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Intro to Chemistry

Intro to Chemistry. 9.27.13. Chemistry: The study of . Chemistry: The study of matter Matter: . Chemistry: The study of matter Matter: Anything with mass that takes up space. The Atom. Atom: Smallest differentiable unit of matter Composed of . The Atom.

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Intro to Chemistry

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  1. Intro to Chemistry 9.27.13

  2. Chemistry: The study of

  3. Chemistry: The study of matter • Matter:

  4. Chemistry: The study of matter • Matter: Anything with mass that takes up space

  5. The Atom • Atom: Smallest differentiable unit of matter • Composed of

  6. The Atom • Atom: Smallest differentiable unit of matter • Composed of protons, neutrons, and electrons

  7. Subatomic Particles • Neutron: • Found in the

  8. Subatomic Particles • Neutron: • Found in the nucleus • Charge of

  9. Subatomic Particles • Neutron: • Found in the nucleus • Charge of 0 • Mass of

  10. Subatomic Particles • Neutron: abbr? • Found in the nucleus • Charge of 0 • Mass of 1 amu(atomic mass unit)

  11. Subatomic Particles • Neutron: n0 • Found in the nucleus • Charge of 0 • Mass of 1 amu(atomic mass unit)

  12. Subatomic Particles • Proton: • Found in

  13. Subatomic Particles • Proton: • Found in the nucleus • Charge of

  14. Subatomic Particles • Proton: • Found in the nucleus • Charge of +1 • Mass of

  15. Subatomic Particles • Proton: • Found in the nucleus • Charge of +1 • Mass of 1 amu

  16. Subatomic Particles • Proton: p+ • Found in the nucleus • Charge of +1 • Mass of 1 amu

  17. Subatomic Particles • Electron: • Found

  18. Subatomic Particles • Electron: • Found orbiting the nucleus at a great distance • Charge of

  19. Subatomic Particles • Electron: • Found orbiting the nucleus at a great distance • Charge of -1 • Mass of

  20. Subatomic Particles • Electron: • Found orbiting the nucleus at a great distance • Charge of -1 • Mass of 0 amu(not actually zero, but mass is so small that it is ignored)

  21. Subatomic Particles • Electron: e- • Found orbiting the nucleus at a great distance • Charge of -1 • Mass of 0 amu(not actually zero, but mass is so small that it is ignored)

  22. Electron Orbitals • Electrons orbit the nucleus in discreet orbits or “shells” • First orbital holds

  23. Electron Orbitals • Electrons orbit the nucleus in discreet orbits or “shells” • First orbital holds 2 e- • 2nd =

  24. Electron Orbitals • Electrons orbit the nucleus in discreet orbits or “shells” • First orbital holds 2 e- • 2nd = 8 e- • 3rd = 8 e- • 4th = 10 e-

  25. Electron Orbitals • Electrons orbit the nucleus in discreet orbits or “shells” • First orbital holds 2 e- • 2nd = 8 e- • 3rd = 8 e- • 4th = 10 e- Important: The outer shell is the only important one for forming bonds with other atoms

  26. S 2 8 3 13 Al Aluminum 26.982

  27. S 2 8 3 13 Al Aluminum 26.982

  28. S 2 8 3 13 Element Symbol Al Aluminum 26.982

  29. S 2 8 3 13 Element Symbol Al Aluminum Element Name 26.982

  30. # of p+ (Atomic Number) S 2 8 3 13 Element Symbol Al Aluminum Element Name 26.982

  31. # of p+ (Atomic Number) S 2 8 3 13 Element Symbol Al Aluminum Element Name 26.982 Average atomic mass (# of p+ + n0)

  32. # of p+ (Atomic Number) S 2 8 3 13 # of e- in each shell Element Symbol Al Aluminum Element Name 26.982 Average atomic mass (# of p+ + n0)

  33. # of p+ (Atomic Number) Physical state at STP (0o @ sea level) S 2 8 3 13 # of e- in each shell Element Symbol Al Aluminum Element Name 26.982 Average atomic mass (# of p+ + n0)

  34. Models of the Atom • Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell)

  35. Models of the Atom • Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell) Mg

  36. Models of the Atom • Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell) B O

  37. Bohr Diagram • Shows complete e- configuration (sometimes shows details of nucleus) • Ex: Mg

  38. Bohr Diagram • Shows complete e- configuration (sometimes shows details of nucleus) • Try: F and Ca

  39. Isotopes • Isotope: An atom with a different # of n0 than normal, which therefore also has a different

  40. Isotopes • Isotope: An atom with a different # of n0 than normal, which therefore also has a different atomic mass

  41. Isotopes • Ex: C-12 vs. C-14 • p+ = p+ =

  42. Isotopes • Ex: C-12 vs. C-14 • p+ = 6 p+ = 6 • n0 = n0 =

  43. Isotopes • Ex: C-12 vs. C-14 • p+ = 6 p+ = 6 • n0 = 6 n0 = 8 • e- = e- =

  44. Isotopes • Ex: C-12 vs. C-14 • p+ = 6 p+ = 6 • n0 = 6 n0 = 8 • e- = 6 e- = 6 • Isotopes only differ in their mass, not in their charge or their bonding behavior

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