Questions on Van der Waals Forces
Multiple-Choice Questions: Van der Waals Forces
1. What are Van der Waals forces?
A) Strong covalent bonds
B) Weak intermolecular forces
C) Ionic bonds
D) Metallic bonds
E) Nuclear forces
2. Which of the following is NOT a type of Van der Waals force?
A) London dispersion forces
B) Dipole-dipole interactions
C) Hydrogen bonding
D) Ion-dipole interactions
E) Metallic bonding
3. Which Van der Waals force is present in all molecules, polar or nonpolar?
A) Dipole-dipole
B) London dispersion forces
C) Hydrogen bonding
D) Ion-dipole
E) Covalent bonding
4. London dispersion forces arise due to:
A) Permanent dipoles
B) Temporary induced dipoles
C) Ionic attraction
D) Hydrogen bonds
E) Metallic bonding
5. Which molecule experiences London dispersion forces only?
A) H₂O
B) NH₃
C) CO₂
D) HCl
E) NaCl
6. Dipole-dipole interactions occur between:
A) Nonpolar molecules only
B) Polar molecules only
C) Ionic compounds only
D) Metals only
E) Noble gases only
7. Which factor increases the strength of London dispersion forces?
A) Smaller molecular size
B) Larger molecular size and more electrons
C) Lower molecular weight
D) Less polarizable electron cloud
E) No electrons
8. Hydrogen bonding is a special type of:
A) Covalent bond
B) Ionic bond
C) Dipole-dipole interaction
D) London dispersion force
E) Metallic bond
9. Which of these atoms must be bonded to hydrogen to form hydrogen bonds?
A) Carbon, nitrogen, oxygen
B) Nitrogen, oxygen, fluorine
C) Fluorine, chlorine, bromine
D) Sulfur, phosphorus, oxygen
E) Hydrogen only
10. Which molecule exhibits hydrogen bonding?
A) CH₄
B) HF
C) CO₂
D) Ne
E) Cl₂
11. Van der Waals forces are strongest in which state of matter?
A) Gas
B) Liquid
C) Solid
D) Plasma
E) None
12. How do Van der Waals forces affect boiling points?
A) Stronger Van der Waals forces increase boiling points
B) They have no effect
C) Stronger forces decrease boiling points
D) Only ionic bonds affect boiling points
E) Only metallic bonds affect boiling points
13. Which molecule would have the highest London dispersion forces?
A) H₂
B) N₂
C) F₂
D) I₂
E) Cl₂
14. Which factor does NOT influence dipole-dipole interactions?
A) Molecular polarity
B) Distance between molecules
C) Molecular size
D) Temperature
E) Number of lone pairs
15. What type of interaction occurs between an ion and a polar molecule?
A) London dispersion forces
B) Ion-dipole interactions
C) Hydrogen bonding
D) Metallic bonding
E) Dipole-dipole interaction
16. Which of the following substances primarily relies on Van der Waals forces for intermolecular attraction?
A) NaCl
B) H₂O
C) O₂
D) MgO
E) HCl
17. Why do larger atoms or molecules have stronger London dispersion forces?
A) They have more protons
B) Their electrons are more easily polarized
C) They have stronger covalent bonds
D) They have ionic bonds
E) They have higher electronegativity
18. Van der Waals forces are significant in which of the following?
A) Formation of ionic crystals
B) Interaction between noble gas atoms
C) Metallic bonding
D) Nuclear fusion
E) Formation of covalent bonds
19. Which is TRUE about hydrogen bonding compared to other Van der Waals forces?
A) It is weaker than London dispersion forces
B) It is stronger than dipole-dipole and London forces
C) It only occurs in nonpolar molecules
D) It is a type of metallic bonding
E) It does not involve hydrogen
20. Which of the following best explains why ice floats on water?
A) Metallic bonding in ice
B) Hydrogen bonding creates an open lattice structure in ice
C) London dispersion forces in ice
D) Ionic bonding in water
E) Van der Waals forces have no role in ice density
- Questions: Molecular Shapes with and without Lone Pairs
- Questions on Bond Polarity
- Questions on Polar Molecules
Answers with Explanations
1. B) Van der Waals forces are weak intermolecular forces.
2. E) Metallic bonding is NOT a Van der Waals force.
3. B) London dispersion forces occur in all molecules.
4. B) They arise from temporary induced dipoles.
5. C) CO₂ is nonpolar and has only London dispersion forces.
6. B) Dipole-dipole occur between polar molecules.
7. B) Larger molecules have more electrons and stronger dispersion forces.
8. C) Hydrogen bonding is a special kind of dipole-dipole interaction.
9. B) N, O, and F bonded to H can form hydrogen bonds.
10. B) HF exhibits hydrogen bonding.
11. C) Van der Waals forces are strongest in the solid state due to close proximity.
12. A) Stronger Van der Waals forces lead to higher boiling points.
13. D) I₂ has the largest atoms and strongest London dispersion forces.
14. E) Number of lone pairs does not directly influence dipole-dipole forces.
15. B) Ion-dipole interactions occur between ions and polar molecules.
16. C) O₂ relies mainly on Van der Waals (dispersion) forces.
17. B) Larger atoms have more polarizable electrons, strengthening dispersion forces.
18. B) Van der Waals forces are important between noble gas atoms.
19. B) Hydrogen bonds are stronger than other Van der Waals forces.
20. B) Hydrogen bonding forms open lattice structure in ice, lowering its density.
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