Answer
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Step 1:I'll solve this Lewis structure problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine the total number of valence electrons
- Total valence electrons: $$4 + (1 \times 2) + (7 \times 2) = 4 + 2 + 14 = 20$$ electrons
- Carbon (C): 4 valence electrons - Hydrogen (H): 1 valence electron × 2 - Chlorine (Cl): 7 valence electrons × 2
Step 3:: Arrange atoms in the molecule
- Place carbon at the center - Arrange hydrogen and chlorine atoms around the carbon
Step 4:: Connect atoms with single bonds
- This uses $$4 \times 2 = 8$$ electrons
- Draw single bonds between carbon and each surrounding atom
Step 5:: Add remaining electrons as lone pairs
- Remaining electrons: $$20 - 8 = 12$$ electrons
- Distribute these as lone pairs on chlorine atoms - Each chlorine atom will have 3 lone pairs
Step 6:: Check octet rule
- Carbon has 4 bonds (full octet) - Each chlorine has 3 lone pairs and 1 single bond (full octet) - Hydrogens have their standard single bond
Final Answer
The best Lewis structure for \mathrm{CH_{2}Cl_{2}} has single bonds between carbon and each surrounding atom, with 3 lone pairs on each chlorine atom.
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