Question

Indicate the major type of intermolecular forces-(1)ionic bonds, (2) dipole-dipole attractions, (3) hydrogen bonds, (4) dispersion forces- that occur. between particles of the following.

a.${\mathrm{CHCl}}_3$${\mathrm{CHCl}}_3$

b. ${\mathrm{H}}_2\mathrm{O}$

c. $\mathrm{LiCl}$

d. ${\mathrm{OBr}}_2$${\mathrm{OBr}}_2$

e. $\mathrm{HBr}$$\mathrm{HBr}$

f.$\mathrm{IBr}$

Short answer

a. (2) dipole-dipole attractions

b. (3) hydrogen bonds

c. (1) ionic bonds

d. (2) dipole-dipole attractions

e. (2) dipole-dipole attractions

f. (4) dispersion forces

Step-by-step solution

Part (a) Given Information

To determine the intermolecular forces present in the molecule.

Part (a) Explanation

• ${\mathrm{CHCl}}_3$is a polar molecule, thus it has dipole-dipole interactions.
• It also has dispersion forces.

• The intermolecular forces present in this molecule are dipole-dipole interactions due to the result of dipoles in a molecule (a result of attraction between a positive and a negative end).

Part (b) Given Information

To determine the intermolecular forces present in the molecule.

Part (b) Explanation

• Water has strong hydrogen bonding as it is composed of hydrogen and oxygen atoms.
• The electronegativity difference between these two atoms results in a polar nature of this compound.

Part (c) Given information

To determine the intermolecular forces present in the molecule.

Part (c) Explanation

• Lithium chloride is an ionic compound, it is composed of lithium and chloride ions.
• The ions are strongly held together by ionic forces or bonds i.e., the type of bond formed between two oppositely charged species.

Part (d) Given Information

To determine the intermolecular forces present in the molecule.

Part (d) Explanation

• The intermolecular forces present in ${\mathrm{OBr}}_2$are Dipole-dipole attractions.
• Oxygen dibromide is a polar molecule, that results in a dipole moment due to which the molecule has dipole-dipole interactions.

Part (e) Given Information

To determine the intermolecular forces present in the molecule.

Part (e) Explanation

• Hydrogen bromide is a polar molecule.
• This molecule exhibits dipole-dipole interactions, due to the large electronegativity difference between hydrogen and bromine atoms.

Part (f) Given information

To determine the intermolecular forces present in the molecule.

Part (f) Explanation

• In the iodine bromide molecule, there are weak London dispersion forces.
• The dipole moment between the iodine and bromine atom is very weak in$\mathrm{IBr}$ molecule.