Question

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

Explanation:

• For option A: In \(SBr_2\), sulfur should have 2 lone pairs (since it has 6 valence electrons, 2 are used in bonding with Br, so \(6 - 2=4\) electrons left, which is 2 lone pairs). This structure is missing lone - pairs on sulfur.
• For option B: In \(PF_2\), phosphorus has 5 valence electrons. If it forms 2 bonds (with F), it should have \(5 - 2 = 3\) non - bonding electrons (1 lone pair and 1 unpaired electron). But the structure has incorrect electron distribution.
• For option C: In \(H_2O\), oxygen has 6 valence electrons. It forms 2 bonds with H, so it should have \(6-2 = 4\) non - bonding electrons (2 lone pairs). This structure is missing lone - pairs on oxygen.
• For option D: In \(SBr_2\), sulfur (valence electrons = 6) forms 2 bonds with Br (each Br has 7 valence electrons). Sulfur has \(6-2=4\) non - bonding electrons (2 lone pairs), and each Br has \(7 - 1=6\) non - bonding electrons (3 lone pairs). This structure correctly shows the bonding and non - bonding electrons.

Answer:

D.