The correct order of increasing C- O bond length of `CO, CO_(3) ^(-2)` and `CO_(2)` is :-

Options

A. `CO_(3)^(-2) lt CO_(2) lt CO`
B. `CO lt CO_(2) lt CO_(3)^(-2)`
C. `CO lt CO_(3)^(-2) lt CO_(2)`
D. `CO_(2) lt CO_(3)^(-2) lt CO`

Answer

To determine the correct order of increasing C-O bond length for CO, CO₃²⁻, and CO₂, we need to analyze the bonding characteristics and hybridization of each compound.

### Step 1: Analyze Carbon Monoxide (CO)
- **Structure**: CO has a triple bond between carbon and oxygen (C≡O).
- **Hybridization**: The carbon in CO is sp hybridized.
- **Bond Length**: Triple bonds are shorter than double or single bonds. Therefore, CO has the shortest C-O bond length.

### Step 2: Analyze Carbon Dioxide (CO₂)
- **Structure**: CO₂ has two double bonds (C=O) with one carbon atom bonded to two oxygen atoms.
- **Hybridization**: The carbon in CO₂ is also sp hybridized.
- **Bond Length**: Double bonds are longer than triple bonds but shorter than single bonds. Therefore, CO₂ has a longer C-O bond length than CO, but shorter than that of carbonate.

### Step 3: Analyze Carbonate Ion (CO₃²⁻)
- **Structure**: The carbonate ion has one carbon atom bonded to three oxygen atoms, with resonance structures showing one C=O double bond and two C-O single bonds.
- **Hybridization**: The carbon in CO₃²⁻ is sp² hybridized.
- **Bond Length**: The presence of both single and double bonds means that the C-O bond length in carbonate is longer than in CO and CO₂. The average bond length is longer due to the single bond character.

### Conclusion
Based on the analysis:
- **CO** (C≡O) has the shortest bond length.
- **CO₂** (C=O) has a longer bond length than CO but shorter than CO₃²⁻.
- **CO₃²⁻** (C-O) has the longest bond length due to the presence of single bonds.

### Final Order of Increasing C-O Bond Length
The correct order of increasing C-O bond length is:
**CO < CO₂ < CO₃²⁻**