Indicate the kinds of intermolecular forces that would occur between the toluene and hexane:

Quick multiple choice questions. Please explain why! uploaded image This molecule indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble A) Hydrogen Bonding B) Dipole-dipole C) Disperson D) Ion-Dipole uploaded image This molecule indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble A) Dispersion only B) Dispersion, dipole-dipole, hydrogen bonding C) Hydrogen bonding only D) Dipole-dipole, ion-dipole uploaded image This molecule indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble A) Hydrogen bonding B) Dipole-dipole C) Dispersion D) Ion-dipole uploaded image This molecule indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble A) Dispersion only B) Dispersion, Dipole-dipole, Hydrogen bonding C) Hydrogen bonding only D) Dipole-dipole, ion-dipole Thanks!

Answer

General guidance

Concepts and reason
The set of repulsive and attractive forces between molecules that result from the polarity is represented as the intermolecular force. There are three types of intermolecular forces: 1)Hydrogen bonding 2)London dispersion force 3)Dipole–dipole force.

Fundamentals

Non-covalent interactions: The intermolecular interactions that exist among the molecules, which are not covalent bonding interactions, are known as non-covalent interactions. The types of intermolecular forces are given below: Vander Waals forces: These are weak forces of attractions that exist in the molecule. Dipole–dipole interactions: It occurs between two polar molecules. The interaction between the partial positive charges of one molecule to the partial positive charge of another molecule is represented as dipole–dipole interaction. Hydrogen bonding: If the hydrogen atom is directly attached to the electronegative atom, it exhibits intermolecular hydrogen bonding. Ion–ion interactions: The compounds having oppositely charged ions attract each other due to the ion–ion interactions. These are strong intermolecular force of attractions. Ion–dipole interactions: The interactions present between the ions and dipole of solvent are known as ion–dipole interactions. London dispersion force: This is a very weak intermolecular force that occurs in the non-polar molecules. The electronegativity difference is very low.

Step-by-step

Step 1 of 8

(1) -
HĆ
CH The wrong choices are A) Hydrogen bonding
B) Dipole - dipole
D) Ion - dipole

The hydrogen bonding is the strongest intermolecular force because it is the interaction between hydrogen and strong electronegative atoms. The dipole–dipole interaction occurs between two polar molecules. Therefore, the above option is incorrect.

Step 2 of 8

Correct option:- C) Dispersion

Part 1

A) Hydrogen bonding B) Dipole-dipole C) Dispersion D) Ion–dipole


In the given molecule, there is no electronegative atom and no polar atom present in the molecule. The molecule is a very weak intermolecular force that occurs in non-polar molecules. The electronegativity difference is very low. Therefore, the given option is correct.

Step 3 of 8

НО.
CH,
HOM.
й
о
H2
Н...
С
ОН
ос
НО
CH-CH
llo
НО The wrong choices, A) Dispersion only
C) Hydrogen bonding only
D) Dipole - dipole, ion - dipole

The given molecule contains electronegative atoms and forms hydrogen bonding, which is the strongest intermolecular force because it is the interaction between hydrogen and strong electronegative atoms. Also, in this molecule, dipole–dipole interaction occurs between two polar atoms. Therefore, the above option is incorrect.

Step 4 of 8

(2) Correct option:- B) Dispersion, dipole - dipole, hydrogen bonding

Part 2

A) Dispersion only B) Dispersion, dipole–dipole, hydrogen bonding C) Hydrogen bonding only D) Dipole–dipole, Ion–dipole


In the given molecule, there is a strong attractive force due to the presence of an electronegative atom. Oxygen can involve in the hydrogen bonding and form a dipole–dipole interaction. Also the molecule has dispersion. Therefore, the above option is correct.

Step 5 of 8

CH3
HỌC
CCH, The wrong choices, A) Hydrogen bonding
B) Dipole - dipole
D) Ion - dipole

The hydrogen bonding is the strongest intermolecular force because it is the interaction between hydrogen and strong electronegative atoms. The dipole–dipole interaction occurs between two polar molecules. Therefore, the above option is incorrect.

Step 6 of 8

(3) Correct option:- C) Dispersion

Part 3

A) Hydrogen bonding B) Dipole–dipole C) Dispersion D) Ion–dipole


In the given molecule, there is no electronegative atom and no polar atom present in the molecule. The molecule is a very weak intermolecular force that occurs in non-polar molecules. The electronegativity difference is very low. Therefore, the given option is correct.

Step 7 of 8

HO The wrong choices are A) Dispersion only
C) Hydrogen bonding only
D) Dipole - dipole, ion - dipole

The given molecule contains electronegative atoms and forms hydrogen bonding, which is the strongest intermolecular force because it is the interaction between hydrogen and strong electronegative atoms. Also, this molecule has a dipole–dipole interaction that occurs between two polar atoms. Therefore, the above option is incorrect.

Step 8 of 8

(4) Correct option:- B) Dispersion, Dipole - dipole, Hydrogen bonding

Part 4

A) Dispersion only B) Dispersion, dipole–dipole, hydrogen bonding C) Hydrogen bonding only D) Dipole–dipole, ion–dipole.


In the given molecule, there is a strong attractive force due to the presence of electronegative atom. Oxygen can involve in the hydrogen bonding and form a dipole–dipole interaction. Also, the molecule has dispersion. Therefore, the above option is correct.

Answer

Part 1

A) Hydrogen bonding B) Dipole-dipole C) Dispersion D) Ion–dipole

Part 2

A) Dispersion only B) Dispersion, dipole–dipole, hydrogen bonding C) Hydrogen bonding only D) Dipole–dipole, Ion–dipole

Part 3

A) Hydrogen bonding B) Dipole–dipole C) Dispersion D) Ion–dipole

Part 4

A) Dispersion only B) Dispersion, dipole–dipole, hydrogen bonding C) Hydrogen bonding only D) Dipole–dipole, ion–dipole.

Leave a Comment