a. definitions 1. chemistry 2. matter chemistry i. introduction
TRANSCRIPT
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
Knowledge moves you towards your goal.