1. Explain the term ionic bond

Question 1 of 20

2. Why do ionic compounds conduct electricity only when molten or in solution?

Question 2 of 20

3. Describe the formation of a covalent bond

Question 3 of 20

4. Describe the bonding in a metal

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5. Give the definition of a covalent bond

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6. Explain why metals are malleable

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7. Alloys contain different sized positive ions. What properties does this give alloys compared to pure metals?

Question 7 of 20

8. Explain, in terms of structure and bonding, why sodium chloride has a very high melting point

Question 8 of 20

9. Why do covalent compounds (e.g H₂O) not conduct electricity?

Question 9 of 20

10. Explain why Silica, SiO₂ is a solid with a high melting point

Question 10 of 20

11. Explain, in terms of its structure, why graphite can conduct electricity.

Question 11 of 20

12. Explain why carbon dioxide gas, CO₂, is a gas at room temperature

Question 12 of 20

13. State the fomula for the two ions in vanadium (V) oxide

Question 13 of 20

14. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of chlorine (Cl₂), how many electrons should be shown in areas 1, 2 and 3?

Question 14 of 20

15. State 3 properties that makes aluminium suitable for power cables

Question 15 of 20

16. What is an alloy?

Question 16 of 20

17. When can ionic substances conduct electricity?

Question 17 of 20

18. A student has drawn a diagram to show the structure of a metallic solid, but forgotten to label the parts. Which of the following correctly lists those parts?

Question 18 of 20

19. Do larger molecules have higher or lower boiling points than smaller molecules?

Question 19 of 20

20. Typically, do covalent substances conduct electricity?

Question 20 of 20