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

Explanation:

Intermolecular bonds exists between seperate molecules or units. Their relative strength determines many physical properties of substances like state of matter, solubility of water, boiling point, volatility, viscosity etc. Examples are Van der waals forces, hydrogen bonds and crystal lattice forces.

In hydrogen sulfide, the intermolecular bond is a dipole-dipole attraction which is a type of van der waals attraction. It occurs as an attraction between polar molecules. These molecules line such that the positive pole of one molecule attracts the negative pole of another.

In water, the intermolecular bond is hydrogen bonds in which an electrostatic attraction exists between the hydrogen atom of one molecule and the electronegative atom of a neighbouring molecule.

Based on their relative strength:

  Van der Waals forces < Hydrogen bonding forces < crystal lattice

This makes water boil at a higher temperature than hydrogen sulfide.