QQuestionChemistry
QuestionChemistry
Draw the Lewis structure (including resonance structures) for the acetate ion ($CH_3 COO^−$). For each resonance structure, use square brackets to denote the overall charge. Include all hydrogen atoms and nonbonding electrons.
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Step 1:I'll solve this step by step, following the LaTeX formatting guidelines precisely:
Step 2:: Identify the atoms and valence electrons
- Total charge: $$-1$$ (acetate ion)
- Carbon atoms: 2 carbons (1 in methyl group, 1 in carboxylate group) - Oxygen atoms: 2 oxygen atoms - Hydrogen atoms: 3 hydrogen atoms in methyl group
Step 3:: Calculate total valence electrons
- Total valence electrons: $$4 + 4 + 12 + 3 + 1 = 24$$ electrons
- Carbon (carboxyl): 4 electrons
Step 4:: Initial bonding structure
- Connect carbons with single bond - Attach hydrogens to methyl carbon - Place oxygens around carboxyl carbon - Distribute remaining electrons as lone pairs
Step 5:: First resonance structure
\begin{bmatrix}
H-C-H \ \mid \ C=O \ \mid \ O^{-} \end{bmatrix}^{-}
Step 6:: Second resonance structure
\begin{bmatrix}
H-C-H \ \mid \ C-O \ \mid \ O^{-} \end{bmatrix}^{-}
Final Answer
Key Observations: - Both oxygen atoms share the - 1 charge - The carbon-oxygen bonds are equivalent in length - Resonance structures show electron delocalization
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