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Chapter 2

Chapter 2. Chemistry of Life. Chemistry Video. http://www.youtube.com/watch?v=m55kgyApYrY. Vocabulary List:. Atom Nucleus Electron Element Isotope Compound Ionic bond Ion Covalent bond Molecule. Q: If you take a stick of chalk and break it in half, are both halves still chalk?. YES.

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Chapter 2

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  1. Chapter 2 Chemistry of Life

  2. Chemistry Video http://www.youtube.com/watch?v=m55kgyApYrY

  3. Vocabulary List: • Atom • Nucleus • Electron • Element • Isotope • Compound • Ionic bond • Ion • Covalent bond • Molecule

  4. Q: If you take a stick of chalk and break it in half, are both halves still chalk? YES NO atomos-unable to cut

  5. ATOM Protons Neutrons Electrons + charge neutral - charge mass mass 1/1840 mass nucleus nucleus space

  6. Element= one type of atom Isotope = atoms of the same element that contain different numbers of neutrons (# of electrons and protons remain constant) If the atomicmass is the sum of protons + neutrons atomicnumber = the # of protons which number changes in an isotope? **Marbles or colored blocks

  7. Compound- substance formed by the chemical combination of 2 or more elements in definite proportions

  8. Atomic Bombs • Nuclear Fission (splitting) of Uranium or Plutonium • Uranium (U) or Plutonium (Pu) = large & unstable (radioactive) • Rapid decay rate --> Release energy needed to hold atom together • Energy release = radiation • Little Boy: 4 tons of fuel = 15 kilotons of TNT Nuclear Fission Video:http://www.youtube.com/watch?v=N7C14UIKuv8

  9. Atomic Bombs continued • Steps: • 1. Explosion from TNT condenses all Pu atoms to “critical mass” • 2. Neutron escapes (energy release) from decaying nuclei and hits another Pu atom • 3. Pu atom that was hit subsequently decays (more energy release) • 4. All the Pu atoms start decaying within seconds

  10. CHEMICAL COMPOUNDS H (gas) + O (gas) Sodium + Chlorine NaCl (table salt) H2O (liquid) Molecule – the smallest unit of compounds whose atoms are joined by covalent bonds

  11. Chemical bonding-involves the electrons surrounding the nucleus of each atom Ionic Bond vs. Covalent Bond Transferring vs. Sharing To do: 2 circles with 8 chairs apiece Q: How can this problem be resolved? Science question: What kind of bond is being modeled?

  12. H20

  13. Dehydration • Water = 50-60% of your body weight • Higher if you have more muscle • Function: • Transport of nutrients and oxygen via bloodstream • Transport white blood cells to fight infection via lymphatics • Rid body of waste • Normal level of H2O loss = 2.5L • 350mL through lungs • 100mL through sweating • 350mL through skin • 1000-2000mL through kidneys

  14. Symptoms of Dehydration: • Headache • Muscle Cramp, Patesthesia (tingling) • Visual Snow • Decreased Blood Pressure (hypotension) • Dizziness/ Fainting upon standing (orthostatic hypotension) • Swelling of Tongue • Sunken eyes • Low urine output • Decreased Heart & Respiratory Rate • Tired • Dry skin • Decreased Metabolism

  15. H2O An oxygen atom has 8 protons Each hydrogen atom has 1 proton 10 protons = 10 shared electrons But will one part of the compound have a greater pull on those electrons? Yes/No…..why? Polar molecules have an uneven distribution of electrons

  16. Slight Negative Charge Water’s Polarity Slight Positive Charge

  17. hydrogen bonding -the attraction between water molecules • 2 polar ends attract each other • A weak bond between the H of one atom and the O of another in water (or any electroneg…) • H20 can hydrogen bond with 4 other H20 molecules

  18. Properties of Water Universal Solvent-due to its polarity -Salts, sugars, acids, bases -Hydrophobic vs hydrophilic

  19. Water Expands When It Freezes Liquid Water Solid Water (Ice) Water becomes less dense due to hydrogen bonds forming between the water molecules, which line up molecules less efficiently (in terms of volume) when water is frozen. http://expertvoices.nsdl.org/polar/2009/02/03/teaching-about-snowflakes-a-flurry-of-ideas-for-science-and-math-integration/ http://cc.oulu.fi/~nmrwww/comp_res4.html

  20. Structure of Ice

  21. COHESIVE and ADHESIVE • Cohesion-attraction to H20 molecules • Adhesion-attraction of H20 molecules to other surfaces

  22. Cohesion Causes Surface Tension

  23. Adhesion

  24. Adhesion (Capillary Action) http://discovermagazine.com/2003/mar/featscienceof http://www.sciencebuddies.org/science-fair-projects/project_ideas/PlantBio_p033.shtml

  25. DRILL-need to have read 1) Draw a molecule of water, indicating its polarity. 2) Explain the truth of the statement: Water can be considered the universal solvent due to its polarity WE NEED A BREAK! Outside…

  26. Dehydration synthesis- build up by removing water Hydrolysis-break down by adding water

  27. Mixture – composed of 2 or more elements/compounds that are mixed physically but not chemically combined Solution – the components are evenly distributed with the solute dissolved in the solvent ex: salt water 2) Suspension – mixture of water and nondissolved material ex: blood is both a suspension (cells) and solution

  28. Acids, Bases and pH pH scale – a measure of the H+ concentration in solution

  29. Lower ph = more H+ Higher ph = fewer H+ ***Pure water is always neutral H2O H+ + OH- in equal amounts Acid-any compound that forms H+ in solution (HCl in the stomach = pH 2.5) Base-any compound that produces OH- in solution (bleach = pH 12.5)

  30. LAB- are foods acidic or basic?

  31. Organic Molecules-study of all compounds that contain bonds between carbon atoms methane isooctane **C-C bonds allow for long chains…Large and complex structures! **4 valence electrons…binds with many other elements

  32. MACROmolecules- giant moleculespolymerization polymers monomers-may be identical/repeating or different

  33. RECALL………Dehydration Synthesis vs Hydrolysis

  34. Dehydration synthesis- build up by removing water Hydrolysis-break down by adding water

  35. 4 ORGANIC MOLECULES

  36. CARBOHYDRATES • Ends in –ose • General formula C1:H2:O1 • Carbohydrate – “carbon hydrate” when CO2 reacts with water to form glucose • major source of ENERGY for all living organisms • source of structural support (plants) Monosaccharide ex. glucose, fructose and galactose Disaccharide ex. Lactose, sucrose Polysaccharide ex. Gycogen, starch and cellulose

  37. Simple vs. Complex Carbohydrates

  38. Simple vs. Complex Carbohydrates Starch 1. stored energy for the plant 2. starch in potatoes, refined wheat and white products are quickly converted into glucose in the body Cellulose 1. major component of plant cell walls 2. does NOT provide energy nor is it digested by our bodies 3. called fiber in our diets & is critical for a healthy digestive system Glycogen 1. animal starch 2. stored form of glucose in our bodies 3. stored in liver to remove glucose from the blood And your resident dietician says…………why?

  39. LIPIDS • Not a polymer- all lipids are grouped together because • hydrophobic- • “scared of water”/ little or no affinitiy for water • ex. You will see oil separate from vinegar in salad dressing

  40. Fats 1. Greasy, oily or waxy to the touch 2. Can be solid or liquid at room temperature 3. If excess calories are consumed, excess stored as fat 4. Stores vitamins and other chemicals 5. Form of insulation for the organism B. Phospholipids-membranes in & around the cells C. Waxes 1. Keep oganism or parts or organisms waterproof & protected 2. Ear was, wax on duck feather D. Steroids 1. Cholesterol a. important component of cell membranes b. harmful if too much in the diet or bloodstream 2. Hormones a. estrogen, progesterone and testosterone control reproductive function b. Anabolic steroids – illegally used to build up muscles - cause serious damage to hear, liver and kidneys

  41. And your resident dietician says………… EXTRA CREDIT: Describe these terms in detail & provide examples: saturated fat unsaturated fat Due: next class

  42. PROTEINS • Amino acid – monomer • Made up different combinations of 20 amino acids • a. 12 nonessential amino acids • b. 8 essential amino acids • Complete proteins-contain all 8 essential amino acids • ex. Meat, eggs, dairy products, fish and tofu • Vegetables have some but not all • a. must be eaten in combination • b. complementary foods (rice and beans) – • together provide a complete protein • Cells recombine aa to build the • proteins necessary for function

  43. Protein = “first or primary”

  44. -some are acidic/basic -polar/nonpolar

  45. LAB: FOOD ANALYSIS

  46. BOGGLE When the timer begins, try to construct as many words as possible using the given letters. You may go in any direction, but not diagonally. Think & write quickly!!!

  47. NUCLEIC ACIDS • Nucleotide - monomer; • - phosphate group, 5 carbon sugar and nitrogenous base • Nucleotides covalently bind to form a nucleic acid • Nucleic acids store and transmit genetic information • 4 Types of nucleotides (A-T/U-C-G) = endless # of different molecules • 2 Types of Nucleic Acids = DNA and RNA

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