorine atom.
After connecting the outer atom come the central atom, count the variety of valence electrons we used till now for making the above structure. A solitary bond developed from two-electron and also in the above structure, we supplied two solitary bonds.
Hence, 4 valence electrons we have used in the above structure from the 20 easily accessible valence electron for drawing the ClO2- Lewis structure.
∴ (20 – 4) = 16
We have actually left through 16 valence electron more.
4. Ar remaining valence electrons beginning from external atom first
It’s time to finish the octet that the external atom first. “The octet rule describes the propensity of atom to choose to have actually eight electrons in the valence shell”.
So, start putting the staying valence electrons on the external atom(oxygen) and complete their octet first.
So, we put the 6 valence electron on every oxygen, as oxygen currently shares two-electron v the assist of a single bond. Every oxygen in the above structure shares 8 electrons, hence completed your octet comfortably.
As we had actually a full of 16 valence electrons and also in the above structure, we supplied 12 more electrons.
∴ (16 – 12) = 4 valence electrons
Now we space still left v 4 an ext valence electrons.
5. Complete main atom octet and also make covalent link if necessary
In ClO2- molecule, chlorine is the central atom and also it needs 8 electrons roughly to finish the octet. As you watch in the framework of the 4th step, chlorine already sharing 4 electrons v the assist of two single bonds connected to oxygen atoms.
So, simply put the 4 leftover valence electrons on chlorine and also complete the octet.
By looking in ~ the over structure, we see both atoms(oxygen and chlorine) in ClO2- molecule completed their octet comfortably and we offered all our 20 complete valence electrons easily accessible for drawing the ClO2- Lewis structure.
But we don’t understand if the over ClO2- Lewis structure is stable or not, so us can’t i think the over structure, together the best and stable lewis framework of ClO2-.
For checking the security of the lewis diagram, we will certainly go with the concept of a official charge.
6. Examine the stability with the help of a formal fee concept
“A formal fee is a charge assigned come an atom in a molecule, assuming that electrons in every chemical binding are shared equally between atoms.”
The structure with the formal charge close to zero or zero is the best and stable lewis structure.
We will certainly calculate the formal fee on the 5th step structure.
⇒ officially charge = (valence electrons – lone pair electrons – 1/2bonded pair electrons)
For chlorine atom –
⇒ Valence electron the chlorine = 7
⇒ Lone pair electrons on chlorine = 4
⇒ bonded pair electrons approximately chlorine = 4
F.C. On chlorine atom = (7 – 4 – 4/2) = +1
For oxygen atom –
⇒ Valence electron that oxygen = 6
⇒ Lone pair electrons on oxygen = 6
⇒ bonded pair electrons about oxygen = 2
F.C. Top top oxygen atom = (6 – 6 – 2/2) = -1
The above structure is not lot stable, as the lewis structure is the many stable once the formal charge on each atom and an all at once formal fee of the molecule is close come zero or zero.
Let’s perform some twists on the above structure to gain the formal charge close come zero.
As we know, chlorine can hold more than 8 electrons since it has d orbital for extra electrons needed for bonding.
So, just take one lone pair native one oxygen atom, transform it to a covalent bond, and also forms a Cl=O bond.
Now again recognize the formal fee on the new ClO2- Lewis structure.
For chlorine atom –
⇒ Valence electron the chlorine = 7
⇒ Lone pair electron on chlorine = 4
⇒ bonded pair electrons roughly chlorine = 6
F.C. ~ above chlorine atom = (7 – 4 – 6/2) = 0
For oxygen atom(left side) –
⇒ Valence electron that oxygen = 6
⇒ Lone pair electron on oxygen = 4
⇒ bonded pair electrons around oxygen = 4
F.C. On oxygen atom = (6 – 4 – 4/2) = 0
For oxygen(right side) –
⇒ Valence electron = 6
⇒ Lone pair electrons on oxygen = 6
⇒ bonded pair electrons about oxygen = 2
F.C. On oxygen atom = (6 – 6 – 2/2) = -1
∴ We obtain (-1) as whole formal charge on the new ClO2- lewis structure and also two atoms have actually zero official charges, hence, this lewis structure of ClO2- is secure and much better than the vault structure(5th action structure).
This is the best and stable lewis dot structure of ClO2- as it has the minimum officially charge, also, fees on chlorine and one oxygen is zero.
ClO2- molecule consists of a negative charge also, so, we placed -1 external the parentheses in the over structure. Also, Chlorite ions can exist in lot of resonant states as result of the changing of bonds.
What is the molecular geometry of ClO2-?
“Molecular geometry is the three-dimensional arrangement of atoms in a molecule”. The molecular geometry that ClO2- is bent or V-shaped.
According to the lewis structure of ClO2-, chlorine is the central atom that has actually 2 lone bag on it, this lone bag occupy more space than bond pair electrons and shot to repel each other. Together a result, bonded pair roughly the oxygen atom pushes apart, this causes oxygen atoms is moved closer together.
Therefore, the resultant molecular geometry the ClO2- shows up like a bent or V-shaped.
Let’s see how to find the molecule geometry that ClO2- using the AXN an approach and VSEPR theory.
That’s exactly how the AXN notation follows as shown in the over picture.
AXN notation for ClO2- molecule:
A represents the main atom, so as per the ClO2- lewis structure, chlorine is the main atom. A = ChlorineX to represent the bonded atoms, as we know, chlorine is fastened to 2 oxygen atoms. Therefore, X = 2N to represent the lone pair, the chlorine atom has two lone bag on it. Hence, N = 2So, the AXN formula for the ClO2- molecule i do not care AX2N2.
According come the VSEPR theory, if a molecule main atom is attached v two bonded atoms and also has two lone pairs then the molecule geometry of that molecule is V-shaped or bent.
Hence, the molecular form or geometry for ClO2- is bent.
ClO2- molecular geometry
The electron geometry because that ClO2- is tetrahedral.
Hybridization the ClO2-
To find the hybridization of an atom, we have to first determine that is hybridization number.
“Hybridization number is the enhancement of a total number of bonded atoms approximately a main atom and the lone pair present on it.”
∴ Hybridization number of ClO2- = (Number the bonded atom attached come chlorine + Lone pair on chlorine)
According to the lewis framework of ClO2-, we have two external inspection atoms(oxygen) attached come the chlorine and also two lone pair present on it.
∴ Hybridization number of ClO2- = (2 + 2) = 4
| Hybridization number | Hybridization |
| 1 | S |
| 2 | Sp |
| 3 | Sp² |
| 4 | Sp³ |
| 5 | Sp³d |
| 6 | Sp³d² |
So, because that a hybridization number of four, we gain the Sp3 hybridization ~ above the chlorine atom in the ClO2- molecule.
The bond edge of ClO2-
“A bond angle is the geometrical angle between two nearby bonds”.
The bond edge of ClO2- is less 보다 109° as result of the presence of two lone bag on chlorine atoms together these lone bag repel each other and also that pushes bonded atoms closer together, hence reasons the reduced bond angle.
Definitely ClO2- is polar in nature as it lacks symmetry since it has actually a molecular geometry that bent, which method dipole generated along with Cl-O bond unable to canceled the end each other offering some dipole minute in the molecule.
The lone pair existence on chlorine causes an unsymmetrical charge circulation in the molecule, for this reason the induced fees on the Cl-O bond do not cancel each various other completely.
Also, the visibility of a an adverse charge over the atoms provides the Cl-O binding polar in nature.
Hence, all these factors lead come ClO2- a polar molecule in nature.
FAQ
Why walk the chlorine in ClO2- lewis structure, has electrons of more than 8 and violate the octet rule? |
Whenever the d-orbitals and beyond to it, take part in bonding with various other atoms then an expanded octet is produced. Chlorine atom in ClO2- lewis structure broadened the octet since it has d-orbitals in the 3rd principal power level, hence, it has extra orbital(d-orbital) for additional electron necessary for bonding. Sulfur, phosphorous, and silicon room some other examples that can increase their octet and also hold electrons much more than 8. |
Why walk the molecular geometry of ClO2- shows up bent in shape? |
This is because of the visibility of 2 lone pairs on chlorine main atom the pushes both oxygen atom closer together, this reasons a lower O-Cl-O shortcut angle, hence, that is shape shows up as bent prefer structure. |