Shortest C-O bond is present in

Options

A. Carbon monoxide
B. Carbon dioxide
C. Carbonate ion
D. Acetone

Answer

To determine which compound has the shortest carbon-oxygen (C-O) bond, we will analyze the bond types present in each of the given options.

### Step-by-Step Solution:

1. **Identify the Compounds**: The compounds we need to analyze are:
- Carbon Monoxide (CO)
- Carbon Dioxide (CO₂)
- Carbonate Ion (CO₃²⁻)
- Acetone (C₃H₆O)

2. **Determine the Bond Types**:
- **Carbon Monoxide (CO)**: In CO, there is a carbon-oxygen triple bond (C≡O). Triple bonds are the shortest and strongest type of covalent bond.
- **Carbon Dioxide (CO₂)**: In CO₂, there are two carbon-oxygen double bonds (C=O). Double bonds are longer than triple bonds but shorter than single bonds.
- **Carbonate Ion (CO₃²⁻)**: The carbonate ion has one carbon-oxygen double bond and two carbon-oxygen single bonds (C=O and C-O). The presence of single bonds makes the overall bond length longer than in CO₂ and CO.
- **Acetone (C₃H₆O)**: Acetone has a carbon-oxygen double bond (C=O) as well, similar to CO₂.

3. **Compare the Bond Lengths**:
- **Triple Bond (C≡O)** in Carbon Monoxide is the shortest.
- **Double Bonds (C=O)** in Carbon Dioxide and Acetone are longer than the triple bond.
- **Mixed Bonds** in Carbonate Ion (C=O and C-O) result in longer bond lengths compared to the triple bond.

4. **Conclusion**: Since the shortest bond is typically found in a triple bond, and carbon monoxide has a carbon-oxygen triple bond, we conclude that the shortest C-O bond is present in Carbon Monoxide (CO).

### Final Answer:
The shortest C-O bond is present in **Carbon Monoxide (CO)**.

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