Select the single best answer. Select the statement that correctly describes the hybridization of phosphorus in \( \mathrm{PF}_{5} \). Phosphorus is \( s p^{2} \) hybridized. Phosphorus is \( s p^{3} \) hybridized. Phosphorus is \( s p^{3} d \) hybridized. Phosphorus is \( s p^{3} d^{2} \) hybridized.

Phosphorus in \( \mathrm{PF}_{5} \) is \( s p^{3} d \) hybridized. This hybridization occurs because phosphorus utilizes its 3s, 3p, and one 3d orbital to form five equivalent sp³d hybrid orbitals, which are arranged in a trigonal bipyramidal geometry around the phosphorus atom. This allows it to effectively bond with five fluorine atoms, facilitating the molecule's stable structure. In the context of hybridization, it’s essential to recognize the role of d orbitals, especially in non-metals like phosphorus that can extend their bonding capabilities. This fascinating aspect of molecular chemistry showcases how elements can adapt their electronic structure to form diverse and complex molecules.