What is the effect of strong intermolecular forces on the boiling point of a substance?

Makes boiling point unpredictable

Which of the following best describes the difference between intermolecular and intramolecular forces?

Intermolecular forces occur between molecules; intramolecular forces occur within molecules.

Intermolecular forces occur within molecules; intramolecular forces occur between molecules.

Why do nonpolar molecules like O $$_2$$ and N $$_2$$ have low boiling points?

They have only London dispersion forces.

They have strong hydrogen bonds.

They have dipole-dipole interactions.

How does molecular size affect the strength of London dispersion forces?

Larger molecules have stronger forces.

Larger molecules have weaker forces.

Smaller molecules have stronger forces.

Size does not affect the forces.

Which of the following statements best explains why hydrogen bonding leads to higher boiling points?

Hydrogen bonds require more energy to break.

Hydrogen bonds are stronger than covalent bonds.

Hydrogen bonds are weaker than London dispersion forces.

Hydrogen bonds do not affect boiling point.

A scientist is comparing the boiling points of H $$_2$$ O, CH $$_3$$ OH, and CH $$_4$$ . Using your knowledge of intermolecular forces, which molecule would you predict to have the lowest boiling point and why?

CH $$_4$$ , because it only has London dispersion forces

H $$_2$$ O, because it has hydrogen bonding

CH $$_3$$ OH, because it has dipole-dipole interactions

CH $$_3$$ OH, because it has hydrogen bonding

You are given two substances: NaCl (ionic solid) and I $$_2$$ (molecular solid). Explain which has stronger intermolecular forces and why.

NaCl, because ionic bonds are stronger than London dispersion forces

I $$_2$$ , because London dispersion forces are stronger than ionic bonds

I $$_2$$ , because it has hydrogen bonding

A liquid has a very high boiling point and is composed of molecules with N-H bonds. What is the most likely explanation for its high boiling point?

Strong London dispersion forces

Weak dipole-dipole interactions

A student claims that the boiling point of CH $$_3$$ CH $$_2$$ CH $$_2$$ CH $$_3$$ (butane) is higher than that of CH $$_4$$ (methane) because of stronger London dispersion forces. Is this claim correct? Justify your answer.

Yes, because butane is larger and has more electrons, leading to stronger London dispersion forces.

No, because methane is more polar.

Yes, because methane has hydrogen bonding.

No, because butane is nonpolar.

Explain why ionic solids generally have higher melting points than molecular solids.

Ionic solids have stronger intermolecular forces due to ionic bonds.

Molecular solids have stronger hydrogen bonds.

Ionic solids have weaker London dispersion forces.

Molecular solids have stronger dipole-dipole interactions.

A mixture contains H $$_2$$ O and CH $$_3$$ OH. Predict whether these two substances will mix well and explain your reasoning based on intermolecular forces.

Yes, because both can form hydrogen bonds with each other.

No, because only CH $$_3$$ OH can form hydrogen bonds.

Yes, because both are nonpolar.

No, because H $$_2$$ O is ionic.

A scientist wants to design a solid with a very high melting point. Which type of intermolecular force should be maximized, and why?

Ionic interactions, because they are much stronger than other intermolecular forces

London dispersion forces, because they are present in all molecules

Hydrogen bonding, because it is the strongest

Dipole-dipole interactions, because they are stronger than ionic interactions

Exploring Intermolecular Forces

11th Grade

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Exploring Intermolecular Forces

Quiz

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Chemistry

•

11th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-3, HS-PS3-4

Standards-aligned

Otto Fadilah

Used 2+ times

FREE Resource

30 questions

Show all answers

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following is an example of an intermolecular force?

Covalent bond

Hydrogen bond

Ionic bond

Metallic bond

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What type of intermolecular force is present in all molecules, regardless of their polarity?

Dipole-dipole interactions

London dispersion forces

Hydrogen bonding

Ionic interactions

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which intermolecular force is the strongest among the following?

London dispersion forces

Dipole-dipole interactions

Hydrogen bonding

Van der Waals forces

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Hydrogen bonding occurs when hydrogen is bonded to which of the following elements?

Carbon, Nitrogen, Oxygen

Nitrogen, Oxygen, Fluorine

Sulfur, Phosphorus, Chlorine

Oxygen, Sulfur, Chlorine

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following molecules can form hydrogen bonds?

Dipole-dipole interactions occur between molecules that are:

Nonpolar

Polar

Ionic

Metallic

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

London dispersion forces are also known as:

Permanent dipole forces

Induced dipole forces

Hydrogen bonds

Ionic bonds

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Exploring Intermolecular Forces

30 questions

Which of the following is an example of an intermolecular force?

What type of intermolecular force is present in all molecules, regardless of their polarity?

Which intermolecular force is the strongest among the following?

Hydrogen bonding occurs when hydrogen is bonded to which of the following elements?

Which of the following molecules can form hydrogen bonds?

Dipole-dipole interactions occur between molecules that are:

London dispersion forces are also known as:

Which intermolecular force is responsible for the high boiling point of water?

What is the effect of strong intermolecular forces on the boiling point of a substance?

In solids, intermolecular forces are generally:

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