1. OR: How do I send an electron a pizza, I need its address
Quantum mechanics
OR:
How do I send an electron a pizza, I need its address

2. Electrons
Bohr established that electrons “live” in orbits, or energy levels. They need a quanta of energy (which Planck calculated to be found by taking frequency x plancks constant, E=hν) to move between energy levels.
This is the n address line.

5. Quantum mechanical orbital
Within the energy levels, we have sub
levels that contain orbitals
An orbital is a fuzzy cloud like area that
contains 1 or 2 electrons
The electron moves so fast it seems to impart its charge to the whole orbital and we cannot know where it is
This is the l address line, the shape of the orbital set
Sub shells are named s, p, d, and f

6. Each orbital has a specific shape, and take up space in a particular coordinate. So the third address line is the ml which tells which axis orbital line follows.
S orbital only one axis, so only number is 0
P orbital has 3 axis, so number is 0, +1 or -1
D orbital has 5 axis, so number is 0, +1,+ 2,-1, -2
F orbital has 7 axis, so number is 0,+1,+2,+3,-1, -2, -3

7. How do we know the shape. It has to do with the amount of vibration
How do we know the shape? It has to do with the amount of vibration. This page has nice graphics that explain

9. ml = Room number Number the rooms, but the middle room has to be zero.
So s room =0
P rooms =
D rooms =
F rooms =

11. Spin number Have to identify whether they are “head up” or “head down”
= + ½
= - ½

12. Principal Quantum Number
Subshell Shape
Angular Quantum Number
Orientation of Subshell Orbital
Magnetic Quantum Number
Spin
symbol = n
symbol = l
symbol = ml
symbol = ms 1
+1/ /2 2
-1, 0 , +1 3
-2, -1, 0 , +1 , +2 4
-3 , -2, -1, 0 , +1 , +2 , +3

13. Start at (n) energy level
Summary of Orbitals
# of shapes
Max # of e-’s
Start at (n) energy level
Shape s 1 2 1
sphere p 3 6 2
peanut
double peanut d 5 10 3 7 14 4 f

14. By Energy Level First Energy Level only s orbital Second Energy Level
Maximum of 2 e- in s
1s2
1 orbital (12)
Second Energy Level
s and p orbitals are available
Maximum of 2 e- in s & 6 in p
2s22p6
4 orbitals (22)

15. By Energy Level Third energy level s, p, and d orbitals
Maximum of 2 e- in s, 6 in p, and 10 in d
3s23p63d10
9 orbitals (32)
Fourth energy level
s,p,d, and f orbitals
Maximm of 2 e- in s, 6 in p, 10 in d, and 14 in f
4s24p64d104f14
16 orbitals (42)

16. By Energy Level
Any more than the fourth and not all the orbitals will fill up.
You simply run out of electrons
The orbitals do not fill up in a neat order.
The energy levels overlap.
Lowest energy fill first. (i.e. – 3d before 4p)

17. Orbitals fill in order Lowest energy to higher energy.
Adding electrons can change the energy of the orbital.
Half filled orbitals have a lower energy than partially filled.
Makes them more stable.
Changes the filling order

18. Write these electron configurations
Titanium - 22 electrons
Vanadium - 23 electrons
Chromium - 24 electrons

19. Write these electron configurations
Titanium - 22 electrons
1s22s22p63s23p64s23d2
Vanadium - 23 electrons
1s22s22p63s23p64s23d3
Chromium - 24 electrons
1s22s22p63s23p64s23d4 expected
But this is wrong!!

20. Exceptions for Electron Configurations (d & f sublevels)

21. Chromium is actually: 1s22s22p63s23p64s13d5 Why?
This gives us two half filled orbitals.
Slightly lower in energy.
The same principal applies to copper.

22. Copper’s electron configuration
Copper has 29 electrons so we expect: 1s22s22p63s23p64s23d9
But the actual configuration is:
1s22s22p63s23p64s13d10
This gives one filled orbital and one half filled orbital.
Exceptions occur at d4& d9