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CHEMISTRY

CHEMISTRY. I . Introduction. A. Why study chemistry?. B. Definitions. 1. Chemistry. 2. Matter. 3. Element. 5. Compound. 4. Molecule. Figure 2.1. Figure 3.4B. II . Atomic Chemistry. A. Particles / Structure. Figure 2.3A. B. Atomic & Mass Number. C. Isotopes & Radioisotopes.

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CHEMISTRY

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  1. CHEMISTRY I. Introduction A. Why study chemistry? B. Definitions 1. Chemistry 2. Matter

  2. 3. Element

  3. 5. Compound 4. Molecule Figure 2.1

  4. Figure 3.4B

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

  6. B. Atomic & Mass Number

  7. C. Isotopes & Radioisotopes Table 2.3 Figure 2.4B 1. Isotopes = more 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. www.Ausetute.com.au

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

  11. III. Molecular Chemistry B. Chemical Bonds A. Definition 1. Definition 2. Types a. Electron Sharing i. Covalent bonds Non-polar Polar 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 Figure 2.8

  15. c. Vander Walls Forces Molecules sharing a charge

  16. C. Formulas & Models 1. Why Important? 2. Types a. Molecular b. Empirical c. Structural

  17. IV. Chemical Reactions A. Definition 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

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

  19. 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

  20. 2. Uses b. Temperature Stabilizer or Regulator a. Solvent Figure 2.11 Figure 2.13

  21. B. Salts 1. Properties 2. Uses

  22. C. Acids, Bases, pH, & Buffers 1. Definitions & Uses 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)

  23. 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+ Why and how does acid precipitation affect vegetation?

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