A. Definitions - PowerPoint PPT Presentation

slide1 n.
Download
Skip this Video
Loading SlideShow in 5 Seconds..
A. Definitions PowerPoint Presentation
Download Presentation
A. Definitions

play fullscreen
1 / 93
A. Definitions
182 Views
Download Presentation
tyrone-savage
Download Presentation

A. Definitions

- - - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript

  1. CHEMISTRY I. Introduction A. Definitions 1. Chemistry 2. Matter

  2. Anything that occupies space and has mass.

  3. 3. Energy

  4. a. Potential

  5. b. Kinetic

  6. c. Forms Chemical Electrical Mechanical Radiant

  7. 4. Elements

  8. II. Atomic Chemistry A. Particles

  9. Figure 2.1

  10. B. Structure

  11. Figure 2.2

  12. C. Atomic & Mass Number

  13. D. Isotopes & Radioisotopes

  14. Figure 2.3

  15. Isotope = atom with moreneutrons Radioisotopesneutrons measurably decay giving off radiation (alpha and beta particles, plus gamma rays) DecayRate = half life

  16. E. Electronegativity & Valence

  17. Electronegativity=> degree of attraction for electrons Valence => number of electrons in the outermost shell Figure 2.5

  18. III. Molecular Chemistry A. Definition B. Chemical Bonds 1. Definition 2. Types a. Electron Sharing

  19. i. Ionic bondsgivingand taking of electrons Figure 2.6a Figure 2.6b

  20. ii. Polar Covalent bondsunequal sharing Figure 2.6

  21. iii.Non-polar covalent bondsequal sharing

  22. iii.Non-polar covalent bondsequal sharing

  23. b. Hydrogen Sharing

  24. Hydrogen bonds sharinga hydrogen atom between molecules Figure 2.10a

  25. IV. Chemical Reactions A. Definition B. Types 1. Synthesis, Dehydration, or Anabolic 2. Decomposition, Hydrolytic, or Catabolic 3. Exchange

  26. A(OH) + B(H) AB + H2O CD + H2O  C(OH) + D(H) AB + CD  AC + BD

  27. Figure 2.11

  28. C. Factors Affecting Rates

  29. V. Inorganic Molecules A. Water 1. Properties

  30. States of Water

  31. Polar Figure 2.7

  32. H-Bonding Potential Figure 2.8

  33. Density

  34. Cohesive Forces

  35. 2. Uses

  36. Solvent Figure 2.12

  37. Temperature Stabilizer or Heat of Vaporization

  38. B. Salt (Electrolytes) 1. Properties

  39. 2. Uses

  40. C. Acids, Bases, pH, & Buffers 1. Definitions & Uses

  41. An acid increases the hydrogen ion concentration H2CO3  HCO3- + H+ (Carbonic) H2SO4  H+ + H+ + SO4 2- (Sulfuric) HCl  H+ + Cl- (Hydrochloric)

  42. A base decreases the hydrogen ion concentration HCl + NaOH NaCl + H2O (Sodium Hydroxide)