# Math Help - chemistry

1. ## chemistry

The theory of hybridization of atomic orbitals was developed to explain molecular geometry. Sketch and name the shape of each of the following hybrid orbitals of a carbon atom in a compound:

a) $sp$
b) $sp^2$
c) $sp^3$

2. Recall the valence electron configuration of carbon: $2s^2 \ 2p^2$

a) The hybridization of one $s$ and one $p$ forms two $sp$ orbitals which leaves two unhybridized $2p$ orbitals, all half-filled. Thus when forming bonds, the two $2p$ orbitals are involved in forming $\pi$-bonds and the $sp$ orbital would form a $\sigma$-bond. This is why we normally associated sp hybrid orbitals with triple bonds.

Consider: $\text{H}-\text{C}\equiv \text{C} - \text{H}$

b) Try using similar reasoning as above. One $s$ and two $p$ orbitals form 3 $sp^2$ hybrid orbitals which leave 1 unhybridized p orbital. The unhybridized p orbital would form a $\pi$-bond with another half-filled p orbital and a $\sigma$-bond when looking at the $sp^2$ orbital. Thus, we normally associate double bonds with $sp^2$ hybrid orbitals.

Consider: $\text{H}_2\text{C}= \text{O}$

c) Consider: $\text{C}\text{H}_4$