Entrance Quiz: Chapters 4 + 5

1. Entrance Quiz: Chapters 4 + 5 1. What are the 4 major macromolecules? 2. A short polymer and a monomer are linked, what is the by-product and term for this process? 3. How many molecules of water are needed to completely hydrolyze a polymer that is ten monomers long? 4. Why are human sex hormones considered lipids? 5. Identify the macromolecule A B C D

2. Entrance Quiz: Chapters 4 + 5 1. What are the 4 major macromolecules? LIPIDS, NUCLEIC ACIDS, PROTEIN, CARBOHYDRATES 2. A short polymer and a monomer are linked, what is the by-product and term for this process? WATER AND DEHYDRATION 3. How many molecules of water are needed to completely hydrolyze a polymer that is ten monomers long? 9 4. Why are human sex hormones considered lipids? THEY ARE HYDROPHOBIC AND NONPOLAR 5. Identify the macromolecule A B C D PROTEIN NUCLEIC ACID LIPID CARBO

3. LIPIDS FUNCTION: Lipids help to store energy, protects organs, insulate the body, and form cell membranes. EXAMPLES:Lipids - include fats, phospholipids, cholesterol and steroids. FOOD SOURCE: Butter, cheese, meats, milk, nuts, oils. STRUCTURE: Monomer is a fatty acid and glycerol. Polymer is a triglyceride

4. PROTEIN FUNCTION: Proteins are used for muscle movement, are part of the cell membrane and are enzymes. EXAMPLES: Amylase, Collagen FOOD SOURCES: Dairy, eggs, fish, meat, nuts, beans. STRUCTURE: Monomer is an amino acid; Polymer is protein in a polypeptide chain Its structure is:

5. There are only 20 amino acids but a million proteins • WHY? • Different lengths • Different combination

6. Carbohydrates FUNCTION: Energy (for Mitochondria) EXAMPLES: Glucose, Starch, Cellulose, Chitin FOOD SOURCES: Sugar, breads, cereal, fruits, milk, pasta, vegetables, rice STRUCTURE: Glucose (monosaccharide) is the monomer. Polyssacharide is the polymer

7. NUCLEIC ACIDS FUNCTION: Transfers genetic information from one generation to the next. EXAMPLES: DNA and RNA FOOD SOURCES: All foods from animals and plants have DNA STRUCTURE: Monomer is a nucleotide (P, S, and B) Its structure is:

8. http://highered.mcgraw-hill.com/sites/0072943696/student_view0/chapter2/animation__protein_denaturation.htmlhttp://highered.mcgraw-hill.com/sites/0072943696/student_view0/chapter2/animation__protein_denaturation.html

9. Make a model to show the primary, secondary, tertiary, a quarternary structure of a proteinMinimum 10 amino acids—pick from each groupYou must have the structure of the amino acids

11. 2nd structure of a proteinH-bondsR groups are NOT involved in H-bonds

12. Tertiary • Interactions with the aqueous solvent, known as the hydrophobic effect results in residues with non-polar side-chains typically being buried in the interior of a protein. • Conversely, polar amino acid side-chains tend to on the surface of a protein where they are exposed to the aqueous milieu.

13. http://bcs.whfreeman.com/thelifewire/content/chp03/0302002.htmlhttp://bcs.whfreeman.com/thelifewire/content/chp03/0302002.html

14. Copy this: “ If I am going to be absent on the day of a test, I will contact Ms. Morris.” TITLE page: Chemistry of Life

15. Chemistry of Life Week 7-8

16. Overview • Living organisms and the world they live in are subject to the basic laws of physics and chemistry. • Biology is a multidisciplinary science, drawing on insights from other sciences. • Life can be organized into a hierarchy of structural levels. • At each successive level, additional emergent properties appear.

17. 2.1 Matter consists of chemical elements in pure form and in combinations called compounds. • Organisms are composed of matter. • Matter is anything that takes up space and has mass. • Matter is made up of elements.

18. 2.1 Matter consists of chemical elements in pure form and in combinations called compounds. • An element is a pure substance that cannot be broken down into other substances by chemical reactions. • There are 92 naturally occurring elements. • Each element has a unique symbol, usually the first one or two letters of the name. Some of the symbols are derived from Latin or German names.

19. 2.1 Matter consists of chemical elements in pure form and in combinations called compounds. A compound is a pure substance consisting of two or more elements in a fixed ratio. • Table salt (sodium chloride or NaCl) is a compound with equal numbers of atoms of the elements chlorine and sodium.

20. Reflect on • Blue green magnets • White-red magnets

21. Essential Elements of Life • Essential elements • Include carbon, hydrogen, oxygen, and nitrogen • Make up 96% of living matter • A few other elements • Make up the remaining 4% of living matter

22. (a) Nitrogen deficiency (b) Iodine deficiency Trace elements • Are required by an organism in only minute quantities • But the absence of trace element can have deadly effects Figure 2.3

23. Radioactive Isotopes • Spontaneously give off particles and energy • Alpha, beta, gamma radiation

24. APPLICATION Scientists use radioactive isotopes to label certain chemical substances, creating tracers that can be used to follow a metabolic process or locate the substance within an organism. In this example, radioactive tracers are being used to determine the effect of temperature on the rate at which cells make copies of their DNA. TECHNIQUE Ingredients including Radioactive tracer (bright blue) Incubators 1 2 3 10°C 15°C 20°C Human cells Ingredients for making DNA are added to human cells. One ingredient is labeled with 3H, a radioactive isotope of hydrogen. Nine dishes of cells are incubated at different temperatures. The cells make new DNA, incorporating the radioactive tracer with 3H. 4 5 6 25°C 30°C 35°C 1 7 8 9 45°C 50°C 40°C The cells are placed in test tubes, their DNA is isolated, and unused ingredients are removed. 2 DNA (old and new) 2 3 4 5 6 7 8 9 1 Biological Uses for Radioactive Isotopes

25. A solution called scintillation fluid is added to the test tubes and they are placed in a scintillation counter. As the 3H in the newly made DNA decays, it emits radiation that excites chemicals in the scintillation fluid, causing them to give off light. Flashes of light are recorded by the scintillation counter. 3 The frequency of flashes, which is recorded as counts per minute, is proportional to the amount of the radioactive tracer present, indicating the amount of new DNA. In this experiment, when the counts per minute are plotted against temperature, it is clear that temperature affects the rate of DNA synthesis—the most DNA was made at 35°C. RESULTS RESULTS Optimum temperature for DNA synthesis 30 20 Counts per minute (x 1,000) 10 0 10 20 30 40 50 Temperature (°C) Figure 2.5

26. Cancerous throat tissue PET(positron-emission tomography)

27. Figure 2.4 Tagging the Brain

28. Covalent Bonds Covalent bonds can be Single—sharing one pair of electrons Double—sharing two pairs of electrons Triple—sharing three pairs of electrons N N C H C C

29. 2.3 The formation and function of molecules depend on chemical bonding between the atoms. Electronegativity: the attractive force that an atomic nucleus exerts on electrons Electronegativity depends on the number of positive charges (protons) and the distance between the nucleus and electrons.

30. Weak Chemical Bonds Hydrogen bonds: attraction between the δ–end of one molecule and the δ+ hydrogen end of another molecule Hydrogen bonds form between H and O and/or H and N. Important with water DNA Proteins

31. Van der Waals Interactions • Van der Waals interactions • Occur when transiently positive and negative regions of molecules attract each other

32. Nitrogen Carbon Hydrogen Sulfur Oxygen Natural endorphin Morphine (a) Structures of endorphin and morphine. The boxed portion of the endorphin molecule (left) binds to receptor molecules on target cells in the brain. The boxed portion of the morphine molecule is a close match. Natural endorphin Morphine Endorphin receptors Brain cell (b) Binding to endorphin receptors. Endorphin receptors on the surface of a brain cell recognize and can bind to both endorphin and morphine. Structure and Function run from large scale body systems through molecules and atoms.Structure and function are what Enzymes are all about Figure 2.17

33. Why do medics pump wounded soldiers with morphine on the battlefield?

34. + 2 H2 + O2 2 H2O Reactants Reaction Product Concept 2.4: Chemical reactions make and break chemical bonds • Chemical reactions • Convert reactants to products

35. Life is the result of Chemical Reactions • Photosynthesis • Is an example of a chemical reaction Figure 2.18

36. Chemical Equilibrium • Chemical equilibrium • Is reached when the forward and reverse reaction rates are equal

37. Take out Water book • Put notes and Hardy Weinberg lab in the center of the table • Make sure there is a post it at the beginning of the lab • If you want to go to a college talk and/or assembly, you MUST have an A or B and no Mi

38. Water: The Molecule That Supports All of Life • Water is the biological medium here on Earth • All living organisms require water more than any other substance • Three-quarters of the Earth’s surface is submerged in water • The abundance of water is the main reason the Earth is habitable

39. – Hydrogenbonds + H – + H + –  – + 3.1: The polarity of water molecules results in hydrogen bonding • The polarity of water molecules • Allows them to form hydrogen bonds with each other • Contributes to the various properties water exhibits

40. 3.2: Four emergent properties of water contribute to Earth’s fitness for life • Cohesion • Moderation of Temperature • Insulation of bodies of water by floating ice • The solvent of life (universal solvent)

41. 1. Cohesion • Cohesion – the hydrogen bonds holding a substance together. (water – water) • Adhesion – the hydrogen bonds holding one substance to another. (water – glass) • Capillary Action – water transport in plants. Uses Cohesion and Adhesion • Transpiration • Surface tension – measure of how difficult it is to stretch or break the surface of a liquid. • Water has a greater surface tensions than most liquids

42. 2. Moderation of Temperature • Kinetic Energy – energy of motion • Thermal Energy (heat) – total energy within a substance • Calorie – amount of heat energy to heat 1g water by 1°C • Kcal – 1000c • Temperature – average kinetic energy per molecule (Celsius Scale)

43. 2. Moderation of Temperature • Specific heat – the amount of heat absorbed or loss for 1g of a substance to change its temperature by 1°C • Water has high specific heat capacity compared to other substances • 1 cal/g/°C

44. 2. Moderation of Temperature • Evaporation • Heat of vaporization – the amount of heat 1g of a liquid must absorb to be converted to a gas • Evaporative cooling – as a liquid evaporates the surface of the remaining liquid cools • This occurs because the “hottest” molecules leave

45. Hydrogen bond Ice Hydrogen bonds are stable Liquid water Hydrogen bonds constantly break and re-form 3. Insulation of bodies of water by floating ice

46. 3. Insulation of bodies of water by floating ice

47. 4. Solvent of Life • Water is claimed to be the universal solvent. • Solution – homogeneous mixture of two or more substances in the same phase • Solute – substance which is dissolved (in case of liquids, substance with the least amount • Solvent – substance which is dissolving another • Aqueous solution – solution involving water • Hydration shell – pocket formed by water molecules in order to dissolve a substance

48. 4. Solvent of life • Hydrophilic – attracted to water • Can be dissolved • Unless molecule is too large • Colloid – stable suspension of fine molecules in a liquid. (blood, milk) • Hydrophobic – repel water • Non-ionic, non-polar, can’t form H-bonds

49. 4. Solvent of Life • Solute concentrations in aqueous solutions • Concentration = g solute / ml solvent • Molarity – moles solute / Liter solution

50. + – H H H + H H H H H Hydroxide ion (OH–) Hydronium ion (H3O+) Figure on p. 53 of water dissociating Acidic and Basic conditions affect living organisms • Water can dissociate • Into hydronium ions and hydroxide ions • H+ (hydrogen ion) is used to represent the hydronium ion • Changes in the concentration of these ions • Can have a great affect on living organisms • Only 1 in 554 mil pure water molecules will diss.