1. Deduce the Lewis structures of molecules and ions for up to four electrons pairs on each atom Predict the shape and bond angles for species with four, three and two negative charge centers on the center atom using the valence shell electron pair repulsion theory (VSEPR) Analyze the physical properties of covalent compounds resulting from single, double and triple bonds Describe and compare the structure and bonding in the three allotropes of carbon; diamond, graphite and fullerene. Describe the structure and bonding of silicon and silicon dioxide

2. DIATOMIC MOLECULES W/ SINGLE BONDS DIATOMIC MOLECULES W/ DOUBLE BONDS DIATOMIC MOLECULES W/ TRIPLE BONDS

3. H O: H : WATER :O= C= O: : CARBON DIOXIDE TWO DOUBLE BONDS CARBON MONOXIDE TRIPLE BOND

4. POLYATOMIC IONS A group of atoms covalently bonded with a charge that form ionic bonds w/ oppositely charged ions AMMONIUM NH4 + HYDROXIDE OH- HYDROGEN CARBONATE CO3 2- SULFATE SO4 2- NITRATE NO3 - CARBONATE CO3 2- PHOSPHATE PO4 3-

5. LOOK AT THE FOLLOWING YOU TUBE VIDEOS FOR STEP BY STEP INSTRUCTIONS ON DRAWING LEWIS STRUCTURES BASIC STEPS TO DRAW LEWIS STRUCTURES http://www.youtube.com/watch?v=PtMifU1py5I POLYATOMIC ION LEWIS STRUCTURES http://www.youtube.com/watch?v=FrICbMseyhs

6. Predict the shape and bond angles for species with four, three and two negative charge centers on the center atom using the valence shell electron pair repulsion theory (VSEPR)

7. http://www.youtube.com/watch?v=sceYMpBrNNo&safe=active http://www.youtube.com/watch?v=xwgid9YuH58 http://www.youtube.com/watch?v=qvPKWcXdo7Y

8. Analyze the physical properties of covalent compounds resulting from single, double and triple bonds DUE TO THE FACT THAT TRIPLE BONDS ARE THE STRONGEST AND SINGLE BONDS ARE THE WEAKEST, IT STANDS TO REASON THAT A MOLECULE WITH A TRIPLE BOND WILL HAVE A MUCH HIGHER MELTING AND BOILING POINT THAN A DOUBLE AND EVEN MORE THAN A MOLECULE WITH A SINGL BOND

9. Describe and compare the structure and bonding in the three allotropes of carbon; diamond, graphite and fullerene. DIAMONDS -hardest substance known to man -brittle (not malleable) -insulator (non-conductor) -insoluble in water -very high melting point GRAPHITE -soft and slippery -brittle -electrical conductor -insoluble in water -very high melting point FULLERENES -soft, slippery and brittle -semi-insulator (conductivity falls between that of graphite and diamond) -Insoluble in water -low melting point solids http://www.youtube.com/watch?v=sUqr6Uk29Z8&safe=active WATCH THE TUTORIAL BELOW FOR MORE INFORMATION

10. Describe the structure and bonding of silicon and silicon dioxide http://www.youtube.com/watch?v=PiYnQLI-ufU&safe=active The structure of silicon dioxide, SiO 2 Silicon dioxide is also known as silicon(IV) oxide. The giant covalent structure of silicon dioxide There are three different crystal forms of silicon dioxide. The easiest one to remember and draw is based on the diamond structure. Crystalline silicon has the same structure as diamond. To turn it into silicon dioxide, all you need to do is to modify the silicon structure by including some oxygen atoms. Notice that each silicon atom is bridged to its neighbours by an oxygen atom. Don't forget that this is just a tiny part of a giant structure extending on all 3 dimensions. T he physical properties of silicon dioxide Silicon dioxide has a high melting point - varying depending on what the particular structure is (remember that the structure given is only one of three possible structures), but around 1700°C. Very strong silicon-oxygen covalent bonds have to be broken throughout the structure before melting occurs. is hard. This is due to the need to break the very strong covalent bonds. doesn't conduct electricity. There aren't any delocalized electrons. All the electrons are held tightly between the atoms, and aren't free to move. is insoluble in water and organic solvents. There are no possible attractions which could occur between solvent molecules and the silicon or oxygen atoms which could overcome the covalent bonds in the giant structure.