a. definitions 1. chemistry 2. matter chemistry i. introduction

A. Definitions

1. Chemistry2. Matter

CHEMISTRYI.

Introduction

Anything that occupies space and has mass.

3. Energy

a. Potential

b. Kinetic

c. FormsChemicalElectrical

Mechanical

Radiant

4. Elements

A. Particles

II. Atomic Chemistry

Figure 2.1

B. Structure

Figure 2.2

C. Atomic & Mass Number

D. Isotopes & Radioisotopes

Figure 2.3

Isotope = atom with more neutronsRadioisotopes neutrons measurably decay giving off radiation (alpha and beta particles, plus gamma rays)Decay Rate = half life

E. Electronegativity & Valence

Electronegativity => degree of attraction for electrons Valence => number of electrons in the outermost shell

Figure 2.5

A. Definition

1. Definition2. Types

III. Molecular Chemistry

B. Chemical Bonds

a. Electron Sharing

i. Ionic bonds giving and taking of electrons

Figure 2.6a

Figure 2.6b

ii. Polar Covalent bonds unequal sharing

Figure 2.6

iii. Non-polar covalent bonds equal sharing

iii. Non-polar covalent bonds equal sharing

b. Hydrogen Sharing

Hydrogen bonds sharing a hydrogen atom between molecules

Figure 2.10a

A. Definition

1. Synthesis, Dehydration, or Anabolic2. Decomposition, Hydrolytic, or Catabolic

IV. Chemical Reactions

B. Types

3. Exchange

A(OH) + B(H) AB + H2O

CD + H2O C(OH) + D(H)

AB + CD AC + BD

Figure 2.11

C. Factors Affecting Rates

A. Water1.

Properties

V. Inorganic Molecules

States of Water

Polar

Figure 2.7

H-Bonding Potential

Figure 2.8

Density

Cohesive Forces

2. Uses

Solvent

Figure 2.12

Temperature Stabilizer or Heat of Vaporization

B. Salt (Electrolytes)1.

Properties

2. Uses

C. Acids, Bases, pH, & Buffers1. Definitions &

Uses

An acid increases the hydrogen ion concentration

H2CO3 HCO3- + H+

(Carbonic)

H2SO4 H+ + H+ + SO4 2-

(Sulfuric)

HCl H+ + Cl- (Hydrochloric)

A base decreases the hydrogen ion concentrationHCl + NaOH NaCl + H2O (Sodium Hydroxide)

pH Scale measures the hydrogen ion concentration

Figure 2.13

A buffer regulates the pH of a solution

HCO3- + H+ H2CO3

HPO4-2 + H+ H2PO4

-

NH3 + H+ NH4+

A. Why Carbon?

VI. Organic Molecules

B. Carbohydrate1.

Atoms2. Arrangement of Atoms

Carbon, Hydrogen, and Oxygen (CH2O)

Figure 2.12

Isomers

3. Types

a. Monosaccharide = glucose, fructose, galactose, or ribose

b. Disaccharide = two simple sugars togetherGlucose + Fructose Sucrose +

H2O

Glucose + Galactose Lactose + H2O

c. Polysaccharides = many simple sugars togetherChitin found in insect

exoskeletons

4. Biological Uses

C. Lipids1.

Atoms2. Arrangement of Atoms3. Types

a. Neutral Fats = glycerol with fatty acid chains (monoglyceride, diglyceride, or triglyceride)

Saturated vs. Unsaturated

b. Phospholipids = glycerol, two fatty acids, and a polar phosphate group.

c. Steroids = carbon ringed with attachments giving different properties

Cholesterol

Estrogen Testosterone

4. Biological Uses

D. Protein1. Atoms2. Arrangement of Atoms

Figure 2.15a

3. Types

Depends on the amino acid sequence conformatio

n vs. denaturation

4. Biological Uses

Proteins vary in function from being Contractile, Defensive, Enzymatic, Signal, Storage, Structural, to Transporter.Everything about a protein’s function is reliant on its conformation, that is dictated by its amino acid sequence.

E. Nucleic Acids1.

Atoms2. Arrangement of Atoms

Nucleotides are one of five types adenine, thymine, cytosine, and guanine in DNA, and substitute uracil for thymine in RNA.

Figure 2.17

3. Types

DNA vs. RNA

Strands double single

Bases A,T,G, & C A, U, G, & CSugars deoxyribose ribose

Size huge portion of DNALocation nucleus nucleus & cytoplasmTypes one three (mRNA, tRNA, & rRNA)

4. Biological Uses

F. Adenosine Triphosphate1.

Atoms2. Arrangement of Atoms3. Types

ATP, TTP, GTP, CTP, & UTP

Figure 2.18

4. Biological Uses

A. Structure

VI. Enzymes

B. Function

1. How enzymes work

Figure 2.20

1. & Why?

Figure 2.21

C. Regulation

1. Competition

2. Feedback Inhibition

3. Allosteric Control

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