1. Why do metals have high melting and boiling points?

Question 1 of 20

2. Explain the term ionic bond

Question 2 of 20

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

Question 3 of 20

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

Question 4 of 20

5. Describe the bonding in a metal

Question 5 of 20

6. State 2 properties that makes aluminium suitable for manufacturing aircraft

Question 6 of 20

7. Explain whether solid ionic compounds conduct electricity

Question 7 of 20

8. Describe the formation of a covalent bond

Question 8 of 20

9. 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 9 of 20

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

Question 10 of 20

11. When can ionic substances conduct electricity?

Question 11 of 20

12. 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 12 of 20

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

Question 13 of 20

14.

State whether covalent substances conduct electricity, and explain why

Question 14 of 20

15. Explain, in terms of its structure, why graphite can act as a lubricant.

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. Explain how the atoms are held together in a hydrogen bromide molecule

Question 17 of 20

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

Question 18 of 20

19. Why is the melting point of a smaller molecule lower than that of a larger molecule?

Question 19 of 20

20. What is a mixture of metals called?

Question 20 of 20