1. CH. 2 CHEMISTRY

2. TERMS & CONCEPTS TO KNOW PRIOR TO CLASS– Mostly Bio 1 topics
BASIC CHEMISTRY
Matter: solid, liquid, gas
Energy: Kinetic, Potential energy
Four chemicals of life
Atomic Structure: protons, neutrons, electrons
Atomic number
Isotopes
Compounds, Molecules and Ions
Chemical Bonds: ionic, covalent (polar & nonpolar), hydrogen
Chemical Reactions: reactants and products; synthesis, decomposition, and exchange reactions
Factors affecting chemical reactions: temperature, concentration, particle size, catalysts

3. TERMS & CONCEPTS TO KNOW PRIOR TO CLASS …
Biochemistry
Inorganic and Organic chemicals, pH scale
Polymers & Monomers
Carbohydrates: monosaccharides, disaccharides, polysaccharides
Lipids: glycerol and fatty acids (saturated and unsaturated), phospholipids
Proteins: amino acids, structural levels of proteins (primary, secondary, and tertiary, and quaternary)
Enzymes, active site, denaturation
Nucleic Acids: RNA and DNA; Adenine, Guanine, Cytosine, Thymine; ATP

4. I. Definition of concepts: Matter & Energy
A. Matter:
States of matter:
B. Energy:
1. Types

5. 2. Forms of Energy 3. Energy Conversions Chemical: Electrical:
Mechanical:
Radiant or electromagnetic
3. Energy Conversions

6. C. Composition of Matter: Atoms & Elements92
Atomic Symbol:
4 elements = 96% of body:
PERIODIC TABLE OF ELEMENTS

7. Other Elements
Deficiencies

8. All atoms are electrically neutral
2. Atoms & = Atomic
Structure
a) Nucleus
Protons (p+)
Neutrons (n0)
b) Electrons (e-)
Orbitals
1st = 2 e-
2nd … = 8 e-
All atoms are electrically neutral
Figure 2.1

9. How related to number of electrons: 4. Atomic Mass Atomic mass unit
3. Atomic Number:
How related to number of electrons:
4. Atomic Mass
Atomic mass unit
Figure 2.1

10. D. Isotopes Protons: Neutrons: Symbol: H-1 or ¹H Atomic weight:
The smaller the isotope, the stronger it is held together
Figure 2.3

11. Radioisotopes
*Radioisotope:
Radioactivity—process of spontaneous atomic decay
PET Scan using glucose

12. E. IONS
Cations
Anions
Importance:
Example
ATOM ION
Na Na+ = Cation

13. IONS …
Anions
ATOM ION
Cl Cl-

14. II. How Matter is Combined: Molecules & Mixtures
A. Molecules
Molecular Weight = weight in grams of 6.02 x 10 to the 23 power
Compound
Figure 2.4

15. B. Mixtures 1. Solutions Solvent Solute Concentration Solute Percent
Weight solute per volume of Solvent
iii) Molarity:

16. C. Chemical Bonds Rule: atoms try to get a full shell of electrons for the outer shell 1. Ionic Bonds Na Cl
Sodium atom (Na) (11p+; 12n0; 11e–)
Chlorine atom (Cl) (17p+; 18n0; 17e–)
Figure 2.6, step 2

17. IONS & IONIC COMPOUNDS
Opposite charges attract each other
ATOMS
IONS  Ionic Compound
Na Cl Na Cl-

18. + – Crystals cation anion Na Cl Na Cl
Sodium atom (Na) (11p+; 12n0; 11e–)
Chlorine atom (Cl) (17p+; 18n0; 17e–)
Sodium ion (Na+)
Chloride ion (Cl–)
Sodium chloride (NaCl)
Figure 2.6, step 3

19. 2. Covalent Bonds:
Figure 2.7a

20. 2 Types of Covalent Bonds
a. Non-polar covalent:
b. Polar bonds:
Polar Molecule:
Why chemicals dissolve
in water:
Figure 2.8

21. Example: double bond (Text p. 52)
Figure 2.7b

22. Comparison of Ionic, Polar & Nonpolar Covalent Bonds
Figure 2.9

23. 3. Hydrogen Bonds
Between: Molecules/compounds, not individual atoms in one molecule or compound
Created by: Polarity
Strength of Bond:
Figure 2.9

24. III. Chemical Reactions A
III. Chemical Reactions A. The Role of Energy in Chemical Reactions chemical energy
Figure 2.10a

25. B. Characteristics of Chemical Reactions. - Reactants. - Products
B. Characteristics of Chemical Reactions Reactants Products - Chemical Equations Na Cl  NaCl Na Cl Na Cl
Sodium atom (Na) (11p+; 12n0; 11e–)
Chlorine atom (Cl) (17p+; 18n0; 17e–)
Sodium ion (Na+)
Chloride ion (Cl–)
Sodium chloride (NaCl)
Figure 2.10a

26. C. Types of Chemical Reactions 1. Synthesis Reactions
Dehydration Synthesis Reaction:
molecule molecule 
OH O O
+ H2O
Figure 2.10a

27. 2. Decomposition Reactions:
a) Hydrolysis Reaction:
H2O
molecule molecule 
O OH O
Figure 2.10b

28. 3. Exchange reaction (AB + CAC + B)
Figure 2.10c

29. 4. Mixed Reactions a) Oxidation-Reduction (Redox) Reactions
Is a Decomposition and Exchange Reaction
Function:
Exchange of: e- and/or hydrogen atoms
Oxidized Reactant:
Reduced Reactant:
Cellular Respiration
C6H12O O2  6CO H2O + ATP
Glucose is oxidized to Carbon Dioxide
Oxygen is reduced to Water

30. D. Reversibility of Chemical Reactions
A + B AB
Indicated by double arrows in opposite directions
Chemical Equilibrium:
Adding or Removing either the reactants or products causes:
An increase in a substance causes:
A decrease in a substance causes:
Example: H2CO HCO H+
If more H+ (acid) is added, then:
If a base is added that reacts with H+, then:

31. E. Factors Influencing the Rate of Chemical Reactions Temperature Concentration Pressure Catalysts - Enzymes

32. Biochemistry I. Inorganic Compounds Types of Chemicals
Examples:
Biochemicals
Inorganic compounds:

33. a) Lubricant/cushioning b) Heat Sink
I. Inorganic Compound …
A. WATER = 60-80%
1. Functions
a) Lubricant/cushioning
b) Heat Sink
c) Chemical Reactions ( text p. 59)
Dehydration Synthesis
Hydrolysis
d) Solvent of living things forming Mixtures
1 Solutioins
Solvent
Solute
Concentration of Solutions:
% solute = (amount solute)
(total amount)
X 100%

34. Concentrations of Solutions …
Milligrams per deciliter of solution
Molarity = moles/liter
1 mole = 6.02 x molecules of a substance
2 Colloids
3 Suspensions

35. B. SALT: ionic compounds not having H+ or OH-
C. ACIDS and BASES
1. Have H+ and OH-
2. Proton (H+) donors and acceptors
3. pH
pH scale

36. 4. BUFFERS—chemicals that can regulate pH change
Are composed of a weak acid and its weak base
Example: Carbonic acid—Bicarbonate system
H2CO3 ----- HCO H+
If H+ is added to the solution:
If OH- is added to the solution:
Figure 2.12

37. II. Organic Compounds Essential to Human Functioning
Carbon & Covalent Bonding
Macromolecules
Polymers and Monomers:
A. Carbohydrates
1. Elements:
2. Functions:
3. Saccharides = Sugars
4. Three Forms
a) Monosaccharides
# carbons
Glucose
Fructose

38. Formation & Decomposition: Sucrose Lactose Maltose (malt sugar)
4. Three Forms …
b) Disaccharieds
Formation & Decomposition:
Sucrose
Lactose
Maltose (malt sugar)
c) Polysaccharides
Glycogen
Starch
Cellulose
Glycogen

39. 5. Isomers
Isomers Glucose
Glucose

40. 6. Combined w other Biochemicals Glycolipids
Glycoproteins
Glycolipid
Galactose
Lipid

41. B. Lipids 1. Contain Elements: Ratio 2. In water 3. Functions:
4. Formation:
5. Types
a) Triglycerides (fat)

42. Triglycerides = Neutral Fats Composition
4. Types …
Triglycerides = Neutral Fats
Composition
Saturated vs. Unsaturated vs. Trans Fats
Omega-3 fatty acids
Phospholipids =
Function
Steroids
Prostaglandins P

43. Structure of amino acid
C. Proteins R
1. Subunit =
Elements:
NH2 (amine) and COOH (carboxyl)
R- group:
Formation
2. Peptide Bond: dehydration synthesis
Dipeptide, …
Polypeptide
Figure 2.16

44. 3. Structural Levels of Proteins (Text p. 73)
Primary:
Secondary:
Often Fibrous
Figure 2.18a–c

45. Structural Levels of Proteins …
Tertiary:
Globular
Fibrous
Quaternary:
Figure 2.18b,d,e

46. 4. Protein Denaturation =
Figure 2.19b

47. 5. over half body’s organic matter 6. Combine with other biochemicals
Glycoproteins & Proteoglycans
Lipoproteins
7. Functions:
Build Structures
Movement
Hormones
Antibodies
Buffers
Transport substances across the
cell membrane or through blood
Enzymes  details next slide
Collagen
Hemoglobin

48. 7. Functions … Enzymes and Enzyme Activity
General Function–Catalyst
Characteristics of Enzymes
Shape
Recycling
Cofactors and
Coenzymes
“ase” ending
Mechanism of
Action  Next Slide
Reactants
Enzyme
Products

49. Mechanism of Enzyme Activity
Active site
Amino acids
Enzyme (E)
Enzyme-substrate
complex (E-S)
Substrates (S) +
1 Enzyme-Substrate Complex
Substrate
Active Site
2 Internal Rearrangement
Breaking of bonds & Formation of new bonds
Energy of Activation
3 Release of Product
Figure 2.21

50. + Active site Amino acids Enzyme (E) Enzyme-substrate complex (E-S)
Internal rearrangements
leading to catalysis
Substrates (S)
H2O +
Figure 2.21

51. + Active site Amino acids Enzyme (E) Enzyme-substrate complex (E-S)
Internal rearrangements
leading to catalysis
Dipeptide product (P)
Free enzyme (E)
Substrates (S)
Peptide bond
H2O +
Figure 2.21

52. D. Nucleic Acids 1. Nucleic Acids = 2. Types: DNA and RNA 3. Elements
4. Nucleotides:
Phosphate
Monosaccharide
Nitrogenous Base
Purines: Adenine and Guanine
Pyrimidines: Cytosine, Thymine, and Uracil
5. Dehydration Synthesis: sugar of one nucleotide to phosphate of another nucleotide
6. Overview of DNA and RNA

53. 6. Overview of DNA and RNA DNA Nitrogenous Bases:
Purines: A and G are two ring bases
Pyrimidines:T, C, and U have one ring bases
Sugar =
Double Helix
Complementary bases
Function
RNA
U replaces T
Single stranded
Types
Released mRNA
Hydrogen Bonds
RNA Molecule

54. 7. Other Related Chemicals Adenosine Triphosphate (ATP)
Function:
Hydrolysis of phosphates
Food + O2 + ADP + Pi ATP + CO2
Phosphorylation
ATP + H2O ADP/AMP + Pi + Energy
energy transfer
energy released

55. Adenosine Triphosphate (ATP) …
Membrane protein P P
Solute
Solute transported
(a)
Transport work
Released Energy is used for:
ADP
ATP + P
Relaxed muscle cell
Contracted muscle cell
(b)
Mechanical work P X P X Y + Y
Reactants
Product made
(c)
Chemical work
Energy liberated during oxidation of food fuels used to regenerate ATP
Figure 2.21

56. END

57. REVIEW QUESTION
1. What is the atomic number and atomic mass of each of the above atoms?

58. Review Question
What sort of chemical reactions do you suppose would be happening during digestion?
What about when your body is making more bone?

59. Review Question
5. What are the 4 major groups of biological organic molecules? What is a major function of each?

61. REVIEW QUESTION
What are 2 variables that can distort the active site of an enzyme and what is the distortion process called?
Dysfunctional
Enzyme

62. REVIEW OF Ch. 1
1a.
1b.
1 a-d. Identify the indicated regions of the body.
1c.
1d.

63. 2. What is the primary organ found in the right hypochondriac region? 3. Name an organ found in hypogastric region?

64. 4. When the response to the effect of a stimulus is in the opposite direction it is called _______________ Feedback.