The trend in halogen boiling points is best explained by:

Answer: Increasing London dispersion forces with size/polarizability All halogens are nonpolar diatomics; only LDF acts. Larger electron clouds (greater polarizability) yield stronger LDF and higher boiling points.

According to the chart, which interaction is generally weakest?

Answer: London dispersion forces London dispersion forces, arising from instantaneous induced dipoles, are typically the weakest among the listed IMFs (though they can be large in big molecules).

The dashed line in the diagram represents:

Answer: A hydrogen bond between H of one water and O lone pair of another The dashed line connects an H attached to O of one molecule with the O of a neighboring water, depicting the directional dipole-dipole interaction known as a hydrogen bond.

AP Chemistry · Topic 3.1

Intermolecular Forces Practice

Part of Properties of Substances and Mixtures.(SAP-5.A)

Practice questions

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Sample questions

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Sample 1difficulty 1/5
$Boiling points of F2, Cl2, Br2, and I2 are plotted against molar mass; the trend is increasing BP with increasing mass.$
$The trend in halogen boiling points is best explained by:$
- A
  $Increasing London dispersion forces with size/polarizability$
  check_circle
- B
  $Hydrogen bonding$
- C
  $Increasing dipole moments$
- D
  $Ionic bonding$
Why
$All halogens are nonpolar diatomics; only LDF acts. Larger electron clouds (greater polarizability) yield stronger LDF and higher boiling points.$
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Sample 2difficulty 1/5
$According to the chart, which interaction is generally weakest?$
- A
  $Hydrogen bonding$
- B
  $London dispersion forces$
  check_circle
- C
  $Dipole-dipole$
- D
  $Ion-dipole$
Why
$London dispersion forces, arising from instantaneous induced dipoles, are typically the weakest among the listed IMFs (though they can be large in big molecules).$
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Sample 3difficulty 1/5
$Two water molecules are drawn with a dashed line connecting an H of one molecule to the O of the other.$
$The dashed line in the diagram represents:$
- A
  $A London dispersion force only$
- B
  $A covalent O-H bond$
- C
  $A hydrogen bond between H of one water and O lone pair of another$
  check_circle
- D
  $An ionic bond$
Why
$The dashed line connects an H attached to O of one molecule with the O of a neighboring water, depicting the directional dipole-dipole interaction known as a hydrogen bond.$
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Sample 4difficulty 2/5
$The plot shows boiling points of group-14, 15, 16, and 17 hydrides versus molar mass; H2O, HF, and NH3 sit far above the trend line.$
$Why do H2O, HF, and NH3 have anomalously high boiling points?$
- A
  $Stronger London dispersion than CH4$
- B
  $Greater molar mass than the trend$
- C
  $Hydrogen bonding between F-H, O-H, or N-H groups$
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- D
  $Ionic bonding$
Why
$H atoms bonded directly to highly electronegative F, O, or N produce strong hydrogen bonds, lifting boiling points well above the dispersion-only trend.$
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Sample 5difficulty 2/5
$The aligned arrangement of HCl molecules represents:$
- A
  $Dipole-dipole attraction$
  check_circle
- B
  $Metallic bonding$
- C
  $Ionic bonding$
- D
  $Hydrogen bonding$
Why
$HCl is polar but H is bonded to Cl (not N, O, or F), so the alignment of partial charges represents dipole-dipole attractions, not H-bonding.$
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