Question

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The boiling point of water (H2O) is 100 °C. Which of the following best predicts the boiling point of hydrogen sulfide (H2S)?
A. Higher than 100 °C because ion dipole interactions in hydrogen sulfide are stronger than hydrogen bonding in water.
B. Lower than 100 °C because hydrogen sulfide has dipole-dipole interactions instead of hydrogen bonding.
C. Lower than 100 °C because the hydrogen bonding in hydrogen sulfide is weaker than it is in water.
D. Higher than 100 °C because the size of a sulfur atom is larger than the size of an oxygen atom.

Answer 1

Answer: B) Lower than 100 °C because hydrogen sulfide has dipole-dipole interactions instead of hydrogen bonding.

Answer 2

B. Lower than 100 °C because hydrogen sulfide has dipole-dipole interactions instead of hydrogen bonding.

Step-by-step explanation:

Boiling point is a physical property which is usually a product of breaking intermolecular bonds.

Both dipole-dipole attractions are intermolecular bonds and they have serious effect on boiling point of a substance.

Hydrogen bonds are very strong intermolecular bonds compared to dipole-dipole attractions. In hydrogen bonding hydrogen atom is directly joined to a highly electronegative atom.

Dipole-Dipole attraction exists between molcules that are polar. Such molecules line up such that the positive pole of one molecule attracts the negative pole of another.

Hydrogen bonds in water are much stronger than the dipole-dipole attraction of hydrogen sulfide.