The boiling point of oxygen is higher than nitrogen's boiling
The reason the boiling point of O2 is higher is not because of increased van der Waals interactions, but simple physics. The mass of a molecule of O2 is greater than that of a molecule of N2, so the molecule of O2 traveling at a speed sufficient to break out of the liquid phase has a greater kinetic energy than an analogous N2 molecule.
The net effect is that more energy must be distributed throughout a sample of O2 to achieve a given vapor pressure (in this case equal to atmospheric pressure) than for a sample of N2. More energy means greater temperature.
Answer:
Explanation:
The attachment or (Bond) that resolves around the atoms of CI2 which is a covalent bond, yet energy is needed to destroy the bond and when new bonds are produced, energy is unleashed while the bond's development makes the molecule equilibrated. In short terms to basically break this bond energy is required and another terms energy is occupied and is the conclusion to your question (I tried my best) Energy is absorbed which is the result of what occurs.
