Which term best describes why a low molecular weight compound could have an unusually high melting point, high boiling point and low vapor pressure?

Dipole-dipole attraction

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Hydrogen bonding

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Van der Waals forces

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Covalent bond

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Solution

The correct option is C Hydrogen bonding
Due to hydrogen bonding, low molecular weight compounds could have high melting point, high boiling point and low vapor pressure.Due to high intermolecular H bonding it becomes tough for a molecule to break and due to this they cannot escape easily, thereby having high melting point, high boiling point and low vapor pressure.

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Similar questions

Why do covalent compounds have low melting and boiling points ?

(a) Compound X consists of molecules.

Choose the letter corresponding to the correct answer from the options A, B, C and D given below :

(i) The type of bonding in X will be :

A. ionic B. electrovalent

C. covalent D. molecular

(ii) X is likely to have a :

A. low melting point and high boiling point,

B. high melting point and low boiling point,

C. low melting point and low boiling point,

D. high melting point and high boiling point.

(iii) In the liquid state, X will :

A. become ionic,

B. be an electrolyte

C. conduct electricity,

D. not conduct electricity.

(b) Electrons are getting added to an element Y :

(i) is Y getting oxidized or reduced ?

(ii) what charge will Y migrate to during the process of electrolysis ?

Explain the following :

(a) Electrovalent compounds conduct electricity in molten or aqueous state.

(b) Electrovalent compounds have a high melting point and boiling point while covalent compounds have low melting and boiling points.

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