Question

Consider 1-propanol, ethyl methyl ether, butane, 2-methylpropane, and 2-methyl-1-propene. The compound with the highest boiling point is 1-propanol because:

a) 1-propanol can only be combusted
b) 1-propanol is an inhibitor
c) 1-propanol is a lock but cannot act as a key
d) 1-propanol has the greatest mass
e) 1-propanol exhibits hydrogen bonding

Answer 1

1-propanol has the highest boiling point among the given compounds because it exhibits hydrogen bonding, which are stronger intermolecular forces compared to the London dispersion forces present in the other compounds.

Step-by-step explanation:

The compound with the highest boiling point among 1-propanol, ethyl methyl ether, butane, 2-methylpropane, and 2-methyl-1-propene is 1-propanol because it exhibits hydrogen bonding. Hydrogen bonds are strong intermolecular forces that occur between a hydrogen atom covalently bonded to a highly electronegative atom, such as oxygen, and another electronegative atom with a lone pair of electrons. This type of bonding is much stronger than the London dispersion forces that the other compounds rely upon for their intermolecular attractions.

For instance, even though some compounds may have similar molar masses, their boiling points can differ significantly due to the presence or absence of hydrogen bonding. Compounds like butane and 2-methylpropane are nonpolar and only exhibit London dispersion forces, which are weaker compared to hydrogen bonds. Hence, 1-propanol has the highest boiling point because its ability to form hydrogen bonds results in the strongest intermolecular forces among the given compounds.