Simple Molecules and Covalent Bonds Quiz
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5 questions, one answer each
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1. Which of the following best describes a covalent bond?
- A. A pair of electrons shared between two atoms
- B. The transfer of electrons from one atom to another
- C. A bond formed between a metal and a non-metal
- D. The attraction between oppositely charged ions
2. In the molecule HCl, how many covalent bonds are present?
- A. Two covalent bonds
- B. One covalent bond
- C. Three covalent bonds
- D. No covalent bonds
3. Why do simple molecular compounds such as H₂O and CH₄ have low melting and boiling points?
- A. Because the covalent bonds within the molecules are weak
- B. Because the intermolecular forces between molecules are weak
- C. Because they do not contain any covalent bonds
- D. Because their electronic configurations are unstable
4. Which statement correctly explains why simple molecular compounds are poor electrical conductors?
- A. They contain covalent bonds which do not allow electron movement
- B. They do not contain ions or delocalised electrons that are free to move and carry electrical charge
- C. Their molecules are too large to allow current to flow
- D. Covalent bonding prevents the formation of any charged particles
5. In molecule N₂, nitrogen atoms form a triple covalent bond. Explain why both nitrogen atoms achieve noble gas electronic configurations through this bonding.
- A. Each nitrogen atom gains three electrons from the other nitrogen atom
- B. Each nitrogen atom shares three pairs of electrons, giving each nitrogen a total of 10 electrons (the electron configuration of neon)
- C. The triple bond creates extra electrons that fill the outer shell of each atom
- D. Nitrogen atoms transfer valence electrons to become isoelectronic with helium