1. Electron Properties and Arrangement Chapter 5
Objectives:
Identify the properties of electrons.
Understand how electrons move in atoms.
Distinguish between atoms based on their different electron arrangements. .

2. Electrons in Atoms What do you know about electrons in atoms?
Using Bohr’s model illustrate and label the sub-particles in the following neutral atoms:
a. H b. C c. Ne-20

3. Electrons and Light Particles
Similarities:
Very tiny particles
Extremely small masses
Move at very high speeds (3.0x108 m/s)

4. Electromagnetic Radiation Spectrum
Electromagnetic Spectrum : Divides light particles into regions based on their wave-like properties.
a. Relationship b/w wavelength and frequency?
Relationship b/w wavelength and energy emission?
Relationship b/w frequency and energy emission?

5. Wave-Like Properties: Wavelength
Wavelength: length of wave from two neighboring crest.
Amplitude: height of wave from origin to crest.

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

7. Wave-Like Properties: Energy
Temperature = energy emitted by light particles.
Photons = light particles that are classified by the amount of energy they emit off.

8. Electromagnetic Spectrum Analysis1
What light particle region has the longest wavelength?
What light particle region has the lowest frequency?
What light particle region emits the highest amount of energy?
As wavelength decreases for a light particle, what happens to frequency?
Sketch a line graph illustrating the relationship between wavelength and frequency.
As frequency increases for a light particle what happens to it its energy?
Sketch a line graph illustrating the relationship between frequency and energy.
In the visible region, (ROYGBIV), does red or violet light particles have a slightly smaller
wavelength?

9. Electromagnetic Spectrum Applications
“Electromagnetic Spectrum Song” by Emerson and Wong Yann

10. Electromagnetic Radiation Spectrum
a. Relationship b/w wavelength and frequency?
Relationship b/w wavelength and energy emission?
Relationship b/w frequency and energy emission?

11. Visible Region: Continuous Spectrum
Continuous Spectrum = Presence of all light particles in the visible region.

12. Visible Region: Absorption Spectrum
Absorption Spectrum = Presence of dark bands that indicate light particles absorbed by matter.
At room temperature we observe light particles reflected.by matter.

13. An Atom’s Interaction with Light Particles

14. Atoms Interaction with Light Particles
Electrons absorb light particles
Electrons absorb specific light particles or photons.
Electrons that absorb photons can move to higher
energy levels.

15. 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.)

16. Electron Movement

17. Flame Test Lab Purpose:
Heat matter (atoms) so that we can observe the emission of photons from electrons.

18. Flame Test Lab Purpose:
Heat matter (atoms) so that we can observe the emission of photons from electrons.
Conclusions:
Electron movement occurs instantaneously.
Elements’ electrons emit off different photons of energy and color.
Identify elements by the distinct color (photons) they emit off.

19. Bell Ringer: Electron Movement
1. Illustrate and explain the movement of electrons in an atom using the following terms:
(photons, absorption, emission, energy levels, ground state, and excited state)
Rank the samples’ color based on the following:
Increasing wavelength.
Decreasing frequency.
Increasing emission of energy.
3. Which sample do you predict had electrons that moved the farthest during the flame test lab.
4. Explain how the flame test lab would be beneficial for forensic scientists.

20. Bell Ringer: Electron Movement
2. Rank the samples’ color based on the following:
a. Increasing wavelength. (data table)
*b. Decreasing frequency. (electromagnetic spectrum)
*c. Increasing emission of energy. (electromagnetic spectrum)

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

22. Electromagnetic Radiation Spectrum
a. Relationship b/w wavelength and frequency?
Relationship b/w wavelength and energy emission?
Relationship b/w frequency and energy emission?

23. Bohr’s Model of the Atom
The electron cloud consists of energy levels.
Electrons reside and move around in these energy levels.
Electrons can move to other energy levels when absorb photons. 23

24. 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.)

25. Infinite Campus Update
Flame Test Lab
*Quiz tomorrow over electron properties, wave-like properties, and electron movement.

26. Electron Movement
1. Explain the difference between the ground state and the excited state of an electron in an atom. 2. In the flame test lab, the color change occurred when electrons ________ photons and dropped down to an energy level closer to the nucleus. (absorbed, reflected, emitted)

27. Continuous Spectrum Review
Continuous Spectrum = Reflection of all light particles by electrons in the visible region.
Ex. sun; white light bulbs

28. Visible Region Absorption Spectrum
Absorption Spectrum = Reveals what light particles are reflected and absorbed by electrons.

29. Emission Spectrum
Emission Spectrum =Reveals what photons are emitted during electron movement.
Ex. Hydrogen Light
chemed.chem.purdue.edu

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

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

33. 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.

34. Locating an Electron
Is it possible to know the exact location and velocity of an electron at any instant in time?
Very difficult to locate an electron because:
- moving extremely fast
-continuously bombarded by light particles
When locate an electron with a photon from a microscope, it changes its velocity in unpredictable ways. 34

35. Heisenberg Uncertainty Principle
After
Before
Photon changes wavelength
Photon
It is not possible to know the exact position and
velocity of an electron at the same time. 35

36. Electron Movement and Arrangement
What principle states that you cannot know the location and velocity of an electron at the same time?
Why is an emission spectrum unique for each element?
What is quantum energy?

37. Electron Movement and Arrangement
What principle states that you cannot know the location and velocity of an electron at the same time?
Why is an emission spectrum unique for each element?
What is quantum energy?
What is the quantum mechanical model?
What is the maximum number of electrons on the 5th energy level?

38. The Quantum Mechanical Model
An atomic model that best explains the probable arrangement and movement of electrons at any moment in time.
Schrodinger provided evidence for this model using
a complex mathematical equation.
Depends upon 4 quantum numbers.
Erwin Schrodinger

39. n-Quantum Number n = energy levels
3-D region of space around the nucleus where an electron can be found.
Each energy level has a specific energy value.
E- must absorb or release a specific quantum of energy to move between energy levels.
E- do not travel in an orbit (exact path) around the nucleus.
Atomic orbitals: Probable paths an electron would take around the nucleus.

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

41. n-Quantum Number Limited number of electrons on each energy level.
2n2 Rule determines the maximum number of electrons on each energy level.

42. 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

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

44. Infinite Campus Update
Electron properties and movement quiz (10pts.)
Flame Test Lab (15 pts.)
Due Today: Electron Probability Lab (15pts.)

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

47. 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
1 (least energy)
P-orbital 2
D-orbital 3
F-orbital
4 (most energy)

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

49. 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.

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

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

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

53. F-orbital Orientations
Maximum # of f-orbital electrons on an energy level?
How many f-orbitals are possible on an energy level? 53

54. Orbital Orientations

55. Electron Configuration
Use the diagram to determine how
many sublevels are in each energy level.
1st: 1
2nd:2
3rd:3
4th:4
5th:4
6th:3 currently
7th:2 currently
What is the maximum number of
electrons in each sublevel? 2
What do you suppose the yellow
arrows represent?
khanacademy.org

56. Electron Arrangement Diagonal Rule
Determine the electron arrangement for each neutral element
Diagonal Rule
Neutral Elements
Electron Configuration
Hydrogen (H):
Lithium (Li) :
Carbon (C):
Oxygen (O):
Neon (Ne):
Sodium (Na):
Chlorine (Cl):
Helium (He) :
Potassium (K):
Vanadium (V):
Cobolt (Co):
Zirconium (Zr):
khanacademy.org

57. 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!)

58. Electron Configuration
Determine the electron configuration for each neutral element:
Diagonal Rule
Neutral Elements
Electron Configuration
Hydrogen (H): 1e-
1s1
Lithium (Li) : 3e-
1s22s1
Carbon (C): 6e-
1s22s22p2
Oxygen (O): 8e-
1s22s22p4
Neon (Ne): 10 e-
1s22s22p6
Sodium (Na): 11e-
1s22s22p63s1
Chlorine (Cl): 17e-
1s22s22p63s23p5
Helium (He) : 2 e-
1s2
Potassium (K): 19e-
1s22s22p63s23p64s1
Vanadium (V): 23e-
1s22s22p63s23p64s23d3
Cobolt (Co): 27e-
1s22s22p63s23p64s23d7
Zirconium (Zr): 40e-
1s22s22p63s23p64s23d104p65s24d2
khanacademy.org

59. Electron Configuration of Elements

60. Electron Configuration Orbital Notation
H: Li: C: V:

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

62. Electron Configuration with Orbital Notation

63. Orbitals and Periodic Table