# Question #1f3e8

Jan 5, 2016

Hybridization is $s {p}^{2}$. See image below.

#### Explanation:

Feb 9, 2016

$s {p}^{2}$

#### Explanation:

The electron pairs arrangement around sulfur is trigonal planar with a bond angle of around ${120}^{\circ}$.

For sulfur to achieve this geometry the orbitals $s$ and $p$ will mix to form three new hybrid orbitals called $s {p}^{2}$ leaving a non hybridized orbital $p$ for the lone pairs on sulfur.

For the oxygen atoms, we should consider the hybrid form of $S {O}_{2}$:

In the hybrid form the electron pairs arrangement around oxygen is also trigonal planar with a bond angle of around ${120}^{\circ}$.

For oxygen to achieve this geometry the orbitals $s$ and $p$ will mix to form three new hybrid orbitals called $s {p}^{2}$ leaving a non hybridized orbital $p$ for one of the two lone pairs and the second will be in a $s {p}^{2}$ hybrid orbital.

Images source: http://bilbo.chm.uri.edu/