Oxygen is more electronegative than chloride. In the series of oxyacids HOCI, `HCIO_(2)`, `HCIO_(3)` and `HCIO_(4)`, an increasing number of oxygen atom is bonded to the chlorine atom. Chlorine forms a number of oxyacids which differ in their stability order.
The hybridisation of CI in `ClO_(2)^(-1)` and its shape are

Options

A. `sp^(3)`, pyramidal
B. `sp^(2)`, angular
C. `sp^(3)`, angular
D. `sp^(2)`, trigonal planar

Explanation

To determine the hybridization of chlorine in the ClO2⁻ ion and its shape, we can follow these steps:

### Step 1: Identify the central atom and its valence electrons
- The central atom in ClO2⁻ is chlorine (Cl).
- Chlorine has 7 valence electrons.

### Step 2: Determine the number of monovalent atoms (M) attached to the central atom
- In ClO2⁻, we have two oxygen atoms. However, since oxygen is divalent (it can form two bonds), we do not count them as monovalent atoms.
- Therefore, the number of monovalent atoms (M) is 0.

### Step 3: Determine the charge on the molecule (C)
- The charge on the ClO2⁻ ion is -1. Thus, C = -1.

### Step 4: Use the hybridization formula
The hybridization can be calculated using the formula:
\[ H = \frac{1}{2} (V + M - C) \]
Where:
- \( V \) = Valence electrons of the central atom (7 for Cl)
- \( M \) = Number of monovalent atoms (0)
- \( C \) = Charge on the molecule (-1)

Substituting the values:
\[ H = \frac{1}{2} (7 + 0 - (-1)) \]
\[ H = \frac{1}{2} (7 + 1) \]
\[ H = \frac{1}{2} (8) \]
\[ H = 4 \]

### Step 5: Determine the hybridization type
- A hybridization value of 4 corresponds to sp³ hybridization.

### Step 6: Determine the shape of the ClO2⁻ ion
- In ClO2⁻, chlorine forms one double bond with one oxygen and a single bond with the other oxygen (which carries the negative charge).
- The chlorine atom will have 2 lone pairs of electrons remaining after bonding.
- When determining the shape, we ignore the lone pairs. The presence of 2 bonded pairs and 2 lone pairs leads to an angular shape.

### Final Answer
- The hybridization of chlorine in ClO2⁻ is **sp³** and its shape is **angular**.