Question

which of the lewis structures in the image is correct?

Explanation:

• Option A: The Lewis structure for \( SBr_2 \) should have lone pairs on sulfur. In this option, sulfur has no lone pairs shown, which is incorrect. Sulfur has 6 valence electrons. In \( SBr_2 \), it forms two single bonds with bromine (using 2 electrons), so there should be 4 electrons (2 lone pairs) remaining on sulfur.
• Option B: For \( PF_3 \), phosphorus has 5 valence electrons. It forms three single bonds with fluorine (using 3 electrons), so there should be 2 electrons (1 lone pair) remaining on phosphorus. In this option, the lone pair on phosphorus is not shown correctly.
• Option C: For \( H_2O_2 \), each oxygen has 6 valence electrons. Each oxygen forms one single bond with hydrogen and one single bond with the other oxygen. Each oxygen should have 2 lone pairs. In this structure, the lone pairs on oxygen are not shown.
• Option D: In \( SBr_2 \), sulfur (6 valence electrons) forms two single bonds with bromine (each bromine has 7 valence electrons). Sulfur has 2 lone pairs (\( 6 - 2\times1= 4 \) electrons, \( 4\div2 = 2 \) lone pairs), and each bromine has 3 lone pairs (\( 7 - 1=6 \) electrons, \( 6\div2 = 3 \) lone pairs). This structure correctly shows the lone pairs on sulfur and bromine.

Answer:

D.