A. Definitions 1. Chemistry 2. Matter CHEMISTRY I. Introduction.
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Transcript of A. Definitions 1. Chemistry 2. Matter CHEMISTRY I. Introduction.
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A. Definitions
1. Chemistry2. Matter
CHEMISTRYI.
Introduction
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Anything that occupies space and has mass.
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3. Energy
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a. Potential
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b. Kinetic
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c. FormsChemicalElectrical
Mechanical
Radiant
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4. Elements
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A. Particles
II. Atomic Chemistry
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Figure 2.1
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B. Structure
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Figure 2.2
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C. Atomic & Mass Number
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D. Isotopes & Radioisotopes
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Figure 2.3
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Isotope = atom with more neutronsRadioisotopes neutrons measurably decay giving off radiation (alpha and beta particles, plus gamma rays)Decay Rate = half life
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E. Electronegativity & Valence
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Electronegativity => degree of attraction for electrons Valence => number of electrons in the outermost shell
Figure 2.5
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A. Definition
1. Definition2. Types
III. Molecular Chemistry
B. Chemical Bonds
a. Electron Sharing
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i. Ionic bonds giving and taking of electrons
Figure 2.6a
Figure 2.6b
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ii. Polar Covalent bonds unequal sharing
Figure 2.6
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iii. Non-polar covalent bonds equal sharing
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iii. Non-polar covalent bonds equal sharing
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b. Hydrogen Sharing
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Hydrogen bonds sharing a hydrogen atom between molecules
Figure 2.10a
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A. Definition
1. Synthesis, Dehydration, or Anabolic2. Decomposition, Hydrolytic, or Catabolic
IV. Chemical Reactions
B. Types
3. Exchange
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A(OH) + B(H) AB + H2O
CD + H2O C(OH) + D(H)
AB + CD AC + BD
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Figure 2.11
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C. Factors Affecting Rates
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A. Water1.
Properties
V. Inorganic Molecules
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States of Water
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Polar
Figure 2.7
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H-Bonding Potential
Figure 2.8
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Density
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Cohesive Forces
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2. Uses
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Solvent
Figure 2.12
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Temperature Stabilizer or Heat of Vaporization
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B. Salt (Electrolytes)1.
Properties
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2. Uses
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C. Acids, Bases, pH, & Buffers1. Definitions &
Uses
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An acid increases the hydrogen ion concentration
H2CO3 HCO3- + H+
(Carbonic)
H2SO4 H+ + H+ + SO4 2-
(Sulfuric)
HCl H+ + Cl- (Hydrochloric)
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A base decreases the hydrogen ion concentrationHCl + NaOH NaCl + H2O (Sodium Hydroxide)
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pH Scale measures the hydrogen ion concentration
Figure 2.13
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A buffer regulates the pH of a solution
HCO3- + H+ H2CO3
HPO4-2 + H+ H2PO4
-
NH3 + H+ NH4+
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A. Why Carbon?
VI. Organic Molecules
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B. Carbohydrate1.
Atoms2. Arrangement of Atoms
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Carbon, Hydrogen, and Oxygen (CH2O)
Figure 2.12
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Isomers
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3. Types
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a. Monosaccharide = glucose, fructose, galactose, or ribose
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b. Disaccharide = two simple sugars togetherGlucose + Fructose Sucrose +
H2O
Glucose + Galactose Lactose + H2O
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c. Polysaccharides = many simple sugars togetherChitin found in insect
exoskeletons
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4. Biological Uses
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C. Lipids1.
Atoms2. Arrangement of Atoms3. Types
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a. Neutral Fats = glycerol with fatty acid chains (monoglyceride, diglyceride, or triglyceride)
Saturated vs. Unsaturated
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b. Phospholipids = glycerol, two fatty acids, and a polar phosphate group.
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c. Steroids = carbon ringed with attachments giving different properties
Cholesterol
Estrogen Testosterone
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4. Biological Uses
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D. Protein1. Atoms2. Arrangement of Atoms
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Figure 2.15a
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3. Types
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Depends on the amino acid sequence conformatio
n vs. denaturation
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4. Biological Uses
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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.
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E. Nucleic Acids1.
Atoms2. Arrangement of Atoms
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Nucleotides are one of five types adenine, thymine, cytosine, and guanine in DNA, and substitute uracil for thymine in RNA.
Figure 2.17
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3. Types
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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)
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4. Biological Uses
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F. Adenosine Triphosphate1.
Atoms2. Arrangement of Atoms3. Types
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ATP, TTP, GTP, CTP, & UTP
Figure 2.18
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4. Biological Uses
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A. Structure
VI. Enzymes
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B. Function
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1. How enzymes work
Figure 2.20
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1. & Why?
Figure 2.21
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C. Regulation
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1. Competition
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2. Feedback Inhibition
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3. Allosteric Control
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Knowledge moves you towards your goal.