The correct order of increasing bond angles in the following species is

Options

A. `Cl_2O lt ClO_2 lt ClO_2^-`
B. `ClO_2 lt Cl_2O lt ClO_2^-`
C. `Cl_2O lt ClO_2^(-) lt ClO_2`
D. `ClO_2^(-) lt Cl_2O lt ClO_2`

Explanation

To determine the correct order of increasing bond angles in the species Cl2O, ClO2, and ClO2^-, we need to analyze the molecular geometry and the factors affecting bond angles in each molecule.

### Step-by-Step Solution:

1. **Identify the Central Atom and Valence Electrons**:
- For Cl2O: Chlorine (Cl) is the central atom. Chlorine has 7 valence electrons, and oxygen (O) has 6 valence electrons.
- For ClO2: Chlorine is again the central atom with 7 valence electrons, and each oxygen contributes 6 valence electrons.
- For ClO2^-: The charge adds an extra electron, so chlorine has 7 valence electrons, and the two oxygens contribute 12 valence electrons (6 each).

2. **Determine the Steric Number**:
- **Cl2O**: The steric number is 4 (2 bonding pairs with O and 2 lone pairs on Cl).
- **ClO2**: The steric number is 3 (2 bonding pairs with O and 1 lone pair on Cl).
- **ClO2^-**: The steric number is 4 (2 bonding pairs with O and 2 lone pairs on Cl).

3. **Predict the Molecular Geometry**:
- **Cl2O**: The geometry is bent due to the presence of lone pairs, leading to a bond angle of approximately 110°.
- **ClO2**: The geometry is also bent, but with only one lone pair, leading to a bond angle of approximately 118°.
- **ClO2^-**: The geometry is tetrahedral due to two lone pairs, leading to a bond angle of less than 109.5°.

4. **Analyze the Bond Angles**:
- **Cl2O**: Approximately 110°.
- **ClO2**: Approximately 118°.
- **ClO2^-**: Less than 109.5°.

5. **Order the Bond Angles**:
- The bond angles can be ordered as follows: ClO2^- < Cl2O < ClO2.

### Final Answer:
The correct order of increasing bond angles is:
**ClO2^- < Cl2O < ClO2**