1. Chapter 4 and 5

4. History Democritus: Tiny particles called atoms and empty space. GREEK Aristotle: Matter was continuous (Hyle) Boyle: Believed in atoms Newton: Believed in atoms. ENGLISH Dalton: Law of Multiple Proportions. JJ Thomson: Electrode. Anode (+), Cathode (-) Cathode Ray : Electrons that travel from Cathode (-) to Anode (+).

8. English cont. Robert Millikan: (1868-1953) Discovered electrons charge, used Thomson’s ideas. French Lavosier and Dalton: Law of Conservation of Mass Law of Definite Proportions Proust and Dalton observed that in chemicals or specific substances; The element ratio is always the same regardless of quantity. IE) NaCl = 1:1 Law of Multiple Proportions The ratio of one element that combines with another element can be expressed in small whole #’s. Concerned with elements that form more than one compound with each other. ( Dalton) IE) Tin (II) Oxide = Sn0 ; Tin (IV) Oxide = SnO 2

11. More information on page 79

20. Average Atomic Mass Neon has two isotopes. Neon (20) has a mass of 19.992u; Neon (22) has a mass of 21.991u. In an average sample of 100 neon atoms, 90 will be Neon (20) and 10 will be Neon (22). Calculate the average mass of neon. Practice Problems Page 112 (17 and 18) 116 and 117(21,22, 23 and 24)

22. PARTY!!!!!

25. Electrons?

30. Electromagnetic Spectrum

32. Magnetosphere

35. Application

36. Images

38. Fun – For Friday

40. 2) Sodium has 3 isotopes. Na23, Na25, Na21. I have 59 atoms of Na; 5 atoms of Na23, 30 atoms of Na25, and 24 atoms of Na21. What is the average atomic mass? 1) Complete the Chart

42. Chapter 5

43. Atomic Structure: Quantum Mechanics De Broglie: Used Planck’s and Einstein’s theory when he studied electrons. E=MC ² and E=h  Equal: MC ²=h  De Broglie Einstein Planck

44. De Broglie substituted V (General Velocity) for C (Velocity of Light) M( V ) ²=h  The equation above shows how electrons move in the same ways as light rays. Wave Particle Duality of Nature Electrons can have a two-sided nature: Particles and Waves . Momentum = (P) P= M x V V  Is Substituted for  M ( V ) ² = h V   = h__ M V _h_ = = M V P  h = P h 

46. Where Are Electrons? Probability = Number of total positions Quantum Theory We know that when an electron moves to a higher or lower energy level light is produced. For example: The Flame Test Quantum Numbers Numbers that describe the electrons in atoms. These numbers are defined by (n, l, m, and s) Number of times an electron is in a certain position.

47. Principle Quantum Number Energy level. The symbol is n . n= 1, 2, 3, 4, 5, 6, 7 We can use the principle quantum number to determine the greatest number of electrons possible in any one level. The formula in use is: (2n ²) where n = 1, 2, 3, 4, 5, 6, 7 So how many electrons can the first energy level in an element hold?

49. l: The Second Quantum Number An energy level can have 5 sublevels: s , p , d , f, g s , p , d , f , g : are identified by (l) The principle quantum number(n) identifies the number of sublevels (l). Orbitals n=1 : L= 0, where 0 means one sublevel (s) n=2: L= 0,1 where 0 and 1 means two sublevels (s,p) n= 3: L=0,1,2 sublevels (s,p,d) n= 4 L= 0,1,2,3 sublevels (s,p,d,f) n= 5 L= 0,1,2,3,4 sublevels (s,p ,d ,f ,g) s – Sublevel contains 1 pair of electrons p – Sublevel contains 3 pair of electrons d – Sublevel contains 5 pair of electrons f – Sublevel contains 7 pair of electrons g – Sublevel contains 9 pair of electrons

55. Energy Levels s , p , d , f : are identified by (l) The principle quantum number identifies the number of sublevels. PQ #_ = PQ #_ = _ Sublevel (_) _ Sublevels (_ , _) PQ #_ = _ Sublevels (_ , _ , _) PQ #_ = _ Sublevels (_ ,_ , _ , _) PQ #_ = _ Sublevels (_ , _ , _ , _ , _) s – Sublevel contains _ pair of electrons p – Sublevel contains _ pair of electrons d – Sublevel contains _ pair of electrons f – Sublevel contains _ pair of electrons g – Sublevel contains _ pair of electrons

57. Hund’s Rule : Every orbital in a sublevel is singly occupied with one electron before any one orbital is doubly occupied. Pauli Exclusion : No two electrons can have the same set of four quantum numbers. Lewis Dot Diagram: The Lewis Dot Diagram tells us the number and position of electrons in the outer most shell of an element. #15 Page 130 Models

60. 8. Sublevels (l), Orbitals (m), Spin (s). 9. Number of possible electrons. 10. Lewis Dot Structure. 11. Isotopes. 12. Explain difference between Newtonian and Quantum mechanics. Study for the test!