CHAPTER 2 CHEMISTRY COMES ALIVE

1
CHAPTER 2CHEMISTRY COMES ALIVE
2

• I. BASIC CHEMISTRY DEFINITION OF CONCEPTS MATTER
  AND ENERGY
• 1. matter
• 2. energy
• a. potential
• b. kinetic

3
FORMS OF ENERGY

• 1. chemical energy
• a. ATP
• 2. electrical energy
• 3. mechanical energy
• 4. radiant energy
• 5. conversion of one form to another results in a
  "loss" - entropy

4
COMPOSITION OF MATTER ATOMS AND ELEMENTS

• 1. atoms
• 2. elements
• 3. periodic table
• a. atomic symbol

5
ATOMIC STRUCTURE

• 1. nucleus
• a. protons
• b. neutrons
• 2. electrons
• a. orbital model

6
(No Transcript)
7
(No Transcript)
8
IDENTIFYING ELEMENTS

• 1. atoms of different elements have different
  numbers of protons, neutrons electrons
• 2. atomic number
• 3. mass number
• a. isotopes
• 4. atomic weight - average of relative weights if
  all isotopes of an element, taking into account
  their relative abundance in nature
• 5. radioisotopes
• a. half-life

9
(No Transcript)
10
HOW MATTER IS COMBINEDMOLECULES AND MIXTURES

• 1. molecule
• 2. compound
• 3. mixtures
• 4. solutions - homogeneous mixtures
• a. solvent
• b. solute

11
MIXTURES

• 1. solution concentrations
• a. percent - parts of solute per 100 parts of
  solvent
• b. molarity - moles per liter
• 1. mole - amount of a substance, in grams, equal
  to its molecular weight
• 2. Avogadro's number - one mole of any substance
  contains exactly the same number of solute
  particles (6.02 x 1023 )

12
MIXTURES

• 2. colloids - heterogeneous mixtures
• a. sol-gel transformations - cytosol
• 3. suspensions - heterogeneous mixtures with
  large visible solutes

13
DISTINGUISHING MIXTURES FROM COMPOUNDS

• 1. none of the properties of atoms or molecules
  are changed in a mixture
• 2. substances in a mixture can be separated by
  physical means
• 3. homogeneous heterogeneous

14
CHEMICAL BONDS

• 1. chemical bonds
• 2. electron shells - energy levels (2,10,18)
• 3. octet rule (valance shell - outermost energy
  level)

15
(No Transcript)
16
(No Transcript)
17
CHEMICAL BONDS

• 1. ionic bonds
• a. ions
• b. anion (-)
• c. cation ()
• 2. covalent bonds
• a. nonpolar molecules
• b. polar molecules - due to shape
• 3. dipole - water

18
(No Transcript)
19
(No Transcript)
20
CHEMICAL REACTIONS

• 1. chemical reaction
• a. chemical equations
• 1. reactants
• 2. products
• 3. molecular formula

21
PATTERNS OF CHEMICAL REACTIONS

• 1. synthesis reaction
• a. a b ----gt ab
• b. anabolic
• 2. decomposition reaction
• a. ab ----gt a b
• b. catabolic

22
(No Transcript)
23
PATTERNS OF CHEMICAL REACTIONS

• 3. exchange or displacement reactions
• a. ab c ----gt ac b
• b. ab cd ----gt ad cb
• 4. oxidation reduction reactions
• a. oxidation - electrons lost or donated
  (oxidized)
• b. reduction - electrons accepted (reduced)

24
(No Transcript)
25
ENERGY FLOW IN CHEMICAL REACTIONS

• 1. exergonic reactions
• 2. endergonic reactions

26
REVERSIBILITY OF CHEMICAL REACTIONS

• 1. all are theoretically reversible
• 2. major direction indicated by length of arrow
• 3. chemical equilibrium

27
FACTORS INFLUENCING RATE OF REACTIONS

• 1. velocity of particle movement
• 2. particle size
• 3. temperature
• 4. concentration
• 5. catalysts
• a. enzymes

28
II. BIOCHEMISTRYWATER

• 1. inorganic compounds - no carbon
• 2. water
• a. high heat capacity
• b. high heat of vaporization
• c. polarity/solvent properties
• 3. universal solvent
• a. hydration layers (f2.11, p40)
• b. association/dissociation
• c. biological colloids - polar proteins water

29
(No Transcript)
30
WATER

• 4. reactivity
• a. hydrolysis reactions
• b. dehydration synthesis
• 5. cushioning

31
SALTS

• 1. an ionic compound with cations other than H
  and anions other than OH-
• 2. electrolytes
• a. kidneys important in electrolyte balance

32
(No Transcript)
33
ACIDS AND BASES

• 1. acid - sour react with metals release H
• a. proton donors
• 2. base - bitter slippery release OH-
• a. proton acceptors
• 3. pH - concentration of hydrogen ions expressed
  in moles per liter (molarity)
• 4. neutralization
• a. neutralization reaction - reaction of acids
  and bases to form salts and water

34
ACIDS AND BASES

• 5. buffers
• a. acidity reflects only free H
• b. strong acids - dissociate completely
  irreversibly in water
• c. weak acids
• d. strong bases
• e. weak bases
• f. carbonic acid -bicarbonate system
• H2CO3 lt----------gt HCO3 H

35
ORGANIC COMPOUNDS

• 1. all contain carbon (except CO, CO2 and
  carbides)
• a. carbon is electroneutral
• 2. carbohydrates
• a. 1-2 of cell mass
• b. C,H,O - HO is 21
• c. monosaccharides
• 1. isomers - glucose, galactose, fructose
• d. disaccharides
• 1. sucrose glucose fructose
• 2. lactose glucose galactose
• 3. maltose glucose glucose

36
(No Transcript)
37
(No Transcript)
38
CARBOHYDRATES

• e. polysaccharides
• 1. polymer
• 2. starch vs. glycogen
• f. functions
• 1. immediate source of cellular energy
• 2. used on cell membranes as "signs" -
  glycoproteins

39
(No Transcript)
40
LIPIDS

• 1. insoluble in water soluble in lipids and
  organic solvents
• 2. C,H,O - HO gt 21
• 3. classified by solubility (table 2.2, p48)
• a. neutral fats
• b. phosopholipids
• c. steroids

41
LIPIDS

• 4. neutral fats - (triglycerides) - fats and oils
  made of glycerol and fatty acids
• a. saturated
• b. unsaturated
• c. saturated fats cholesterol - arteriosclerosis

42
(No Transcript)
43
LIPIDS

• 5. phosopholipids - modified triglycerides with 2
  fatty acids (hydropHobic) and a pHospHate group
  (hydropHilic)
• 6. steroids - used hydrocarbon rings instead of
  chains
• a. cholesterol - essential for membranes
  hormones, vitamin D bile salts

44
(No Transcript)
45
(No Transcript)
46
PROTEINS

• 1. 10-30 of cell mass
• 2. amino acids
• 3. peptide bonds
• 4. macromolecules

47
(No Transcript)
48
PROTEINS

• 5. structural levels
• a. primary - linear sequence
• b. secondary - twisted and folded - alpHa helix
  beta pleated sheet
• c. tertiary - folded secondary structure
• d. quaternary - aggregates of two or more
  polypeptide units

49
(No Transcript)
50
PROTEINS

• 6. fibrous proteins - (structural) - extended
  strand like usually secondary but may be
  quaternary (collagen)
• 7. globular proteins - (functional) - compact
  spHerical usually tertiary or quaternary
  (antibodies hormones)
• 8. protein denaturation
• a. results when temp. or pH causes unfolding and
  loss of shape
• b. active sites

51
(No Transcript)
52
PROTEINS

• 9. enzymes
• a. globular proteins biological catalysts
• b. speed up reaction rates up to 1 million times
• c. cofactor - enzymes ions
• d. coenzyme - enzymes vitamins
• e. -ase ending
• f. activation energy is reduced
• g. induced fit model

53
(No Transcript)
54
NUCLEIC ACIDS

• 1. DNA - (table 2.4, p57)
• a. nucleotides
• b. DNA
• 1. deoxyribose sugar
• 2. A G - purines
• 3. T C - pyrimidines
• 4. complementary bases
• 5. double helix

55
NUCLEIC ACIDS

• 2. RNA
• a. ribose sugar
• b. single strand
• c. uracil

56
NUCLEIC ACIDS

• 3. ATP - Adenosine Triphosphate (f2.23, p58)
• a. high energy bonds

57
(No Transcript)
58
CLINICAL TERMS

• 1. acidosis - low pH of blood (lt7.35)
• 2. alkalosis - high pH of blood (gt7.45)
• 3. heavy metals - metals with toxic effects
• 4. ionizing radiation - causes atoms to ionize
  (x-rays, radioisotopes)
• 5. ketosis - acidosis from excessive ketones due
  to breakdown of fats (starvation, diabetes
  mellitus)
• 6. radiation sickness