1. Quantum Theory

2. Quantum Theory (based partly on Heisenberg’s Uncertainty Principle)
The position and the momentum of a moving object cannot simultaneously be measured and known exactly
There is an inherent limitation to knowing both where a particle is at a particular moment and how it is moving in order to predict where it will be in the future

3. Quantum Theory
An electron is in an orbital – probability space where an electron can be found a certain percentage of the time as defined by Shrodinger’s equations
An orbital can hold 2 electrons (this means the bigger the energy level, the more orbitals it has)
Schrodinger’s equations (once all the math has been done) describe where a particular electron is likely to be found

4. We can know 4 pieces of information about the location of any electron within an atom.
1. Energy Level (n)
Distance from the nucleus
Options: 1 – 7
2. Sublevel (l)
Shape
3. Magnetic Orientation (lm)
Direction the shape is pointing (think; x, y, z)
4. Spin (ls)
How the electron is spinning (the options are up or down)
We write an up electron as a half arrow up ( ) and a down electron as a half arrow down ( )

5. This table (p.8) summarizes what we can know.
Type of information
Label
What it represents
How many options?
How many e- can it hold?
Energy Level n
Distance from the nucleus
n=1 through n=7
2n2
Sublevel l
Shape
n = 1  1 sublevel (s)
n = 2  2 sublevels (s, p)
n = 3  3 sublevels (s, p, d)
n = 4  4 sublevels (s, p, d, f)
Level 1 = ______
Level 2 = ______
Level 3 = ______
Level 4 = ______
Level 5 = ______
Magnetic lm
Orientation of Orbital (which direction it is pointing)
Depends on the number of sublevels.
p-orbitals follow the x, y, and z axes (one orbital per axis)
(each orbital can hold 2 electrons)
Spin ls
How electron is spinning
Up = + ½
Down = - ½
The spinning of electrons generates an electric field.
For 2 electrons to occupy the same orbital they must have opposite spin. 2 8 18 32 50

6. Shapes (remember, these are plotted using Schrodinger’s Equation)
s sublevels are spheres:
p sublevels look like peanuts (maybe?) (notice the orientation along the x, y, or z axis):

7. Shapes
d sublevels look like… (don’t worry about the orientation, you need to know there are 5 of them):
f sublevels look like…? (you need to know there are 7 of them)

8. Shapes
Also, g sublevels are a theoretical thing…but we haven’t made any elements that require them in their ground state yet.

9. Describing the Location of Electrons in an Atom
To determine the electron configuration of an atom, 3 guidelines are followed:
3. Pauli Exclusion Principle: (electron self esteem)
No two electrons in the same atom have the same 4 quantum numbers.
Taken together, the four quantum numbers describe the state of a particular electron. For example, an electron may have these quantum numbers: 1, 0, 0, -1/2 (corresponding to n, l, lm and ls). Think of these as a social security number for an individual, or a street address for a house. No two are identical.

10. Describing the Location of Electrons in an Atom
To determine the electron configuration of an atom, 3 guidelines are followed:
1. Aufbau Principle: (electrons are lazy)
Electrons are added one at a time to the lowest energy available orbital.
1s is filled first, then 2s, 2p, 3s, 3p …

11. Describing the Location of Electrons in an Atom
To determine the electron configuration of an atom, 3 guidelines are followed:
2. Hund’s Rule: (electrons are mildly antisocial)
Electrons occupy equal energy orbitals so the maximum number of unpaired electrons result.
Equal energy orbitals are “degenerate orbitals”; for example, px, py, and pz are degenerate orbitals. (This means they are equal energy.)

12. Summary of energy levels, sublevels, and orbitals
Principal energy level
Sublevel
Orbitals
n = 1 1s
1s (one)
n = 2
2s, 2p
2s (one) + 2p (three – x,y,z)
n = 3
3s, 3p, 3d
3s (one) + 3p (three – x,y,z) + 3d (five – xy,xz, etc.)
n = 4
4s, 4p, 4d, 4f
4s (one) + 4p (three – x,y,z) + 4d (five – xy,xz, etc.) + 4f (seven – xyz, etc.)

13. Number of electrons in each sublevel
Number of Orbitals
Maximum # of electrons (two per orbital) s p d f 1 2 3 6 5 10 7 14

14. This diagram helps show the differences in energy for each sublevel within an electron cloud. Working from bottom to the top, you can see how each atom’s electrons fill. Use it to write in the electrons for a neutral atom of Phosphorous (15 electrons)

15. Neutral atom of Phosphorous (15 electrons)