Multiple Choice
Which of the following best describes the molecular polarity of XeF_4?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following best describes the polarity of a carbon dioxide (CO_2) molecule?
A
CO_2 is a polar molecule because it contains polar bonds.
B
CO_2 is a polar molecule because the oxygen atoms are more electronegative than carbon.
C
CO_2 is a nonpolar molecule because its linear geometry causes the dipole moments to cancel.
D
CO_2 is a nonpolar molecule because it contains only nonpolar bonds.
Verified step by step guidance1
Step 1: Identify the molecular geometry of CO_2. Carbon dioxide has a linear shape because the central carbon atom forms two double bonds with oxygen atoms, and there are no lone pairs on the carbon.
Step 2: Determine the polarity of each individual bond. The C=O bonds are polar because oxygen is more electronegative than carbon, creating a dipole moment pointing from carbon to oxygen.
Step 3: Analyze the overall molecular polarity by considering the vector sum of the bond dipoles. Since CO_2 is linear, the two bond dipoles are equal in magnitude but point in opposite directions.
Step 4: Understand that because the bond dipoles are equal and opposite, they cancel each other out, resulting in no net dipole moment for the molecule.
Step 5: Conclude that despite having polar bonds, the linear geometry of CO_2 causes the dipole moments to cancel, making the molecule nonpolar overall.
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