Intermolecular forces

Intermolecular forces

9th - 12th Grade

12 Qs

quiz-placeholder

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Assessment

Quiz

Chemistry

9th - 12th Grade

Hard

Created by

Penny Mullan

Used 2+ times

FREE Resource

12 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following statements is true?

Vapour pressure increases with temperature.

Hydrogen bonds are interatomic bonds.

Intermolecular forces hold the atoms in a molecule together.

Dispersion forces are generally stronger than dipole forces.

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which one of the following factors is NOT a consequence of hydrogen bonding between water molecules?

Water has its greatest density at 4oC rather than at 0oC

Water expands on freezing

Water has a relatively high boiling point

An oxygen atom is bonded to two hydrogen atoms in the water molecule.

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

At normal room temperature ammonia gas will liquefy when under pressure whereas nitrogen gas will not. The type of intermolecular forces found in ammonia and nitrogen respectively are:

Polar covalent and pure covalent forces.

Dipole-dipole and temporary dipole forces.

Hydrogen bonds and London forces.

Hydrogen bonds and dipole-dipole forces

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which one of the following best describes the attractive forces between iodine molecules in the solid phase?

Ionic bonding forces

Covalent bonding forces

Ion-dipole forces

London dispersion forces

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

When noble gases liquefy the forces between the particles can best be classified as:

London forces

Dipole-dipole forces

Hydrogen bonds

Molecular forces

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The intermolecular forces in a crystal of ice are:

London forces

Hydrogen bonds

Covalent bonds

Polar covalent bonds

7.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Dry ice (solid carbon dioxide) sublimes on heating because the forces are:

Pure covalent bonds

Polar covalent bonds

Forces between temporary dipoles

Dipole-dipole forces

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