1. Notes One Unit Eight Molecules Cross Word Answers State the three laws that support the existence of atoms List the five principles of Dalton's atomic theory. Calculate the masses of atoms in amu and gram units. Describe how the atomic mass unit was chosen. Calculate Average Atomic Mass Reading Assignment Two unit Two Next Class http://www.teachersdomain.org/special/nova/n ova.physics.ato/http://www.teachersdomain.org/special/nova/n ova.physics.ato/ Pages 72-81

2. Laws of proportions What is the proportion for(?)… H 2 O H 2 O 2 N 2 O 3 N 2 O 5 N 2 O N 2 O 4 2:1 1:1 2:3 2:5 2:1 1:2 Multiple Proportions Definite Proportions

3. Law of conservation of mass DEMO NaOH/HCl phenolphthalein on a balance NaOH(aq)+HCl(aq)  H 2 O(l)+NaCl(aq)

4. Law of conservation of mass 2H 2 (g) + 1O 2 (g)  2H 2 O(l) H= H= O= O= Mass is conserved! 3H 2 (g) + 1N 2 (g)  2NH 3 (l) N= H= 2C 2 H 6 (g)+ 7O 2 (g)  4CO 2 (g) + 6H 2 O(l) C= H= O= 44 22 22 66 4 4 12 14 8 12 + 6=14

5. Three laws that support the existence of atoms 1. Law of definite proportions 2. E=MC 2 3. Law of multiple proportions

6. List the five(Four?) principles of Dalton's atomic theory. 1.All matter is made of indivisible and indestructible atoms. 2. All atoms of a certain element are identical in mass and properties. 3. Compounds can be formed by using two or more different kinds of atoms. 4. A chemical reaction is a rearrangementof atoms.

7. Carbons Mass in amu and gram units 1 amu=1/12 C-12 1 C-12 mass = 12.00000000 amu 1amu = 1.66053X10 -24 grams. 12.0000000 grams/Mole!

8. Mass Spectroscope Neon gas e -1 beam heating element negative grid NeNe +1 20 Ne +1 21 Ne +1 22 Ne +1

9. Calculating Average Atomic Mass E amu % product C-12 C-13 12.000000 13.003355 98.90 1.10 = 1186.8 = 14.3036905 x x 1187 + 14 1201 + 14.3 1187 98.90 % + 1.10 % 100.00 % ÷100.00= 12.01amu 4 sd5 sd4 sd 1201

10. Notes Two Unit Eight The Nucleus Quiz Average Atomic Mass Describe the evidence for the existence of electrons and their presence in atoms. Explain how Rutherford's experiments led to the discovery of the nucleus. Discuss atoms of different elements in terms of the numbers of electrons, protons, and neutrons they contain. Pages 82-90

11. Horse Shoe Magnet Vacuum Chamber

12. Potassium Gas- K(g) e -1 Beam To Vacuum Pump K +1 ions Vacuum Chamber Magnet FaceTo Vacuum Pump 39 K +1 40 K +1 41 K +1 K +1 K Photographic Plate

13. Calculating Average Atomic Mass E amu % product 79 Br 81 Br 78.9183376 80.9162913 50.697 49.317 = 4000.922961 = 3990.548738 x x + 3990.5 4000.9 50.697 % +49.317 % 100.014 % ÷100.014= 79.9028136 amu 5 sd6 sd5 sd 7991.4 = 79.903 amu

14. Cathode Ray Demo Electrons(e -1 ) leave the cathode Cathode  e -1   Anode - +

15. Cathode Ray Devices

16. Van de Graff Demo Van de Graff generator   Leyden Jar

17. Millikan's oil-drop experiment Charge of e -1 is equal to -1.602189 x 10 -19 Coulombs. X-ray ... -2  (+) plate  (-) plate  perfume sprayer Oil drops  0 hole  battery 

18. Rutherford's experiments Characteristics of atoms Radium  Lead Gold Foil  Microscope  Alpha particle   +2 8000   10,000 atoms thick 7999  pass through mostly empty space Small(1/10,000), 4 2 He +2 dense, and heavy positive charge core +79  +2

19. Atoms and their electrons, protons, and neutrons Proton(P +1 ) + Neutrons(n 0 )= Mass #(Z) AZElementP +1 n0n0 SymbolName HydrogenH 1 1 1 0 11 12 1 1 H 2 1 1 3 12H 3 1 816Oxygen 8 8O 16 8 Oxygen 2657 Iron 2631 Fe 57 26 Iron -2 -3 -16 -57

20. Nuclear Reactions A reaction, as in fission, fusion, or radioactive decay, that alters the energy, composition, or structure of an atomic nucleus. 235 92 U +n  1 0 Xe + 135 54 + n 1 0 Sr 100 38 Fission: Fusion: 1 0 n+ 7 3 Li  3 1 H 4 2 + He + 1 0 n Decay: 238 92 U  234 Th + 90 4 2 He Alpha Decay 234 90 Th  234 91 Pa + 0  Beta Decay(e -1 )

21. Notes Three Unit Eight The Structure of the Atom’s Shell Describe the nature of light and how it is produced. Explain how the wavelengths of light emitted by an atom provide information about electron energy levels. Flame Tests Lab B Pages 92-95

22. Atomic Model Rutherford model *Mostly Empty Space Very Small, Very Dense, Positive Charged, *Nucleus… Where were the electrons? What are the electrons doing? +

23. Particle Model of The Electron Neils Bohr e -1 found in the empty space. He used light to define their actions. e -1 region +

24. Electromagnetic Spectrum gamma ray X-ray UV IRradarFM TV Short wave AM Visible Light Short wavelength Long wavelength Low Energy High Energy

25. Bohr’s Model of the shell *Particle Model *Circular orbits * Hydrogen only Light’s Energy e -1

26. The Spectroscope Helium Tube slit Prism spectrograph Bright-line Emission Spectrum

27. Solar Spectrum  hydrogen  helium  mercury  uranium  (92 elements)

28. Spectrum Example #1 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

29. Spectrum Example #2 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

30. Spectrum Example #3 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

31. Spectrum Example #4 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

32. Identifying Elements with Flame Tests NaKLiBa

33. Notes Four Unit Eight Electron Arrangements For Elements Compare the atomic models of Rutherford and Bohr. Describe the quantum mechanical interpretation of electrons in atoms. State Pauli's exclusion Principle, the aufbau principle, and Hund's rule, and describe their roles in determining the electron configuration of atoms. Pages 96-103

34. Atomic Model Rutherford model *Mostly Empty Space Very Small, Very Dense, Positive Charged, *Nucleus… Where were the electrons? What are the electrons doing? + Quantum Amount Bohr model

35. De Broglie’s Wave model for Electrons Wave Nature Different solutions for e -1 actions. e -1 ’s act as a particle or a wave. e -1 ’s absorb or release Quantum Amount of NRG. Demo of waves on a string

36. Standing Waves

37. S Orbital X-axis y-axis z-axis

38. p Orbitals Shapes x-axis z-axis y-axis

39. p Orbitals Assembled x-axis z-axis y-axis

40. Quantum Model for The Shell of The Atom

41. Electron Order of Filling Aufbau principle fill the lowest energy level first

42. Orbital Filling Diagram Write the orbital filling diagram for Ne. How many electrons does Ne have? Final Answer Short Hand Answer 10 e -1        1s 2 2s 2 2p 6 [He] 2s 2 2p 6 attract

43. Orbital Filling Diagram Write the orbital filling diagram for Na. How many electrons does Na have? Final Answer Short Hand Answer 11 e -1        1s 2 2s 2 2p 6 [Ne] 3s 1 1 

44. Orbital Filling Diagram Write the orbital filling diagram for Cl. How many electrons does Cl have? Final Answer Short Hand Answer 17 e -1            1s 2 2s 2 2p 6 3s 2 3p 5 [Ne] 3s 2 3p 5

45. Notes Five Unit Eight Electron Dot diagrams Quantum Numbers Pages 96-103

46. Electron Dot Diagram for Neon        [He] 2s 2 2p 6 Ne ● ● ● ● ● ● ● ●

47. Electron Dot Diagram for Sodium        [Ne] 3s 1  Na ●

48. Electron Dot Diagram for Chlorine            [Ne] 3s 2 3p 5 ● ● ● ● ● ● ● Cl

49. Quantum Numbers Addresses for electrons Four numbers for each address No two addresses are the same First number is n=1, 2, 3, 4, 5, 6, 7(Distance From the Nucleus) Second number is l = 0, 1, 2, 3 s p d f Third number is m l = 0 = +1, 0, -1 = +2, +1, 0, -1, -2 = +3, +2, +1, 0, -1, -2, -3 p orbital d orbital f orbital Forth number is m s = +1/2 or -1/2 s orbital

50. NodalPlane

51. P orbital Nodal planes ( l =0) X-axis y-axis z-axis ?

52. P orbital Nodal planes ( l =1) x-axis z-axis y-axis

53. x y z Nodal planes ( l =2)

54.  n= l=l= m l =ms =ms = 32-2+1/2 Quantum Numbers l = 0(s), 1(p), 2(d), 3(f) = m s = +1/2 or -1/2 =  

55.  n= l=l= m l =ms =ms = 310-1/2 Quantum Numbers l = 0(s), 1(p), 2(d), 3(f) = m s = +1/2 or -1/2 =  

56.  n= l=l= m l =ms =ms = 700+1/2 Quantum Numbers l = 0(s), 1(p), 2(d), 3(f) = m s = +1/2 or -1/2 =  

57. n=ml =ml =ms =ms = 43+2-1/2 l=l=  Quantum Numbers

58. Quantum Number for Last e -1 in In  n=5 l=l= 1ml=ml=+1 ms=ms=+1/2 Many e -1 does In have? 49 e -1 Short hand element? Kr Many e -1 does Kr have? 36 e -1    How many e -1 to account for? 13 e -1 Quantum #’s for Last e -1 Short-hand fills to where? Fill-in Valence13 e -1

59. Final quiz Review

60. Average Atomic mass quiz Example AMU Abundance(%) K 39 38.963708 93.20 K 40 39.963999 0.012 K 41 40.961825 6.73 X = 3631.417586 0.479567988 275.6730823 3631 0.48 276 3631 + 276 3907 93.20 + 6.73 0.01 99.94 3907÷ 99.94= 39.09 4 SD 0

61. Spectrum Example #3 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

62. Orbital Filling Diagram Write the orbital filling diagram for Cu. How many electrons does Cu have? Final Answer Short Hand Answer 29 e -1                1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 9 [Ar] 4s 2 3d 9 

63. Electron Dot Diagram for Selenium                [Ar] 4s 2 3d 10    4p 4 Se ● ● ● ● ● ●

64. Quantum Number for Last e -1 in Cd n=4 l=l= 2ml=ml=-2 ms=ms=-1/2 How many e -1 does Cd have? 48 e -1 Short hand element? Kr Many e -1 does Kr have? 36 e -1     How many e -1 to account for? 12 e -1 Quantum #’s for Last e -1 Short-hand fills to where? Fill-in Valence12 e -1 l = 0(s), 1(p), 2(d), 3(f) = m s = +1/2 or -1/2 =  

65. Nuclear Reactions 235 92 U +n  1 0 Cs + 136 55 + n 1 0 Rb 99 37 Fission: Decay: 238 92 U  235 Th + 90 3 2 He Alpha Decay

66. Wave model for shell of the atom

67. Hund's rule Hund's rule: every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied.

68. Pauli's exclusion Principle