A concept map for four types of intermolecular forces and a certain type of bond is shown. No

Yes

Are ions

present?

No

No

Are molecules

with permanent

dipoles present?

Are polar

molecules

present?

Yes

Yes

Yes

Is H atom

bonded to F, O, or

Natom?

No

A

С

D

E

Compare the relative strength of the two forces A and B. Explain how you determined this comparison by identifying the forces.

Answer is explained in the explanation section below.

Explanation:

Solution:

From the concept map given:

A = Londen forces or dispersion forces:

Dispersion Forces: Type of intermolecular forces between non-polar molecules having no dipole moment

For example: CO2 -- CO2 bonding

B =  Dipole - Dipole intermolecular forces: Type of intermolecular forces between molecules having permanent dipole moment.

For example: HCL --- HCL bonding.

C = Hydrogen Bonding: Type of intermolecular forces exist between H of one molecule with electronegative (F/O/N) of other molecule.

For example: H20 -- H20 bonding

D = Ion - Dipole intermolecular forces: Type of intermolecular forces exists between ions and molecules having dipoles.

For Example: NaCl

Comparison between C and D:

Ion-Dipole forces are stronger than H-bonding because the charge of any ion is greater than the partial charge of polar molecules. That is why ions bind better to polar molecules than polar - polar molecules.

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.