QQuestionChemistry
QuestionChemistry
Draw the Lewis structure of SF^2 , showing all lone pairs.
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Answer
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Step 1:I'll solve this Lewis structure problem step by step, following the specified formatting guidelines:
Step 2:: Determine the total number of valence electrons
- Total valence electrons: $$6 + (2 \times 7) = 20$$ electrons
- Sulfur (S) is in Group 16, so it has 6 valence electrons - Fluorine (F) is in Group 17, so each F has 7 valence electrons
Step 3:: Arrange atoms and create skeletal structure
\begin{array}{c}
- Sulfur will be the central atom - Place two fluorine atoms around the sulfur F-S-F \end{array}
Step 4:: Distribute electrons to create bonds
- Remaining electrons: $$20 - 4 = 16$$ electrons
- Create single bonds between S and each F - Each single bond uses 2 electrons F-S-F \end{array} - Bonds used: 4 electrons
Step 5:: Add lone pairs
\begin{array}{c}
- Distribute remaining 16 electrons as lone pairs - Place 3 lone pairs on each fluorine - Place 2 lone pairs on sulfur :F-S-F: \quad \quad \ddot{:}\ddot{:} \quad \ddot{:}\ddot{:} \end{array}
Final Answer
\begin{array}{c} :F-S-F: \quad \quad \ddot{:}\ddot{:} \quad \ddot{:}\ddot{:} \end{array}
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