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
- Ccheck_circle
Hydrogen bonding between F-H, O-H, or N-H groups
- D
Ionic bonding
Explanation
H atoms bonded directly to highly electronegative F, O, or N produce strong hydrogen bonds, lifting boiling points well above the dispersion-only trend.