1. For each property give an explanation see e.g.
Iodine
water
Carbon dioxide
Sodium chloride
Copper (II) suphate
Iron (I) oxide
Diamond
Quartz
graphite .
Type of bonding with definition
Melting and boiling point
Hard, sort or brittle ?
Brittle
Because forms a giant ionic lattice, when one layer of ions pushed over another layer opposite charges line up and repel each other, breaking off layers of the lattice.
Conducts ?
For each property give an explanation see e.g.

2. Metallic bonding Starter 1. write title
2. In which type of elements does metallic bonding take place ?
3. Name 3 substances where you will find metallic bonding.
4. List the properties of metals.
EXTENSION what is an alloy and what are its properties ?

3. Metallic bonding
2. In which type of elements does metallic bonding take place ? Metals 3. Name 3 substances where you will find metallic bonding. Any metal Or metal alloy

4. Metallic bonding
4. List the properties of metals Strong High melting point High boiling point Conduct electricity Conduct heat Malleable (easily beaten into shape) Ductile (easily pulled into wires)

5. Metallic bonding
Aims.
To be able to describe and draw the metallic bonding
To know the properties of metals
To relate the properties of metals to their structure
Extension to practise past exam paper questions on metallic bonding
Extension to comparing types of bonding.

6. To be able to describe and draw the metallic bonding
Key point-metals easily lose their outer electrons
Extension why ?
Metals have less number of valence electrons while non metals have more number of them. If there are less valence electrons it is easy to lose them in order to attain stability or reach the electronic configuration of noble gas.

7. To be able to describe and draw the metallic bonding
Key point-Outer electrons are free to move-DELOCALISED -Leaving behind a metal CATION

8. Copy: Metal Structure
Write the EXAM description and Definition (WRITE THIS IN YOUR BONDING COMPARISON TABLE also)
Description- “An Array of positive metal ions in a sea of delocalised electrons”
Definition -the attraction between the array of positive metal ions and the sea of delocalised electrons.
2. Draw the metallic bonding in sodium (page 20)
Delocalised electrons from outer shells of metal
3. Extension draw the metallic bonding in Magnesium

9. Copy: Metal Structure
3. Extension draw the metallic bonding in Magnesium (for 9 magnesium cations there should be 18 electrons) e- e- e-
Mg2+
Mg2+
Mg2+ e- e- e- e- e-
Mg2+
Mg2+
Mg2+ e- e- e- e- e- e-
Mg2+
Mg2+
Mg2+ e- e- e- e-

10. Copy: Metal Structure
Use page 20 to explain why sodium can be easily cut with a knife but magnesium can not.
Mg2+ e-

11. Copy: Metal Structure
Use page 20 to explain why sodium can be easily cut with a knife but magnesium can not.
1. In sodium the attraction between the seas of delocalised electrons and array of metal ions is weaker
-In sodium there is only one electron per Na+
-In magnesium there is two electrons and a 2+ positive charge on the magnesium
2. The ions do not pack very efficiently.

12. 2. To know the properties of metals
You should have written this down from the starter.....if not you will need to do this for homework use page in the text book.

13. 3. To relate the properties of metals to their structure
Strong- Powerful attractions between
_______ metal ions and the ________
___________________
B. High melting and boiling points- Metals form g_____ m_____ s_____. There are _____ attractions between _________________
Extension Q. 4 pg 32.-comparison of bonding

14. 3. To relate the properties of metals to their structure
Strong- Powerful attractions between
_______ metal ions and the ________
___________________
B. High melting and boiling points- Metals form g_____ m_____ s_____. There are _____ attractions between _________________
Extension Q. 4 pg 32.-comparison of bonding
Array of Positive
Sea of
Delocalised electrons
etallic
tructure
iant
Strong
The array of positive metal ions and the sea of delocalised electrons

15. Metals conduct electricity because.....
Metallic Bonding
Metals conduct electricity because.....
Metallic Bonding

16. Metals conduct heat because.....
Metallic Bonding
Metals conduct heat because.....
Metals conduct heat because.....
Metallic Bonding

17. Dr Brown’s Chemistry. http://www. docbrown
Great quizzes to quickly test yourself. Only look at the parts of the specification you need to (Higher, or triple) Make sure you go to the edexcel IGCSE link
Chemguide
Good videos and revision notes. Make sure you go to the edexcel IGCSE link
Knockhardy publishing
Great power points but not IGCSE specific, a good place to get clear explanations
FROG
Past papers and mark schemes a must! Also revision power points and notes.

18. Metals conduct heat because.....
Metallic Bonding
Metals conduct heat because.....
Metals conduct heat because.....
Electrons pick up energy and move throughout the structure.
As electrons move heat energy is transferres
Metallic Bonding

19. Metals are ductile and malleable because.....
Metals are made of an array of positive metal ions and a sea of delocalised electrons
The Metal ions are arranged in layers
3. When a force is applied layers can slide over each other
The attraction between the ions and electrons remains e.g. The metallic bonds are still there
Metallic Bonding
Metallic Bonding

20. Ductile-draw into a wire

21. Ductile-draw into a wire

22. Independent work Use page 25 draw a labelled diagram of an alloy
Explain how alloys can make a metal harder
Name 3 alloys and for each one give a property and use.
Exam paper

23. Alloys

24. Complete the past paper
Mark your past paper writing down the correct answer.

25. Metallic bonding Plenary How did I get on ?
To be able to describe and draw the metallic bonding
To know the properties of metals
To relate the properties of metals to their structure
Extension to practise past exam paper questions on metallic bonding
Extension to comparing types of bonding.