CH. 2 CHEMISTRY

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

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

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

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

C. Composition of Matter: Atoms & Elements 92 Atomic Symbol: 4 elements = 96% of body: PERIODIC TABLE OF ELEMENTS

Other Elements Deficiencies

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

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

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

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

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

IONS … Anions ATOM ION Cl Cl-

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

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

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

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

+ – 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

2. Covalent Bonds: Figure 2.7a

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

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

Comparison of Ionic, Polar & Nonpolar Covalent Bonds Figure 2.9

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

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

B. Characteristics of Chemical Reactions. - Reactants. - Products B. Characteristics of Chemical Reactions - Reactants - Products - Chemical Equations 2Na + Cl2  2NaCl 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

C. Types of Chemical Reactions 1. Synthesis Reactions Dehydration Synthesis Reaction: molecule 1 molecule 2  1 OH O O + H2O Figure 2.10a

2. Decomposition Reactions: a) Hydrolysis Reaction: H2O molecule 1 molecule 2  O OH O Figure 2.10b

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

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 C6H12O6 + 6O2  6CO2 + 6H2O + ATP Glucose is oxidized to Carbon Dioxide Oxygen is reduced to Water

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: H2CO3 HCO3- + H+ If more H+ (acid) is added, then: If a base is added that reacts with H+, then:

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

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

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%

Concentrations of Solutions … Milligrams per deciliter of solution Molarity = moles/liter 1 mole = 6.02 x 10 23 molecules of a substance 2 Colloids 3 Suspensions

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

4. BUFFERS—chemicals that can regulate pH change Are composed of a weak acid and its weak base Example: Carbonic acid—Bicarbonate system H2CO3 ----- HCO3- + H+ If H+ is added to the solution: If OH- is added to the solution: Figure 2.12

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

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

5. Isomers Isomers Glucose Glucose

6. Combined w other Biochemicals Glycolipids Glycoproteins Glycolipid Galactose Lipid

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

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

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

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

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

4. Protein Denaturation = Figure 2.19b

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

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

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

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

+ 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

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

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

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

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

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

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

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

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

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

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

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