carbon in carbon dioxide is

Options

A. `sp` hybridization
B. `sp^(2)` hybridization
C. `sp^(3)` hybridization
D. `d^(2)sp^(3)` hybridised.

Answer

To determine the hybridization of carbon in carbon dioxide (CO₂), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Valency of Carbon:**
- Carbon has a valency of 4, meaning it can form four bonds.

2. **Determine the Number of Bonds in CO₂:**
- In carbon dioxide, carbon is bonded to two oxygen atoms. Each carbon-oxygen bond is a double bond.
- Therefore, carbon forms a total of 2 double bonds (which counts as 4 bonds).

3. **Calculate the Steric Number:**
- The steric number is calculated as the number of bonds plus the number of lone pairs on the central atom (carbon in this case).
- Since carbon in CO₂ has no lone pairs and forms 2 double bonds, the steric number is:
\[ \text{Steric Number} = \text{Number of Bonds} + \text{Number of Lone Pairs} = 2 + 0 = 2 \]

4. **Determine the Hybridization:**
- The hybridization can be determined from the steric number:
- A steric number of 2 corresponds to **sp hybridization**.

5. **Identify the Geometry:**
- The geometry of a molecule with sp hybridization and a steric number of 2 is **linear**.

### Final Answer:
The hybridization of carbon in carbon dioxide (CO₂) is **sp**, and its shape is **linear**.

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