The single, double and triple bond lengths of carbon in carbon dioxide are respectively

Options

A. 1.15, 1.22 and 1.10 Å
B. 1.22,1.15 and 1.10 Å
C. 1.10,1.15 and 1.22 Å
D. 1.15 , 1.10 and 1.22 Å

Explanation

To determine the bond lengths of carbon in carbon dioxide (CO₂), we need to understand the types of bonds present in the molecule and how they compare to single, double, and triple bonds.

### Step-by-Step Solution:

1. **Identify the Structure of Carbon Dioxide (CO₂)**:
- Carbon dioxide consists of one carbon atom (C) and two oxygen atoms (O).
- The molecular structure can be represented as O=C=O, indicating that the carbon is double-bonded to each oxygen atom.

2. **Understand Bond Types**:
- **Single Bond**: A bond formed by the sharing of one pair of electrons (e.g., C–C or C–O).
- **Double Bond**: A bond formed by the sharing of two pairs of electrons (e.g., C=O).
- **Triple Bond**: A bond formed by the sharing of three pairs of electrons (e.g., C≡C).

3. **Bond Lengths**:
- **Single Bond Length**: Typically longer than double and triple bonds due to less electron density between the atoms.
- **Double Bond Length**: Shorter than a single bond due to increased electron density, which pulls the atoms closer together.
- **Triple Bond Length**: The shortest bond length because of the highest electron density.

4. **Bond Lengths in CO₂**:
- In CO₂, there are no single or triple bonds present; only double bonds exist between carbon and oxygen.
- Therefore, we can conclude:
- **Single Bond Length**: Not applicable in CO₂.
- **Double Bond Length**: The bond length of C=O in CO₂ is approximately 120 pm (picometers).
- **Triple Bond Length**: Not applicable in CO₂.

5. **Conclusion**:
- The bond lengths in carbon dioxide can be summarized as follows:
- Single Bond Length: Not applicable
- Double Bond Length: Approximately 120 pm
- Triple Bond Length: Not applicable