1. Chemistry of Life

2. What is an element? How about an atom??? What is Matter?
Anything that has mass and takes up space
What is an element?
A substance that cannot be further broken down
How about an atom???

3. What are the most common elements of life?
Trace elements?

4. Symptom of an iodine deficiency
Iron deficiency?
Fluoride deficiency

5. Locations and charges of protons?
Neutrons?
Electrons?

6. Arrangement of electrons in the electron shells

7. Atomic number = number of protons in an atom
Atomic mass = number of protons + number of neutrons

8. What makes an atom stable???

10. If an atoms outer electron shell is not full it will react with other atoms (form bonds) in order to fill it
Diagram showing how two hydrogen atoms share a pair of electrons so that each has a filled outer shell
*** COVALENT BOND
Molecular formula (shows how many atoms of each element are present in the molecule)
Structural formula
shows how the different atoms are connected
the solid line connecting 2 atoms indicates a
covalent bond

15. Ionic Bond

16. isotopes

20. pH …. What do you know about this?

21. (Higher concentration of H+) (Lower concentration of H+)
pH scale 1
Battery acid 2
Lemon juice, gastric juice 3
Grapefruit juice, soft drink,
vinegar, beer
(Higher concentration of H+)
Increasingly ACIDIC
Acidic solution 4
Tomato juice 5
Rain water 6
Human urine
Saliva
NEUTRAL
[H+]=OH–] 7
Pure water
Human blood,
tears 8
Seawater
Neutral solution 9
Figure 2.15 The pH scale represents the relative concentration of H+ and OH–. 10
(Lower concentration of H+)
Increasingly BASIC
Milk of magnesia 11
Household ammonia 12
Household bleach 13
Oven cleaner
Basic solution 14

22. Figure 2.15 The pH scale represents the relative concentration of H+ and OH–.

23. Why is pH important?
Different areas of the body have different pH values
Ex: stomach
blood
If the pH varies from this value, proteins lose their shape and don’t work
Role of buffers in the body
Keep the pH in a narrow range (keep pH values steady)

26. Water Electrons are shared, but not shared equally
-spend more time around the Oxygen
-form a POLAR COVALENT bond
(–) O
Figure 2.9 A water molecule. H H
(+)
(+)

27. Hydrogen bond
Figure 2.10 Hydrogen bonds between water molecules.

28. pH In pure water, some water molecules split apart forming
hydrogen ions (H+)
hydroxide ions (OH–)
Teaching Tips
1. Discussions of pH are enhanced by lab activities that permit students to test the pH of everyday items (foods and household solutions). If students do not have opportunities to conduct such tests in labs, consider testing a few items during your class (pH paper or a basic pH meter will, of course, be necessary).
If the water is pure then the amounts of hydrogen ions (H+) is equal to the amounts of hydroxide ions (OH-)

29. pH
If something is added to pure water to disrupt this equality, the substance is an acid or a base
Acids
Have more H+ than OH-
Bases
Have more OH- than H+
Teaching Tips
1. Discussions of pH are enhanced by lab activities that permit students to test the pH of everyday items (foods and household solutions). If students do not have opportunities to conduct such tests in labs, consider testing a few items during your class (pH paper or a basic pH meter will, of course, be necessary).

30. A pH scale is used to describe whether a solution is acidic or basic
pH ranges from 0 (most acidic) to 14 (most basic)
A solution that is neither acidic or basic is neutral (pH = 7)
Teaching Tips
1. Discussions of pH are enhanced by lab activities that permit students to test the pH of everyday items (foods and household solutions). If students do not have opportunities to conduct such tests in labs, consider testing a few items during your class (pH paper or a basic pH meter will, of course, be necessary).

31. Cohesion of water  water sticking to itself
Does this because of hydrogen bonding
Results in water having surface tension
“film” on top of water

32. Temperature moderation
Water resists changes in temperature
Water can absorb and release a lot of heat energy with a small change in temperature

33. Absorbs a lot of energy when heating up
Releases energy when cooling down

34. Adhesion  water sticking to something else
Meniscus

36. Transpiration
Uses cohesion and adhesion to move water from the roots to top of a tree

37. Adhesion of water
To cells of xylem
Cohesion of water to itself

38. Density Water is densest at 4℃ Ice is less dense than liquid water
Provides insulation and allows wildlife to survive under a layer of ice

39. Water is an almost universal solvent
In a solution the SOLVENT is the substance in a greater amount
The SOLUTE is the substance present in a lesser amount
Ionic compounds (like salt) will dissolve in water
Polar molecules will dissolve in water
(sugar)

40. Glucose

42. Ionic Bond Occur when atoms gain or lose electrons, forming ions
Form ions to have outer electron shell full
Ions of opposite charges attract

43. What is an isotope?

44. Isotopes use to diagnose disease
Cancerous throat tissue

45.                                                         The illustration shows the concentration of radioactive tracer bound to monoamine oxidase B (MAO B). Red shows the highest concentration.
MAO B is important because it breaks down the chemicals that allow nerve cells to communicate and regulate blood pressure.

46. Buffers Molecules that can accept or release H+ resist change in pH
Are usually weak acid/base pairs

50. Organic Chemistry

51. Hydrocarbons