QQuestionChemistry
QuestionChemistry
"What is the electron geometry and molecular shape of carbon tetrabromide (CBr4) without making a model? Do you expect the bonds in this molecule to be polar?"
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Answer
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Step 1:Let's solve this step by step:
Step 2:: Determine the central atom and valence electrons
- Total valence electrons: $$4 + (4 \times 7) = 32$$ electrons
- The central atom is carbon (C) - Carbon has 4 valence electrons - Each bromine (Br) contributes 7 valence electrons
Step 3:: Draw the Lewis structure
- Carbon will form 4 single bonds with bromine atoms - Each Br atom will complete its octet - All 32 valence electrons will be used in bonding
Step 4:: Determine electron domain geometry
- $$\text{Electron geometry} = \text{Tetrahedral}
- Carbon has 4 single bonds - Using VSEPR theory, this means 4 electron domains around the central carbon - The electron geometry is tetrahedral
Step 5:: Determine molecular shape
- $$\text{Molecular shape} = \text{Tetrahedral}
- All 4 electron domains are bonding domains - No lone pairs on the central carbon
Step 6:: Analyze bond polarity
- $$\text{Net molecular polarity} = \text{Nonpolar}
- C-Br bonds are polar due to electronegativity difference - However, the tetrahedral symmetry means these polar bonds cancel out
Final Answer
- Electron geometry: Tetrahedral - Molecular shape: Tetrahedral - Molecular polarity: Nonpolar (despite polar C-Br bonds)
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