1. Biochemistry I: Chemistry Basics

2. I. Basic Concepts/Vocabulary:

3. 1. Matter: anything that occupies space and has mass

4. -4 states of matter
1. Solid
2. Liquid
3. Gas
4. Plasma

5. 2. Mass: the amount of matter an object has
-constant throughout universe

6. 3. Weight: the force of gravity on an object

7. 4. Element: a pure substance which cannot be broken down into simpler kinds of matter

8. -4 types of elements
Non-metals
Metals
Inert (noble) gases
Metalloids

9. II. Periodic Table of Elements

10. -Developed by Dmitri “Wild man” Mendeleev

11. -tabular arrangement by increasing atomic number

12. -organized by rows (periods) and columns (groups)

13. -physical and chemical properties repeat themselves

14. III. Atomic Theory - the atom model

15. Atom: the simplest particle of an element that retains all the properties of that element

16. 3 subatomic particles Proton: (+) charge; nucleus
Neutron: (0) charge; nucleus
Electron: (-) charge; electron cloud
-electron cloud makes up most of the volume
-nucleus makes up the mass

17. Atomic Number: the # of protons in an atom
Atomic # = 7; Nitrogen

18. Atomic Mass: the number of protons plus the number of neutrons

19. Ion: an atom in which protons don’t equal electrons; charged atom
Two Types:
Cation: a positively charged ion (lost electrons)
Anion: a negatively charged ion (gained electrons)
(Neutral atom: protons = electrons)

20. Electrons: high energy particles that pair up in energy levels
Electron Energy Levels: Level Number of Electrons K 2 L 8 M 18 N 32

21. IV. Chemical Bonding 3 Types:
Ionic Bond: bond formed from the attraction of oppositely charged ions
(metal and non-metal)
Covalent Bond: bond formed when atoms share one or more pairs of electrons
(between non-metals)
Hydrogen Bond: bond formed between partially charged molecules

22. Ionic Bond: between metals & non-metals

23. Covalent Bond: between non-metals

24. Hydrogen Bond

25. Compound: combination of atoms from two or more elements

26. V. Chemical Reactions

27. Catalyst: substance that reduces the amount of energy required to activate a reaction
Ex. Enzymes, chlorophyll

28. VI. Solutions

29. Solution: a mixture in which one or more substances are uniformly distributed in another substance
2 Components
Solute: substance dissolved in solution
Solvent: substance in which solute is dissolved

30. Concentration: a measurement of the amount of solute dissolved in a solution

31. Saturated Solution: no more solute can be dissolved

32. Aqueous Solution: a solution in which water is the solvent

33. VII: pH Scale: a scale developed to measure the strength of Acids and Bases
Compares concentrations of hydronium (H+) and Hydroxide (OH-) ions in solution
Range 0 to 14

35. Acid: a compound that releases hydronium (H+) in solution
Properties:
Good conductor of electricity
Sour taste
Reacts with metals
Examples: HCL

36. Base: a compound that releases hydroxide ions (OH-) in solution
Properties:
Conduct electricity
Slippery in solution
Do not react with metals
Examples:

37. Neutralization: making an acid or base neutral by mixing them together
Buffer: chemical substance that neutralize an acid or base solution
Neutralization Reaction: Acid + Base  Salt + water

38. VIII: Water: The Molecule of Life
-Most common chemical compound on Earth - Universal compound in chemical reactions
Properties
Freezing point 0; boiling point 100
Universal solvent
A polarized molecule
Cohesive to allow free flow (transport)
Temp rises and falls slowly
Tends to remain a liquid
Less dense as a solid
Most dense a 4 C

39. Biochemistry II: Biological Macromolecules

40. Most Common Elements in LIfe
Carbon: C
Hydrogen: H
Oxygen: O
Nitrogen: N

41. Two groups of Carbon Molecules:
Monomer: a subunit (building block) of a larger marcromolecule
Polymer: a large molecule of repeating monomers

42. Biological Carbon Compounds:

43. 1. Carbohydrates: organic compounds in which there are twice as many hydrogen atoms as oxygen atoms
3 Types:
Monosaccharide: monomers of carbohydrates that six carbon, simple sugars (glucose – C6H12O6)
Disaccharide: twelve carbon double sugars
Polysaccharide: numerous monosaccharides linked together (cellulose – starch in plants)

44. 2. Lipids: organic compounds that feel greasy and will not dissolve in water
Ex. Fats, waxes, oils, steroids Fatty acids: the monomers (building blocks) of lipids and fats Phospholipids : lipids that consist of a phosphate head and two lipid tails (found in cell membranes)

45. 3. Nucleic Acids – the acids of life
- Found in the nucleus of cells
Contain genetic information
Deoxyribonucleic acid (DNA)
Ribonucleic Acid (RNA)
Monomers are nucleotides
Four bases: Adenine (A), thymine (T), cytosine (C), Guanine (G)

46. 4. Proteins: a polymer formed by linking numerous amino acids together.
Ex. Hemoglobin, enzymes, insulin Amino Acids: monomers of proteins -consist of an amine group and an acid group