QQuestionChemistry
QuestionChemistry
Draw the Lewis structure for the sulfur monoxide (SO) molecule.
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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
- Total valence electrons: $$6 + 6 = 12$$ electrons
- Sulfur (S) is in Group 16, so it has 6 valence electrons - Oxygen (O) is in Group 16, so it also has 6 valence electrons
Step 3:: Arrange atoms and create single bond
- Remaining electrons: $$12 - 2 = 10$$ electrons
- Place sulfur and oxygen atoms next to each other - Create an initial single bond between S and O
Step 4:: Distribute remaining electrons as lone pairs
- Remaining electrons: $$4$$ electrons
- Add lone pairs to oxygen first (needs 8 electrons to complete octet) - Place 3 lone pair sets (6 electrons) around oxygen - Place remaining 2 electrons as a lone pair on sulfur
Step 5:: Check formal charges
- Sulfur: $$6 - 4 - 1 = 1$$ formal charge
- Oxygen: 6 - 6 - 0 = 0 formal charge
Final Answer
The Lewis structure for SO shows a single bond between S and O, with 3 lone pairs on oxygen and 1 lone pair on sulfur. [Diagram would show S-O with 3 lone pairs on O and 1 lone pair on S]
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