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

Question 1 of 20

2. Do ionic substances conduct electricity?

Question 2 of 20

3. Describe the structure of metals

Question 3 of 20

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

Question 4 of 20

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

Question 5 of 20

6. Draw a diagram to show the bonding in a metal

Question 6 of 20

7. Describe the structure of an ionic compound, e.g NaCl.

Question 7 of 20

8. When are ions attracted to each other?

Question 8 of 20

9. 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 9 of 20

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

Question 10 of 20

11. Why are alloys harder than pure metals?

Question 11 of 20

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

Question 12 of 20

13. Explain why methane gas, CH₄, is a gas at room temperature

Question 13 of 20

14. Give the definition of a covalent bond

Question 14 of 20

15. Describe the formation of a covalent bond

Question 15 of 20

16. A substance is found not to conduct electricity even when molten. What type of bonding does the substance have?

Question 16 of 20

17. What is a mixture of metals called?

Question 17 of 20

18. What does the word malleable mean?

Question 18 of 20

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

Question 19 of 20

20. State 3 properties that makes iron suitable for saucepans

Question 20 of 20