Multiple Choice
In a molecule of hydrogen chloride (HCl), which atom does the electron density shift toward, indicating the direction of polarity?
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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 SF_6 (sulfur hexafluoride)?
A
SF_6 is a nonpolar molecule because its symmetrical octahedral shape causes the dipole moments to cancel.
B
SF_6 is a polar molecule due to the presence of lone pairs on the sulfur atom.
C
SF_6 is a polar molecule because the sulfur atom is more electronegative than fluorine.
D
SF_6 is a nonpolar molecule because it contains only nonpolar covalent bonds.
Verified step by step guidance1
Identify the molecular geometry of SF_6. Sulfur hexafluoride has six fluorine atoms bonded to a central sulfur atom, which results in an octahedral shape due to six bonding pairs and no lone pairs on sulfur.
Recall that molecular polarity depends on both the polarity of individual bonds and the overall shape of the molecule. Each S-F bond is polar because fluorine is more electronegative than sulfur, creating bond dipoles.
Analyze the symmetry of the molecule. In an octahedral geometry, the six bond dipoles are arranged symmetrically around the central atom, pointing in opposite directions and thus canceling each other out.
Conclude that because the bond dipoles cancel due to the symmetrical shape, the overall molecular dipole moment is zero, making SF_6 a nonpolar molecule.
Eliminate incorrect options: SF_6 does not have lone pairs on sulfur, sulfur is less electronegative than fluorine, and the bonds are polar covalent, not nonpolar covalent.
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