1. Why Study Chemistry in Biology?

2. I. The Atom A. Definition: smallest particle of an element
BOTH FOR LIVING AND NON LIVING
A. Definition: smallest particle of an element

3. B. Composition Proton +1 1 Nucleus Neutron Electron -1
Subatomic Particle
Charge
Mass
Location
Proton +1 1
Nucleus
Neutron
Electron -1
1/1840 the mass of a proton
Orbiting nucleus

4. outermost electrons participate in BONDING
Location of Electrons
outermost electrons participate in BONDING

5. II. Elements A. Definition: substance that cannot be broken
down into other substances
B. Biologically important elements
i. Major: C H O N P S
(Carbon, Hydrogen, Oxygen, Nitrogen, Phosphorus, Sulfur)

6. Radioactive Isotopes
Thyroid- Uses Iodine- If use an isotope they can trace how much iodine is picked up
Reactor Radioisotopes (half-life indicated)
Iodine-125 (60 d): Used in cancer brachytherapy (prostate and brain), also diagnostically to evaluate the filtration rate of kidneys and to diagnose deep vein thrombosis in the leg. It is also widely used in radioimmuno-assays to show the presence of hormones in tiny quantities.
Iodine-131 (8 d)*: Widely used in treating thyroid cancer and in imaging the thyroid; also in diagnosis of abnormal liver function, renal (kidney) blood flow and urinary tract obstruction. A strong gamma emitter, but used for beta therapy.
Radioisotopes can be manufactured in several ways. The most common is by neutron activation in a nuclear reactor- add or remove neutrons
nucleus of a radioisotope usually becomes stable by emitting

7. Radioactive bairum- white drink- xrays examine stomach esophagous

8. Bohr Atomic Model

9. Atoms Space

10. Why if atoms have so much space can we be solid?
DO NOW
Why if atoms have so much space can we be solid?

13. III. Chemical Compounds
A. Compound definition:
a substance containing two or more
elements in a fixed ratio
Ex: H2O, NaCl, CO2

14. B. Bonds: complete share exchange
Atoms want to fill their outer energy
levels to be
To do this, they will meet up with other atoms and either or
electrons
complete
share
exchange

15. C o v a l e n t B o n d : s h a ri n g I s c a r I n g
Atoms share electrons

16. Examples of covalent molecules

17. ii. Ionic Bonds: gimme’ that electron!
Atoms transfer electrons, becoming (+) or (-) charged
The attraction brings them together
Ex: Na+ and Cl- = NaCl!

18. JOKE- Don’t Have to write this.
A NEUTRON walks into a diner and sits down to order a meal.
When the waitress brings the food over the neutron says “Can you bring the check? I am in a hurry!”
The waitress replies, “Don’t worry about it, there is NO CHARGE for you.”

19. JOKE- Don’t have to write this.
Two atoms walk down the street and collide.
One atom says to the other, “Are you okay?”
The second atom replies, “I think I lost an electron.”
The first atom says, “Are you sure?”
The second one says, “Yeah, I’m POSITIVE!”

21. iii. Molecules definition: two or more atoms held together by COVALENT bonds

22. LIFE DEPENDS ON THE UNIQUE PROPERITIES OF WATER
V. WATER
LIFE DEPENDS ON THE UNIQUE PROPERITIES OF WATER
Use water ppt from chemistry

24. Questions to think about
Why do put salt on the roads?
Why do we add salt to a pot of pasta water?
At a higher altitude why must we cook “boil” something longer?

25. Human Composition:
Cells are 70–90% water

26. B. Plant Composition
As much as 95% plants can be made of water

27. C. Formula:
H2O

28. D. Bonds: i. Hydrogen bonds: Hydrogens from one water molecule are
ATTRACTED to the
oxygen of ANOTHER
water molecule: they
develop a weak bond

29. i. Cohesion
1. Definition: Water “sticks” to each other Ex.: Surface tension
1-inch paperclip
over-filled water
3oz Dixie cup
Where did we see this is the lab?

30. Jesus Christ Lizard

31. ii. Adhesion
1. Definition: Water molecules attracted to other molecules.
2. Ex. In trees/plants water goes against gravity
Called capillary action

33. Water is the a Universal Solvent
Water is able to dissolve other Polar & ionic compounds when mixed by causing the ions to break away and surround them.
Water dissolves Salt (Na+Cl-)
DOES THIS BC CHARE
Know that water is your solvent and salt is your solute

34. iii. Temperature and Water
Boiling Point: 100 oC / 212 oF
When you heat molecules move faster
When you cool molecules move slower
Water takes more energy to heat because energy must break hydrogen bonds

35. Does water boil faster if you add salt to it?
Water Boils when it has enough energy for the molecules to leave

36. Freezing Point
0 oC or 32 oF
What would happen if our oceans did not have salt in them?
Why do we put salt on our roads?
Why at effect does salt have on FREEZING POINT?

37. Why is this important for life?
Water Boiling Point
Ethanol Boiling Point

38. Why are higher altitude must we cook “boil” something longer?
Because of the lower atmospheric pressure, water boils at a lower temperature. Boil at 95 degrees not at 100- boil for longer than to get to t

39. Why do we need salt in our ice, when making ice cream? Watch Video

40. LOW DENSITY OF ICE Density- amount of matter in a volume
In most substances the solid state is more dense than the liquid state
Water is the opposite
ICE IS LESS DENSE THAN WATER and will FLOAT

41. LOW DENSITY OF ICE
WHY?
Hydrogen bonds in ice (solid) keep molecules spaced out

42. LOW DENSITY OF ICE Floats
Ice insulates the liquid water below allowing life to persist