Problem: Which of the following solids has the highest melting point: Ar(s), CCl4(s), LiCl(s), CH3OH(s)?

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We are asked to determine which of the following solids has the highest melting point: Ar(s), CCl4(s), LiCl(s), CH3OH(s). 


Intermolecular forces of attraction (IMF) can be used to predict the melting point of substances. 

The stronger the IMFs, the higher the Heat of Fusion (heat required for substances to melt)


Here are the relative strengths of the IMF’s of compounds:

Ionic bonding > H bonding > dipole-dipole > London dispersion (Van der Waals) 

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Problem Details

Which of the following solids has the highest melting point: Ar(s), CCl4(s), LiCl(s), CH3OH(s)?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Intermolecular Forces and Physical Properties concept. If you need more Intermolecular Forces and Physical Properties practice, you can also practice Intermolecular Forces and Physical Properties practice problems.

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Based on our data, we think this problem is relevant for Professor Littlepage's class at NOTRE DAME.