Final answer:
When comparing the boiling points of 2-methylhexane and 2-methylheptane, we would expect 2-methylheptane to have a higher boiling point. This is because it has a larger molecular size, resulting in stronger intermolecular forces.
Step-by-step explanation:
When comparing the boiling points of two organic compounds, such as 2-methylhexane and 2-methylheptane, we need to consider the intermolecular forces present in each compound. The boiling point of a compound is affected by the strength of these forces.
In general, the strength of intermolecular forces increases with increasing molecular size, so we would expect 2-methylheptane to have a higher boiling point than 2-methylhexane. This is because 2-methylheptane has a larger molecular size, which allows for stronger London dispersion forces between its molecules compared to 2-methylhexane.
London dispersion forces are the dominant intermolecular forces in hydrocarbons and are caused by temporary fluctuations in electron distribution. These forces increase with increasing molecular size due to the larger number of electrons present in larger molecules.