3. Structure and Bonding

Question 1

1. What is ionic bonding?

Answer 1

1. When an atom transfers electrons to another atom to form ions

Question 2

2. What type of elements form ionic bonds between them?

Answer 2

2. A metal and a non-metal

Question 3

3. What force holds ions together in ionic compounds?

Answer 3

3. Electrostatic forces

Question 4

4. What type of structure do ionic compounds form?

Answer 4

4. Giant lattices

Question 5

5. What is the charge on a Group 1 metal ion?

Answer 5

5. +1

Question 6

6. What is the charge on a Group 6 element’s ion?

Answer 6

6. -2

Question 7

7. How many electrons are in the outer shell of an ion?

Answer 7

7.Full outer shell (e.g. 8 or if the first shell 2)

Question 8

9. Do ionic compounds have high or low melting and boiling points?

Answer 8

9. High

Question 9

10. Why?

Answer 9

10. Strong ionic bonds need a lot of energy to break them.

Question 10

11. When do ionic compounds conduct electricity?

Answer 10

11. Molten (melted) or in solution

Question 11

12. Why?

Answer 11

12. The ions are free to move

Question 12

13. What is covalent bonding?

Answer 12

13.Sharing of electrons

Question 13

14. What type of elements form covalent bonds between them?

Answer 13

14. Non-metals

Question 14

15. What type of structure do covalent compounds such as chlorine, water and methane form?

Answer 14

15. Simple covalent molecules

Question 15

17. Do small molecules have high or low melting and boiling points?

Answer 15

17. Low

Question 16

18. Why do small molecules have low boiling point?

Answer 16

18. Weak intermolecular forces (forces between the small molecules)

Question 17

19. Do larger molecules have higher or lower melting and boiling points?

Answer 17

19. Higher

Question 18

20. Do small covalent molecules conduct electricity?

Answer 18

20. No

Question 19

21. Why don’t small molecules conduct electricity?

Answer 19

21. No charged particles

Question 20

22. Why are polymers solid at room temperature?

Answer 20

22. Relatively strong intermolecular forces

Question 21

23. What is the bonding in a polymer?

Answer 21

23. Covalent

Question 22

24. Do giant covalent structures have high or low melting and boiling points?

Answer 22

24. High

Question 23

25. Why do giant covalent have high melting points?

Answer 23

25. It is the covalent bonds that are broken and they are strong so need a lot of energy to break them.

Question 24

26. Why is diamond hard?

Answer 24

8. Strong covalent bonds (4 per carbon)

Question 25

27.       Can diamond conduct electricity? Explain why.

Answer 25

9.            No. No free (delocalised) electrons.

Question 26

28.       Why is graphite a hard, solid at room temperature?

Answer 26

10.       Strong covalent bonds (3 per carbon)

Question 27

29.       Why can graphite be used as a lubricant?

Answer 27

11.       Layers can slide over each other (weaker intermolecular forces between layers

Question 28

30.       Can graphite conduct electricity? Explain why.

Answer 28

12.       Yes. Free (delocalised) electrons can move and carry charge.

Question 29

31.       What is graphene?

Answer 29

13.       Single layer of graphite

Question 30

32.       What properties make it useful?

Answer 30

14.       Very good conductor of electricity, strong.

Question 31

33.       What is metallic bonding?

Answer 31

15.       Attraction between delocalised (free) electrons and positive ions

Question 32

34.       Why can metals conduct electricity and thermal energy?

Answer 32

16.       Delocalised (free) electrons can move and carry charge

Question 33

35.       Why are alloys harder than pure metals?

Answer 33

17.       Different sized metal atoms so the layers can’t slide over each other.