Chlorine Bleach Chlorine combines with oxygen in several proportions. Dichlorine monoxide (Cl2O
) is used in the manufacture of bleaching agents. Potassium chlorate KCLO3
is used in oxygen generators aboard aircraft. Draw the Lewis structures for CL2O
and CLO3
.
The Correct Answer and Explanation is:
Lewis Structures and Explanation for Cl₂O and ClO₃⁻
1. Lewis Structure of Cl₂O (Dichlorine Monoxide)
Structure:
- Oxygen is the central atom.
- Two single bonds connect oxygen to each chlorine atom.
- Oxygen has two lone pairs.
- Each chlorine atom has three lone pairs.
rubyCopyEdit :Cl: :Cl:
| |
.. O .. .. O ..
| |
In simplified form:
mathematicaCopyEditCl–O–Cl
Each atom has a full octet. No formal charges are present.
2. Lewis Structure of ClO₃⁻ (Chlorate Ion)
Structure:
- Chlorine is the central atom.
- Three oxygen atoms surround chlorine.
- Two of the oxygen atoms are singly bonded and carry a negative charge.
- One oxygen is double bonded.
- Chlorine has one lone pair.
mathematicaCopyEdit ..
:O:
|
:O–Cl=O:
|
..
Formal charges:
- Each singly bonded O: −1
- Chlorine: 0
- Overall charge: −1
Resonance is present. The double bond shifts among the three oxygen atoms, making all Cl–O bonds equivalent in reality.
Explanation
Dichlorine monoxide (Cl₂O) consists of two chlorine atoms and one oxygen atom. The oxygen atom has six valence electrons and needs two more to complete its octet. Each chlorine atom has seven valence electrons and requires one additional electron. Oxygen forms single covalent bonds with each chlorine atom, contributing one electron to each bond. This sharing satisfies the octet rule for all atoms. The molecule is bent due to the lone pairs on the oxygen atom, which repel the bonding pairs. The chlorine atoms are more electronegative than oxygen, but oxygen is central because of its ability to form two bonds and accommodate lone pairs.
Chlorate ion (ClO₃⁻) has chlorine in the center surrounded by three oxygen atoms. Chlorine has seven valence electrons and can expand its octet due to available d-orbitals. The total valence electron count for ClO₃⁻ is 26: chlorine contributes 7, each oxygen 6, and one extra electron accounts for the negative charge. One oxygen forms a double bond with chlorine, while the other two form single bonds and hold the extra electrons as lone pairs. Formal charge analysis shows this configuration minimizes charges, placing the negative charges on the more electronegative oxygen atoms. The ion exhibits resonance, as the position of the double bond can rotate among the three oxygen atoms. This delocalization stabilizes the ion. All Cl–O bonds are equivalent due to this resonance. Chlorine in this ion uses an expanded octet (more than 8 electrons) to accommodate all bonding and lone pairs, which is permissible for third-period elements.
These structures illustrate the flexibility of atoms like chlorine and oxygen in forming compounds with different oxidation states and resonance forms, which is essential in chemical applications such as bleaching and oxygen generation.
