QQuestionChemistry
QuestionChemistry
"Write a Lewis structure that obeys the octet rule for SOCl^2 (S is the central atom) and assign formal charges to each atom.
Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons and formal charges."
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Answer
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Step 1:I'll solve this Lewis structure problem step by step:
Step 2:: Determine the total number of valence electrons
6 + 6 + (7 \times 2) = 26 \text{ valence electrons}
- Sulfur (S): 6 valence electrons - Oxygen (O): 6 valence electrons - Chlorine (Cl): 7 valence electrons × 2
Step 3:: Place the central sulfur atom and arrange the other atoms
- S will be the central atom - Arrange O and two Cl atoms around the sulfur
Step 4:: Connect atoms with single bonds
\text{Total electrons used in single bonds: } 4 \times 2 = 8 \text{ electrons}
- Draw single bonds from S to O and each Cl
Step 5:: Distribute remaining electrons as lone pairs
- Remaining electrons: $$26 - 8 = 18 \text{ electrons}
- Place lone pairs on terminal atoms first * Each Cl gets 3 lone pairs * O gets 2 lone pairs - Remaining electrons go on central S atom
Step 6:: Calculate formal charges
- Cl atoms: $$7 - 6 - (2 \div 2) = 0
- Formal charge = (Valence electrons) - (Lone pair electrons) - (Bonding electrons ÷ 2)
Final Answer
The Lewis structure shows: - S as the central atom with a + 2 formal charge - O single-bonded to S with no formal charge - Two Cl atoms single-bonded to S, each with no formal charge - Complete octet for O and Cl atoms - Lone pairs distributed as described in Step 4 Note: While this structure follows the octet rule, the + 2 formal charge on sulfur suggests potential resonance structures or alternative bonding configurations might exist.
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