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ACS GENERAL CHEMISTRY 2 FINAL EXAM
2026-2027: COMPLETE STUDY GUIDE – 200+
GRADED A+ QUESTIONS WITH RATIONALES –
FIRST-TIME PASS GUARANTEED
# SECTION 1: INTERMOLECULAR FORCES, LIQUIDS & SOLIDS (25
Questions)
**Q1.** What are the four types of intermolecular forces listed from weakest to
strongest?
A) Dipole-dipole, London dispersion, hydrogen bonding, ion-dipole
B) London dispersion, dipole-dipole, hydrogen bonding, ion-dipole
C) Hydrogen bonding, dipole-dipole, London dispersion, ion-dipole
D) Ion-dipole, hydrogen bonding, dipole-dipole, London dispersion
**Answer: B** – Rationale: The four types of intermolecular forces in order of
increasing strength are: London dispersion forces (weakest), dipole-dipole
interactions, hydrogen bonding, and ion-dipole forces (strongest). London forces
are present in all molecules, while ion-dipole forces are the strongest due to full
ionic charges interacting with polar molecules .
**Q2.** Which substance will have the highest boiling point due to intermolecular
forces?
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A) CH₄ (methane)
B) H₂O (water)
C) CO₂ (carbon dioxide)
D) F₂ (fluorine)
**Answer: B** – Rationale: Water exhibits hydrogen bonding, the strongest type
of intermolecular force among neutral molecules. Hydrogen bonding occurs when
hydrogen is bonded to N, O, or F. Methane, carbon dioxide, and fluorine only
exhibit London dispersion forces, which are significantly weaker .
**Q3.** Which type of intermolecular interaction is present in **all** molecules?
A) Hydrogen bonding
B) London dispersion forces
C) Ion-dipole forces
D) Dipole-dipole interactions
**Answer: B** – Rationale: London dispersion forces are present in all molecules,
regardless of polarity. They arise from temporary fluctuations in electron
distribution creating temporary dipoles. They are the only IMF in nonpolar
substances and contribute to attractions in all substances .
**Q4.** For which of the following would hydrogen bonding **not** be an
important intermolecular force?
A) HF
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B) H₂O
C) NH₃
D) CH₄
**Answer: D** – Rationale: Hydrogen bonding requires a hydrogen atom bonded
to a small, highly electronegative atom (N, O, or F). Methane has only C–H bonds,
so no hydrogen bonding. HF, H₂O, and NH₃ all have H bonded to F, O, or N .
**Q5.** What effect do intermolecular forces have on surface tension?
A) Surface tension decreases as strength of IMF increases
B) Surface tension increases as strength of IMF increases
C) Surface tension is not affected by IMFs
D) Surface tension is only affected by temperature
**Answer: B** – Rationale: Stronger intermolecular forces create a greater "pull"
on surface molecules, increasing surface tension. Liquids with strong IMFs (like
water with hydrogen bonding) have high surface tension, while liquids with weak
IMFs (like hexane) have low surface tension .
**Q6.** What effect do intermolecular forces have on viscosity?
A) Viscosity decreases as strength of IMF increases
B) Viscosity increases as strength of IMF increases
C) Viscosity is not affected by IMFs
D) Viscosity is only affected by molecular weight
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**Answer: B** – Rationale: Viscosity is a measure of a fluid's resistance to flow.
Stronger intermolecular forces create greater resistance as molecules attempt to
slide past each other, resulting in higher viscosity .
**Q7.** Which compound exhibits hydrogen bonding as its primary
intermolecular force?
A) HCl
B) H₂S
C) HF
D) CH₄
**Answer: C** – Rationale: HF has hydrogen bonded to fluorine, which is one of
the three elements (N, O, F) that exhibit hydrogen bonding. HCl does have a polar
bond, but chlorine is not electronegative enough for hydrogen bonding .
**Q8.** Which molecule would have the highest viscosity?
A) CH₃CH₂OH (ethanol)
B) CH₃OCH₃ (dimethyl ether)
C) C₆H₁₄ (hexane)
D) HOCH₂CH₂OH (ethylene glycol)
ACS GENERAL CHEMISTRY 2 FINAL EXAM
2026-2027: COMPLETE STUDY GUIDE – 200+
GRADED A+ QUESTIONS WITH RATIONALES –
FIRST-TIME PASS GUARANTEED
# SECTION 1: INTERMOLECULAR FORCES, LIQUIDS & SOLIDS (25
Questions)
**Q1.** What are the four types of intermolecular forces listed from weakest to
strongest?
A) Dipole-dipole, London dispersion, hydrogen bonding, ion-dipole
B) London dispersion, dipole-dipole, hydrogen bonding, ion-dipole
C) Hydrogen bonding, dipole-dipole, London dispersion, ion-dipole
D) Ion-dipole, hydrogen bonding, dipole-dipole, London dispersion
**Answer: B** – Rationale: The four types of intermolecular forces in order of
increasing strength are: London dispersion forces (weakest), dipole-dipole
interactions, hydrogen bonding, and ion-dipole forces (strongest). London forces
are present in all molecules, while ion-dipole forces are the strongest due to full
ionic charges interacting with polar molecules .
**Q2.** Which substance will have the highest boiling point due to intermolecular
forces?
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A) CH₄ (methane)
B) H₂O (water)
C) CO₂ (carbon dioxide)
D) F₂ (fluorine)
**Answer: B** – Rationale: Water exhibits hydrogen bonding, the strongest type
of intermolecular force among neutral molecules. Hydrogen bonding occurs when
hydrogen is bonded to N, O, or F. Methane, carbon dioxide, and fluorine only
exhibit London dispersion forces, which are significantly weaker .
**Q3.** Which type of intermolecular interaction is present in **all** molecules?
A) Hydrogen bonding
B) London dispersion forces
C) Ion-dipole forces
D) Dipole-dipole interactions
**Answer: B** – Rationale: London dispersion forces are present in all molecules,
regardless of polarity. They arise from temporary fluctuations in electron
distribution creating temporary dipoles. They are the only IMF in nonpolar
substances and contribute to attractions in all substances .
**Q4.** For which of the following would hydrogen bonding **not** be an
important intermolecular force?
A) HF
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B) H₂O
C) NH₃
D) CH₄
**Answer: D** – Rationale: Hydrogen bonding requires a hydrogen atom bonded
to a small, highly electronegative atom (N, O, or F). Methane has only C–H bonds,
so no hydrogen bonding. HF, H₂O, and NH₃ all have H bonded to F, O, or N .
**Q5.** What effect do intermolecular forces have on surface tension?
A) Surface tension decreases as strength of IMF increases
B) Surface tension increases as strength of IMF increases
C) Surface tension is not affected by IMFs
D) Surface tension is only affected by temperature
**Answer: B** – Rationale: Stronger intermolecular forces create a greater "pull"
on surface molecules, increasing surface tension. Liquids with strong IMFs (like
water with hydrogen bonding) have high surface tension, while liquids with weak
IMFs (like hexane) have low surface tension .
**Q6.** What effect do intermolecular forces have on viscosity?
A) Viscosity decreases as strength of IMF increases
B) Viscosity increases as strength of IMF increases
C) Viscosity is not affected by IMFs
D) Viscosity is only affected by molecular weight
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**Answer: B** – Rationale: Viscosity is a measure of a fluid's resistance to flow.
Stronger intermolecular forces create greater resistance as molecules attempt to
slide past each other, resulting in higher viscosity .
**Q7.** Which compound exhibits hydrogen bonding as its primary
intermolecular force?
A) HCl
B) H₂S
C) HF
D) CH₄
**Answer: C** – Rationale: HF has hydrogen bonded to fluorine, which is one of
the three elements (N, O, F) that exhibit hydrogen bonding. HCl does have a polar
bond, but chlorine is not electronegative enough for hydrogen bonding .
**Q8.** Which molecule would have the highest viscosity?
A) CH₃CH₂OH (ethanol)
B) CH₃OCH₃ (dimethyl ether)
C) C₆H₁₄ (hexane)
D) HOCH₂CH₂OH (ethylene glycol)
