1. Organic Molecules
Mrs. Woodard arnold

2. The Universal Solvent – WATER
Day One
The Universal Solvent – WATER

3. Background Information
Atom- basic unit of matter
Proton and neutron- subatomic particles in the nucleus
Electron- subatomic particle in charge of bonding on the outside of the nucleus
Covalent Bond- Bond in which electrons are shared
Ionic Bond- bond in which electrons are donated or received
Hydrogen bond- bond caused by differences in charges on a polar covalent molecule

4. Why is water So important?
Water is polar which makes it the universal solvent
Hydrophilic – polar substances that are easily dissolved in water (i.e. sugar)
Hydrophobic – nonpolar substances that are not easily dissolved in water (i.e. oil)
Has a neutral pH (acidity vs. basicity)
Water forms H+ and OH- ions

5. Why is Water So Important?
Water has a high specific heat so it can help normalize temperature changes
Specific heat is how much heat is required to change the temp of a substance by 1 degree
Water floats when it freezes

6. Why is Water So Important?
Cohesion and Adhesion –
Water is attracted to water molecules
Water is attracted to other substances
Allows for molecules to synthesized or hydrolyzed
Synthesis – put together
Hydrolysis – break apart

7. pH scale Compares how acidic substances are Closer to 0 is more acidic
Closer to 14 is more basic

8. Buffers
Weak acids or bases in a cell that serve as protection against changes in pH
Our blood is a buffer solution maintaining a neutral pH of about 7.35 – very close to waters pH

9. Most Important Elements to Living Things:
C, H, N, O, P, S
Carbon
Hydrogen
Nitrogen
Oxygen
Phosphorous
Sulfur

10. Bell Ringer __________________ is the basic unit of life.
__________________ is a weak acid or base that protects a solution from changes in pH
______________, __________________, _________________, ________________, _________________, and _______________ are the most important elements of life.

11. Day Two
MACROmolecules

12. Organic Compounds Compounds that contain hydrogen and carbon
Macromolecules are LARGE organic compounds

13. Carbon Carbon has 4 electrons in outer shell
Carbon can form covalent bonds with as many as 4 other atoms (elements)
Usually with C, H, O or N
Example: CH4(methane)

14. Macromolecules Large organic molecules Also called POLYMERS
Made up of smaller “building blocks” called MONOMERS
Examples:
1. Carbohydrates
2. Lipids
3. Proteins
4. Nucleic acids (DNA and RNA)

15. How are macromolecules made?

16. Dehydration Synthesis
Also called “condensation reaction”
Forms polymers by combining monomers by “removing water”.

17. How are macromolecules separated or digested?

18. Hydrolysis
Separates monomers by “adding water”

19. Bell Ringer
Macromolecules are separated or digested through _____________________.
______________________ ______________________ creates macromolecules.
Carbon contains ____________ electrons in its outer shell which allows for it to make ____________ bonds with four other molecules.

20. Carbohydrates and Lipids
Day Three
Carbohydrates and Lipids

21. Recap: 4 types of organic Compounds
Carbohydrate
Lipids
Proteins
Nucleic Acids

22. Carbohydrates Most carbohydrates are sugars
Sugar suffix – ose
Ex. Glucose, Sucrose, Fructose (high fructose corn syrup)
Glucose is the most important organic molecule in the human body!

23. Carbohydrates (cont.) Elements in carbohydrates are always:
C:H:O – Carbon:Hydrogen:Oxygen
1:2:1 Ratio
Ex. C6H12O6
Monomers – Monosaccharides
Ex. Glucose, Fructose, galactose
Polymers – Polysaccharides
Ex. Chitin, Cellulose

24. Polysaccharides Have two uses:
Used as short term energy storage for the human body
Are the FIRST source of energy for the body
Used as structure
Chitin – fungi cell wall, exoskeleton of arthropods
Cellulose – plantae cell wall, fiber in our body

25. Examples of Carbohydrates
Bread, pasta, rice, potatoes, sugar, fruits, vegetables

26. Lipids Elements- C, H, O contains more carbon and hydrogen than oxygen
Monomer Glycerol and 3 Fatty Acids (triglyceride)
Examples - fats, waxes, oils, steroids

27. Lipids Uses of lipids Second source of stored energy Cell membrane
Insulation
Steroid which forms cholesterol
Male and female hormones

28. Examples of Lipids
Butter, Cooking Oil, Lard, Milk Products like Ice Cream, Cheese and Sour Cream

29. Fatty Acids
Fatty acids are identified as have a carboxyl group in their chain

30. 3 Types of Lipids Fats Phospholipids Steroids
Saturated Fats - No double bonds so they stack well forming solid lipids
Unsaturated Fats - Double bonds do not stack well forming liquids
Phospholipids
Steroids

31. Saturated Fats
Saturated fats are bad for the human body because they solidify in the blood vessels
Solid saturated fats form plaque that clogs arteries (arteriosclerosis)

32. Arteriosclerosis
leads to high blood pressure, heart attacks (blockage to heart) and strokes (blockage to brain)
Trans Fats - worst kind include extra hydrogens
Manufacturers add hydrogens to vegetable oils making them able to stack, increasing their melting point and shelf life

33. Bell Ringer
________________ ____________ have no double bonds and stack nicely in the body which can lead to ________________.
Carbohydrates have a ratio of ____________ meaning that if C6 then H =___ and O= _______________.
The suffix for sugar is always _____________.

34. Proteins and Nucleic Acids
Day 4
Proteins and Nucleic Acids

35. Proteins Proteins are also called polypeptides
Proteins are amino acids
There are 20 amino acids but the human body can only manufacture 11 of them
9 amino acids must be ingested into the body

36. Proteins Elements- C, H, O, N, and sometimes S Monomers- Amino Acids
Examples-
insulin, human growth hormone, hemoglobin
Proteins are the body’s last energy source

37. Amino Acid Shapes

38. Uses of Proteins Last energy source for the body Building Blocks,
Component of Cell Membrane
ENZYMES
Antibodies
Some hormones
Hair & nails

39. Proteins in Food
Eggs, Nuts, Peanut Butter, Meat, Soy Beans

40. Nucleic acids Elements- C, H, O, N, P Monomers- Nucleotides Examples-
DNA-Deoxyribonucleic Acid
RNA-Ribonucleic Acid

41. Uses of Nucleic Acids
Uses- Genetic Material that codes for the production of proteins
Nucleotide has three parts:
5 carbon sugar
Phosphate Group
Nitrogen Base

42. Bell Ringer ______________ are the monomers that make up DNA and RNA.
_______________, ___________________, _______________________ are examples of proteins in the BODY.
A nucleotide is made up of three parts a _______________ base, a _____________ sugar, and a ______________ group.

43. Enzymes and molecule formation
Day 5
Enzymes and molecule formation

44. Enzymes Reminder – ENZYMES are PROTEINS
Enzymes lower the energy of activation
Energy of Activation – energy required to start a reaction
Enzymes are specific – they only fit a certain substrate
Lock in key model
Catalysts – speed up a chemical reaction without changing in the process

45. Lowering the Activation Energy

46. Lock and Key Model

47. 3 Factors Affecting Enzyme ActivitypH
Denature - enzyme active site changes shape and can no longer bind with the substrate.
Enzyme will denature at the wrong pH which is enzyme specific.

48. 3 Factors Affecting Enzyme Activity
Temperature
Molecules move faster when they are warm, slower when they are cool
they bump into the substrate more frequently
Too high, will cause the enzyme to denature (change shape) and the substrate can not bind with the active site

49. 3 Factors Affecting Enzyme Activity
Concentration of Enzyme or Substrate
The more enzyme, the greater the chance of the substrate bumping into it.
Increases the rate of the reaction until all of the substrate has been used.
The more substrate, the greater the chance of the enzyme bumping into it.
Increases the rate of the reaction until all the enzymes have substrate in them and the reaction will level off

50. Carbohydrates Structure

51. Protein Structure

52. Lipid/Triglyceride Structure