Question

which of the lewis structures in the image is correct?

Explanation:

Step1: Analyze option A

Phosphorus has 5 valence electrons. In the given structure, phosphorus forms 3 single bonds with chlorine atoms. Each single bond contributes 1 electron. So, \(3\times1 = 3\) electrons from bonds. And there is a lone pair (2 electrons). Total valence electrons around P: \(3 + 2=5\). Chlorine has 7 valence electrons. In the structure, each Cl forms 1 single bond (1 electron) and has 3 lone pairs (\(3\times2 = 6\) electrons). Total for Cl: \(1+6 = 7\). This follows the octet rule (for Cl) and valence electron count for P.

Step2: Analyze option B

Sulfur has 6 valence electrons. In the given structure, sulfur forms 2 single bonds (2 electrons). Each oxygen has 6 valence electrons. One oxygen forms a single bond (1 electron) and has 3 lone pairs (6 electrons), total 7 (violates octet as O should have 8). Another oxygen forms a single bond (1 electron) and has 3 lone pairs (6 electrons), total 7 (violates octet).

Step3: Analyze option C

Carbon has 4 valence electrons. In the given structure, carbon forms a double - bond (counts as 2 electrons) with sodium (but sodium is a metal and forms ionic bonds, not covalent bonds in this Lewis - structure - like representation. Also, carbon has only 3 electron - pair groups (one double bond and one single bond) which is incorrect for its valence electron distribution.

Step4: Analyze option D

Carbon has 4 valence electrons. In the given structure, carbon forms 2 single bonds (2 electrons) and has a lone pair (2 electrons). Total 4 (violates octet as it should have 8). Bromine has 7 valence electrons. One Br forms a single bond (1 electron) and has 3 lone pairs (6 electrons), total 7 (violates octet as Br should have 8). Another Br forms a single bond (1 electron) and has 3 lone pairs (6 electrons), total 7 (violates octet).

Answer:

A. Option Text