QQuestionChemistry
QuestionChemistry
a. Draw the Lewis structure of acetone, (CH3)2CO (C in the middle, with two C's and an O bonded to it). What is the hybridization on each carbon atom in the molecule?
b. On the Lewis structure, identify every bond as a sigma or pi bond (σ or π).
c. For the Carbon-Hydrogen bond, what are the orbitals that overlap to make that bond?
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Draw the Lewis Structure of Acetone
* Carbon in the center * One oxygen double-bonded to the central carbon \begin{array}{c} \text{H}_{3}C - \text{C} = \text{O} \ \quad \text{H}_{3}C \end{array}
Step 3:: Hybridization of Carbon Atoms
* Hybridization is $$sp^{3}
- Central carbon: * Has three bonds (two single C-C bonds, one double C=O bond) - Methyl carbon atoms: * Have four single bonds
Step 4:: Bond Identification
- Carbon-hydrogen bonds: All $$\sigma$$ bonds
- Central carbon to methyl carbons: Single \sigma bonds
Step 5:: Carbon-Hydrogen Bond Orbital Overlap
- Methyl carbons ($$sp^{3}$$): Overlap of $$sp^{3}$$ hybrid orbital with hydrogen 1s orbital
- Creates a \sigma bond through head-on orbital overlap
Final Answer
- Central carbon hybridization: sp^{2} - Methyl carbon hybridization: sp^{3} - Bonds: Mixture of \sigma and \pi bonds - C-H bonds formed by sp^{3} hybrid orbital overlapping with hydrogen 1s orbital
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