After drawing the Lewis structure of BrCl3, what is the ideal bond angle around the central bromine atom?

• A. 120°
• B. 109.5°
• C. 180°
• D. 90°

Answer: (D)

Verified step by step guidance

1. Identify the central atom in BrCl\_3, which is bromine (Br), and count the total number of valence electrons around it, including those from the bonded chlorine atoms and any lone pairs on bromine.
2. Draw the Lewis structure of BrCl\_3, placing three chlorine atoms bonded to bromine and then distribute the remaining electrons to satisfy the octet rule, noting any lone pairs on bromine.
3. Determine the electron pair geometry around the central bromine atom by counting both bonding pairs and lone pairs of electrons. This will help predict the molecular shape using VSEPR theory.
4. Use VSEPR theory to find the ideal bond angles based on the molecular geometry. For BrCl\_3, which has three bonded atoms and two lone pairs, the shape is T-shaped, and the ideal bond angles are approximately 90° and 180°.
5. Conclude that the ideal bond angle around the central bromine atom in BrCl\_3 is 90°, consistent with the T-shaped molecular geometry caused by the lone pairs repelling the bonded atoms.