1. 4.3. Bonding References:

2. Atoms that bond Covalent bonding occurs when pairs of electrons are shared by atoms (like F 2, H 2, ). Octet Rule: Each atom would then have 8 ( an octet of ) electrons in its last electron shell

3. Nonpolar Covalent Bond: A bond characterized by the equal sharing of a pair of electrons between atoms. Hydrogen molecule (nonpolar covalent ) Chlorine molecule (nonpolar covalent)

4. Polar covalent bond Polar Covalent Bond: A bond characterized by the sharing of one of more pairs of electrons between two different atoms.

5. Determine the atoms with higher electronegativity in water and HCl molecules

6. Single covalent bond Determine the number of the shared electron pairs between one H and C atom

7. Multiple covalent bond Draw the forming of molecules of Oxygen and Carbon dioxide

8. Diamond and Graphite – extended lattice

9. carbon A wonderful image released by Michael Ströck under the GNU Free Documentation License: The structures of eight allotropes of carbon: a) Diamond b) Graphite c) Lonsdaleite d) C60 (Buckminsterfullerene) e) C540 Fullerene f) C70 Fullerene g) Amorphous carbon h) Single-walled carbon nanotube

10. Carbon's most recently discovered allotrope, graphene. Here the graphene surface hosts an indium tin oxide nanoparticle, which helps secure two platinum nanoparticles (blue) for improved catalysis in a fuel cell. Carbon's most recently discovered allotrope

11. Nature Chemistry Volume: 2, Pages: 450–453 Year published: (2010) Nature Chemistry Volume: 2, Pages: 450–453 Year published: (2010) QUANTUM CHEMICAL MODELLING EXPLAINS FOUR CRITICAL STEPS IN A TOP-DOWN MECHANISM OF FULLERENE FORMATION: (I) LOSS OF CARBON ATOMS AT THE EDGE OF GRAPHENE, LEADING TO (II) THE FORMATION OF PENTAGONS, WHICH (III) TRIGGERS THE CURVING OF GRAPHENE INTO A BOWL-SHAPED STRUCTURE AND WHICH (IV) SUBSEQUENTLY ZIPS UP ITS OPEN EDGES TO FORM A CLOSED FULLERENE STRUCTURE. Nature Chemistry 2010

12. Atoms that don’t bond He

13. Look at Table 4.3.3., p. 125 copy the table for the students and work through it

14. A rough diamond prac /fun p.124 Prac p.128 Model building

15. Ionic Bonds form when electrons are transferred from one atom to another, forming charged Ions which are attracted to each other by Electrostatic Forces. Elements tend to loose or gain electrons, forming Ions, to get a 'full other shell'. Ionically bonded substances, such as Sodium Chloride, can from crystals known as Giant Ionic Lattices with bonds forming a network of connections between atoms.

16. Forming a positive ion (cation)

17. Forming a negative ion (anion)

18. Ions – aim to have stable outer shell

19. When substances can conduct electricity? Charges should move Solution of NaCl

20. When substances can conduct electricity? Charges should move

21. Exercises on p. 123 Ese the question: Which electrons are give out? (For example)

22. Precious metals, like gold, are impervious to oxygen. Gold remains lustrous even after being exposed to the elements. (Source: Perth Mint) Metallic bonds are bonds between metal atoms that involve sharing of electrons. Metallic bonds are very flexible, which is why metals can be put into many different shapes.

23. Metal bond

24. Physical properties of metals GOLD is soft, very malleable high melting point and boiling temperature found as solids at normal temperatures high ability to conduct an electric current bend easily (malleable) able to be drawn out into a wire (ductile) shiny when pure.

25. Chemical properties of metals