refer to intermolecular forces and energy and give reason why H20 and HF deviate from the trend in boiling point observed for the others?

Update:

what conclusion can you draw from looking at the trend? (excluding H2o and HF)

give an explantation for this trend

2 Answers

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  • 3 years ago

    The H-O and H-F bonds are exceptionally polar because of the very high electronegativity values of O and F. Therefore, the dipole-dipole attraction between these molecules is much stronger than other dipole-dipole attractions, and is given a different name--Hydrogen bonding. So, H2O and HF deviate from the trend in boiling points because of this strong hydrogen bonding between their molecules.

    Among the other compounds, the boiling points increase with increasing molar masses. While these other molecules may be somewhat polar and exhibit some dipole-dipole interactions, the boiling point trends are mainly affected by size. This is the result of increasing dispersion forces between the molecules.

  • DrBob1
    Lv 7
    3 years ago

    Trend: Higher molecular weight - higher boiling point. Deviation: Hydrogen bonding overrules all the other forces.

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