📚 Topic Summary
Molecular solids are substances held together by relatively weak intermolecular forces (IMFs) rather than strong covalent or ionic bonds. These IMFs—such as London dispersion forces, dipole-dipole interactions, and hydrogen bonding—dictate the physical properties of these solids, including their melting points and solubilities. The stronger the IMFs, the higher the melting point. Understanding the types of IMFs present in a molecular solid is crucial for predicting its behavior. 🤓
🧪 Part A: Vocabulary
Match the term to its correct definition:
| Term |
Definition |
| 1. Hydrogen Bonding |
A. Temporary attractive force resulting from instantaneous dipoles in molecules. |
| 2. Dipole-Dipole Interactions |
B. Strongest IMF; occurs between molecules with H bonded to N, O, or F. |
| 3. London Dispersion Forces |
C. Solid composed of discrete molecules held together by IMFs. |
| 4. Molecular Solid |
D. Attractive forces between polar molecules. |
| 5. Intermolecular Forces |
E. Attractive or repulsive forces between neighboring molecules. |
Match the correct letter (A-E) with each number (1-5).
📝 Part B: Fill in the Blanks
Complete the following paragraph using the words provided (words may be used once, more than once, or not at all): melting point, intermolecular forces, covalent bonds, London dispersion forces, hydrogen bonding, dipole-dipole.
The physical properties of molecular solids are largely determined by the strength of their __________. Solids with strong __________ tend to have higher __________. Even nonpolar molecules exhibit weak attractions due to __________. Additionally, molecules containing hydrogen bonded to oxygen, nitrogen, or fluorine can form strong attractions via __________. The atoms within a single molecule are held together by __________.
🤔 Part C: Critical Thinking
Explain how the types of intermolecular forces present in a substance affect its solubility in different solvents.