# Question #c0c79

Nov 2, 2016

I disagree with the answer Methane is a classic example of $s {p}^{3}$ hybridization.

#### Explanation:

In its ground state of $1 {s}^{2} 2 {s}^{2} 2 {p}^{2}$ only the unpaired set of two p electrons are able to bond. This would give rise to a formula of $C {H}_{2}$ not $C {H}_{4}$

Carbon monoxide is an example of Carbon bonding in the ground state not the $s {p}^{3}$ hybridized state. CO has formed only two bonds. A double bond between the Carbon and the Oxygen The Lewis dot structure would look like this.
..
: C :: O:

Methane $C {H}_{4}$ has formed four bonds requiring the the $s {p}^{3}$ hybridization.