Which of the following molecules primarily interacts through induced dipole interactions?

A. H2O

B. CH4

C. HCl

D. NaCl

Which factor does NOT affect the strength of van der Waals forces?

A. Size of the molecule

B. Shape of the molecule

C. Charge of the molecule

D. Number of electrons in the molecule

Which of the following is NOT a requirement for the formation of hydrogen bonds?

A. Presence of a hydrogen atom

B. Presence of a highly electronegative atom

C. Presence of a metal atom

D. A significant difference in electronegativity between the bonded atoms

Which of the following molecules can form hydrogen bonds?

A. CH4

B. NH3

C. Cl2

D. Ne

Why is water (H2O) a liquid at room temperature while methane (CH4) is a gas?

A. Water has ionic bonds

B. Methane has stronger covalent bonds

C. Water can form hydrogen bonds

D. Methane has a larger molecular size

a) Define the term "induced dipole interactions" and explain how they arise in non-polar molecules. [3]

b) Why are induced dipole interactions also referred to as "van der Waals forces"? [2]

a) Describe the factors that affect the strength of van der Waals forces in non-polar molecules. [3]

b) Given two non-polar molecules, one larger and one smaller, which one would you expect to have stronger van der Waals forces and why? [2]

a) What is a "hydrogen bond", and how does it differ from other types of dipole-dipole interactions? [3]

b) Explain the significance of hydrogen bonding in the structure of water. [2]

a) Explain the difference between a dipole-dipole interaction and an induced dipole interaction. [3]

b) Why do non-polar molecules, which lack permanent dipoles, still exhibit van der Waals forces? [2]

c) How do the strengths of these interactions compare to covalent bonds? [2]

a) What is the significance of hydrogen bonding in the structure of DNA? [3]

b) Why are hydrogen bonds crucial for the double helix structure of DNA? [2]

c) How do hydrogen bonds compare in strength to covalent bonds and other intermolecular forces? [3]

Which of the following molecules is polar?

A. CO2

B. CH4

C. H2O

D. O2

Which type of intermolecular force is the weakest?

A. Ionic bond

B. Covalent bond

C. Hydrogen bond

D. Van der Waals forces

Which of the following molecules has the highest boiling point due to its ability to form hydrogen bonds?

A. CH4

B. NH3

C. BF3

D. CCl4

Why does DNA have a stable structure?

A. It forms ionic bonds

B. It forms covalent bonds

C. It forms hydrogen bonds

D. It forms metallic bonds

Which of the following molecules is non-polar and interacts primarily through induced dipole interactions?

A. H2O

B. HF

C. CO2

D. H2

a) Describe the factors that are necessary for the formation of hydrogen bonds. [3]

b) Why is water's boiling point unusually high for a molecule of its size? [2]

c) How does the presence of hydrogen bonds affect the density of ice compared to liquid water? [3]

a) Explain the term "van der Waals forces" and how they differ from hydrogen bonds. [3]

b) Why do larger molecules generally have stronger van der Waals forces? [2]

c) How do van der Waals forces contribute to the properties of non-polar substances like noble gases? [3]

a) Describe the nature of induced dipole interactions and explain how they arise in non-polar molecules. [3]

b) How do the strengths of induced dipole interactions vary with the size and shape of molecules? [3]

c) Explain the term "hydrogen bond" and identify two substances, other than water, where hydrogen bonding is significant. [3]

d) How do the properties of substances with hydrogen bonds differ from those with only induced dipole interactions? [3]

a) What factors are necessary for a molecule to form hydrogen bonds? [3]

b) Explain the significance of hydrogen bonding in the structure and properties of DNA. [3]

c) Why do substances with hydrogen bonds often have higher boiling points than those without? [2]

d) How do van der Waals forces and hydrogen bonds contribute to the solubility of substances in water? [4]

a) Describe the difference between a hydrogen bond and a covalent bond. [3]

b) Why is ice less dense than liquid water? [3]

c) How do induced dipole interactions contribute to the properties of noble gases? [2]

d) Explain the role of van der Waals forces in the liquefaction of gases. [4]