# How do we describe the orbital hybridization in the water molecule?

The oxygen atom has $3 \times p - \text{orbitals}$, i.e. $2 {p}_{x}$, $2 {p}_{y}$, and $2 {p}_{z}$
And these three orbitals can be mathematically hybridized with the $\text{s-orbital}$ to form $4 \times s {p}^{3}$ orbitals..........and this forms $2 \times O - H$ bonds, and TWO filled lone pairs.......:stackrel(ddot)OH_2.