1. Electron Movement and Organization 3.30.15
Objectives:
Identify electron properties
Understand how electrons move within an atom.

2. Electron Movement and Organization 3.31.15
Objectives:
Identify electron properties
Understand how electrons move within an atom.

3. Characteristics of Electrons
What are some properties of electrons?
How do electrons move within an atom?

4. Electron Movement and Organization 3.18.15
Objectives:
Identify electron properties
Understand how electrons move within an atom.

5. Electron Movement and Organization 4.1.15
Objectives:
Identify electron properties
Understand how electrons move within an atom.

6. Like Properties: Wavelength
Wavelength: length of wave from two neighboring crest.

7. Wave-Like Properties: Frequency
Frequency (Hz) : how many waves pass a certain point per second. Units: Hertz (Hz.)= (waves/second)

8. Wave-Like Properties: Energy
Temperature : Represents amount of energy emitted from light particles.
Photons: Light particles classified by energy emitted.
*Electron movement dependent upon type of photons absorbed or released.

9. Electrons: Wave-Like Properties
a. Relationship b/w wavelength and frequency?
Relationship b/w wavelength and energy emission?
Relationship b/w frequency and energy emission?

10. Electron Movement Electrons can take different paths
around the nucleus.
*Electrons constantly move to different
energy levels in the electron cloud.
*Direction of e- movement is
dependent upon energy absorbed or released.
Erwin Schrodinger

11. Electron Movement Around Nucleus
A maximum of 2 electrons can move in each orbital.

12. Electron Movement Electrons can take different paths
around the nucleus.
*Electrons constantly move to different
energy levels in the electron cloud.
*Direction of e- movement is
dependent upon energy absorbed or released.
Erwin Schrodinger

13. Electron Movement Ground state of H Atom (lowest energy level for e-)
Ground state of H Atom (lowest energy level for e-)
A photon (light particle) is absorbed by H’s electron.
Electron becomes excited and jumps to higher energy level.
3. E- returns to ground state and emits (releases) the photon.
Emitted photon’s wavelength can be detected by scientists.
(Infrared region at room temp; Visble region at higher temps.)

14. Flame Test Lab
Purpose: To classify atoms and identify electron movement in atoms.

15. Electron Movement and Organization 4.13.15
Objectives:
Identify electron properties
Understand how electrons move within an atom.
Understand how electrons are arranged in an atom.

16. Electromagnetic Spectrum Analysis
a. Relationship b/w wavelength and frequency?
Relationship b/w wavelength and energy emission?
Relationship b/w frequency and energy emission?

18. Emission Spectrums
Emission spectrum for each element is unique.

19. Visible Region of EM Spectrum
loke.as.arizona.edu

21. Electron Movement and Organization 4.14.15
Objectives:
Identify electron properties
Understand how electrons move within an atom.
Understand how electrons are arranged in an atom.

22. Electron Probability Lab
Purpose: To determine which energy level an electron would prefer to be on in an atom. Class’s Hypothesis: -1st energy level-closest to nucleus (12 students) -Highest energy level-farthest from nucleus(6 students)

23. Energy Levels and the Periodic Table Associate energy levels with rows on periodic table.

24. Electron Movement and Organization 4.15.15
Objectives:
Identify electron properties
Understand how electrons move within an atom.
Understand how electron arrangement determines chemical reactivity.

25. Electron Probability Lab
Class’s Hypothesis: -1st energy level-closest to nucleus (12 students) -Highest energy level-farthest from nucleus(6 students) Class’s Results:
Lab Group
Energy Level 1
(# of times)
Energy Level 2
Energy Level 3 1 2 3 4 5 6 7 8 9

26. Electromagnetic Spectrum Analysis Qts.

27. Emission Spectrums
Emission spectrum for each element is unique.

28. Locating an Electron
Is it possible to know the exact location of an electron at any moment in time?
Very difficult to locate an electron because:
- moving extremely fast
-continuously bombarded by light particles, which changes the path of the electron.
-When locate an electron with a photon from a microscope, it changes its direction in unpredictable ways. 28

29. Heisenberg Uncertainty Principle
After
Before
Photon changes wavelength
Photon
It is not possible to know the exact location of an
electron, just probable location. 29

30. Energy Levels Limited number of electrons on each energy level.
2n2 Rule determines the maximum number of electrons on each energy level.

31. Electron Arrangement
Different for each element.

32. Periodic Table and Valence Electrons

33. Electron Arrangement
Different for each element.
Valence Electrons

34. Electron Movement in Energy Levels
Quantum of energy:
Specific energy that is absorbed or emitted by electrons.
Energy difference between two energy levels.
Scientist can calculate energy emitted by electrons.
Determine what energy levels electrons move between in an atom.

35. Electron Probability Lab

36. l–Quantum Number l -number : Sublevels within an energy level.
Sublevels identify the shape of the orbitals.
There are four different sublevels: s, p, d, f

37. Orbital Shapes
A maximum of 2 electrons can move in each orbital.

38. Orbitals and Energy Requirement
Electron movement defines orbital shapes for each sublevel.
Electrons need energy to move in orbital shapes.
Sublevel’s Orbitals
Energy for electron movement
(Rank in increasing amount of energy)
S-orbital
P-orbital
D-orbital
F-orbital

39. Electron Configuration
Electron Configuration: The probable arrangement of electrons in the ground state of an atom.
Electron Configuration Rules:
Aufbau Principle: Electrons will move in an orbital of lower energy first. (Electrons are lazy!)
Pauli Exclusion Principle: Only two electrons can move in an orbital at the same time.
Hund’s Rule: When electrons can move in orbitals of the same energy, they will prefer to be alone before pairing up. (Electrons are selfish!)

40. Electron Movement and Organization 3.25.15
Due:
Electron Probability Lab
Objectives:
Understand how electrons move within atoms.
Distinguish between atoms based on their different electron arrangements.

41. Bell Ringer: Electron Arrangement
1. What atomic model best explains electron arrangement?
2. a. What is the n-quantum number?
b. T or F: Electron move around the nucleus in
an exact path.
3. a. What is the l-quantum number?
b. Illustrate the s, p, d, f atomic orbitals?
c. How many electrons can move in each atomic orbital at any one time?

42. Orbital Shapes
A maximum of 2 electrons can move in each orbital.

43. Orbitals and Periodic Table

45. Bell Ringer: Electron Arrangement
1. What atomic model best explains electron arrangement?
2. a. What is the n-quantum number?
b. T or F: Electron move around the nucleus in
an exact path.
3. a. What is the l-quantum number?
b. Illustrate the s, p, d, f atomic orbitals?
c. How many electrons can move in each atomic orbital at any one time?

46. Electron Configuration

49. Electron Configuration: Bell Ringer
What is electron configuration for an element?
2. How does the periodic table help you determine electron configuration for an element? Be specific with your explanation.

50. Electron Sublevels (atomic orbitals) Diagonal Rule
3. Use the diagram to determine the type
of sublevels (orbitals) in each energy level?
1st:
2nd:
3rd:
4th:
5th:
6th:
7th:
2. What do you suppose the yellow
arrows represent?
khanacademy.org

51. Periodic Table and Electron Configuration

52. Orbital Shapes
A maximum of 2 electrons can move in each orbital.

53. Electron Configuration: Exit Slip
Br: Ar: Fe

56. Electron Configuration
Electron Configuration: The probable arrangement of electrons in the ground state of an atom.
Electron Configuration Rules:
Aufbau Principle: Electrons will move in an orbital of lower energy first. (Electrons are lazy!)
Pauli Exclusion Principle: Only two electrons can move in an orbital at the same time.
Hund’s Rule: When electrons can move in orbitals of the same energy, they will prefer to be alone before pairing up. (Electrons are selfish!)

57. m- Quantum Number m –number: Orientations for each atomic orbital.
Orbital orientations: The different ways an electron can make an orbital in 3-D space.

58. S-Orbital Orientation
Maximum # of s-orbital electrons on an energy level?
How many s-orbital orientations are possible on an energy level?

61. P-orbital Orientations
Maximum # of p-orbital electrons on an energy level?
How many p-orbital orientations are possible on an energy level?

63. D-orbital Orientations
Maximum # of d-orbital electrons on an energy level?
How many d-orbital orientations are possible on an energy level?

65. F-orbital Orientations
Maximum # of f-orbital electrons on an energy level?
How many f-orbital orientations are possible on an energy level? 65

67. Orbital Orientations

68. Electron Movement and Organization 11.05.14
Infinite Campus:
Electron Probability Lab (15pts.)
Objectives:
Understand how electrons move within atoms
Distinguish between atoms based on their different electron arrangements.

69. Electron Configuration with orbital notation
1. Define the first three quantum numbers. 2. Write the electron configuration (n,l,m quantum numbers) for each element below: H: Li: C: V:

70. Electron Configuration Orbital Notation

71. S-Quantum Numbers S-number :
The direction an electron spins in an orbital.
If paired, the electrons will spin in opposite directions.

72. Electron Configuration: Bell Ringer
a. Determine the electron configuration of a neutral Br atom and include the orbital notations.
b. How many unpaired electrons?
c. How many valence electrons does Br have?
d. How many types of sublevels (orbitals) use Hund’s rule?

73. Orbitals and Periodic Table

74. Nuclear Chemistry and Electron Arrangement Exam

75. Balancing Redox Reactions: Acidic Solutions
Cu (s) + NO3- (aq) ----> Cu2+ (aq) + NO2 (g)