📚 Quick Study Guide
🔍 Intermolecular forces (IMFs) are attractive or repulsive forces between molecules.
💡 IMFs are weaker than intramolecular forces (e.g., covalent bonds).
⚛️ Strong IMFs lead to higher boiling points and melting points.
🧊 Types of IMFs:
➡️ Hydrogen bonding: Strongest IMF, occurs when H is bonded to O, N, or F.
➡️ Dipole-dipole forces: Occur between polar molecules.
➡️ London dispersion forces: Weakest IMF, present in all molecules, strength increases with molecular size.
🧪 Practice Quiz
Question 1: Which of the following compounds exhibits the strongest intermolecular forces?
A) $CH_4$
B) $H_2O$
C) $CO_2$
D) $N_2$
Question 2: Which intermolecular force is primarily responsible for the high boiling point of water ($H_2O$) compared to methane ($CH_4$)?
A) London dispersion forces
B) Dipole-dipole forces
C) Hydrogen bonding
D) Ionic bonding
Question 3: Which of the following compounds has the weakest intermolecular forces?
A) $CH_3OH$
B) $CH_3CH_2OH$
C) $CH_3CH_2CH_3$
D) $CH_3CH_2NH_2$
Question 4: Which of the following molecules primarily interacts through London Dispersion Forces?
A) $NH_3$
B) $H_2S$
C) $CH_4$
D) $H_2O$
Question 5: Which of the following compounds would you predict to have the highest boiling point?
A) $C_2H_6$
B) $C_3H_8$
C) $C_4H_{10}$
D) $C_5H_{12}$
Question 6: Which of the following molecules can form hydrogen bonds with itself?
A) $CH_3OCH_3$
B) $CH_3CHO$
C) $CH_3COOH$
D) $CH_3Cl$
Question 7: What type of intermolecular force exists between molecules of $SO_2$?
A) London dispersion forces only
B) Hydrogen bonding
C) Dipole-dipole forces and London dispersion forces
D) Ionic forces
Click to see Answers
1: B
2: C
3: C
4: C
5: D
6: C
7: C