1. What causes what you are seeing?
Electrons
What causes what you are seeing?

2. Sample
Flame color
Flame description

3. Electron Configuration
Mapping the electrons

4. Electron Configuration
The way electrons are arranged around the nucleus.

5. Quantum Mechanical Model
1920’s
Werner Heisenberg (Uncertainty Principle)
Louis de Broglie (electron has wave properties)
Erwin Schrodinger (mathematical equations using probability, quantum numbers)

6. Heisenberg uncertainty principle
it is impossible to determine simultaneously both the position and velocity of an electron or any other particle with any great degree of accuracy or certainty.

7. Erwin Schrodinger
Formulated equation that describes behavior and energies of subatomic particles.
Incorporates both particle and wave behavior in terms of wave function:
is proportional to the probability of finding an electron.
Leads to Quantum Mechanics: we cannot pinpoint an electron in an atom but we can define the region where electrons can be in a particular time……… called a Probability map….a 3-dimensional area in space called an ORBITAL

8. Like building a house….. Orbitals are like a house.
There are floors, rooms, closets and balconies.
Keep that in mind……

9. Principal Quantum Number, n
Indicates main energy levels
n = 1, 2, 3, 4…
This is like how many floors your house has
Each main energy level has sub-levels
This is like what kind of rooms are on each floor

10. Energy Sublevels
s p d f

12. The principle quantum number, n, determines the number of sublevels within the principle energy level. Basically each floor can only have certain types of rooms-answer questions….

13. Orbital Quantum Number, ℓ (Angular Momentum Quantum Number)
Indicates shape of orbital sublevels
ℓ = n-1
ℓ sublevel
0 s
1 p
2 d
3 f
4 g

14. Orbital
The space where there is a high probability that it is occupied by a pair of electrons. How many in a pair?
Orbitals are solutions of Schrodinger’s equations.

15. Orbitals

16. Visualizing the orbitals
Back to the house……
Orbitals are the rooms that hold 2 people per room.

17. Orbitals in Sublevels Sublevel # Orbitals # electrons s 1 2 p 3 6d f

18. Three rules are used to build the electron configuration:
Aufbau principle
Pauli Exclusion Principle
Hund’s Rule

19. Aufbau Principle Electrons occupy orbitals of lower energy first.
Like building a house- lower floors fill up first

20. Orbital Diagram

21. Filling Order diagram

22. -Pauli Exclusion Principle (Wolfgang Pauli, Austria, 1900-1958) -Electron Spin Quantum Number
An orbital can hold only two electrons and they must have opposite spin.
Electron Spin Quantum Number (ms):
+1/2, -1/2
Imagine people in a house one on feet……

23. Hund’s Rule
In a set of orbitals, the electrons will fill the orbitals in a way that would give the maximum number of parallel spins (maximum number of unpaired electrons).
Analogy: Students could fill each seat of a school bus, one person at a time, before doubling up.

24. Orbital Diagram for Hydrogen

25. Orbital Diagram for Helium

26. Orbital Diagram for Lithium

27. Orbital Diagram for Beryllium

28. Orbital Diagram for Boron

29. Orbital Diagram for Carbon

30. Orbital Diagram for Nitrogen

31. Rappers Resort

32. Orbital Diagram

33. Orbital Diagram for Fluorine

34. Notations of Electron Configurations
Standard
Shorthand

35. Standard Notation – electron configurations
If I had to send mail to someone living in the house you just built how would I address the envelope?
I would have to do the following.
Floors I have to climb to get to you
Type of rooms I pass
How many people are living in the rooms

36. Match up Who is who in this situation? Floors I have to climb
electrons
Type of rooms I pass
Principle energy levels
How many people are living in the rooms
orbitals

37. ALWAYS!!!
ROW
BLOCK
# OF BLOCKS

38. Color it in!

39. What do you notice about the d block?
the d block ______________ ________ so instead of 4d it is _____.
Why? It’s like closets in bedrooms.

40. Standard Notation of Fluorine
Number of electrons
in the sub level 2,2,5
1s2 2s2 2p5
Main Energy Level Numbers 1, 2, 2
Sublevels

41. Practice He Li P O Fe

42. Shorthand Notation- Noble gas configurations
Use the last noble gas that is located in the periodic table right before the element.
Write the symbol of the noble gas in brackets.
Write the remaining configuration after the brackets.
Ex: Fluorine: [He] 2s2 2p5

43. Practice Ca Al Br Cu

44. Lewis Dot Structures
Models to show how many valence electrons are in the A group elements.
This doesn’t apply to group B
Group # = Dots!

45. Examples

46. You try! Xe Cs Sr I

47. Electrons get excited!
Electrons can gain energy and move to an excited state and emit energy in specific wavelengths of light we can see!
How?

48. Ground state
Electrons have a ground state – or a state in which they normally exist. When energy is added to the system they jump to the next level
ON the RETURN to ground level they emit light in our visible spectrum.

49. Visible spectrum

50. Flame test.
We are going to solve a crime…….
See flame test worksheets

51. That’s it
Good luck on your test!