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Atoms, Ions and the Periodic Table

Atoms, Ions and the Periodic Table. Chemistry 131 Chapter 2. Dalton’s Atomic Theory. Structure of the Atom. Atomic Mass. Periodic Table. Ions. Dalton’s Atomic Theory. Two Key Ideas led to Atomic Theory. Law of Conservation of Mass. 1787 - Lavoisier. Law of Definite Proportions.

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Atoms, Ions and the Periodic Table

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  1. Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2

  2. Dalton’s Atomic Theory Structure of the Atom Atomic Mass Periodic Table Ions

  3. Dalton’s Atomic Theory

  4. Two Key Ideas led to Atomic Theory

  5. Law of Conservation of Mass 1787 - Lavoisier

  6. Law of Definite Proportions 1804 - Proust

  7. Published in 1808 with Four Postulates Dalton’s Atomic Theory

  8. All matter is composed of exceedingly small, invisible particles called Atoms.

  9. Atoms of an element have a given mass and properties, atoms of differing elements differ in mass and properties.

  10. Atoms are not created or destroyed in a chemical reaction.

  11. Atoms combine is simple, fixed, whole-number ratios to form compounds

  12. Structure of the Atom

  13. Dalton perceived Atoms as the smallest unit of matter.

  14. Positive Charge Thomson’s discovery of the electron posited a different model. Negative Charge Electron

  15. Rutherford’s Gold Foil experiments led to yet another revision

  16. The Nuclear Model of the Atom

  17. Even atoms have sub-structure.

  18. Hydrogen

  19. Proton Mass = 1.6726×10-24 gCharge = +1.6022×10-19 C

  20. Neutron Mass = 1.6749×10-24 g Charge = 0

  21. Electron Mass = 9.1094×10-28 g Charge = -1.6022×10-19 C

  22. Atomic Number = Number of protons Mass Number=#Protons + # Neutrons

  23. Isotopes Hydrogen Also Hydrogen

  24. Ions

  25. Number of Electrons = Number of Protons, if the atom is neutral.

  26. Ions +1 Li

  27. Atomic Mass

  28. 1.6749×10-24 g isn’t a lot

  29. Atomic Mass Unit (amu)

  30. 1 amu = 1/12 the mass of 1 Carbon-12 atom

  31. All atomic masses are therefore relative to Carbon-12

  32. The atomic masses on the periodic table are relative atomic masses

  33. Relative Atomic Mass=(Isotope 1 mass × Abundance 1) +(Isotope 2 mass × Abundance 2)+…

  34. Example (Silver)107Ag 106.9051 amuis 51.82%109Ag 108.9048 amuis 48.18%

  35. 106.9051 amu × 0.5182 = 55.40 amu108.9048 amu × 0.4818 = 52.47 amu55.40 amu+52.47 amu =107.87 amu

  36. Problem Given the following information, calculate the relative atomic mass of Magnesium. 24Mg = 23.985 amu at 20.00% 25Mg = 24.985 amu at 20.00% 26Mg = 25.983 amu at 60.00%

  37. Problem The copper mined on Earth consist of 63Cu (62.93 amu) and 65Cu (64.93 amu). Which isotope is more abundant? Why?

  38. Periodic Table

  39. Review Problems

  40. Review Problem 1 How many carbon atoms are present in each sample? 120 amu 12,000 amu 7.22 × 1024amu

  41. Review Problem 2 During a typical physical exam blood tests measure the cholesterol level. A high result is anything over 240.0 mg/dL. What is this in pounds/fluid ounce? If a typical human has 5.000 L of blood, how many pounds of cholesterol are present in the blood of a patient with a total cholesterol of 260.0 mg/dL?

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