A. Why study chemistry?

1. Chemistry2. Matter

CHEMISTRYI.

IntroductionB. Definitions

3. Elements

4. Molecule

5. Compound

Figure 2.3

Figure 5.3

A. Particles / Structure

II. Atomic Chemistry

Figure 2.5

B. Atomic & Mass Number

C. Isotopes & Radioisotopes

Figure 2.7

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?

E. Electrons

Figure 2.8

Figure 2.9

Figure 2.6

Figure 2.10

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

Electronegativity degree of attraction for electrons

Figure 2.9

A. Definition

1. Definition2. Types

III. Molecular Chemistry

B. Chemical Bonds

a. Electron Sharing

i. Covalent bonds = sharing of valence electrons

Figure 2.11

Non-polar covalent bonds

Figure 2.12

Polar

Figure 2.13

Figure 2.15

Figure 2.14

ii. Ionic = giving and receiving electrons

b. Hydrogen Sharing

Hydrogen bonds sharing a hydrogen

Figure 2.16

Hydrogen bonds sharing a hydrogen

Figure 3.2

c. VanderWalls Forces

VanderWalls Forces sharing a charge

1. Why Important?C. Formulas & Models

Figure 2.17

Figure 2.18

c. Structural

b. Empirical

a. Molecular

A. Definition

1. Synthesis, Dehydration, or Anabolic2. Decomposition, Hydrolytic, or Catabolic

IV. Chemical Reactions

B. Types

3. Exchange

A(OH) + B(H) AB + H2O

AB + H2O A(OH) + B(H)

AB + CD AC + BD

C. Factors Affecting Rates

A. Water1. Properties

V. Inorganic Molecules

States of Water

Polar

H-Bonding Potential

Figure 3.2

Density

Figure 3.6

Cohesive Forces

Figure 3.4

Cohesive ForcesFigure

3.3

2. Uses

Solvent

Figure 3.6Figure 3.8

Temperature Stabilizer or Regulator

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 concentration

HCl + NaOH NaCl + H2O (Sodium Hydroxide)

pH Scale measures the hydrogen ion concentration

Figure 3.10

A buffer regulates the pH of a solution

HCO3- + H+ H2CO3

HPO4-2 + H+ H2PO4

-

NH3 + H+ NH4+

How does acid precipitation affect vegetation?

Knowledge will always forbear over stupidity.