1. CHEMISTRY I. Introduction A. Why study chemistry? B. Definitions
1. Chemistry (study of matter)
2. Matter (mass and space)

2. 3. Element (natural stable particles of matter)

3. 4. Molecule (combining atoms) 5. Compound (atoms in a fixed ratio)
Figure 2.1

4. Figure 3.4B

5. II. Atomic Chemistry
A. Particles / Structure
Figure 2.3A

6. B. Atomic Number & Mass Number

7. C. Isotopes & Radioisotopes
Figure 2.4B
Table 2.3
1. Isotopes = varied number of neutrons but stable
2. Radioisotopes = nucleus decay giving off alpha and beta particles, plus gamma rays.
3. Decay = half life
How and why would this activity be so bad for cells?

8. D. Electrons
1. Shells  electron organization
Figure 2.5

9. Sub shell Electron Configuration
Atom
No. Electrons
Sub shell Electron Configuration
Ion H 1
1s1 H-
1 + 1 = 2
1s2 He 2 Li 3
1s2 2s1
Li+
3 - 1 = 2 Be 4
1s2 2s2
Be2+
4 - 2 = 2 B 5
1s2 2s2 2p1
B3+
5 - 3 = 2 C 6
1s2 2s2 2p2
C4+
6 - 4 = 2 N 7
1s2 2s2 2p3
N3-
7 + 3 = 10
1s2 2s2 2p6 O 8
1s2 2s2 2p4
O2-
8 + 2 = 10 F 9
1s2 2s2 2p5 F-
9 + 1 = 10 Ne 10 Na 11
1s2 2s2 2p6 3s1
Na+
= 10 Mg 12
1s2 2s2 2p6 3s2
Mg2+
= 10 Al 13
1s2 2s2 2p6 3s2 3p1
Al3+
= 10 Si 14
1s2 2s2 2p6 3s2 3p2
Si4+
= 10 P 15
1s2 2s2 2p6 3s2 3p3
P3-
= 18
1s2 2s2 2p6 3s2 3p6 S 16
1s2 2s2 2p6 3s2 3p4
S2-
= 18 Cl 17
1s2 2s2 2p6 3s2 3p5
Cl-
= 18 Ar 18

10. 2. Valence  number of electrons in the outermost shell
Figure 2.5
2. Valence  number of electrons in the outermost shell
3. Electronegativity  degree of attraction for electrons

11. III. Molecular Chemistry
A. Definition
B. Chemical Bonds
1. Definition (how atoms interact)
2. Types
a. Electron Sharing
i. Covalent bonds
Non-polar (equal sharing of e-)
Polar (unequal sharing of e-)
Figure 2.6

12. Table 2.6

13. ii. Ionic (giving and receiving electrons)
Figure 2.7A
Figure 2.7B

14. b. Hydrogen Sharing
Molecules sharing a hydrogen atom
Figure 2.8

15. b. Hydrogen Sharing
Molecules sharing a hydrogen
Figure 2.8

16. c. Charge Sharing
Molecules sharing a charge
i. van der Waals Forces

17. C. Formulas & Models
1. Why Important? (explains structure to function)
2. Types
a. Molecular (atom ratio)
b. Empirical (simplest ratio)
c. Structural (actual shape)

19. IV. Chemical Reactions A. Definition (how they react and why) B. Types
1. Synthesis, Dehydration, or Anabolic
2. Decomposition, Hydrolytic, or Catabolic
3. Exchange
A(OH) + B(H)  AB + H2O
AB + H2O  A(OH) + B(H)
AB + CD  AC + BD

20. C. Factors Affecting Rates
3. ???
2. ???
1. Concentration
4. Others?

21. V. Inorganic Molecules A. Water 1. Properties c. H-bonding a. States
b. Polar
Figure 2.6
Figure 2.8
d. Density
e. Cohesive Forces
Figure 2.12
Figure 2.10

22. 2. Uses b. Temperature Stabilizer or Regulator a. Solvent Figure 2.11

23. B. Salts
1. Properties (combining two nonmetals by ionic bond, make ions in solution)
2. Uses (Potential energy and move water)

24. C. Acids, Bases, pH, & Buffers
1. Definitions
a. An acid (increases the hydrogen ion concentration)
H2CO3  HCO3- + H+ (Carbonic)
H2SO4  H+ + H+ + SO4 2- (Sulfuric)
HCl  H+ + Cl- (Hydrochloric)
b. A base (decreases the hydrogen ion concentration)
HCl + NaOH  NaCl + H2O (Sodium Hydroxide)

25. d. A buffer (regulates the pH of a solution)
c. pH Scale (measures the hydrogen ion concentration)
Figure 2.14
d. A buffer (regulates the pH of a solution)
HCO3- + H+  H2CO3
HPO4-2 + H+  H2PO4-
NH3 + H+  NH4+
2. Uses & Misuses Why and how does acid precipitation affect vegetation?