Lewis structure for PF4

Lewis structure for PF4+

The correct answer and explanation is:

The Lewis structure of PF4+PF_4^+ (phosphorus tetrafluoride cation) consists of phosphorus (P) as the central atom, bonded to four fluorine (F) atoms, and carrying a +1 charge.

Steps to Draw the Lewis Structure of PF4+PF_4^+:

1. Determine the total number of valence electrons:
   • Phosphorus (P) is in group 15, so it has 5 valence electrons.
   • Fluorine (F) is in group 17, so each fluorine has 7 valence electrons.
   • Since there are four fluorine atoms, their total contribution is 4 × 7 = 28 electrons.
   • The +1 charge means one electron is lost, reducing the total count by 1.
   Total valence electrons = 5 + 28 – 1 = 32 electrons.
2. Identify the central atom and arrange the atoms:
   • Phosphorus is the central atom because it is less electronegative than fluorine.
   • The four fluorine atoms are symmetrically arranged around phosphorus.
3. Form single bonds between phosphorus and fluorine:
   • Each P–F single bond requires 2 electrons.
   • With 4 bonds, 4 × 2 = 8 electrons are used.
4. Distribute the remaining electrons:
   • After forming bonds, 32 – 8 = 24 electrons remain.
   • These electrons are placed as lone pairs on the fluorine atoms (each gets 6 electrons to complete the octet).
5. Check for formal charges:
   • Formal charge on phosphorus: (5 – 0 – 4) = +1.
   • Each fluorine has a formal charge of (7 – 6 – 1) = 0.
   • Since the molecule has an overall +1 charge, the structure is correct.

Molecular Shape and Hybridization:

• The electron geometry is tetrahedral.
• Due to the +1 charge, the molecule is somewhat distorted compared to a neutral PF4PF_4.
• The hybridization of phosphorus in PF4+PF_4^+ is sp³.

Here is the Lewis structure image of PF4+PF_4^+:

Here is the Lewis structure of PF4+PF_4^+ with the correct arrangement of atoms, bonds, lone pairs on fluorine, and the +1 charge. Let me know if you need further explanations!