Question

What is the hybridization of the carbon atom in \(CO_2\)?

• A. \(sp^3\)
• B. \(sp^2\)
• C. \(sp\)
• D. \(sp^3d\)

Hint:

If the central atom has:
• 2 regions of electron density → \(sp\)
• 3 regions → \(sp^2\)
• 4 regions → \(sp^3\) Carbon in \(CO_2\) has two regions, hence \(sp\) hybridization.

Answer 1

The Correct Option is C

Step 1: Understanding the Question:
We need to find the hybridization of the central Carbon atom in Carbon Dioxide (\( CO_2 \)) based on its bonding environment.
Step 2: Key Formula or Approach:
Hybridization can be determined by calculating the Steric Number (\( SN \)):
\[ SN = (\text{Number of sigma bonds}) + (\text{Number of lone pairs on the central atom}) \]
Step 3: Detailed Explanation:
1. Carbon has 4 valence electrons. In \( CO_2 \), it forms two double bonds (\( O=C=O \)).
2. Each double bond consists of one sigma (\( \sigma \)) bond and one pi (\( \pi \)) bond.
3. Therefore, Carbon has 2 sigma bonds and 0 lone pairs.
4. Steric Number \( = 2 + 0 = 2 \).
5. A steric number of 2 corresponds to \( sp \) hybridization.
This results in a linear geometry with a bond angle of \( 180^\circ \).
Step 4: Final Answer:
The hybridization of Carbon in \( CO_2 \) is \( sp \).