Question detail
Does diamond conduct electricity? Why or why not?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Structure and bonding of carbon
Question
- A. Yes, because it has free electrons
- B. No, because it has no delocalised electrons
- C. Yes, because it has ionic bonds
- D. No, because it is a metal
Answer
The correct option is No, because it has no delocalised electrons. This answer is correct because it matches the approved learning objective to explain that each carbon atom in diamond forms four covalent bonds in the subtopic Diamond.
Explanation
The correct option is No, because it has no delocalised electrons. No, because it has no delocalised electrons is correct because it directly supports the approved learning objective to explain that each carbon atom in diamond forms four covalent bonds. This belongs to the subtopic Diamond within Structure and bonding of carbon, so the explanation must stay tied to that curriculum context. The other options are incorrect because they either do not answer this learning objective, use a vague statement, or move away from Diamond.
Common mistake
Misunderstanding Carbon Bonds in Diamond
Students often state that each carbon atom in diamond forms three covalent bonds instead of four.
Remember that in diamond, each carbon atom forms four covalent bonds, creating a strong and rigid structure.
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