Question

Explain hybridization of central atom in :$H_{2}O$

Answer 1

$\bullet$ In $H_{2}O$, $O$ is the central atom and its one $2s$

of three $2p$ orbitals hybridized to give four $s{p}^3$ hybrid orbitals.

$\bullet$ Two $s{p}^3$ hybrid orbitals having unpaired electrons overlap with the s-orbital of $H$ to form two $H-O$ $s{p}^3=s$ bonds.

$\bullet$ Geometry is tetrahedral.

$\bullet$ Bond angle $n^{\prime }s$ reduced to $104.5°$ from $109.5°$ due to more lone pair repulsion and hence the molecule requires a $V-shape$..