1. Carbon Chemistry

2. Properties of Carbon Atomic number is 6 4 valence electrons available for bonding Each carbon atom can form 4 bonds and can combine with itself and other elements in many ways. Carbon atoms can form straight chains, branched chains, and rings.

3. Examples

4. 4 Forms of Pure Carbon 1. Diamond - a crystalline form of carbon in which each carbon atom is bonded strongly to four other carbon atoms. Extremely hard and nonreactive. Melting point is greater than 3500 degrees C (as hot as the surface of some stars)

5. Diamond structure

6. 2. Graphite - each carbon atom is bonded tightly to three other carbon atoms in flat layers. Bonds between layers are very weak, so layers slide past one another easily. Used in lead pencils and is slippery. Makes a good lubricant in machines.

7. Graphite

8. 3. Fullerene - carbon atoms arranged in the shape of a hollow sphere. Made by scientists in 1985. Named after Buckminster Fuller One type of fullerene is called a “buckyball”

9. Buckyball

10. 4. Nanotube - carbon atoms are arranged in the shape of a long, hollow cylinder. Like a sheet of graphite rolled into a tube. Made in 1991. Tiny, light, flexible, and extremely strong. Good conductors of heat and electricity.

11. Nanotube

12. Carbon Compounds More than 90% of all known compounds contain carbon (that’s nearly everything you can think of!) Compounds containing carbon are called Organic compounds. Scientists once thought that organic compounds could only be produced by living things. (Can now be made artificially from petroleum, or crude oil.) Many organic compounds have similar properties in terms of melting points(low), boiling points(low), odor(strong), electrical conductivity(none), and solubility(none).

13. Hydrocarbons Simplest organic compounds. Contain only the elements carbon and hydrogen. Mix poorly with water. Flammable (used as fuels). Simplest is methane (CH 4 ) 2 carbons = Ethane (C 2 H 6 ) 3 carbons = Propane (C 3 H 8 ).

14. Saturated Hydrocarbons A hydrocarbon in which each carbon atom in the molecule shares a single bond with each of four other atoms. Covalent bonds. “saturated” because no other atoms can be added without replacing an atom that is part of the molecule. These are called Alkanes.

15. First 4 Alkanes

16. Unsaturated Hydrocarbons A hydrocarbon in which at least two carbon atoms share a double bond or a triple bond. Double bonded hydrocarbons are called Alkenes Triple bonded hydrocarbons are called Alkynes “unsaturated” because double or triple bond can be broken to allow more atoms to be added to the molecule.

17. Alkenes and Alkynes

18. Aromatic Hydrocarbons Most are based on benzene. Often have strong odors.

19. Other Organic Compounds Alcohols and phenols (antioxidants) Organic acids/ Carboxylic acids (asprin) Esters, thiols, disulfides (anesthetics) Halogen containing (CFC’s) Amines and Amides/ Alkyl halides Aldehdyes and Ketones (Vanilla, formaldehyde, acetone Carbohydrates, Lipids, Proteins, Nucleic acids

20. This weeks Project Nutrition chart

21. Name of food Serving size (you can convert this later) Total calories, fat, carbohydrates, protein, vitamin A, vitamin C, vitamin D, calcium, iron, sodium