Question

which of the lewis structures in the image is correct? c b a d

Explanation:

Step1: Analyze Structure A

In \(SBr_3\), sulfur should have lone pairs. Structure A misses lone pairs on sulfur.

Step2: Analyze Structure B

In \(PF_2\), fluorine should have full - octet (3 lone pairs). Structure B has incorrect lone - pair distribution on fluorine.

Step3: Analyze Structure C

In \(H_3O\), oxygen should follow octet rule. \(H_3O\) is not a stable species as written (correct is \(H_2O\) with oxygen having 2 lone pairs).

Step4: Analyze Structure D

For \(SBr_4\), sulfur has 6 valence electrons. In \(SBr_4\), sulfur forms 4 single bonds (uses 4 electrons) and has 1 lone pair (2 electrons). Each bromine has 3 lone pairs (6 electrons) and 1 bonding pair (2 electrons), satisfying the octet rule.

Answer:

D