Draw the most stable Lewis structure for H2CS and complete the following statements.

I: The total number of nonbonding pairs of electrons on the sulfur atom is
[ Select ]
0
3
1
2
.
II: The bond between the carbon and sulfur atoms is a
[ Select ]
triple bond
double bond
single bond
.

07A

Question

Draw the most stable Lewis structure for H2CS and complete the following statements.

I: The total number of nonbonding pairs of electrons on the sulfur atom is 
[ Select ]
0
3
1
2
 .
II: The bond between the carbon and sulfur atoms is a 
[ Select ]
triple bond
double bond
single bond
 .

07A

BlackTom AI · Accepted Answer

We start by identifying the key pieces of information needed for the Lewis structure of H2CS.
- Total valence electrons: H (2 × 1) + C (4) + S (6) = 12 electrons.
- The most plausible backbone is H2C=S, where carbon is bonded to two hydrogens and double-bonded to sulfur; this follows common valence patterns for carbon and sulfur in such species.

Analyzing option I (number of nonbonding electron pairs on sulfur):
- If sulfur has two lone pairs (2 × 2 = 4 electrons) in the H2C=S structure, that accounts for the typical octet fulfillment for sulfur when it forms a double bond to carbon.
- If we tried 0 lone pairs on sulfur, sulfur would have only the bonding electrons and would not satisfy the octet in the expected resonance forms, and the total electron accounting would be inconsistent with the stable Lewis structure for this molecule.
- If we tried 3 lone pairs, sulfur would hold 6 electrons as lone pairs, which would exceed its typical valence capacity in this bonding context and lead to an incorrect octet distribution.
- If we tried 1 lone pair, sulfur would have 2 electrons as a lone pair, which still would not align with the standard valence and octet considerations for a C=S double bond in this molecule.
Therefore, 2 nonbonding pairs is the correct count for sulfur in the most stable Lewis structure.

Now analyzing option II (the C–S bond order):
- In the H2C=S structure, carbon forms a double bond to sulfur to satisfy carbon’s tetravalence (two H atoms and one C–S bond to complete four bonds for carbon) and to place sulfur in a reasonable valence state with lone pairs.
- A triple bond between carbon and sulfur would overbond carbon relative to the available valence distribution and would not align with the standard valence framework for this molecule; it would also disrupt the octet on sulfur and carbon.
- A single bond would underbond carbon, leaving it short of four bonds and forcing an unusual distribution of lone pairs that does not match common stable Lewis structures for H2CS.
- Therefore, the correct bond between carbon and sulfur is a double bond, consistent with the typical formal charges and octet fulfillment in H2CS.

Putting it together, the two correct selections are: sulfur has 2 nonbonding electron pairs, and the C–S bond is a double bond. The alternative options for either choice fail because they violate octet rules, typical valence, or conventional bonding patterns for this molecule.

CHEM 1210 AU2025 (15738) Exam 4- Requires Respondus LockDown Browser

Draw the most stable Lewis structure for H2CS and complete the following statements. I: The total number of nonbonding pairs of electrons on the sulfur atom is [ Select ] 0 3 1 2 . II: The bond between the carbon and sulfur atoms is a [ Select ] triple bond double bond single bond . 07A

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