1. Inorganic Chemistry Atoms – Smallest unit of matter Elements – Different types of matter –92 in nature, 15 in life, 4 major elements in life Molecules – 2 or more atoms ex) H 2, O 2, N 2 Compounds – 2 or more elements ex) H 2 O

2. Atomic Structure Particles – protons +, electrons -, neutrons n Nucleus – contains protons & neutrons Energy levels – electrons orbit nucleus –1 st – 2 electrons max –2 nd – 8 electrons max –3 rd – 8 electrons max

3. Characteristics of atoms Atomic Number - # of Protons = # of Electrons Atomic Mass - # Protons + # Neutrons What atoms like to be….. 1) Neutral 2) Full outer energy level

4. Elements of Life Hydrogen – 1 proton, 0 neutrons, 1 electron –1 outer electron (1 needed) Carbon – 6 protons, 6 neutrons, 6 electrons –4 outer electrons (4 needed) Nitrogen – 7 protons, 7 neutrons, 7 electrons –5 outer electrons (3 needed) Oxygen – 8 protons, 8 neutrons, 8 electrons –6 outer electrons (2 needed)

5. Electron Configuration

6. Isotopes Different forms or the same element – Carbon 14 vs. Carbon 12 –Hydrogen 2 or 3 vs. Hydrogen 1 –Nitrogen 15 vs. Nitrogen 14 –Oxygen 18 vs. Oxygen 16 Tracers – use of radioisotopes to trace chemical pathways in living things.

7. Isotopes

8. Chemical Bonding Covalent Bonds Ionic Bonds Hydrogen Bonds

9. Covalent Bonding Covalent bonding – sharing electron pairs Single – share 1 pr. of electrons (H 2 ) Double – share 2 prs. of electrons (O 2 ) Triple – share 3 prs. of electrons (N 2 )

10. Methane

11. Polar Covalent Bonds Unequal sharing of the electrons creates partial charges on the molecule –Ex) Water Hydrogen bonds form between partial positive and negative charges on atoms

12. Ionic Bonding Ionic bonding – transfer of electrons from one atom to another atom. –Ex) NaCl -  Na+ & Cl- Ions – charged atoms or groups of atoms

13. Ionic Bonds

14. Salt dissolves in water

15. Organic Chemistry Compounds found in living things. Contain C,H,O, but based on carbon. Form long chains, branched chains, rings. 4 Types: Carbohydrates Proteins Lipids Nucleic Acids

16. Carbohydrates Characteristics Contain C, H, O & H:O ratio = 2:1 Primary energy source for living things. Form ring structures Names end in –ose.

17. Carbohydrates Building Blocks Monosaccharide ex) Glucose – C 6 H 12 O 6 Galactose, Fructose Isomers – Different forms of the same molecule Disaccharide ex) Maltose, Lactose, Sucrose C 12 H 22 O 11 Dehydration Synthesis – Remove water to make a larger molecule. Polysaccharide ex) Starch, Cellulose, Glycogen

18. Monosaccharides

19. Dehydration Synthesis

20. Lipids Characteristics Contain C,H,O, but much less oxygen Cell membranes, secondary energy source Lipids are NOT soluble in water Common examples: Fats, oils, waxes

21. Lipids Building Blocks Glycerol + 3 Fatty Acids Glycerol has 3 –OH groups Fatty Acids have –COOH group Dehydration Synthesis removes 3 waters.

22. Lipid formation

23. Fatty Acid Chains Saturated –Maximum # of hydrogen atoms Unsaturated –1 double bond, 2 less hydrogens Polyunsaturated –Many double bonds, much fewer hydrogens Cholesterol – forms from saturated F.A.’s

24. Fatty Acid Chains

25. Proteins Characteristics Contain C,H,O,N (S) Cell structures, pigments, hormones, antibodies, contractile materials, enzymes. Forms: helixes, folded chains, globular. Names end in _______.

26. Proteins Building Blocks Amino Acids – 20 different types Central carbon atom Amino group –NH 2 Acid Group –COOH Single Hydrogen 20 different ® groups

27. Charged Amino Acids

28. Polar & Special Amino Acids

29. Hydrophobic Amino Acids

30. Proteins Dipeptide – 2 Amino acids Dehydration synthesis forms peptide bond. Polypeptide – many amino acids.

31. Dehydration Sysnthesis

32. 4 levels of structural organization 1) Order of amino acids 2) Initial folding (helix, sheets) 3) Folding of folds (globular) 4) Multiple polypeptide chains together 3-D shape determines protein function Hydrogen bonds hold molecule in it’s shape

33. 3.5 – Part 1 Figure 3.5 – Part 1 figure 03-05a.jpg

34. 3.5 – Part 2 Figure 3.5 – Part 2 figure 03-05b.jpg

35. Enzymes Proteins that act as catalysts to speed up chemical reactions in a cell. Active Site – reaction part of enzyme. Substrate – substance enzyme acts on. Lock & key theory – substrate exactly fits into enzyme active site to perform reaction. Enzyme is not affected by the reaction.

36. Characteristics of Enzymes Enzymes are Reusable. Only need a little. Work best at an Optimal Temperature. Work best at an Optimal pH. Rate depends on concentration of both the enzyme and the substrate. Co-enzymes assist enzyme action. Most work inside cells, some outside.