Multiple Choice
Is a phosphate group polar or nonpolar?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following Lewis structures represents a molecule that is polar?
A
N2: N≡N
B
HCl: H—Cl
C
O2: O=O
D
CO2: O=C=O
Verified step by step guidance1
Step 1: Understand that molecular polarity depends on the presence of polar bonds and the overall molecular geometry. A molecule is polar if it has a net dipole moment, meaning the dipoles from individual bonds do not cancel out.
Step 2: Analyze each molecule's Lewis structure and determine if the bonds are polar. Bonds between atoms with different electronegativities are polar; bonds between identical atoms are nonpolar.
Step 3: For N2 (N≡N) and O2 (O=O), both consist of two identical atoms, so the bonds are nonpolar, and the molecules are nonpolar overall.
Step 4: For CO2 (O=C=O), although the C=O bonds are polar, the molecule is linear and symmetrical, so the bond dipoles cancel out, making CO2 nonpolar.
Step 5: For HCl (H—Cl), the bond is between hydrogen and chlorine, which have different electronegativities, creating a polar bond. Since it is a diatomic molecule, the molecule is polar overall.
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