The linear shape of `CO_(2)` is due to ……….

Options

A. `sp^(3)` hybridisation of carbon
B. sp hybridisation of carbon
C. `p pi - p pi` bonding between carbon and oxygen
D. `sp^(2)` hybridisation of carbon

Explanation

To answer the question regarding the linear shape of carbon dioxide (CO₂), we can break down the explanation into several steps:

### Step-by-Step Solution:

1. **Understanding the Molecular Structure**:
- Carbon dioxide (CO₂) consists of one carbon atom and two oxygen atoms. The arrangement of these atoms determines the shape of the molecule.

2. **Hybridization of Carbon**:
- The carbon atom in CO₂ undergoes hybridization. In this case, carbon is sp hybridized. This means that one s orbital and one p orbital from carbon mix to form two equivalent sp hybrid orbitals.

3. **Bond Formation**:
- Each of the sp hybrid orbitals forms a sigma (σ) bond with an oxygen atom. Additionally, there are two unhybridized p orbitals on the carbon that form pi (π) bonds with the p orbitals of the oxygen atoms. This results in a double bond between carbon and each oxygen atom.

4. **Bond Angles**:
- The geometry of the molecule is influenced by the hybridization. In sp hybridization, the bond angle is 180 degrees. This means that the two oxygen atoms are positioned at opposite ends of the carbon atom, leading to a linear shape.

5. **Conclusion**:
- Therefore, the linear shape of CO₂ is primarily due to the sp hybridization of the carbon atom and the formation of pi bonds between carbon and oxygen.

### Final Answer:
The linear shape of CO₂ is due to its sp hybridization and the formation of pπ-pπ double bonds.

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