1. The Chemistry of Life:  The nature of matter  Properties of water

2. Atoms Basic unit of matter Greek (atomos)  unable to be cut Subatomic particles  protons, neutrons, electrons Nucleus  protons and neutrons

3. Elements and Isotopes  Elements  a pure substance that consists entirely of one type of atom Number of protons= element’s atomic#  Isotopes Same element  different number of neutrons (same chemical properties) Atomic mass # = weighted average mass of the isotopes  Radioactive Isotopes Nuclei are unstable and break down at a constant rate Can be used as a dating tool, treatment for cancer, food sanitation, tracers to follow movement in bodies.

4. Chemical compounds and bonds  Compound – Formed by the chemical combination of 2 or more elements in definite proportions Example: C 6 H 12 O 6 (glucose)  Chemical bonds: Ionic bonds  Electrons are transferred from one atom to another Covalent bonds (strongest bond)  Electrons are shared between atoms  Forms molecules Van der Waals Forces  Intermolecular forces – an attraction between oppositely charged regions of nearby molecules

5. Computer Modeling:  Intermolecular forces Use the handout from this activity as notes.

6. The water molecule  Polarity Uneven distribution of electrons between the H and O atoms Hydrogen end  slightly positive Oxygen end  slightly negative  Hydrogen bonds Negative to positive attractions btw molecules Strongest bond that can form btw molecules Cohesion = attraction between molecules of the same substance (ex. Water on a penny) Adhesion = attraction between molecules of different substances (ex. meniscus)

7. Solutions and Suspensions  Mixture = 2 or more elements or compounds physically mixed (not chemically) 2 types = solutions and suspensions  Solutions Components are evenly distributed Solvent (dissolves the solute) ex. water Solute (substance that is dissolved) ex. salt  Suspensions Mixtures of water and nondissolved material Movement keeps material suspended  Blood  solution and suspension! Made of mostly water with many dissolved components (solution) Also contains nondissolved material like blood cells (suspension)

8. Acids, Bases, and pH

9.  pH scale = factor of 10 btw steps  Acids (strong acid = 0/weak acid = 6) Forms H + ions in solution The higher the concentration of H +  more acidic  Bases (strong base = 14/weak base = 8) Forms OH- ions in solution and low concentrations of H+ The lower the concentration of H +  more basic  Buffers Weak acids or bases that can react with strong acids and bases to prevent sharp changes in pH Helps to maintain homeostasis in the body (pH of the body = 6.5 – 7.5)

10. Computer Modeling:  Properties of Water and hydrogen bonding: Use the handout from this activity as notes.

11. Chemistry of Life  Carbon compounds  Chemical Reactions and Enzymes

12. The chemistry of carbon  Organic chemistry: The study of all compounds that contain carbon Can form single, double, or triple covalent bonds with other carbon molecules  Macromolecules: Monomers – small organic compound units Polymers – many monomers strung together 4 groups = carbohydrates, lipids, nucleic acids, and proteins

13. Carbohydrates  Main energy source for living things  Can also be used for structural purposes (ex. cell wall in plants)  Made up of C, H, and O  ratio of 1:2:1  Monomer = glucose (sugar molecule) or monosaccharides  Polymer = starch or polysaccharides

14. Computer Modeling:  Carbohydrates: Use the handout from this activity as notes.

15. Carbohydrate Constructed Response (formative assessment)  How do intermolecular attractions play a role in the behavior of polysaccharides? Be sure to include how starch and cellulose compare in your response.

16. Lipids (fats)  Generally not soluble in water  Used to store energy, found in membranes, waterproof coverings, and used as chemical messengers  Typically = glycerol molecule combined with fatty acid molecules  Saturated – maximum # of hydrogen bonds (no double bonds) in a fatty acid  Unsaturated – at least one carbon-carbon double bond in a fatty acid

17. Computer Modeling:  Lipids: Use the handout from this activity as notes.

18. Caption: Write captions that explain what is happening to the phospholipids in the two pictures. In Water:In Oil: Caption:

19. Bellwork (for the next day): True or False: Water and Oil repel each other. Why do you think that?

20. Protein  Contain N, C, H, O  Some proteins control the rate of reactions (enzymes), regulate cell processes, form bone and muscle, cell transport, and fight disease  Monomer = amino acids  Polymer = polypeptide or protein

21. Computer Modeling:  Proteins: Use the handout from this activity as notes.

22. Nucleic Acids  Contains H, O, N, C, and P  Stores, transmits hereditary/genetic information  2 kinds = RNA and DNA  Monomer = nucleotide (a 5C sugar, phosphate group, and a nitrogenous base)  Polymer = polynucleotide or nucleic acid

23. Chemical Reactions  A process that changes one set of chemicals into another Always involves the breaking and formation of bonds  Reactants Enter into a reaction Bonds are broken  Products Result from a reaction New bonds are formed

24. Energy in Reactions  Energy changes Release energy  spontaneous Absorb energy  needs energy to proceed  Where does this energy come from in plants? Animals?  Activation energy Energy needed to get a reaction started

25. Activation energy: Energy-Absorbing ReactionEnergy-Releasing Reaction products Reactants Activation energy products Reactants

26. Enzymes  Catalyst = substance that speeds up a chemical reaction  Lowers activation energy  Type of Protein

27. The graphs to the left show the same reaction: X + Y  XY, where X reacts with Y, producing XY. A student gives the opinion that Graph A requires less energy to start the reaction. Is this student right or wrong in their interpretation of the graphs? Interpret what the graphs show (including whether the reaction is energy releasing or energy absorbing) and why the student was right or wrong.