Why do covalent compounds have low melting and boiling points?

Weak VanderWaals force of attraction between molecules.

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Strong VanderWaals force of attraction between molecules.

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Large amount of energy required to break the force of attraction.

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None of the above

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Solution

The correct option is A
Weak VanderWaals force of attraction between molecules.

The molecules of covalent compounds are held by weak intramolecular forces. Thus, a very small amount of energy is required to break the bonds between two or more molecules. That is why they have low melting and boiling points.

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Similar questions

Q. Covalent compounds are usually liquids or gases due to the weak force of attraction between their molecules.

Q. Assertion :Ionic compounds have high melting points. Reason: Ionic compounds have strong electrostatic forces of attraction between the ions. Therefore, it requires a lot of energy to overcome these forces.

Which of the following statements are usually correct for carbon compounds?

These :

(a) are good conductors of electricity.

(b) are poor conductors of electricity.

(d) do not have strong forces of attraction between their molecules.

Statement 1: Ionic compounds have high boiling points.
Statement 2: The oppositely charged ions are held together by strong electrostatic forces of attraction and require more heat energy to break the bonds.

State True or False.

The boiling point is directly proportional to the van der Waals' forces between the atoms/molecules. More is the force of attraction, higher is the temperature required to overcome these binding force and higher will be the boiling point.

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