Identify the Lewis structure of hydrogen sulfide. Select the correct answer below: HI: $ HIS H-S -H none of the above
The Correct Answer and Explanation is:
The correct Lewis structure for hydrogen sulfide is:
H–S–H
This structure represents a molecule with a central sulfur atom single-bonded to two hydrogen atoms and carrying two lone pairs of electrons. To explain this, let’s walk through the logic and electron accounting step by step.
Hydrogen sulfide has the molecular formula H₂S. Hydrogen (H) has one valence electron, and sulfur (S), found in Group 16 of the periodic table, has six valence electrons. Therefore, the total number of valence electrons in the molecule is:
2 hydrogen atoms × 1 electron = 2 1 sulfur atom × 6 electrons = 6 Total = 8 valence electrons
In Lewis structures, each single bond represents two electrons. Sulfur will form two single bonds, each connecting it to one hydrogen atom, which uses up four electrons in total.
That leaves four remaining valence electrons. These are placed as two lone pairs on the sulfur atom. As a result, sulfur ends up surrounded by eight electrons (two from each hydrogen bond and four from its lone pairs), which satisfies the octet rule. Each hydrogen atom, by sharing a pair of electrons in a bond with sulfur, achieves a full valence shell with two electrons.
The molecular geometry is bent, not linear, because the two lone pairs on sulfur repel the bonded pairs. This leads to a bond angle of about 92 degrees, which is narrower than the ideal tetrahedral angle due to lone pair repulsion.
Among the provided options, only H–S–H is a valid Lewis structure for hydrogen sulfide. The other options include incorrect notations or impossible charges for a neutral molecule like H₂S. Thus, H–S–H is the correct answer.
