Multiple Choice
Which of the following statements about the polar and non-polar nature of a molecule is true?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following molecules is nonpolar?
A
H2O (water)
B
CO2 (carbon dioxide)
C
NH3 (ammonia)
D
SO2 (sulfur dioxide)
Verified step by step guidance1
Step 1: Understand that molecular polarity depends on both the polarity of individual bonds and the geometry (shape) of the molecule. A molecule is nonpolar if the bond dipoles cancel out due to symmetrical arrangement.
Step 2: Analyze the molecular geometry of each molecule using VSEPR theory: H2O is bent, NH3 is trigonal pyramidal, SO2 is bent, and CO2 is linear.
Step 3: Consider the electronegativity differences and bond dipoles: all molecules have polar bonds because of differences in electronegativity between atoms (e.g., C and O, H and O, N and H, S and O).
Step 4: Evaluate the symmetry of the molecules: CO2 is linear and symmetrical, so the two polar C=O bonds point in opposite directions and their dipoles cancel out, making CO2 nonpolar.
Step 5: Conclude that H2O, NH3, and SO2 have bent or pyramidal shapes causing an uneven distribution of charge, making them polar, while CO2 is nonpolar due to its linear and symmetrical shape.
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