When PCl₅ solidifies it forms PCl₄⁺cations and PCl₆^- anions.According to valence bond theory,what hybrid orbitals are used by phosphorus in the PCl₄⁺cation?

Question

Quizplus · Accepted Answer

In the PCl₄⁺ cation, the phosphorus atom has lost one electron and is now in a +1 oxidation state. Phosphorus in this state has three valence electrons and would require three hybrid orbitals to bond with three chlorine atoms. In valence bond theory, hybrid orbitals are created by mixing atomic orbitals to form new, hybridized orbitals. The hybridization of phosphorus in the PCl₄⁺ cation would require the promotion of one of the 3s electrons to the 3p orbital, followed by hybridization between the 3s and two 3p orbitals. This results in three sp³ hybrid orbitals, which are all used to form sigma bonds with the three chlorine atoms. Therefore, the best choice is C.

When PCl5 Solidifies It Forms PCl4+cations and PCl6- Anions

When PCl₅ Solidifies It Forms PCl₄⁺cations and PCl₆^- Anions