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. Chemistry as it related to biology
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 chem rxn
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
(mass)
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

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. A carbon with eight rather than six neutrons is unstable; it releases rays and subatomic particles and is a radioactive isotope.
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?
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
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. S orbital: innermost, hold 2 elections
E. Electrons and Energy 1. 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. B. Ionic Bonding
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

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

23. C. Covalent Bonding Strongest type of bond
Covalent bonds: when two atoms share electrons so each atom has octet of electrons in the outer shell.
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. In nonpolar covalent bonds, sharing of electrons is equal = no charge
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 bonds create surface tension.
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

32. water 1. High Specific Heat 2. High heat of vaporization
Examples of charts
Property
Explanation
Importance
Example
1. High Specific Heat
2. High heat of vaporization
3. Universal solvent
4. Cohesive and Adhesive
5. Ice Floats
water
Property 1
Property 2
Property 3
Property 4
Property 5
Explanation
Pg 29-31
example

33. 1. All living things are 70.90% water.
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.

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.

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

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
not water… Ice floats!
H bonds form a crystal
allowing life to survive the winter
Ice! I could use more ice!
Most (all?) substances are more dense when they are solid, but not water…
Lower density as a solid = Ice floats!
H bonds form a crystal
And this has made all the difference!

40. Hydrophobic vs Hydrophilic

41. 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 1 2 3 4 5 6 7 8 9
Amount of base added
Buffering
range pH
Exercise = acidic in muscles
CO2 = carbonic acid
lactic acid
body uses buffers to counter act this

42. BICARBONATE BUFFER SYSTEM:
H2O + CO2  H2CO3  HCO3 -+ H+
HCO3- = Bicarbonate (weak base)
H2CO3 = Carbonic acid (weak acid)
Major buffer system in blood
Maintains blood pH between 7.38 and 7.42

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 OH ions; thus, its pH is neutral. 3. Water dissociates into hydrogen and hydroxide ions: 

44. Acid molecules dissociate in water, releasing hydrogen ions (H+) ions: HCl ¨ H+ + Cl-.
Bases are 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..

46. Acids Base Substances with hydrogen ions (H+) Taste sour
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 10 times less H+
10–1
H+ Ion
Concentration
Examples of Solutions
Stomach acid, Lemon juice 1 pH
100
Hydrochloric acid
10–2 2
10–3
Vinegar, cola, beer 3
10–4
Tomatoes 4
10–5
Black coffee, Rainwater 5
10–6
Urine, Saliva 6
10–7
Pure water, Blood 7
10–8
Seawater 8
10–9
Baking soda 9
10–10
Great Salt Lake 10
10–11
Household ammonia 11
10–12
Household bleach 12
10–13
Oven cleaner 13
10–14
Sodium hydroxide 14
pH Scale
tenfold change in 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+
In pure water only 1 water molecule in every 554 million is dissociated
tenfold change in 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 gonna earn a Darwin Award!
Any Questions?

51. 1. The only atom that has a nucleus with no neutrons is _________.
A) argon
B) carbon
C) oxygen
D) hydrogen
2. Which of the following elements is NOT one of the six that make up 98% of most organisms' body weight?
A) hydrogen
B) nitrogen
C) carbon
D) iron

52. Which of the following statements is true?
A) All isotopes give off subatomic particles.
B) All isotopes are radioactive.
C) All isotopes have the same number of protons.
D) All isotopes have the same number of neutrons.
What type of bond is formed when atoms share electrons?
A) ionic
B) covalent
C) hydrogen

53. The three isotopes of carbon 12C, 13C and 14C have different numbers of _______?
A) electrons
B) protons
C) neutrons
The combined number of ___________ will determine the number of electrons in orbital(s) around a neutral atom.
A) orbitals
B) neutrons
C) bonds
D) protons

54. If an atom has an atomic number of 17 and an atomic mass of 35, the number of neutrons in its nucleus equals _____.
A) 17
B) 18
C) 52
Which bond is most easily broken?
A) a hydrogen bond
B) a triple covalent bond
C) a single covalent bond

55. Which of the following statements is true?
A) There are two polar covalent bonds in water.
B) There are two ionic bonds in water.
C) There is one ionic and one covalent bond in water.
D) Electrons are less attracted to oxygen than hydrogen.
The two parallel strands of DNA are held together by _______ bonds.
A) nonpolar
B) hydrogen
C) ionic
D) covalent

56. The calcium ion (Ca2+) _____.
A) has accepted two protons
B) has given away two electrons
C) will form a covalent bond with the chlorine ion (Cl-)
D) All of these
Hydrogen bonds form when ___________.
A) atoms share electrons
B) a slightly negative atom is attracted to a slightly positive atom
C) atoms gain electrons
D) atoms lose protons

57. Which of the following has a basic pH?
A) lemon juice
B) milk of magnesia
C) tomatoes
D) hydrochloric acid
Aquatic living things are able to survive the winter thanks to which property of water?
A) It is less dense as a solid than as a liquid.
B) It is cohesive and adhesive.
C) It is the universal solvent.
D) It resists changes of state (from liquid to ice or liquid to steam).

58. Hydrophobic molecules tend to be _________.
A) nonpolar
B) inorganic minerals
C) ionic
D) water soluble