QOD: In a group of 4, each pick one paragraph of the article to read. (note: paragraph 2 is the hardest one, the back

1. QOD: In a group of 4, each pick one paragraph of the article to read. (note: paragraph 2 is the hardest one, the back page will be more helpful) When you are done reading, discuss as a group and try to answer the question: Why does the doctor not recommend the use of external cooling (such as ice baths, cold water or even air conditioners) to reduce a fever.

2. 2.1  Chemical Elements Chemistry as it related to biology

3. A. Matter What is matter?

4. Matter “stuff” Made up of elements: substance that cannot be broken down into other substances by a chemrxn Compound: consist of 2 or more elements in a fixed ratio

5. Six elements (C, H, N, O, P, S) make up 98% of living things. • C, H, O and N make up about 96%

6. B. Atomic Structure

7. Periodic Table The atomic mass of an atom is about equal to the sum of its protons and neutrons All atoms of an element have the same number of protons, the atom's atomic number (mass)

8. Interactive Periodic Table  |  Cartoon Periodic Table

9. Isotopes Isotopes are atoms with the same number of protons but differ in number of neutrons; e.g., a carbon atom has six protons but may have more or less than usual six neutrons.

10. Carbon 14  - Break it Down! Carbon- 12 is the most common form of carbon, it has 6 protons, 6 electrons, and 6 neutrons It is called Carbon 12 because that is its weight  (6 + 6 ) Carbon 14 has 2 extra neutrons, its weight is 14  (6 + 8 ); it is an isotope of carbon

11. Sample Question: A 200 g sample of muskopfonian is left in a container , the half life of muskopfonian is 1 hour. How much of the sample will be left after 4 hours? A carbon with eight rather than six neutrons is unstable; it releases rays and subatomic particles and is a radioactive isotope. Answer: 200 x .5 =  100 (hour 1) 100 x .5  =  50  (hour 2)50 x .5 = 25 (hour 3)25 x .5 = 12.5 (hour 4) or 200 x .54 = 12.5

12. Low levels of radiation such as radioactive iodine or glucose allow researchers to trace the location and activity of  the atom in living tissues; therefore these isotopes are called tracers which are used in CAT scans

13.  High levels of radiation can cause cancerous tissues and destroy cells; careful use of radiation in turn can sterilize products and kill cancer cells.

14. Pick your favorite element from the table.  Turn and tell your lab partner what it is, how many protons, electrons and neutrons it has, and what it's atomic weight is.

15. E. Electrons and Energy1. Electrons occupy an orbital at some level near or distant from the nucleus of the atom. S orbital: innermost, hold 2 elections P orbital: after s, holds 8 elections

16. 3. When atoms absorb energy during photosynthesis, electrons are boosted to higher energy levels. 4. The innermost shell of an atom is complete with two electrons; all other shells are complete with eight electrons. 5. The outermost shell is the valance shell, and the number of valance e-in the outermost shell determine many of the atoms properties

17. DRAW IT!     QUICK!! 1. Draw six protons in the nucleus of the atom.  2. Draw six neutrons in the nucleus of the atom. 3. Draw two electrons in the first energy level and label them with their charge. 4. Draw four electrons in the second energy level and label them with their charge. 5. What element is it!? __________                           (the future of the human race depends on it!)

19. 2.2 Elements and Compounds Compounds:When two or more different elements react or bond together, they form a compound (e.g., H2O).  Electrons possess energy and bonds that exist between atoms in molecules contain energy. Glycine

20. Ionic bonds:when electrons are transferred from one atom to another. • Attraction of oppositely charged ions holds the two atoms together in an ionic bond. • Losing or gaining elections gives ions a filled outer shell, so they are more stable • Ex: sodium (Na+) and Chlorine (Cl- ) make NaCl B. Ionic Bonding

21. Cation: positively charged ion anion: negatively charged ion

23. Covalent bonds: when two atoms share electrons so each atom has octet of electrons in the outer shell. C. Covalent Bonding • Hydrogen can give up an electron to become a hydrogen ion (H+) or share an electron with another atom to complete its outer shell of two electrons. • Strongest type of bond

24. Structural formulas represent shared atom as a line between two atoms; e.g., single covalent bond (H-H), double covalent bond (O=O) Carbon has amazing bonding properties, as we will learn in the next chapter on BIOCHEMISTRY

25. Bonds can be represented using structural formation, where a line represent the sharing of 2 elections

26. D. Nonpolar and Polar Covalent Bonds In nonpolar covalent bonds, sharing of electrons is equal= no charge With polar covalent bonds, the sharing of electrons is unequal. = charge Ex: water molecule (H2O), sharing of electrons by oxygen and hydrogen is not equal; the oxygen atom with more protons dominates the H2O association.              *The oxygen then assumes a small negative charge *

27. Hydrogen Bond:weak attractive force between slightly positive hydrogen atom of one molecule and slightly negative atom in another or the same molecule. • Weakest bond • mainly between O, N, F and an atom of hydrogen • Many hydrogen bonds taken together are relatively strong. • Hydrogen bonds between complex molecules of cells help maintain structure and function. Hydrogen bonds create surface tension.

28. Van der Waals Interactions When you have a molecule which is electrically dipolar (equal but opposite in charge) you have attraction between the negative pole of one molecule and positive pole of the other molecule. They are usually weaker than hydrogen bounds but exist in all matter

29. Notice the e- spend more time around the oxygen molecule: it’s has more protons to attract the elections *the shape allows for one side to be more + and the other more -

30. Biological molecules recognize and interact with each other with specificity based on their shape

31. Title: Properties of water In your notebook, create a chart listing the properties of water, and why each property is important. Include example whenever possible use pages 29-31 http://vimeo.com/37064053

32. Examples of charts water Property 1 Property 2 Property 3 Property 4 Property 5 Explanation Pg 29-31 example

33. 2.3. Chemistry of Water A. Facts 1. All living things are 70.90% water. 2. Because water is a polar molecule, water molecules are hydrogen bonded to each other.3. With hydrogen bonding, water is liquid between 0 C and 100 C which is critical for life. http://www.johnkyrk.com/H2O.html

34. B. Properties of Water High Specific Heat: The temperature of liquid water rises and falls more slowly than that of most other liquids. a. Calorie is amount of heat energy required to raise temperature of one gram of water 1o C.b. Because water holds more heat, its temperature falls more slowly than other liquids; this protects organisms from rapid temperature changes and helps them maintain normal temperatures. http://science.howstuffworks.com/environmental/458-how-water-works-video.htm

35. 2. Water has a high heat of vaporization. a. Hydrogen bonds between water molecules require a large amount of heat to break.b. This property moderates earth's surface temperature; permits living systems to exist here.c. When animals sweat, evaporation of the sweat takes away body heat, thus cooling the animal.

36. Organisms rely on heat of vaporization to remove body heat Evaporative cooling Heat of vaporization

37. 3. Water is universal solvent, and facilitates chemical reactions both outside of and within living systems.. a. Water is a universal solvent because it dissolves a great number of solutes.b. Ionized or polar molecules attracted to water are hydrophilic.c. Nonionized and nonpolar molecules that cannot attract water are hydrophobic. Solvents dissolve other substances (solutes) and do not lose their own properties. If we use a simple and easy example, we can get a handle on the idea. Take a glass of warm water, put a teaspoon of table salt in it, and stir it. The salt will dissolve in the water and "disappear" from view. The water is the solvent here, the salt is the solute in this example, and the resulting salt water is a solution that we created. It's that simple.

38. 4. Liquid water is cohesive & adhesive Cohesion= H bonds between water molecules; H2O molecules tend to stick together. Adhesive= ability of water to cling to other polar molecules importance= Higher surface tension Transport H2O against gravity in plants

39. 5. Ice floats • Most (all?) substances are more dense when they are solid, but • notwater… Ice floats! • H bonds form a crystal • allowing life to survive the winter Ice!I could use more ice! And this hasmade all the difference!

40. Hydrophobic vs Hydrophilic

41. 9 8 7 6 Buffering range 5 pH 4 3 2 1 0 0 1 2 3 4 5 Amount of base added Buffers & cellular regulation • pH of cells must be kept ~7 Buffers are solutions used to stabilize the pH of a solution • Control pH by using buffers • reservoir of H+ • donate H+ when [H+] falls • absorb H+ when [H+] rises

42. BICARBONATE BUFFER SYSTEM: H2O + CO2 H2CO3 HCO3 -+ H+ HCO3- = Bicarbonate (weak base) H2CO3 = Carbonicacid (weakacid) Major buffer system in blood Maintainsblood pH between 7.38 and7.42

43. C. Acids and Bases 1. Covalently bonded water molecules ionize; the atoms dissociate into ions. 2. When water ionizes or dissociates, it releases a small (107 moles/liter) but equal number of H+ and OHions; thus, its pH is neutral.3. Water dissociates into hydrogen and hydroxide ions: 

44. Acidmolecules dissociate in water, releasing hydrogen ions (H+) ions: HCl ¨ H+ + Cl-. Basesare molecules that take up hydrogen ions or release hydroxide ions. NaOH ¨ Na+ + OH-. See also:  Acid & Base Coloring

45. 6. The pH scale indicates acidity and basicity (alkalinity) of a solution. 1) One mole of water has 107 moles/liter of hydrogen ions; therefore, has neutral pH of 7.2) Acid is a substance with pH less than 7; base is a substance with pH greater than 7.3) As logarithmic scale, each lower unit has 10 times the amount of hydrogen ions as next higher pH unit; * Buffers keep pH steady and within normal limits in living organisms.. http://www.johnkyrk.com/pH.html

46. Chemistry in Biology Acids Base • Substances with hydrogen ions (H+) • Taste sour • pH lower than 7 • Substances with hydroxide ions (OH–) • Taste bitter • Feel slippery • pH greater than 7 • Examples • Stomach acid • Citrus fruit: orange • vinegar • Examples • Soap • Baking soda • Cleaning products

47. Create a Venn Diagram Comparing Acids and Bases • Stomach acid • Citrus fruit: orange • Soap • Cleaning products • Baking soda • vinegar • Substances with hydrogen ions (H+) • Substances with hydroxide ions (OH–) • Taste sour • Taste bitter • Feel slippery • pH greater that 7 • pH lower that 7 Neutral = pH of 7

48. H+ Ion Concentration Examples of Solutions pH 100 0 Hydrochloric acid 10–1 1 10–2 2 Stomach acid, Lemon juice Vinegar, cola, beer 10–3 3 Tomatoes 10–4 4 10–5 5 Black coffee, Rainwater 10–6 6 Urine, Saliva 7 Pure water, Blood 10–7 Seawater 8 10–8 Baking soda 10–9 9 Great Salt Lake 10–10 10 10–11 Household ammonia 11 10–12 12 Household bleach 10–13 13 Oven cleaner 10–14 14 Sodium hydroxide pH Scale tenfold changein H+ ions pH1  pH2 10-1 10-2 10 times less H+ pH8  pH7 10-8 10-7 10 times more H+ pH10  pH8 10-10 10-8 100 times more H+

49. He’s gonnaearn a Darwin Award! AnyQuestions?