Multiple Choice
Which of the following best describes the polarity of the molecule CH_4 (methane)?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following best describes the molecular polarity of CH2F2 (difluoromethane)?
A
CH2F2 is a nonpolar molecule because its dipoles cancel out.
B
CH2F2 is a polar molecule because it has a net dipole moment.
C
CH2F2 is nonpolar due to its linear geometry.
D
CH2F2 is polar only in the solid state.
Verified step by step guidance1
Step 1: Identify the molecular geometry of CH2F2. The central atom is carbon, bonded to two hydrogen atoms and two fluorine atoms. Since carbon forms four single bonds, the geometry is tetrahedral.
Step 2: Consider the electronegativities of the atoms involved. Fluorine is highly electronegative compared to hydrogen and carbon, so the C-F bonds are polar with dipole moments pointing toward the fluorine atoms.
Step 3: Analyze the symmetry of the molecule. In CH2F2, the two fluorine atoms are not opposite each other, so their dipole moments do not cancel out completely.
Step 4: Determine the net dipole moment by vector addition of individual bond dipoles. Because the dipoles from C-F bonds are stronger and not symmetrically opposed, the molecule has a net dipole moment.
Step 5: Conclude that CH2F2 is a polar molecule due to its tetrahedral shape and the presence of polar C-F bonds that do not cancel out, resulting in an overall molecular polarity.
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