How do you know which compound has a higher boiling point?

In general, larger molecules have higher boiling points than smaller molecules of the same kind, indicating that dispersion forces increase with mass, number of electrons, number of atoms or some combination thereof.

How do you compare the boiling points of compounds?

Intermolecular forces (IMFs) can be used to predict relative boiling points. The stronger the IMFs, the lower the vapor pressure of the substance and the higher the boiling point. Therefore, we can compare the relative strengths of the IMFs of the compounds to predict their relative boiling points.

Which of the following compounds should have the lowest boiling point?

Cal2 has the maximum covalent character and the least boiling point.

How can you tell which compound has stronger intermolecular forces?

If the molecules have similar molar masses and similar types of intermolecular forces, look for the one that is the most polar or that has the most electronegative atoms or the most hydrogen bonding groups. That one will have the strongest IMF’s overall.

Which of the following molecules would boil at the lowest temperature?

Liquid helium has the lowest boiling point of all — about -452 degrees Fahrenheit, only 4.2 degrees Celsius above absolute zero.

Which among the three substances has the lowest melting point?

The chemical element with the lowest melting point is Helium and the element with the highest melting point is Carbon.

Which of the following compound has the lowest melting point?

This means that calcium iodide ($Ca{I_2}$) has the lowest melting point.

Which of the following compounds has the lowest boiling point image?

Dipropyl ether (letter b) has the lowest boiling point.

Which of the following has weakest intermolecular forces?

Hint: London dispersion force is the weakest intermolecular force.

What are the strongest to weakest intermolecular forces?

In order from strongest to weakest, the intermolecular forces given in the answer choices are: ion-dipole, hydrogen bonding, dipole-dipole, and Van der Waals forces. Ionic bonding is stronger than any of the given intermolecular forces, but is itself NOT an intermolecular force.