1. Why do ionic substance have high melting and boiling points?

Question 1 of 20

2. 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 2 of 20

3. Explain why nitrogen gas, N₂, is a gas at room temperature

Question 3 of 20

4. Describe the formation of a covalent bond

Question 4 of 20

5. Typically, do covalent substances conduct electricity?

Question 5 of 20

6. Why are alloys harder than pure metals?

Question 6 of 20

7. Describe the structure of metals

Question 7 of 20

8. What holds ions together?

Question 8 of 20

9. What is needed to complete this diagram to show the ionic bonding in potassium oxide, K₂O ?

Question 9 of 20

10. Do ionic substances conduct electricity?

Question 10 of 20

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

Question 11 of 20

12. Give the definition of a covalent bond

Question 12 of 20

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

Question 13 of 20

14. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of ethane (C₂H₆), how many electrons should be shown in areas 1, 2, 3, 4, 5, 6 and 7?

Question 14 of 20

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

Question 15 of 20

16. State two properties of aluminium that make it suitable for use in food cans

Question 16 of 20

17. Suggest why buckminsterfullerene, C₆₀, has a low melting point.

Question 17 of 20

18. What does the word malleable mean?

Question 18 of 20

19. What is an alloy?

Question 19 of 20

20. Explain whether solid ionic compounds conduct electricity

Question 20 of 20