1. To describe Rutherford’s model of the atom
Objectives
To describe Rutherford’s model of the atom
To explore the nature of electromagnetic radiation
To see how atoms emit light

2. Rutherford’s Atom – But what are those electrons doing?

3. How can different colored fireworks be made. Why do we get colors
How can different colored fireworks be made? Why do we get colors? Why do different chemicals give us different colors? 

4. To understand e-s, we study electromagnetic radiation.
2. Energy and Light
To understand e-s, we study electromagnetic radiation.
GAMMA-prolonged exposure?
ROY G. BIV, Micro, Radio

5. TThe rainbow is more beautiful than the pot of gold.

6. 2. Energy and Light
How are the types of light different?
Wavelength, λ
Energy travels in wave motion. Shorter wavelength, more energy. Spring Demo.

7. Electromagnetic Radiation
One of the ways that energy travels through space.
Characteristics:
Wavelength ( ) – distance between two peaks or troughs in a wave. 
Frequency ( ) – number of waves (cycles) per second that pass a given point in space
Speed (c) – speed of light (2.9979×108 m/s) or (3×108 m/s)

8. How are the types of light different?
2. Energy and Light
How are the types of light different?
PhET Wave on a String
PhET Radio Waves
PhET Microwave

9. Different wavelengths carry different amounts of energy. (Drill Demo)
2. Energy and Light
Different wavelengths carry different amounts of energy. (Drill Demo)

10. 3. Emission of Energy by Atoms
Atoms can give off light.
They first must receive energy and become excited.
The energy is released in the form of a photon.

11. Dual nature of light Double Slit Experiment
2. Energy and Light
Energy is mass E = mc2
Dual nature of light Double Slit Experiment
Wave vs Photon – packet of energy

12. 2. Energy and Light
Dual nature of light- show PhET wave on a string- no end, increase frequency and amplitude until you see the photons as part of the wave…PhET Wave on a String

13. To describe Rutherford’s model of the atom
Objectives Review
To describe Rutherford’s model of the atom
To explore the nature of electromagnetic radiation
To see how atoms emit light
Work Session: Page 365 # 1-6

14. To learn about Bohr’s model of the hydrogen atom
Objectives
To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy
To learn about Bohr’s model of the hydrogen atom
To understand how the electron’s position is represented in the wave mechanical model

15. Refraction of White Light (Continuous Spectrum)

16. The Line Spectrum of Hydrogen (Line Spectrum)

17. Energy of the electron in the hydrogen atom is quantized. WHY?
Significance
Only certain energies (photons) are allowed for the electron in the hydrogen atom.
Energy of the electron in the hydrogen atom is quantized.
WHY?

18. 1. The Energy Levels of Hydrogen
Atomic states
Excited state – atom with excess energy
Ground state – atom in the lowest possible state
When an H atom absorbs energy from an outside source it enters an excited state.

19. 1. The Energy Levels of Hydrogen
Energy level diagram
Energy in the photon corresponds to the energy used by the atom to get to the excited state.

20. 1. The Energy Levels of Hydrogen
Quantized Energy Levels
Since only certain energy changes occur the H atom must contain discrete energy levels.

21. Bohr’s model of the atom
Quantized energy levels
Electron moves in a circular orbit
Electron jumps between levels by absorbing or emitting photon of a particular wavelength

22. 2. The Bohr Model of the Atom
Bohr’s model of the atom was not totally correct.
Electrons do not move in a circular orbit.

23. 3. The Wave Mechanical Model of the Atom
Orbitals (de Broglie and Schrödinger)
Nothing like orbits
Probability of finding the electron within a certain 3-D space
Darker means higher probability

24. What happens when electrons lose their energy?
Objectives Review
What happens when electrons lose their energy?
Which has lower energy, 0.5 kg of steak or 0.5 kg of hamburger? Why?
Why does metal spark when placed in a microwave?
They get Bohr’d
Hamburger, ground state

25. To learn about Bohr’s model of the hydrogen atom
Objectives Review
To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy
To learn about Bohr’s model of the hydrogen atom
To understand how the electron’s position is represented in the wave mechanical model
Work Session: Page 370 # 2-6

26. To learn about the shapes of the s, p and d orbitals
Objectives
To learn about the shapes of the s, p and d orbitals
To review the energy levels and orbitals of the wave mechanical model of the atom
To learn about electron spin

27. Hydrogen has discrete energy levels. Called principal energy levels
1. The Hydrogen Orbitals
Hydrogen Energy Levels
Hydrogen has discrete energy levels.
Called principal energy levels
Labeled with whole numbers 1, 2, 3, 4

28. Each principal energy level is divided into sublevels.
1. The Hydrogen Orbitals
Hydrogen Energy Levels
Each principal energy level is divided into sublevels.
Labeled with numbers and letters (s, p, d, f)
Indicate the shape of the orbital

29. Principal Energy Levels 1 - 8
1. Orbitals Summary
Principal Energy Levels 1 - 8
Orbitals 4 - s, p, d, f each with unique shapes
Level 1 has 1 orbital (s)
Level 2 has 2 orbitals (s, p)
Level 3 has 3 orbitals (s, p, d)
Level 4 has 4 orbitals (s, p, d, f)
Level 5 has 4 orbitals (s, p, d, f)
Level 6 has 3 orbitals (s, p, d)
Level 7 has 2 orbitals (s, p)
Level 8 has 1 orbital (s) symmetry

31. Each suborbital can hold a max of 2 e-s
1. Orbitals Summary
Each orbital (s, p, d, f) can be broken down into suborbitals (sublevels)
s - 1
p - 3
d - 5
f – 7
Each suborbital can hold a max of 2 e-s

32. Orbitals do not have sharp boundaries.
1. The Orbitals
Orbitals do not have sharp boundaries.

33. 1. The Orbitals Entanglement
Heisenburg Uncertainty Principle- LINK
The more precisely the position is determined, the less precisely the momentum is known in this instant, and vice versa.

35. 1s Orbital

36. Two Representations of the Hydrogen 1s, 2s, and 3s Orbitals

37. 2px Orbital

38. 2py Orbital

39. 2pz Orbital

40. The Boundary Surface Representations of All Three 2p Orbitals

41. 3dx2-y2 Orbital

42. 3dxy Orbital

43. 3dxz Orbital

44. 3dyz Orbital

45. Orbital

46. The Boundary Surfaces of All of the 3d Orbitals

47. f suborbitals (7)

48. Principal Energy Levels 1 - 8
2. Orbitals Summary
Principal Energy Levels 1 - 8
Orbitals 4 - s, p, d, f each with unique shapes
Level 1 has 1 orbital (s)
Level 2 has 2 orbitals (s, p)
Level 3 has 3 orbitals (s, p, d)
Level 4 has 4 orbitals (s, p, d, f)
Level 5 has 4 orbitals (s, p, d, f)
Level 6 has 3 orbitals (s, p, d)
Level 7 has 2 orbitals (s, p)
Level 8 has 1 orbital (s) balance, top

49. Each suborbital can hold a max of 2 e-s
2. Orbitals Summary
Each orbital (s, p, d, f) can be broken down into suborbitals (sublevels)
s - 1
p - 3
d - 5
f – 7
Each suborbital can hold a max of 2 e-s
How can the orbitals be a volume with 1 e-?
Helicopter, laser pointer, lighted top

50. Why can an H atom have so many orbitals and only 1 electron?
2. The Orbitals
Why can an H atom have so many orbitals and only 1 electron?
An orbital is a potential space for an electron.
Atoms can have many potential orbitals.
They are always there, waiting to be used.
But not always detectable until an electron gains enough energy to occupy
Magician Car Accident
Schrödinger’s cat….Lottery
Cat put in box- given poisoned food– after a while, it is simultaneously dead and alive—although when we look in, it is either, but not both.
Lottery- before you look at the winning numbers, ??
I had an accident with a magician, - he just appeared out of nowhere!

51. 3. The Wave Mechanical Model: Further Development
Atoms Beyond Hydrogen
The Bohr model was modified because it did not apply to all atoms.
Atoms beyond hydrogen have an equal number of protons and electrons.
Need one more property to determine how the electrons are arranged
Spin – electron spins like a top or like the earth

52. 3. The Wave Mechanical Model: Further Development
Atoms Beyond Hydrogen
Pauli Exclusion Principle - an atomic suborbital can hold a maximum of 2 electrons and those 2 electrons must have opposite spins to maintain balance
………………. car spin, 1st car

53. To learn about the shapes of the s, p and d orbitals
Objectives Review
To learn about the shapes of the s, p and d orbitals
To review the energy levels and orbitals of the wave mechanical model of the atom
To learn about electron spin
Work Session: Page 376 # 2-6

54. To learn about valence electrons and core electrons
Objectives
To understand how the principal energy levels fill with electrons in atoms beyond hydrogen
To learn about valence electrons and core electrons
To learn about the electron configurations of atoms with Z < 18
To understand the general trends in properties in the periodic table

55. 1. Electron Arrangements in the First 18 Atoms
H atom (Descriptive Notation)
Electron configuration – electron arrangement – 1s1
Orbital diagram – orbital is a box grouped by sublevel containing arrow(s) to represent electrons

56. 1. Electron Arrangements in the First 18 Atoms
He atom
Electron configuration– 1s2
Orbital diagram

57. 1. Electron Arrangements in the First 18 Atoms
Li atom
Electron configuration– 1s2 2s1
Orbital diagram

58. Orbital Energies

59. 1. Electron Arrangements in the First 18 Atoms
Be atom – 4 e-s
(1s22s22p63s23p6)
1s22s2
______ ______ ______ ______ ______ ______ ______ ______ ______
1s s p s p

60. 1. Electron Arrangements in the First 18 Atoms
B atom – 5 e-s
(1s22s22p63s23p6)
1s22s22p1
______ ______ ______ ______ ______ ______ ______ ______ ______
1s s p s p

61. 1. Electron Arrangements in the First 18 Atoms
C atom – 6 e-s
(1s22s22p63s23p6)
1s22s22p2
* When filling in the orbital diagram, start with the lowest energy level. Work up through each sublevel, being sure to have opposite spins for paired electrons. All suborbitals must contain one e- before any suborbital can be completely filled (p suborbitals).
______ ______ ______ ______ ______ ______ ______ ______ ______
1s s p s p

62. 1. Electron Arrangements in the First 18 Atoms
Draw the electron configuration and orbital diagram for: N O F Ne Al P S Cl
______ ______ ______ ______ ______ ______ ______ ______ ______
1s s p s p

63. 1. Electron Arrangements in the First 18 Atoms
Draw the electron configuration for:
N 1s22s22p3 1s22s2p3
O 1s22s22p4 1s22s2p4
F 1s22s22p5 1s22s2p5
Ne 1s22s22p6 1s22s2p6
Al [Ne] 3s2p1
P [Ne] 3s2p3
S [Ne] 3s2p4
Cl [Ne] 3s2p5

64. 1. Electron Arrangements in the First 18 Atoms
1s22s22p63s23p6 Don’t have to memorize!
Properties of families related to valence configuration
K [Ar] you might think 3d1, however, properties hint to 4s1
Ca [Ar] you might think 3d2, however, properties hint to 4s2
Less predictability with larger atoms-less F(mag)

65. 1. Electron Arrangements in the First 18 Atoms
Classifying Electrons
Valence electrons – electrons in the outermost (highest) principal energy level of an atom (designated by group Roman # I - VIII)
Core electrons – inner electrons
Elements with the same valence electron arrangement show very similar chemical behavior.

66. 2. Electron Configurations and the Periodic Table
1s s p s
Li ______ ______ ______ ______ ______ ______
Na ______ ______ ______ ______ ______ ______
Notice the pattern in the valence shell.
Notice the energy level and the row on the periodic table.
Notice the ionic charge that these make.

67. 2. Electron Configurations and the Periodic Table
1s s p
Cl ______ ______ ______ ______ ______ ______ ______ ______ ______
1s s p s p
Notice the pattern in the valence shell, the energy level and the row on the periodic table, and the ionic charge that these make.
F ______ ______ ______ ______ ______ ______ (EXCITED)
1s s p s

68. 2. Electron Configurations and the Periodic Table
Look at electron configurations for K through Kr
Cr and Cu have non-patternistic e- configurations
Transition Elements
Larger atomic radii have more variety

69. 2. Electron Configurations and the Periodic Table
W [Xe]4f145d46s2
W [Xe]4f146s25d4
Order can get mixed around in notation because of the preference to find the balance between showing the energy levels in order and showing which orbitals fill first.
Variations can also be caused by individual preferences, arbitrary convention, or printing space availability.

70. 2. Electron Configurations and the Periodic Table
Orbital filling and the periodic table (Wave Mechanical Model)
Periodic

71. 2. Electron Configurations and the Periodic Table
Group number tells the number of valence electrons!

72. 3. Atomic Properties and the Periodic Table
Metals and Nonmetals
Metals tend to lose electrons to form positive ions.
Nonmetals tend to gain electrons to form negative ions.

73. 3. Atomic Properties and the Periodic Table
Atomic Size
Size tends to increase down a column.
Size tends to decrease across a row.
Biggest at lower left

74. 3. Atomic Properties and the Periodic Table
Ionization Energies
Ionization Energy – energy required to remove an electron from an individual atom (gas)
Tends to decrease down a column
Tends to increase across a row
Biggest upper right

75. 3. Atomic Properties and the Periodic Table
Ionization Energies
Ionization Energy – energy required to remove an electron from an individual atom (gas)
The key criticism of the Bohr model was that although it accurately predicted the ionization energies for hydrogen, it was lacking in its description of the ionization energies for the other atoms.

76. 3. Atomic Properties and the Periodic Table
Ionization Energies
Ionization Energy – energy required to remove an electron from an individual atom (gas)
Lithium
Sodium and Potassium
Rubidium and Cesium
Francium Bomb

77. To learn about valence electrons and core electrons
Objectives Review
To understand how the principal energy levels fill with electrons in atoms beyond hydrogen
To learn about valence electrons and core electrons
To learn about the electron configurations of atoms with Z < 18
To understand the general trends in properties in the periodic table
Work Session: Page 390 # 1-7