QQuestionChemistry
QuestionChemistry
Determine whether the following molecules are polar or nonpolar using the Lewis structures.
a. Ammonia, NH₃
b. Difluoromethane, CH₂F₂
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Answer
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Step 1:I'll solve this problem step by step, focusing on molecular polarity determination.
Step 2:: Understand Molecular Polarity Criteria
Molecular polarity depends on: - Molecular geometry - Electronegativity differences between atoms - Symmetry of electron distribution
Step 3:: Analyze Ammonia (NH₃)
\text{NH}_3 \text{ is POLAR}
Lewis Structure Analysis: - Central nitrogen atom - Three hydrogen atoms bonded - One lone pair of electrons on nitrogen Molecular Geometry: Electronegativity: - Nitrogen electronegativity: 3.04 - Hydrogen electronegativity: 2.20 - Difference creates polar bonds Polarity Assessment: - Asymmetric electron distribution - Net dipole moment exists - Lone pair creates uneven charge distribution Conclusion for NH₃:
Step 4:: Analyze Difluoromethane (CH₂F₂)
\text{CH}_2\text{F}_2 \text{ is POLAR}
Lewis Structure Analysis: - Central carbon atom - Two fluorine atoms - Two hydrogen atoms Molecular Geometry: Electronegativity: - Carbon electronegativity: 2.55 - Fluorine electronegativity: 3.98 - Hydrogen electronegativity: 2.20 - Significant differences in bond electronegativities Polarity Assessment: - Asymmetric distribution of electronegative fluorine atoms - Unequal bond dipoles - Net dipole moment exists Conclusion for CH₂F₂:
Final Answer
a. NH₃: Polar molecule b. CH₂F₂: Polar molecule
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