1. Schrödinger & Heisenberg Model

2. 2 Ar 8 8 18 bright line spectrum
Recall Bohr’s model of the atom: Bohr’s model of the atom was famous because it could explain the ____________________________________. 2 Ar 8 8 18
bright line spectrum

4. continuous discontinuous discrete bands
The spectrum of white light is _________________, it shows all the colours of the rainbow
The spectrum of energized gas is _________________, it shows _________________.
discontinuous
discrete bands

5. Each spectrum is a unique “fingerprint.”

8. E1
Ground state

9. E1
Ground state
1st excited state

10. E1 E1 packet of light photon Ground state 1st excited state

11. E2
Ground state

12. 2nd excited state

13. E2-E1 E2 E2 1st excited state Ground state 2nd excited state

15. When particles are exposed to energy
ground state (lowest energy state) atoms absorb specific energy and become “excited”
an electron moves to a higher shell
excited atoms then release the energy at specific frequencies to get back to ground state
the electron moves back to its original shell, emitting a photon (packet of light)
the difference between two particular energy levels is called the quantum
the lines in the spectrum are produced when electrons de-excite

16. quantum

17. Bohr’s model was proven significantly wrong in 2 ways:
electrons don’t revolve around the nucleus in circles
the model can only predict energies in H

18. Recap What does “ground state” refer to? A. A hydrogen atom
B. Lowest energy state of an atom
C. Highest energy state of an atom
D. When the atom is on the ground

19. Recap How does an electron become “excited?”
A. The atom it resides in reacts with another atom
B. It absorbs energy and jumps shells
C. It absorbs specific amounts of energy and jumps shells
D. When it sees a particle of opposite charge

20. Recap What is a photon? A. A packet of light B. An excited proton
C. An excited electron
A Chinese wonton stuffed with Vietnamese noodles

21. Dalton
Thomson
Rutherford
Bohr
Schrödinger

24. Schrödinger’s model describes the probability of where to find an electron in an atom
orbital: the region of space around a nucleus where an electron can be found
orbitals are described by quantum numbers

25. 1st or principal quantum number (n)
Symbols
What does it mean?
1st or principal quantum number (n)
2nd quantum number (l)
3rd quantum number (m)
4th quantum number (ms)
1, 2, 3 …
Size and energy level

26. 2s

27. 1st or principal quantum number (n)
Symbols
What does it mean?
1st or principal quantum number (n)
2nd quantum number (l)
3rd quantum number (m)
4th quantum number (ms)
1, 2, 3 …
Size and energy level
s, p, d, f
Orbital shape

28. s orbital
p orbital
d orbital
f orbital

29. 1st or principal quantum number (n)
Symbols
What does it mean?
1st or principal quantum number (n)
2nd quantum number (l)
3rd quantum number (m)
4th quantum number (ms)
1, 2, 3 …
Size and energy level
s, p, d, f
Orbital shape
x, y, z
Orbital orientation

34. 1st or principal quantum number (n)
Symbols
What does it mean?
1st or principal quantum number (n)
2nd quantum number (l)
3rd quantum number (m)
4th quantum number (ms)
1, 2, 3 …
Size and energy level
s, p, d, f
Orbital shape
x, y, z
Orbital orientation
½ or -½
Electron spin

35. # of Orbitals in a Subshell Maximum # of Electrons in Subshell
Each energy level has a specific set of orbitals and each one represents where a maximum of 2 electrons can be found.
Orbital Type
Begins at n=
# of Orbitals in a Subshell
Maximum # of Electrons in Subshell s 1 1 2 p 2 3 6 d 3 5 10 f 4 7 14

36. Recap What is an orbital?
A. The path an electron takes around the nucleus
B. Lobes
C. The shape of the nucleus
D. Mathematical description (probability) of where to find an electron in an atom

37. Let’s zoom in to each of the Bohr shells
Let’s zoom in to each of the Bohr shells. What’s really going on at each shell?

38. Energy Level Diagram
Shell 4 3
orbitals 2
subshells 1

39. electron-electron repulsion
Rules to follow when filling orbitals:
Fill orbitals from lowest to highest energy (Aufbau Principle)
Place one electron in each orbital of a sub-shell
When each orbital of a sub-shell has one electron, go back and pair the electrons (Hund’s Rule)
If two electrons are in a orbital, they must have opposite spin (Pauli Exclusion Principle)
These rules ensure that the electron configuration gives the ___________ energy, most __________ atom by reducing ________________________________.
lowest
stable
electron-electron repulsion

41. More About Shells
Shell 4 3 2 1
1s22s22p63s23p64s23d104p6 2 8 8 18

42. How can you write the electron configuration without the energy level diagram???

44. 1s 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 5d 6p 6d 7s 4f 5f

46. Ar:
1s2
2s2
2p6
3s2
3p6
3p5
3p3
3p1
3p2
3p4

47. Ga:
1s2
2s2
2p6
3s2
3p6
4s2
3d10
4p1

48. Ag:
1s2
2s2
2p6
3s2
3p6
4s2
3d10
4p6
5s2
4d9

49. Rn:
1s2
2s2
2p6
3s2
3p6
4s2
3d10
4p6
5s2
4d10
5p6
6s2
4f14
5d10
6p6

51. 1s2 2s2 2p6 3s2 3p6 K
[Ar]
4s1
1s2 2s2 2p6 3s2 3p6
[Ar] Ti
4s2 3d2
1s2 2s2 2p6 3s2 3p6 Ni
[Ar]
4s2 3d8
1s2 2s2 2p6 3s2 3p6
[Ar] Ga
4s2 3d10 4p1
1s2 2s2 2p6 3s2 3p6 Kr
[Ar]
4s2 3d10 4p6 Ar

52. [Ar]
4s2 3d 5

53. Example: Write the electron configuration for Ga using core notation.
Closest previous noble gas element: ______
Core notation:___________________ Ar
[Ar] 4s23d104p1

54. Practice: Write the electron configuration for the following elements.
Zn _______________________________
K ________________________________
Kr _______________________________
[Ar]4s23d10
[Ar]4s1
[Ar]4s23d104p6