What is the bond angle of (OClO) in ClO₂-

A. 90
B. 120

C. 105
D. 111

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To determine the bond angle of ( \text{ClO}_2^{-} ), we need to consider the electron pair geometry around the central atom, chlorine.

Step-by-Step Explanation:

  1. Determine Hybridization:

    • The central chlorine atom in ( \text{ClO}_2^{-} ) has two lone pairs and forms two sigma bonds with oxygen atoms.
    • Hence, the chlorine atom exhibits sp³ hybridization.
  2. Effect of Lone Pairs:

    • In an ideal sp³ hybridized system (like methane, CH₄), the bond angle is ( 109.5^\circ ).
    • However, ( \text{ClO}_2^{-} ) has two lone pairs on chlorine. Lone pairs exert greater repulsion compared to bonding pairs, leading to a decrease in bond angles.
  3. Lone Pair Repulsion:

    • Due to lone-pair lone-pair repulsions, the bond angle is reduced.
    • This reduction from the ideal tetrahedral bond angle of ( 109.5^\circ ) is typically around ( 5^\circ ), leading to an actual bond angle of approximately ( 105^\circ ).

Therefore, the bond angle in ( \text{ClO}_2^{-} ) is around 105 degrees.


The correct bond angle of ( \text{ClO}_2^{-} ) is C. 105 degrees.

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