A. Definitions 1. Chemistry 2. Matter CHEMISTRY I. Introduction
Anything that occupies space and has mass.
3. Energy
a. Potential
b. Kinetic
c. Forms Chemical Electrical 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 neutrons Radioisotopes 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. Definition 2. 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 Anabolic Decomposition, Decomposition, Hydrolytic, Hydrolytic, or or Catabolic IV. Chemical Reactions B. Types 3. Exchange
A (OH) + B (H) AB + H2OH2O CD + H 2 O C (OH) + D (H) AB + CD AC + BD
Figure 2.11
C. Factors Affecting Rates
A. Water 1. 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, & Buffers 1. Definitions & Uses
An acid increases the hydrogen ion concentration H 2 CO 3 HCO H + (Carbonic) H 2 SO 4 H + + H + + SO 4 2- (Sulfuric) HCl H + + Cl - (Hydrochloric)
A base decreases the hydrogen ion concentration HCl + NaOH NaCl + H 2 O (Sodium Hydroxide)
pH Scale measures the hydrogen ion concentration Figure 2.13
A buffer regulates the pH of a solution HCO H + H 2 CO 3 HPO H + H 2 PO 4 - NH 3 + H + NH 4 +
A. Why Carbon? VI. Organic Molecules
B. Carbohydrate 1. Atoms 2. Arrangement of Atoms
Carbon, Hydrogen, and Oxygen (CH 2 O) Figure 2.12
Isomers
3. Types
a. Monosaccharide = glucose, fructose, galactose, or ribose
b. Disaccharide = two simple sugars together Glucose + Fructose Sucrose + H2OH2O Glucose + Galactose Lactose + H2OH2O
c. Polysaccharides = many simple sugars together Chitin found in insect exoskeletons
4. Biological Uses
C. Lipids 1. Atoms 2. Arrangement of Atoms 3. 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. Protein 1. Atoms 2. Arrangement of Atoms
Figure 2.15a
3. Types
Depends on the amino acid sequence conformation 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 Acids 1. Atoms 2. 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, & C Sugars deoxyribose ribose Size huge portion of DNA Location nucleus nucleus & cytoplasm Types one three (mRNA, tRNA, & rRNA)
4. Biological Uses
F. Adenosine Triphosphate 1. Atoms 2. Arrangement of Atoms 3. 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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