Question

Using VSEPR theory, predict the species which has square pyramidal shape.

• A. \(SnCl_{2} \)
• B. \(CCl_{4} \)
• C. \(SO_{3} \)
• D. \(BrF_{5}\)

Hint:

In VSEPR theory, the presence of lone pairs affects the geometry of the molecule. Square pyramidal geometry occurs when there are 5 bonding pairs and 1 lone pair around the central atom.

Answer 1

The Correct Option is D

Step 1: Grasp VSEPR theory.
VSEPR (Valence Shell Electron Pair Repulsion) theory forecasts molecular geometry by considering the repulsion among electron pairs in the central atom's valence shell. 
Molecular shape is dictated by the quantity of bonding and lone pairs surrounding the central atom. 
Step 2: Examine each species. 
\(SnCl_{2}\): The central atom, Sn, possesses 2 bonding pairs and 1 lone pair, resulting in a bent or V-shaped geometry. 
\(CCl_{4}:\) The central atom, C, has 4 bonding pairs and no lone pairs, yielding a tetrahedral geometry. 
\(SO_{3}\): The central atom, S, features 3 bonding pairs and no lone pairs, producing a trigonal planar geometry. 
\(BrF_{5}\): The central atom, Br, is bonded to 5 atoms and has 1 lone pair, leading to a square pyramidal geometry. 
Step 3: Identify the correct solution. 
\(BrF_{5}\) exhibits a square pyramidal structure owing to the presence of 5 bonding pairs and 1 lone pair around the central bromine atom.