1. A Real Diamond Geezer http://news.bbc.co.uk/player/nol/newsid_65000 00/newsid_6504800/6504813.stm?bw=bb&mp= wm&news=1&bbcws=1 This diamond used to be a man: How is this possible?

2. C2 – structures and properties Objectives Giant covalent structures Outcomes I can list some giant covalent structures (E) and describe their properties (C) explain why graphite conducts electricity (A) Key Words; covalent, giant structure, boiling melting point, inter molecular

3. Questions; 1.Which group is carbon in? 2.What is carbons electronic configuration? 3.How many electrons does carbon have? 4.How many protons does carbon have? 5.Draw the electronic structure of carbon 6.How many bonds can carbon make? 7.Name a compound that carbon is in

4. Atoms that share electrons can form giant covalent structures. Examples; Diamond, graphite, fullerenes, silica http://www.yo utube.com/wat ch?v=zQAK4x xPGfM

5. Diamond Properties very Diamond is very hard, transparent. Making it ideal for jewellery. High melting point http://www.youtube.com/watch?v=zQ AK4xxPGfM http://www.youtube.com/watch?v=zQ AK4xxPGfM Chemically unreactive http://www.youtube.com/watch?v= zQAK4xxPGfM/www.youtube.com/ watch?v=zQAK4xxPGfM Each carbon atom forms 4 strong covalent bonds with other carbon atoms. Many bonds to break means a lot of energy is needed to melt it. Useful? Explain http://www.youtube.com/watc h?v=fuinLNKkknI&feature=pla yer_embedded#http://www.youtube.com/watc h?v=fuinLNKkknI&feature=pla yer_embedded#!

6. GIANT COVALENT Diamond is a ______ covalent _______. It has a high ______ & ______ point. Each carbon atoms makes ____ bonds with other _____ atoms. Silica is a ______ covalent ______. Each silicon makes ____ bonds with _____ atoms. Many bonds take a lot of _____ to break them. 3. Graphite is soft and slippery, each carbon makes ___ bonds with other _____ atoms. The spare electron becomes _______ allowing graphite to ______ electricity. 4. Fullerenes are involved with nanoscience technology. They have a ____surface area. They look like _____, they can hold things. This makes them useful for _____ delivery

7. C2 – structures and properties Objectives Simple Covalent compounds Outcomes I can list substances made of simple molecules (E) and describe their properties (C) I can explain why simple molecules have low melting and boiling points (A) Key Words; covalent, simple molecules, boiling melting point, inter molecular

8. Starter; Draw dot and cross diagrams for the following molecules Hydrogen H-H Oxygen O = O Hydrogen chloride H- Cl Water H - O - H What type of bond is this? How does this bond form? What overall charge do these molecule have?

9. Intermolecular forces The covalent bond is not broken, the intermolecular force is, this doesn’t require much energy, this is why simple molecules have low boiling and melting points (grade A)

11. Simple covalent structure (1mark) Share electrons (1 mark) Correct formula of the molecule (1 mark) Draw dot and cross correctly (1mark)

12. Giant metallic Structure force Metals conduct heat and electricity because the electrons are free ‘delocalised’ to carry the charge. Metals are malleable (can bend and be shaped) because the atoms can slide over each other. Page 137

13. Giant Covalent Structures: Diamond: Find an image of the bonding in diamond. Use it to explain why diamond is hard. Give some uses of diamond, and explain how its properties mean that it is good at this job. Graphite: Find an image of the bonding in graphite. Use it to explain: Why graphite is a soft, slippery material. Why it can conduct heat and electricity. Give some uses of graphite, and explain how its properties mean that it is good at this job. Find some more examples of giant covalent structures.