Question

what is the hybridization of the central atom in the phosphorus tetrabromate (pbr4^ -) anion?

Explanation:

Step1: Determine the number of valence - electron groups around the central atom

Phosphorus has 5 valence electrons. In the $PBr_{4}^{-}$ anion, it has 4 bonding pairs (with 4 bromine atoms) and 1 non - bonding pair (due to the negative charge). So the total number of electron groups around the central P atom is 4 (bonding) + 1 (non - bonding)=5.

Step2: Relate the number of electron groups to hybridization

The number of hybrid orbitals is equal to the number of electron groups around the central atom. When there are 5 electron groups, the hybridization is $sp^{3}d$.

Answer:

$sp^{3}d$