1. S2 Science
Ions and Ionic Bonding

2. Learning Outcomes
We are Learning about ionic bonding

3. Success Criteria
I can describe what an ion is and describe their formation
I can describe an ionic bond and explain that it usually consists of a metal/non-metal combination
I can state that ionic substances form lattice structures
I can state that the forces of attraction between oppositely charged ions in a lattice structure are strong
I can state the properties of ionic compounds

4. Ions
Ions are charged particles

5. Ions Ions are charged particles
The simplest ions are atoms that have lost or gained electrons

6. Ions Ions are charged particles
The simplest ions are atoms that have lost or gained electrons
Atoms lose or gain electrons to become like the noble gasses

7. Why Ions Form
The lithium atom has the electron configuration 2,1
The target diagram would be - Li 3+
2,1

8. Why Ions Form
To achieve the stable electron arrangement of the noble gas the lithium atom would have to lose its outer electron.

9. Why Ions Form
The lithium ion has the electron configuration of just 2
The target diagram would be - 3+ 2
Li+

10. Why Ions Form
The lithium ion now has the same electron configuration as helium and so is very stable.

11. Why Ions Form It has 3 protons but only 2 electrons
The extra proton gives it a positive charge.

12. Why Ions Form
The fluorine atom has 7 electrons in its outer shell
The target diagram would be - 9+
2,7 F

13. Why Ions Form
To become like the noble gases it must either lose or gain electrons.

14. Why Ions Form
To become like the noble gases it must either lose or gain electrons.
It cannot lose 7 electrons so it must gain just 1 to complete the shell

15. Why Ions Form
The fluoride ion has 8 electrons in its outer shell
The target diagram would be - 9+
2,8 F-

16. Why Ions Form
The fluorine ion has 10 electrons and 9 protons.

17. Why Ions Form The fluoride ion has 10 electrons and 9 protons.
The extra electron gives it a negative charge.

18. Ions Summary
Metals lose electrons to form positive ions.

19. Ions Summary Metals lose electrons to form positive ions.
Non metals gain electrons to become negative ions.

20. Ions Summary Metals lose electrons to form positive ions.
Non metals gain electrons to become negative ions.
Metal and non-metal ions attract each other to form ionic compounds

21. Ions Summary Metals lose electrons to form positive ions.
Non metals gain electrons to become negative ions.
Metal and non-metal ions attract each other to form ionic compounds
The attraction between positive and negative ions is called the ionic bond.

22. Ions Summary Group Number 1 2 3 4 5 6 7 8 Valency/combining power
Charge on the ion

23. Ions Summary Group Number 1 2 3 4 5 6 7 8 Valency/combining power
Charge on the ion

24. Ions Summary Group Number 1 2 3 4 5 6 7 8 Valency/combining power
Charge on the ion 1+ 2+ 3+ 3- 2- 1-

25. The Ionic Bond Sodium chloride is a typical ionic compound
Sodium forms a positive ion Na+
Chlorine forms a negative ion Cl-
The negative chloride ion is attracted strongly to the positive sodium ion

26. Solid, liquid or solution
Conductivity tests
Substance
Solid, liquid or solution
conductor
iron
solid
sugar
solution
Sodium chloride
water
liquid
Copper sulphate
ethanol
Zinc chloride
Zinc iodide

27. Solid, liquid or solution
Conductivity tests
Substance
Solid, liquid or solution
conductor
iron
solid 
sugar
solution
Sodium chloride
water
liquid
Copper sulphate
ethanol
Zinc chloride
Zinc iodide

28. Conductivity tests
Compounds which contain only non metals do not conduct electricity.

29. Conductivity tests
All metals conduct electricity

30. Conductivity tests All metals conduct electricity
Compounds containing metals do not conduct when solid but do conduct when molten or in solution

31. Conductivity tests All metals conduct electricity
Compounds containing metals do not conduct when solid but do conduct when molten or in solution
These compounds are called ionic compounds

32. Compounds
Ionic compounds contain ions

33. Compounds Ionic compounds contain ions
Only when the ions can move freely will the compound conduct electricity

34. Compounds Ionic compounds contain ions
Only when the ions can move freely will the compound conduct electricity
In a solid the ions cannot move and so cannot conduct electricity

35. Electrolysis
Electrolysis means the breaking up of a compound by the action of electricity.
(‘electro’ = electricity; ‘lysis’ = breaking apart)

36. Electrolysis DC
Carbon
electrodes
copper chloride

37. Electrolysis of copper chloride
Observations Made
At positive rod
At negative rod

38. Electrolysis of copper chloride
Observations Made
At positive rod
At negative rod
Colourless gas
Brown solid

39. Electrolysis of copper chloride
The metal copper was formed at the negative rod
The gas chlorine was formed at the positive rod.

40. Ions on the move
An electrolyte is a liquid or solution that conducts electricity by ions moving through it.
An electrode is a rod where the electricity enters or leaves the electrolyte.

41. Ions on the move
The ions always move towards oppositely charged electrodes.

42. Ions on the move
The ions always move towards oppositely charged electrodes.
Positive metal ions move towards the negative electrode

43. Ions on the move
The ions always move towards oppositely charged electrodes.
Positive metal ions move towards the negative electrode
Negative non metal ions move towards the positive electrode