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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.

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

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.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.