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Of the following substances, only _____ has London dispersion forces as its only intermolecular force.

A) CH3OH B) NH3 C) H2S D) CH4 E) HCl

Explain the reasoning. (PLEASE EXPLAIN!!!!!!)

Respuesta :

Answer:

A

Explanation:

a) C6H14, C8H18 – London-dispersion force

Since both substances have the same intermolecular force, the substances with the

larger molecular mass with have the higher boiling point. In this case, C8H18 will

have the higher boiling point.

b) C3H8 – London-dispersion force

CH3OCH3 –Dipole-dipole

The higher boiling point belongs to CH3OCH3 because is has the stronger

intermolecular force, dipole-dipole interaction.

c) CH3OH – Hydrogen bonding

CH3SH – Dipole-dipole interaction

Hydrogen bonding is the strongest intermolecular force, so CH3OH will have the

higher boiling point.

d) NH2NH2 – Hydrogen bonding

CH3CH3 – London-dispersion force

Hydrogen bonding is the strongest intermolecular force, so NH2NH2 will have the

higher boiling point.

The only intermolecular interaction present in the methane molecule is London dispersion forces.

The following points can be considered:

  • The electronegativity of the carbon and hydrogen is closer in values. Therefore the carbon to hydrogen bond in the methane molecule is not polar.
  • The only intermolecular interaction present in the molecule is a weak London dispersion force.
  • Methanol is having dipole-dipole interactions, hydrogen bonding interactions.
  • Ammonia is a polar molecule and hence there are dipole-dipole interactions.
  • Hydrogen sulphide possesses a change in the electronegativity of sulphur and hydrogen. So the molecule is polar in nature.
  • The HCl molecule is polar in nature, possess dipole-dipole interactions.

Therefore, the correct answer is D)CH4 that is methane.

Learn more about Methane:

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