Final answer:
Boiling point depends on intermolecular forces. Compounds with stronger intermolecular forces have higher boiling points. Arrange the compounds in each set in order of increasing boiling point temperature based on their intermolecular forces.
Step-by-step explanation:
Boiling point depends on the strength and types of intermolecular forces present in the compounds. In general, stronger intermolecular forces result in higher boiling points. Let's arrange each set of compounds in order of increasing boiling point temperature:
(a) HCl, H₂O, SiH₄: SiH₄ < HCl < H₂O. SiH₄ is a nonpolar molecule with only weak London dispersion forces. HCl is a polar molecule that exhibits dipole-dipole interactions. H₂O is a polar molecule that forms hydrogen bonds, which are stronger than dipole-dipole interactions.
(b) F₂, Cl₂, Br₂: F₂ < Cl₂ < Br₂. These compounds are all nonpolar and exhibit London dispersion forces. As the number of electrons increases, the strength of the London dispersion forces increases, resulting in higher boiling points.
(c) CH₄, C₂H₆, C₃H₈: CH₄ < C₂H₆ < C₃H₈. These compounds are all nonpolar and exhibit London dispersion forces. The boiling point increases with increasing molecular mass.
(d) O₂, NO, N₂: N₂ < O₂ < NO. These compounds are all nonpolar and exhibit London dispersion forces. However, NO also exhibits dipole-dipole interactions, which make it have a slightly higher boiling point than O₂.