Covalent Bonding Quiz
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5 questions, one answer each
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1. What is a covalent bond?
- A. The transfer of electrons between atoms
- B. The sharing of a pair of electrons between atoms
- C. The attraction between a metal ion and delocalised electrons
- D. The attraction between oppositely charged ions
2. Why does solid carbon dioxide (dry ice) sublime easily at a relatively low temperature?
- A. Its covalent bonds are weak and break easily
- B. It has weak intermolecular forces between simple CO2 molecules that require little energy to overcome
- C. It is a giant covalent structure
- D. It contains free ions
3. Why does diamond not conduct electricity, while graphite does?
- A. Diamond has no carbon atoms
- B. Graphite has delocalised electrons free to move between layers, while diamond has all electrons held in fixed covalent bonds
- C. Diamond is a compound, graphite is an element
- D. Graphite is ionic and diamond is covalent
4. Which trend is generally true for simple molecular substances as relative molecular mass increases?
- A. Melting and boiling points decrease
- B. Melting and boiling points generally increase
- C. Melting and boiling points stay exactly the same
- D. They stop conducting electricity
5. A student argues that boiling water breaks the covalent O–H bonds within water molecules. Why is this incorrect, and what actually happens?
- A. It is correct — covalent bonds do break on boiling
- B. It is incorrect; boiling only overcomes the weak intermolecular forces between water molecules, leaving the covalent O–H bonds intact
- C. It is incorrect because water has no covalent bonds
- D. It is incorrect because water is an ionic compound