Which of the following best describes the Lewis dot structure of a neutral H2S molecule?

• A. Sulfur atom in the center with two double bonds to hydrogen atoms and no lone pairs on sulfur.
• B. Sulfur atom in the center with two single bonds to hydrogen atoms and no lone pairs on sulfur.
• C. Sulfur atom in the center with two single bonds to hydrogen atoms and two lone pairs on sulfur.
• D. Sulfur atom in the center with one single bond and one double bond to hydrogen atoms and one lone pair on sulfur.

Answer: (C)

Verified step by step guidance

1. Step 1: Identify the total number of valence electrons in the H2S molecule. Hydrogen has 1 valence electron each, and sulfur has 6 valence electrons, so total valence electrons = 2 × 1 + 6 = 8 electrons.
2. Step 2: Determine the central atom, which is sulfur because it is less electronegative than hydrogen and can form more bonds.
3. Step 3: Draw single bonds between the sulfur atom and each hydrogen atom. Each single bond represents 2 electrons, so 2 bonds use 4 electrons.
4. Step 4: Distribute the remaining valence electrons as lone pairs on the sulfur atom. Since 4 electrons are used in bonds, 4 electrons remain, which form two lone pairs on sulfur.
5. Step 5: Confirm that each hydrogen has a full valence shell (2 electrons) and sulfur has an octet (8 electrons total: 4 from bonds and 4 from lone pairs), ensuring the Lewis structure is complete and neutral.