The false one from the following statements has to be identified – (a) Dipole-dipole interactions between molecules are greatest if the molecules possess only temporary dipole moments. (b) All compounds containing hydrogen atoms can participate in hydrogen-bond formation. (c) Dispersion forces exist between all atoms, molecules, and ions. Concept Introduction: Intermolecular forces are the force of attraction between the molecules in a compound. The physical state of a substance depends on the strength of the intermolecular forces present in the molecules of that substance. Very strong intermolecular forces bind the molecules together tightly and form “solids”. The molecules are held together strongly in solids that they hardly move from their respective position. Liquid molecules have relatively low strength of intermolecular forces between them. Thus they move freely and because of this liquids do “flow”. Gaseous substances have weakest intermolecular forces between them. Usually intermolecular forces are considered negligible in case of gaseous compounds. Gaseous molecules exhibit very rapid and random movement. The classification of intermolecular forces can be summarized as follows – There are three types of intermolecular forces - London dispersion forces, dipole-dipole forces and hydrogen bonding. These forces are collectively known as Van der Waals forces . London dispersion forces exist in non-polar covalent compounds consists of temporary or instant dipoles and almost all type of compounds. Dipole-dipole forces present in polar covalent compounds consists of permanent dipoles. Hydrogen bonding is formed in polar covalent compounds containing direct bond between Hydrogen and other high electronegativity like Fluorine, Oxygen or Nitrogen . It is relatively the strongest one.

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Chapter 12, Problem 12.91QP

Interpretation Introduction

Interpretation:

The false one from the following statements has to be identified –

(a) Dipole-dipole interactions between molecules are greatest if the molecules possess only temporary dipole moments.

(b) All compounds containing hydrogen atoms can participate in hydrogen-bond formation.

(c) Dispersion forces exist between all atoms, molecules, and ions.

Concept Introduction:

Intermolecular forces are the force of attraction between the molecules in a compound.

The physical state of a substance depends on the strength of the intermolecular forces present in the molecules of that substance.

Very strong intermolecular forces bind the molecules together tightly and form “solids”. The molecules are held together strongly in solids that they hardly move from their respective position.

Liquid molecules have relatively low strength of intermolecular forces between them. Thus they move freely and because of this liquids do “flow”.

Gaseous substances have weakest intermolecular forces between them. Usually intermolecular forces are considered negligible in case of gaseous compounds. Gaseous molecules exhibit very rapid and random movement.

The classification of intermolecular forces can be summarized as follows –

There are three types of intermolecular forces - London dispersion forces, dipole-dipole forces and hydrogen bonding. These forces are collectively known as Van der Waals forces.

London dispersion forces exist in non-polar covalent compounds consists of temporary or instant dipoles and almost all type of compounds.

Dipole-dipole forces present in polar covalent compounds consists of permanent dipoles.

Hydrogen bonding is formed in polar covalent compounds containing direct bond between Hydrogen and other high electronegativity like Fluorine, Oxygen or Nitrogen. It is relatively the strongest one.

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