Final answer:
The differences in boiling points between compounds can be attributed to the strengths of intermolecular forces. Methanol (CH3OH) has higher boiling point due to stronger hydrogen bonding compared to Methanethiol (CH2SH). Xe is a liquid at lower temperature than Ar due to stronger London dispersion forces in Xe. The boiling point differences between Kr and Cl2 can be explained by the stronger dispersion forces in Cl2 compared to Kr.
Step-by-step explanation:
The differences in boiling points between CH3OH and CH2SH can be attributed to the intermolecular forces present in each compound. CH3OH, or methanol, has stronger intermolecular forces, specifically hydrogen bonding, which requires more energy to overcome, resulting in a higher boiling point. On the other hand, CH2SH, or methanethiol, has weaker intermolecular forces, such as dispersion forces, which are easier to overcome, leading to a lower boiling point.
The difference in boiling points between Xe and Ar can be explained by their different intermolecular forces. Xe is a liquid at atmospheric pressure and 120 K because it exhibits London dispersion forces, which increase with increasing molecular size. Ar, on the other hand, is a gas under the same conditions because its smaller size and weaker London dispersion forces allow it to exist in the gas phase at lower temperatures.
The higher boiling point of Kr compared to Cl2 can be attributed to the different intermolecular forces in these compounds. Kr, despite its larger atomic mass, has weaker London dispersion forces compared to Cl2, which has stronger dispersion forces due to the presence of polar covalent bonds. Therefore, Cl2 requires more energy to overcome its intermolecular forces and transition from the liquid phase to the gas phase, resulting in a higher boiling point compared to Kr.