When a water molecule forms a hydrogen bond with another water molecule, which atoms are involved in the interaction?

a hydrogen from one molecule and an oxygen from the other molecule

a hydrogen from one molecule and a hydrogen from the other molecule

an oxygen from one molecule and an oxygen from the other molecule

an oxygen and a hydrogen from the same molecule

two hydrogens from one molecule and one hydrogen from the other molecule

Which of the following statements are incorrect concerning drawing III?

These molecules exhibit ionic bonding.

Electrostatic interactions exist between the molecules.

The molecules find the best compromise between attraction and repulsion.

OCS exhibits this type of interaction.

Two of these statements are incorrect.

The freezing point of helium is −270°C. The freezing point of xenon is −112°C. Both of these are in the noble gas family. Which of the following statements is supported by these data?

The London dispersion forces between the helium molecules are less than the London dispersion forces between the xenon molecules.

Helium and xenon form highly polar molecules.

As the molecular weight of the noble gas increases, the freezing point decreases.

The London dispersion forces between the helium molecules are greater than the London dispersion between the xenon molecules.

Which of the following statements about liquids is true?

London dispersion forces arise from a distortion of the electron clouds within a molecule or atom.

Droplet formation occurs because of the higher stability associated with increased surface area.

Substances that can form hydrogen bonds will display lower melting points than predicted from periodic trends.

Liquid rise within a capillary tube because of the small size lowers the effective atmospheric pressure over the surface of the liquid.

The boiling point of a solution is dependent solely on the atmospheric pressure over the solution.

When a nonpolar liquid displays a convex meniscus, which of the following explains this behavior?

The cohesive forces are stronger than the adhesive forces to the glass.

It has a low surface tension, and therefore clings to the glass.

The adhesive forces to the glass are stronger than the cohesive forces.

Which of the following is paired incorrectly?

gold metal—simple cubic unit cell

crystalline solids—highly regular arrangement of their components

amorphous solids—considerable disorder in their structures

unit cell—the smallest repeating unit of the lattice

Which of the following statements about steel is false ?

It contains carbon atoms in the holes of its iron crystals.

The presence of carbon-iron bonds in the alloy make steel harder and stronger than pure iron.

Pure iron is relatively soft and ductile because it lacks directional bonding.

The amount of carbon directly affects the properties of steel.

Which of these statements is incorrect?

Molecular solids have high melting points.

The binding forces in a molecular solid include London dispersion forces.

Ionic solids have high melting points.

All of these statements are correct.

A solid crystal of NaCl is

hard, high melting, a poor electrical conductor

soft, low melting, a good electrical conductor

hard, high melting, a good electrical conductor

soft, low melting, a poor electrical conductor

soft, high melting, a poor electrical conductor

How would you expect the melting point of $$\\mathrm{CCl_4}$$ to compare to that of $$\\mathrm{NaCl}$$ ?

It should be lower because $$\\mathrm{NaCl}$$ forms an extended ionic crystal lattice, whereas $$\\mathrm{CCl_4}$$ is a covalently-bonded small molecule.

It should be similar since they are both ionic solids.

It should be higher because the bonds are stronger due to the higher charge on C $$(+4)$$ .

It should be higher because $$\\mathrm{CCl_4}$$ is larger than $$\\mathrm{NaCl}$$ .

It is not possible to say anything about their melting points without more information.

On a relative basis, the weaker the intermolecular forces in a substance,

the greater its vapor pressure at a particular temperature

the greater its heat of vaporization

the more it deviates from ideal gas behavior

You are given the following boiling point data. Which one of the liquids would you expect to have the highest vapor pressure at room temperature? water, H 2 O — 100°C methanol, CH 3 OH — 64.96°C ethanol, CH 3 CH 2 OH — 78.5°C diethyl ether, CH 3 CH 2 —O—CH 2 CH 3 — 34.5°C ethylene glycol, HO—CH 2 —CH 2 —OH — 198°C

diethyl ether, CH 3 CH 2 —O—CH 2 CH 3

ethylene glycol, HO—CH 2 —CH 2 —OH

Consider the compounds $$\\mathrm{CH_3OH}$$ , $$\\mathrm{CCl_4}$$ , and $$\\mathrm{CH_3Br}$$ . For each compound, list the strongest intermolecular force that operates within a sample of that compound.

H-bonding is the strongest intermolecular force in $$\\mathrm{CH_3OH}$$ , dispersion is the strongest intermolecular force in $$\\mathrm{CCl_4}$$ , and dipole-dipole is the strongest intermolecular force in $$\\mathrm{CH_3Br}$$ .

Dispersion is the strongest intermolecular force in $$\\mathrm{CH_3OH}$$ , dispersion is the strongest intermolecular force in $$\\mathrm{CCl_4}$$ , and dispersion is the strongest intermolecular force in $$\\mathrm{CH_3Br}$$ .

Ion-dipole is the strongest intermolecular force in $$\\mathrm{CH_3OH}$$ , Ion-dipole is the strongest intermolecular force in $$\\mathrm{CCl_4}$$ , and dipole-dipole is the strongest intermolecular force in $$\\mathrm{CH_3Br}$$ .

Dipole-induced dipole is the strongest intermolecular force in $$\\mathrm{CH_3OH}$$ , dispersion is the strongest intermolecular force in $$\\mathrm{CCl_4}$$ , and dipole-dipole is the strongest intermolecular force in $$\\mathrm{CH_3Br}$$ .

Ion-induced dipole is the strongest intermolecular force in $$\\mathrm{CH_3OH}$$ , dispersion is the strongest intermolecular force in $$\\mathrm{CCl_4}$$ , and H-bonding is the strongest intermolecular force in $$\\mathrm{CH_3Br}$$ .

Which of the following is indicative of the existence of strong intermolecular forces of attraction in a liquid?

a very low heat of vaporization

Which of the following pair of molecules could form hydrogen bonds between them?

$$\\mathrm{(CH_3)_2NH}$$ and $$\\mathrm{(CH_3)_3N}$$

$$\\mathrm{CH_3OH}$$ and $$\\mathrm{HBr}$$

$$\\mathrm{C_2H_6}$$ and $$\\mathrm{HOCH_2CH_2OH}$$

$$\\mathrm{FCH_2CH_2F}$$ and $$\\mathrm{HCl}$$

$$\\mathrm{Na^+}$$ and $$\\mathrm{H_2O}$$

Intermolecular Forces and Boiling Point Questions

Authored by Mary Januea Fleck

Chemistry

University

NGSS covered

Intermolecular Forces and Boiling Point Questions

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest.

dipole-dipole, London dispersion, ionic, and hydrogen-bonding

London dispersion, dipole-dipole, hydrogen-bonding, and ionic

hydrogen-bonding, dipole-dipole, London dispersion, and ionic

dipole-dipole, ionic, London dispersion, and hydrogen-bonding

London dispersion, ionic, dipole-dipole, and hydrogen-bonding

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Hydrogen bonds account for which of the following observation?

Hydrogen naturally exists as a diatomic molecule.

Hydrogen is easily combustible with oxygen.

Water molecules are bent or "V-shaped."

Air is more dense than hydrogen gas.

For its molar mass, water has a high boiling point.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following would you expect to have the highest boiling point?

All of these have the same boiling point.

Which of the following should have the lowest boiling point?

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the species below would you expect to show the least hydrogen bonding?

NH₃

H₂O

CH₄

all the same

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The molecules in a sample of solid SO₂ are attracted to each other by a combination of

London forces and H-bonding

H-bonding and ionic bonding

covalent bonding and dipole-dipole interactions

London forces and dipole-dipole interactions

none of these

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

In which of the following groups of substances would dispersion forces be the only significant factors in determining boiling points?
I. Cl₂ II. HF III. Ne IV. KNO₂ V. CCl₄

I, III, V

I, II, III

II, IV

II, V

III, IV, V

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Intermolecular Forces and Boiling Point Questions

Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest.

Hydrogen bonds account for which of the following observation?

Which of the following would you expect to have the highest boiling point?

Which of the following should have the lowest boiling point?

Which of the species below would you expect to show the least hydrogen bonding?

The molecules in a sample of solid SO₂ are attracted to each other by a combination of

In which of the following groups of substances would dispersion forces be the only significant factors in determining boiling points?
I. Cl₂ II. HF III. Ne IV. KNO₂ V. CCl₄

Which substance involves no bonding forces except London dispersion forces?

In general, the density of a compound as a gas is closer in value to that of the compound as a liquid than the density of the compound as a liquid is in value to that of the compound as a solid.

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Popular Resources on Wayground

Discover more resources for Chemistry

Intermolecular Forces and Boiling Point Questions

Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest.

Hydrogen bonds account for which of the following observation?

Which of the following would you expect to have the highest boiling point?

Which of the following should have the lowest boiling point?

Which of the species below would you expect to show the least hydrogen bonding?

The molecules in a sample of solid SO2 are attracted to each other by a combination of

In which of the following groups of substances would dispersion forces be the only significant factors in determining boiling points?I. Cl2 II. HF III. Ne IV. KNO2 V. CCl4

Which substance involves no bonding forces except London dispersion forces?

In general, the density of a compound as a gas is closer in value to that of the compound as a liquid than the density of the compound as a liquid is in value to that of the compound as a solid.

Access all questions and much more by creating a free account

Popular Resources on Wayground

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The molecules in a sample of solid SO₂ are attracted to each other by a combination of

In which of the following groups of substances would dispersion forces be the only significant factors in determining boiling points?
I. Cl₂ II. HF III. Ne IV. KNO₂ V. CCl₄