Shape of `ClO_(2)^(-)` ion is

Options

A. Liner
B. angular
C. pyramid
D. None

Answer

To determine the shape of the `ClO2^(-)` ion, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Central Atom**:
- In the `ClO2^(-)` ion, chlorine (Cl) is the central atom because it is less electronegative than oxygen (O).

2. **Draw the Lewis Structure**:
- Start by counting the total number of valence electrons. Chlorine has 7 valence electrons, and each oxygen has 6. Since there are two oxygens, that gives us a total of 12 electrons from oxygen. Additionally, we have one extra electron due to the negative charge of the ion. Thus, the total is:
\[ 7 + 6 + 6 + 1 = 20 \text{ valence electrons} \]
- Place Cl in the center and connect it to the two O atoms. One O will form a double bond with Cl, and the other will form a single bond with Cl, which also carries a negative charge.

3. **Assign Electrons to Bonds and Lone Pairs**:
- In the Lewis structure:
- The double bond between Cl and one O uses 2 electrons.
- The single bond between Cl and the other O uses 1 electron.
- This leaves us with:
\[ 20 - (2 + 1) = 17 \text{ electrons remaining} \]
- Place 6 electrons (3 lone pairs) on the double-bonded O and 6 electrons (3 lone pairs) on the single-bonded O. The chlorine atom will have 2 lone pairs remaining.

4. **Determine Hybridization**:
- The central atom (Cl) has:
- 2 bonding pairs (one double bond and one single bond)
- 2 lone pairs
- This gives a total of 4 regions of electron density around the chlorine atom, indicating `sp^3` hybridization.

5. **Determine the Molecular Geometry**:
- The electron geometry is tetrahedral due to the four regions of electron density.
- However, the presence of two lone pairs will affect the shape. The shape of the molecule is determined by the positions of the atoms, which leads to an angular (or bent) shape.

6. **Conclusion**:
- The shape of the `ClO2^(-)` ion is angular or bent due to the presence of the two lone pairs on the chlorine atom.

### Final Answer:
The shape of the `ClO2^(-)` ion is **angular**.