2. BASIC CHEMISTRY n 1. Matter n (a) states n (b) physical changes-chemical n changes n (c elements---atoms; periodic table n (d) structure of atoms n (e) oxidation-reduction

3. ATOMS n 1. COMPOSITION (sub atomic particles) n 2. CHARGE n 3. THREE WAYS OF IDENTIFYING n AN ATOM OR ELEMENT n 4. ISOTOPES (definition); naturally occurring artifically made; n 5. Combine to form molecules.

4. MOLECULES & COMPOUNDS n 1. How molecular wt. Is computed. n 2. Definition of a molecule. n 3. Examples: n (a) calcium chloride n (b) hydrochloric acid n (c sucrose

5. MATTER-ENERGY COMPLEX n 1. Atom n (a) cloud (b) dumbell (c sphere n (d) haze n 2. Shells-orbitals-energy levels n 3. Two dimensional representation n 4. Restriction of number of electrons n each can contain.

6. MATTER-ENERGY COMPLEX contd. n 5. Energy Levels (K, L, M, N, O, P, Q ) n 6. * OCTET RULE n 7. Electron-Nucleus relationship n 8. Analogy: cliff with steps and rocks n 9. The attracting force of the nucleus for the electron is inversely proportional to the distance the electron is from the nucleus.

7. MATTER-ENERGY COMPLEX contd. n 10. Chemical reactions take place primarily between electrons in the outer energy levels of separate atoms. n 11. Bonding capacity of atom is determined by : the number of electrons in its outer orbit. n 12. Rearrangement of electrons in outermost energy level (bonding).

8. CHEMICAL BONDING n 1. Rearrangement involves one of two possibilities: n (a) one atom will give up one or more electrons to the other--ionic bonding n (b) each atom will share one or more of its electrons with the other. --covalent bonding. n 2. Bonding capacity of atoms is determined by the number of electrons n in the outer 0rbit.

9. CHEMICAL BONDING contd. {Ionic} n 3. Ionic bond (use sodium & chlorine) n 4. Atom is stable when its outer energy n level is filled with electrons. n 5. Use calcium and chlorine to illustrate that atoms do not always react in 1-1 ratio.

10. CHEMICAL BONDING contd. {Covalent} n 6. Carbon atom n 7. Models: (a) methane (b) paraffin series (c water (d) methyl alcohol n (e) carbon dioxide (f) ethylene (g) acetylene n 8. Ways to present relationships of shared electrons

11. CHEMICAL BONDING contd. {Hydrogen} n 9. Bond angles and the geometry of molecules. n 10. Hydrogen bond--definition n 11. Polarity of molecules--(use water as n example) n FORMATION OF DOUBLE BONDS n DIATOMIC MOLECULES & RINGS