A. A. Why study chemistry? 1. 1. Chemistry 2. 2. Matter CHEMISTRY I. Introduction B. B. Definitions.
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Transcript of A. A. Why study chemistry? 1. 1. Chemistry 2. 2. Matter CHEMISTRY I. Introduction B. B. Definitions.
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A. Why study chemistry?
1. Chemistry2. Matter
CHEMISTRYI.
IntroductionB. Definitions
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3. Elements
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4. Molecule
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5. Compound
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Figure 2.3
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Figure 5.3
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A. Particles / Structure
II. Atomic Chemistry
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Figure 2.5
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B. Atomic & Mass Number
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C. Isotopes & Radioisotopes
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Figure 2.7
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Isotopes = more neutrons but stable
Radioisotopes = nucleus decay giving off alpha and beta particles, plus gamma rays.
Decay = half life
Why would this activity be so bad for cells?
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E. Electrons
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Figure 2.8
Figure 2.9
Figure 2.6
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Figure 2.10
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Atom No. Electrons Sub shell Electron Configuration Ion No. Electrons Sub shell Electron Configuration
H 1 1s1 H- 1 + 1 = 2 1s2
He 2 1s2
Li 3 1s2 2s1 Li+ 3 - 1 = 2 1s2
Be 4 1s2 2s2 Be2+ 4 - 2 = 2 1s2
B 5 1s2 2s2 2p1 B3+ 5 - 3 = 2 1s2
C 6 1s2 2s2 2p2 C4+ 6 - 4 = 2 1s2
N 7 1s2 2s2 2p3 N3- 7 + 3 = 10 1s2 2s2 2p6
O 8 1s2 2s2 2p4 O2- 8 + 2 = 10 1s2 2s2 2p6
F 9 1s2 2s2 2p5 F- 9 + 1 = 10 1s2 2s2 2p6
Ne 10 1s2 2s2 2p6
Na 11 1s2 2s2 2p6 3s1 Na+ 11 - 1 = 10 1s2 2s2 2p6
Mg 12 1s2 2s2 2p6 3s2 Mg2+ 12 - 2 = 10 1s2 2s2 2p6
Al 13 1s2 2s2 2p6 3s2 3p1 Al3+ 13 - 3 = 10 1s2 2s2 2p6
Si 14 1s2 2s2 2p6 3s2 3p2 Si4+ 14 - 4 = 10 1s2 2s2 2p6
P 15 1s2 2s2 2p6 3s2 3p3 P3- 15 + 3 = 18 1s2 2s2 2p6 3s2 3p6
S 16 1s2 2s2 2p6 3s2 3p4 S2- 16 + 2 = 18 1s2 2s2 2p6 3s2 3p6
Cl 17 1s2 2s2 2p6 3s2 3p5 Cl- 17 + 1 = 18 1s2 2s2 2p6 3s2 3p6
Ar 18 1s2 2s2 2p6 3s2 3p6
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Valence => number of electrons in the outermost shell
Figure 2.9
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Electronegativity degree of attraction for electrons
Figure 2.9
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A. Definition
1. Definition2. Types
III. Molecular Chemistry
B. Chemical Bonds
a. Electron Sharing
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i. Covalent bonds = sharing of valence electrons
Figure 2.11
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Non-polar covalent bonds
Figure 2.12
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Polar
Figure 2.13
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Figure 2.15
Figure 2.14
ii. Ionic = giving and receiving electrons
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b. Hydrogen Sharing
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Hydrogen bonds sharing a hydrogen
Figure 2.16
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Hydrogen bonds sharing a hydrogen
Figure 3.2
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c. VanderWalls Forces
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VanderWalls Forces sharing a charge
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1. Why Important?C. Formulas & Models
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Figure 2.17
Figure 2.18
c. Structural
b. Empirical
a. Molecular
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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
AB + H2O A(OH) + B(H)
AB + CD AC + BD
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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
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H-Bonding Potential
Figure 3.2
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Density
Figure 3.6
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Cohesive Forces
Figure 3.4
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Cohesive ForcesFigure
3.3
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2. Uses
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Solvent
Figure 3.6Figure 3.8
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Temperature Stabilizer or Regulator
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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 concentration
HCl + NaOH NaCl + H2O (Sodium Hydroxide)
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pH Scale measures the hydrogen ion concentration
Figure 3.10
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A buffer regulates the pH of a solution
HCO3- + H+ H2CO3
HPO4-2 + H+ H2PO4
-
NH3 + H+ NH4+
How does acid precipitation affect vegetation?
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Knowledge will always forbear over stupidity.