Notes One Unit Eight Molecules

1. Notes One Unit EightMolecules • 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/nova.physics.ato/ Pages 72-81

2. Laws of proportions Definite Proportions • What is the proportion for(?)… • H2O • H2O2 • N2O3 • N2O5 • N2O • N2O4 Multiple Proportions 2:1 1:1 2:3 Multiple Proportions 2:5 2:1 1:2

3. Law of conservation of massDEMO NaOH/HCl phenolphthalein on a balance NaOH(aq)+ HCl(aq) H2O(l)+ NaCl(aq)

4. Law of conservation of mass 4 4 2H2(g) + 1O2(g)2H2O(l) H= H= O= O= Mass is conserved! 3H2(g) + 1N2(g)2NH3(l) N= N= H= H= 2C2H6(g)+ 7O2(g) 4CO2(g) + 6H2O(l) C= C= H= H= O= O= 2 2 2 2 6 6 4 4 12 12 14 8 + 6= 14

5. Three laws that support the existence of atoms 1. Law of definite proportions 2. E=MC2 3. Law of multiple proportions

6. List the five(Four?) principles of Dalton's atomic theory. • 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 heating element negative grid Neon gas Ne Ne+1 e-1 beam 20Ne+1 21Ne+1 22Ne+1

9. Calculating Average Atomic Mass E amu% product C-12 98.90 = 1186.8 12.000000 x 13.003355 x = 14.3036905 C-13 1.10 1187 1187 98.90 % + 14.3 + 14 + 1.10 % 1201 100.00 % 1201 ÷100.00 = 12.01amu 4 sd 5 sd 4 sd

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. Vacuum Chamber Horse Shoe Magnet

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

13. Calculating Average Atomic Mass E amu% product 79Br 50.697 78.9183376 x = 4000.922961 = 3990.548738 80.9162913 x 81Br 49.317 4000.9 50.697% + 3990.5 +49.317% 7991.4 100.014 % 7991.4 ÷100.014 = 79.9028136 amu 5 sd 6 sd 5 sd = 79.903 amu

14. Cathode Ray Demo Electrons(e-1) leave the cathode - + e-1 e-1 e-1 e-1 Cathode 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. Oil drops  perfume sprayer hole  (+) plate -2 . -1 . X-ray . 0 battery  (-) plate

18. Rutherford's experiments Alpha particle Lead Radium +2 8000   Microscope 7999  pass through 42He+2 Gold Foil 10,000 atoms thick +2 Characteristics of atoms mostly empty space Small(1/10,000), +79 dense, and heavy positive charge core

19. Atoms and their electrons, protons, and neutrons Proton(P+1) + Neutrons(n0)= Mass #(Z) 1 1 1 Hydrogen 0 H Hydrogen -1 1 1 Hydrogen 1 H Hydrogen -2 1 2 1 2 1 1 Hydrogen 1 2 H 3 Hydrogen -3 3 1 8 16 Oxygen -16 8 16 Oxygen 8 O 8 Iron Fe Iron -57 26 57 26 31 57 26

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

21. Notes Three Unit EightThe Structure of the Atom’s Shell Pages 92-95 • 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

22. Atomic Model Rutherford model *Mostly Empty Space *Nucleus… Very Small, Very Dense, Positive Charged, 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 Visible Light Short wave gamma ray X-ray IR radar FM UV TV AM Short wavelength Long wavelength Low Energy High Energy

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

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

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

28. Spectrum Example #1 n=6 Violet indgo Blue Yellow Orange Red Green n=5 n=4 Excited State n=3 n=2 Quantum Amount n=1 Ground State energy

29. Spectrum Example #2 n=6 Violet indgo Blue Yellow Orange Red Green n=5 n=4 Excited State n=3 n=2 Quantum Amount n=1 Ground State energy

30. Spectrum Example #3 n=6 Violet indgo Blue Yellow Orange Red Green n=5 n=4 Excited State n=3 n=2 Quantum Amount n=1 Ground State energy

31. Spectrum Example #4 n=6 Violet indgo Blue Yellow Orange Red Green n=5 n=4 Excited State n=3 n=2 Quantum Amount n=1 Ground State energy

32. Identifying Elements with Flame Tests Na K Li Ba

33. Notes Four Unit EightElectron 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 Bohr model *Mostly Empty Space *Nucleus… Very Small, Very Dense, Positive Charged, Where were the electrons? What are the electrons doing? Quantum Amount +

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 y-axis z-axis X-axis

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

39. p Orbitals Assembled y-axis z-axis x-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 6 2p attract   2s 2 6  [He] 2p 

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 6 1 2p 3s   3s 1  [Ne] 

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 2p 3s 3p 2s 2    2 6 2 5      3s [Ne] 3p 5 2  

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

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

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

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

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

50. NodalPlane