Question

Using the VSEPR model, the shape of \( \text{PCl}_4^+ \) ion is:

• A. Tetrahedral
• B. Square planar
• C. Trigonal pyramidal
• D. Bent

Hint:

For a molecule with 4 bonding pairs and no lone pairs on the central atom, the shape is tetrahedral.

Answer 1

The Correct Option is A

Step 1: VSEPR Theory.
VSEPR (Valence Shell Electron Pair Repulsion) theory predicts molecular geometry by considering electron pair repulsion. Molecular shape is determined by the count of bonding and lone electron pairs around the central atom.

Step 2: Analysis of \( \text{PCl}_4^+ \).
For the \( \text{PCl}_4^+ \) ion:- Phosphorus (P) is the central atom.- It is bonded to 4 chlorine atoms, resulting in 4 bonding pairs.- The \( +1 \) charge indicates one electron deficit compared to a neutral atom, meaning there are no lone pairs on the phosphorus atom.With 4 bonding pairs and 0 lone pairs, VSEPR theory dictates a tetrahedral shape.

Step 3: Conclusion.
The \( \text{PCl}_4^+ \) ion exhibits a tetrahedral shape, aligning with option (1).