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

3. Element (natural stable particles of matter)

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

Figure 3.4B

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

B. Atomic Number & Mass Number

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?

D. Electrons 1. Shells  electron organization Figure 2.5

Sub shell Electron Configuration www.Ausetute.com.au 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+ 11 - 1 = 10 Mg 12 1s2 2s2 2p6 3s2 Mg2+ 12 - 2 = 10 Al 13 1s2 2s2 2p6 3s2 3p1 Al3+ 13 - 3 = 10 Si 14 1s2 2s2 2p6 3s2 3p2 Si4+ 14 - 4 = 10 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 Cl 17 1s2 2s2 2p6 3s2 3p5 Cl- 17 + 1 = 18 Ar 18

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

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

Table 2.6

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

b. Hydrogen Sharing Molecules sharing a hydrogen atom Figure 2.8

b. Hydrogen Sharing Molecules sharing a hydrogen Figure 2.8

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

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

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

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

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

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

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

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)

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?