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 given species, we will analyze each molecule step by step.

### Step 1: Analyze ClO2⁻ (Chlorite Ion)
- **Structure**: Chlorine (Cl) is the central atom bonded to two oxygen (O) atoms and has two lone pairs of electrons.
- **Electron Count**: Cl has 7 valence electrons, and with the addition of one extra electron due to the negative charge, we have a total of 8 electrons.
- **Bonding**: The structure will have two single bonds to oxygen and two lone pairs on chlorine.
- **Bond Angle**: According to VSEPR theory, the presence of two lone pairs will cause maximum repulsion, resulting in a smaller bond angle.

### Step 2: Analyze Cl2O (Dichlorine Monoxide)
- **Structure**: Oxygen (O) is the central atom bonded to two chlorine (Cl) atoms and has two lone pairs.
- **Electron Count**: O has 6 valence electrons, and with two Cl atoms forming single bonds, we have a total of 8 electrons around O.
- **Bonding**: The structure will have two single bonds to chlorine and two lone pairs on oxygen.
- **Bond Angle**: Similar to ClO2⁻, the two lone pairs will cause repulsion, leading to a smaller bond angle.

### Step 3: Analyze ClO2 (Chlorine Dioxide)
- **Structure**: Chlorine (Cl) is the central atom bonded to two oxygen (O) atoms and has one lone pair.
- **Electron Count**: Cl has 7 valence electrons, and with two double bonds to oxygen, we have a total of 6 electrons used in bonding and one lone pair remaining.
- **Bonding**: The structure will have two double bonds to oxygen and one lone pair on chlorine.
- **Bond Angle**: The presence of one lone pair will cause less repulsion compared to two lone pairs, resulting in a larger bond angle.

### Step 4: Compare Bond Angles
- **ClO2⁻**: Smallest bond angle due to two lone pairs.
- **Cl2O**: Similar bond angle to ClO2⁻, but slightly larger due to the same number of lone pairs.
- **ClO2**: Largest bond angle due to only one lone pair.

### Conclusion
Based on the analysis, the correct order of increasing bond angles is:
**ClO2⁻ < Cl2O < ClO2**

### Final Answer
The correct order of increasing bond angles in the following species is:
**ClO2⁻ < Cl2O < ClO2**