1 / 10

BASIC CHEMISTRY

BASIC CHEMISTRY. 1. Matter (a) states (b) physical changes-chemical changes (c elements---atoms; periodic table (d) structure of atoms (e) oxidation-reduction. ATOMS. 1. COMPOSITION (sub atomic particles) 2. CHARGE

hiroko
Download Presentation

BASIC CHEMISTRY

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

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

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

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

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

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

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

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

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

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

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

More Related