We’re being asked to use intermolecular forces to explain the difference in enthalpy values of the given compounds.
The intermolecular forces are responsible for holding the liquid together. The enthalpy of vaporization is, roughly, a measure of how much energy is required to break those intermolecular forces apart.
That is, the stronger the intermolecular forces, the larger the enthalpy of vaporization will be.
Recall that we have different intermolecular forces:
Intermolecular Forces (IMF) are the attractive forces between 2 molecules.
▪ strongest IMF
▪ deals with the attraction between an ion and a polar compound.
• Hydrogen Bonding
Consider the following values for enthalpy of vaporization (kJ/mol) of several organic substances.
Use intermolecular forces, including hydrogen-bonding interactions where applicable, to explain your responses.
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