What is the electron pair geometry for P in PF2Cl3? Are there lone pairs around the central atom, and what is the geometry of PF2Cl3?

The electron pair geometry for phosphorus (P) in PF₂Cl₃ is based on the arrangement of its bonding and lone pairs. In this molecule, phosphorus is the central atom surrounded by two fluorine atoms and three chlorine atoms.

First, we need to determine the number of valence electrons for phosphorus. Phosphorus has five valence electrons. In PF₂Cl₃, it forms two bonds with fluorine and three bonds with chlorine, using up all five of its valence electrons. However, there are no lone pairs left on the phosphorus atom because all electrons are engaged in bonding.

Considering this bonding situation, we can categorize the electronic geometry using VSEPR (Valence Shell Electron Pair Repulsion) theory. Since phosphorus is bonded to five atoms and has no lone pairs, its electron pair geometry is classified as trigonal bipyramidal.

To summarize, in PF₂Cl₃, the absence of lone pairs leads us to conclude that the geometry remains trigonal bipyramidal. Therefore, the final geometry of PF₂Cl₃ is also trigonal bipyramidal.