1. Electron Orbitals
Cartoon courtesy of lab-initio.com

2. Quantum Mechanical Model of the Atom
The model says that the nucleus is surrounded by a space in which electrons orbit- the electron cloud.

3. The model says that the electron cloud is divided the following parts:
The electron cloud is divided into energy levels (n) numbered 1,2,3,4,… to infinity(∞)
Each energy level is divided into sublevels. (s,p,d,f)
Each sublevel is divided into orbitals. Regardless of which energy level it resides, sublevel s has 1 orbital. Sublevel p has 3 orbitals. Sublevel d has 5 orbitals. Sublevel f has 7 orbitals. (Note: the pattern continues to go up by odd numbers.)
4) Each orbital can hold a maximum of 2 electrons with opposite spins.

4. 1) Electron Energy Levels
“n” is also known as the Principle Quantum number
Formula to find the total number of electrons that can fit in an energy level:
2n2
n 1 is closest to the nucleus.

5. The electron cloud is divided into energy levels (n) numbered 1,2,3,4,… to infinity(∞)
n1 is closest to the nucleus.
The farther out from the nucleus the more energy the level has.

6. 2) Each energy level is divided into sublevels
2) Each energy level is divided into sublevels. -Level 1 has 1 sublevel (s). -Level 2 has 2 sublevels (s,p). - Level 3 has 3 sublevels (s,p,d). -Level 4 has 4 sublevels (s,p,d,f). Sublevels continue to be labeled with letters. After s,p,d,f they just go through the rest of the alphabet (g,h,i, etc.).

7. 3) Each sublevel is divided into orbitals.

8. What is an Electron Orbital?
An orbital is a region within an energy level where there is a probability of finding an electron.
Orbital shapes are defined as the surface that contains 90% of the total electron probability.

9. Scientists can not draw the path the electrons take in the orbital because…
To plot a path for something you need to know exactly where the object is and be able to work out exactly where it's going to be an instant later. You can't do this for electrons.

10. Heisenberg Uncertainty Principle
“One cannot simultaneously determine both the position and momentum of an electron.”
You can find out where the electron is, but not where it is going.
OR…
You can find out where the electron is going, but not where it is!
Werner
Heisenberg

11. Orbital shapes
Regardless of which energy level it resides, sublevel s has 1 orbital.
Sublevel p has 3 orbitals.
Sublevel d has 5 orbitals.
Sublevel f has 7 orbitals.

12. s Orbital shape The s orbital has a spherical shape centered around
the origin of the three axes in space.

13. p orbital shape
There are three dumbbell-shaped p orbitals in each energy level above n = 1, each assigned to its own axis (x, y and z) in space.

14. d orbital shapes
Things get a bit more complicated with the five d orbitals that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbbells”
…and a “dumbbell
with a donut”!

15. Shape of f orbitals

16. Electron Spin
4) Each orbital can hold a maximum of 2 electrons with opposite spins.
Electron spin describes the behavior (direction of spin) of an electron within a magnetic field.
Possibilities for electron spin:
Forward, backward

17. Pauli Exclusion Principle
Two electrons occupying the same orbital must have opposite spins
Wolfgang
Pauli

18. Principles of electron configurations:
Aufbau Principle: Electrons enter the orbital of the lowest energy level first.
Hund’s Rule: Electrons enter the orbital of equal energy and then pair up.
Pauli Exclusion Principle: Two electrons occupying the same orbital must have opposite spins
Let’s Practice!!!

19. Orbital filling table

21. Electron configuration of the elements of the first three series

22. Element
Atomic #
Configuration
notation
Orbital notation
Lithium, 3
p+= 3
e- = 3
____ ____ ____ ____ ____
1s s p
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neo

23. Periodic Trends Blocks can be grouped according to the sublevels
s block – Group 1A ands 2A
p block – Group 3A through 8A
d block – the transition metals/elements
f block – the Inner Transition Metals

24. Practice
Then a few more things….

26. Examples Beryllium – row 2 =period 2, block 2s Be- 1s2 2s2
Row number = period = energy level
Hydrogen- row 1= period 1, block 1s
H-1s1
Beryllium – row 2 =period 2, block 2s
Be- 1s2 2s2
Carbon – row 2 =period 2, block 2p
C- 1s2 2s2 2p2

28. The Exceptions!
1. Transition elements (d sublevel)-
The energy level is 1 less than the row/period #
Ex: Sc- period 4d but it will end in 3d!
Sc- 1s2 2s2 2p6 3s2 3p6 4s2 3d1
2. Inner transition metals (f sublevel)-
The energy level is 2 less than the row /period #
Ex: Dy- period 6f but it will end in 4f!
Dy- 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4P6 5s2 4d10 5p6 6s2 4f9