Question

The hybridization of carbon atom in \(CH_4\) molecule is:

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

Hint:

Shortcut: \[ \text{Steric number}=4 \Rightarrow sp^3 \] Methane is the most common example of \(sp^3\) hybridization.

Answer 1

The Correct Option is C

Concept: Hybridization is the mixing of atomic orbitals having comparable energies to form equivalent hybrid orbitals. Carbon electronic configuration: \[ 1s^2\,2s^2\,2p^2 \] In methane: \[ CH_4 \] carbon forms four equivalent sigma bonds.

Step 1: Determine number of sigma bonds around carbon.
In methane: \[ CH_4 \] carbon forms: \[ 4 \] single covalent bonds with hydrogen atoms. Thus total sigma bonds around carbon: \[ 4 \]

Step 2: Relate sigma bonds with hybridization.
Hybridization pattern: \[ 2 \text{ sigma bonds } \rightarrow sp \] \[ 3 \text{ sigma bonds } \rightarrow sp^2 \] \[ 4 \text{ sigma bonds } \rightarrow sp^3 \] Since carbon forms four sigma bonds: \[ \text{Hybridization}=sp^3 \]

Step 3: Determine geometry.
\(sp^3\) hybridization leads to: \[ \text{Tetrahedral geometry} \] with bond angle: \[ 109.5^\circ \] Hence, the correct answer is: \[ \boxed{sp^3} \]