Which compound below would be expected to have the highest boiling point?
a) CH3-CH2-CH2-CH2-CH2-CH2-CH3
b) CH3-CH2-CH2-CH2-CH-CH3
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CH3
c) CH3-CH-CH2-CH-CH3
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CH3 CH3
d) CH3
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CH3-CH-C-CH3
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CH3 CH3
I think its A?
I would expect that to be a.
You are correct. Compound A, CH3-CH2-CH2-CH2-CH2-CH2-CH3, would be expected to have the highest boiling point. Boiling point is influenced by the strength of intermolecular forces, such as hydrogen bonding and London dispersion forces. In this case, compound A has a longer carbon chain, leading to more London dispersion forces, which are stronger with increased surface area. This results in a higher boiling point compared to the other compounds.
To determine which compound would be expected to have the highest boiling point, we need to consider the structure and molecular size of the compounds.
In this case, compound A has a straight-chain structure with seven carbon atoms. It has a greater molecular size compared to the other compounds. Larger molecules generally have higher boiling points because they have stronger intermolecular forces, which require more energy to break and transition from a liquid to a gas state. Therefore, compound A is a likely candidate for having the highest boiling point.
On the other hand, compounds B, C, and D are branched isomers of compound A. Branching reduces the molecular size and surface area, which decreases the strength of intermolecular forces. As a result, compounds B, C, and D are expected to have lower boiling points compared to compound A.
To summarize, based on the given information and considering molecular size and structure, compound A (CH3-CH2-CH2-CH2-CH2-CH2-CH3) is likely to have the highest boiling point among the given compounds.