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.
The VSEPR (Valence Shell Electron Pair Repulsion) model helps predict the geometry of molecules based on the repulsion between electron pairs. The shape of a molecule depends on the number of bonding pairs and lone pairs around the central atom.

Step 2: Analyzing \( \text{PCl}_4^+ \).
For the \( \text{PCl}_4^+ \) ion: - The central atom is phosphorus (P). - It is surrounded by 4 chlorine atoms, forming 4 bonding pairs of electrons. - The charge on the ion is \( +1 \), which means there is one fewer electron than the neutral molecule, so there are no lone pairs on the phosphorus atom. Therefore, with 4 bonding pairs and no lone pairs, the shape is tetrahedral according to VSEPR theory.

Step 3: Conclusion.
Thus, the correct shape of the \( \text{PCl}_4^+ \) ion is tetrahedral, corresponding to option (1).