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13. Liquids, Solids & Intermolecular Forces

Intermolecular Forces

13. Liquids, Solids & Intermolecular Forces

Intermolecular Forces

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Intermolecular Forces Concept 1

Intermolecular Forces Concept 2

Intermolecular Forces Example 2

Intermolecular Forces Example 1

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Multiple Choice

The dominant forces between molecules (intermolecular forces) are ____ in origin.

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Multiple Choice

Intermolecular forces are:

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Multiple Choice

Which of the following intermolecular forces are found in ALL molecules?

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Multiple Choice

Which of these molecules exhibit the highest number of different intermolecular forces?

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Multiple Choice

It is common to add Epson salts to bath water when one has been over exercising and has sore muscles. What is the primary intermolecular force that exists between magnesium sulfate, the primary in Epson salts, and the water in the bathtub?

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Multiple Choice

Which species is expected to have the largest dispersion forces?

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Textbook Question

Ethanol 1CH CH OH 2 dissolves in hexane 1C H 2. Give the strongest type of intermolecular force between two sol- ute molecules, between two solvent molecules, and between a solute and solvent molecule. (LO 13.1) (a)

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Textbook Question

(a) Which kind of intermolecular attractive force is shown in each case here? (b) Predict which of the four interactions is the weakest. [Section 11.2] (i)

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Textbook Question

List the three states of matter in order of (b) increasing intermolecular attrac- tion.

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Textbook Question

List the three states of matter in order of (a) increasing molecular disorder

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Textbook Question

(a) How does the average kinetic energy of molecules com- pare with the average energy of attraction between mole- cules in solids, liquids, and gases?

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Textbook Question

What types of intermolecular forces exist in a sample of acetone? (LO 8.8)

(a) Dispersion forces (b) Dispersion forces and dipole–dipole forces (c) Dipole–dipole forces (d) Dispersion forces, dipole–dipole forces, and hydrogen bonding

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Textbook Question

At room temperature, Si is a solid,CCl4 is a liquid, and Ar is a gas. List these substances in order of (a) increasing intermo- lecular energy of attraction and

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Textbook Question

The DNA base thymine dissolves in water due to hydrogen bonding. Which of the following hydrogen bonds drawn between thymine and surrounding water molecules are valid? (LO 8.10) (a) I and II (b) I, II, IV (c) I, II, III (d) III and IV

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Textbook Question

(c) Which type of intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom?

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Textbook Question

(b) Which type of intermolecular attractive force operates only between polar molecules?

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Textbook Question

(a) Which type of intermolecular attractive force operates between all molecules?

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Textbook Question

(b) Which of these kinds of interactions are broken when a liquid is converted to a gas?

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Textbook Question

Would you expect that an anion would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?

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Textbook Question

Describe the intermolecular forces that must be overcome to convert these substances from a liquid to a gas: (b) CH3COOH,

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Textbook Question

Which type of intermolecular force accounts for each of these differences? (b) Xe is a liquid at atmospheric pressure and 120 K, whereas Ar is a gas under the same conditions.

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Textbook Question

True or false: (b) For the noble gases the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table.

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Textbook Question

True or false: (e) The larger the atom, the more polarizable it is.

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Textbook Question

Which member in each pair has the greater dispersion forces?(c) SiH4 or GeH4.

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Textbook Question

Which member in each pair has the greater dispersion forces? (a) H2O or H2S,

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Textbook Question

Which member in each pair has the stronger intermolecular dispersion forces? (c) CH3CH2CH2Cl or (CH3)2CHCl

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Textbook Question

(b) Which of the following molecules can form hydrogen bonds with other molecules of the same kind: CH3F, CH3NH2, CH3OH, CH3Br?

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Textbook Question

A number of salts containing the tetrahedral polyatomic anion, BF4-, are ionic liquids, whereas salts containing the somewhat larger tetrahedral ion SO42 - do not form ionic liquids. Explain this observation.

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Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. d. HF

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Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. a. Kr

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Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. b. NCl3

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Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. d. He

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Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. d. I2

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Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. c. CH3OH

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Textbook Question

The critical temperatures and pressures of a series of haloge- nated methanes are as follows:

(a) List the intermolecular forces that occur for each compound.

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Textbook Question

When ethyl alcohol, CH3CH2OH, dissolves in water, how many hydrogen bonds are formed between one ethyl alcohol molecule and surrounding water molecules? Sketch the hydro- gen bonding interactions. (Hint: Add lone pairs of electrons to the structure before drawing hydrogen bonds.)

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Textbook Question

Intermolecular forces are important in creating ordered arrangements in liquid crystals. What types of intermolecu- lar forces exist in a sample of the following compound?

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Textbook Question

Two isomers of the planar compound 1,2-dichloroethylene are shown here.

(a) Which of the two isomers will have the stronger dipole– dipole forces?

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Textbook Question

The table below shows the normal boiling points of benzene and benzene derivatives.

(a) How many of these compounds exhibit dispersion in- teractions?

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Textbook Question

What is the difference between London dispersion forces and dipole–dipole forces?

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Textbook Question

Which substance in each of the following pairs would you expect to have larger dispersion forces? (b) HCl or HI

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Textbook Question

Of the substances Xe, CH3Cl, and HF, which has: (a) The smallest dipole–dipole forces?

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Textbook Question

1,3-Propanediol can form intramolecular as well as intermolecular hydrogen bonds. Draw a structure of 1,3-propanediol showing an intramolecular hydrogen bond.

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Textbook Question

Dimethyl ether has the following structure.

(b) Which of the following illustrations depicts the hydrogen bonding that occurs between dimethyl ether and water? (i)

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Textbook Question

Propanol (PrOH) and methyl methacrylate (MMA) asso-ciate in solution by an intermolecular force, forming an adduct represented as PrOH•MMA. The equilibrium con- stant for the association reaction is Kc = 0.701 at 298 K. (b) Draw a plausible structure for the PrOH • MMA adduct. Use to signify an intermolecular interaction.

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Identify which of the following molecules can exhibit hydrogen bonding as a pure liquid.

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Which substances exhibit only london (dispersion) forces?

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Classify each substance based on the intermolecular forces present in that substance.

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In the molecule below, how many atoms could make hydrogen bonds with water?

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Which of the substances have polar interactions (dipole–dipole forces) between molecules?

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Which molecules exhibit only london (dispersion) forces?

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Which of the following molecules can form hydrogen bonds?

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Which of the substances has polar interactions (dipole–dipole forces) between molecules?

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Identify the predominant type of intermolecular force in each of the following compounds.

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Which of the following would be expected to form hydrogen bonds with water?

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Identify the intermolecular forces present in the substances in each pair

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Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

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Identify which of the following molecules can exhibit hydrogen bonding as a pure liquid. check all that apply.

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Arrange the following molecules according to the strength of their dispersion forces.

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Arrange the molecules by the strength of the london (dispersion) force interactions between molecules.

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Which one of the following substances should exhibit hydrogen bonding in the liquid state?

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Which of the statements describe hydrogen bonding between water molecules or describe properties of water that lead to hydrogen bonding between water molecules?

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If present in a molecule, which atom is least likely to participate in hydrogen bonds with water?

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Rank the following molecules in order of increasing strength of intermolecular forces.

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In which of the following compounds will the molecules not form hydrogen bonds with each other?

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What intermolecular forces are present between two molecules of HI?

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