1. Chapter 3 The Atom

2. HISTORY OF THE ATOM NOTES BLACK CIRCLE ACTIVITY Day One and Day Two

3. Black Circles You and your partner will be given a black circle. Within the black circle is a ball and some barrier Your job is to figure out what shape the barrier is….

4. The Greek Philosophers Democritus Greek Philosopher Nature must be small particles which were indivisible Aristotle Greek Philosopher Matter was continuous Table (chop forever)

6. John Dalton 1.Matter = particles with definite size & mass 2. All atoms that make up an element have the same mass.

7. John Dalton 3. Atoms of 2 different elements have different masses. 4. Atoms come together in definite ratios to form compounds. H 2 O

9. Thomson Studied the Cathode Ray Tubes Rays appear on phosphorescent screen when an electrical current is sent through Atoms are neutral How could the magnet affect these particles? Must be smaller positive and negative particles

10. J.J. Thomson

11. Rutherford Gold Foil Experiment What did he expect? – Majority of particles to hit straight across opening

13. What actually happened? Most went through Few particles hit foil and bounced back

14. Conclusions from the Gold Foil Experiment 1.Atom is mostly empty space 2.Mass is concentrated in the center 3.Nucleus is positive

15. RUTHERFORD MARBLE ACTIVITY Day Three

16. Rutherford: Measuring what you cannot see

17. LAB WRITE-UP REVIEW FOR QUIZ Day Four

18. Dalton 1.What is the name of his theory? 2.What are elements made of? 3.An atom of hydrogen and an atom of carbon are ________ 4.What are compounds made of?

19. J.J. Thomson 1.What did Thomson discover? 2.What is the charge of an electron?

20. Rutherford 1.What is the charge of an alpha particle? 2.Why is Rutherford’s experiment called the gold foil experiment? 3.How did he know the atom was mostly empty space?

21. Rutherford 4. What happened to the alpha particles as they hit the gold foil? 5. How did he know that the nucleus was positively charged?

22. LECTURE: NUCLIDE SYMBOLS QUIZ: HISTORY OF ATOMIC STRUCTURE Day Five

23. Structure of the Atom Proton – Nucleus – Positive Charged Neutron – Nucleus – Neutrally charged Electron – Outside the nucleus – Negatively charged

24. Nuclide Symbols Atomic Number Mass Number

25. Nuclide Symbol Write the nuclide symbol for a potassium atom that has 21 neutrons.

26. Lets Try a Few Write the Nuclide Symbols A lithium atom with 4 neutrons A sulfur atom with 15 neutrons

27. Assignment Page 20 – Practice Problems: Writing Nuclide Symbols First Four

28. LECTURE: NUCLIDE SYMBOLS & ISOTOPES Day Six

29. Nuclide Symbols Mass Number Atomic Number

30. Lets Try a Few!! Write the nuclide symbols for the following: – Copper- 64 – A Sulfur with has 17 neutrons – Potassium- 39

31. Isotopes Atoms of the same number of protons but different number of neutrons

32. Assignment Page 20 and 21

33. Day Seven LECTURE: NUCLIDE SYMBOLS AND IONS

34. Nuclide Symbols

35. Nuclide Symbols for Ions What is an ion? – An ion is a charged particle It could be positive or negative What does that do to the number of protons, electrons, and neutrons?

36. Example 40 K +1, Determine the number of protons, neutrons, and electrons.

37. Lets Try a Few! Determine the number of electrons, protons, and neutrons in the following: 81 Br -1 18 N -3

38. Radioactivity Three types of Radioactivity – Alpha – Beta – Gamma

39. Assignment Page 22 – Complete the first table

40. NUCLIDE SYMBOLS/ RADIOACTIVITY PRE-LAB FLAME TEST Day Eight

41. Radioactivity Three types of Radioactivity – Alpha – Beta – Gamma

42. Example

43. Properties of Electrons Most of the atom’s mass is made up of ______ Most of the atom’s volume is made up of _____ Found in __________

44. Properties of Electrons The closer the electron is to the nucleus the less energy it has

45. Ground vs. Excited States Ground State Close to nucleus as possible Excited State – Electrons receive energy move farther away – Release E to drop back down to ground state (LIGHT) – Light can be seen in different colors – Elements can be identified by observing the colors it releases

46. Assignment Radioactivity Worksheet

47. FLAME TEST REVIEW FOR NUCLIDE AND RADIOACTIVITY QUIZ Day Nine

48. QUIZ: NUCLIDE AND RADIOACTIVITY LAB WRITE-UP Day Ten

49. ELECTRON CONFIGURATION Day Eleven

50. Locating/Mapping Electrons Energy Levels (n) – Higher the n farther away from the nucleus – More Energy Sublevels – Number of sublevels is related to the energy level – N=1 : 1 sublevel, N=2: 2 sublevels – N= 3 : ? Sublevels, N=4 : ???, N= 5: ???

51. Shapes and Orbitals Orbital: – Most probable location of the electrons – Each orbital can hold a maximum of 2 electrons Shapes – 4 different orbitals that have four different shapes – s, p, d, f

53. Lets try to summarize this: (Page 28) Sublevels (Symbol) # of orbitals # of electrons in EACH orbital TOTAL # of electrons possible in sublevel s p d f

54. ELECTRON CONFIGURATION Day Twelve

55. Lets try to summarize this: (Page 28) Sublevels (Symbol) # of orbitals # of electrons in EACH orbital TOTAL # of electrons possible in sublevel s p d f

56. Lets dig a little deeper: (Page 28) Energy Level (n) # of Sublev els Type of sublevels # of electrons possible in each orbital Total # of electrons possible in Energy Level 1 2 3 4 5 6 7

57. So how do we “map” out the location of the electrons? Aufbau Principle: – Electrons will always fill up an atom from lowest to highest energy CARBON

58. Assignment Page 29 – Oxygen, Boron, Helium, Sulfur, Magnesium

59. ELECTRON CONFIGURATION Day Thirteen

60. What about the bigger elements? Potassium

61. 1s 2s2p 3s3p3d 4s4p4d4f 5s5p5d5f 6s6p6d6f 7s7p7d7f

62. Assignment Page 30 – #1-10

63. QUIZ: ELECTRON CONFIGURATION MODEL OF THE ATOM Day Fourteen

64. REVIEW FOR TEST MODEL OF THE ATOM Day Fifteen

65. TEST Day Sixteen