1. Electron Configuration Notes

2. Ground State –
The lowest energy state of an atom.
Excited State –
State in which an atom has a higher potential energy then it has in its ground state.

3. Heisenberg Uncertainty Principle –
It is impossible to determine simultaneously both the position and velocity of an electron or any other particle. (Can’t exactly predict where electrons will be, just give a general idea.)
Orbital –
Three dimensional region around the nucleus that indicates the probable location of an electron.

4. Principle Quantum Number –
Quantum Numbers –
Numbers that specify the properties of atomic orbital’s and the properties of electrons in orbital’s.
Principle Quantum Number –
(n) The main energy level occupied by the electron.
Positive numbers only  1, 2, 3, etc

5. Angular Momentum Quantum Number – (l) The shape of the orbital.
Starts at 0 and then positive integers till n – 1 is reached
Ex. If n = 2, then l = 0, 1
Ex. If n = 4, then l = 0, 1, 2, 3

6. Orbital Letter Designationss 1 p 2 d 3 f

7. Magnetic Quantum Numbers –
(m) The orientation of an orbital around the nucleus.
Starts at –l and it each integer to l
Ex. If l = 2, then m = -2, -1, 0, 1, 2
Ex. If l = 3, then m = -3, -2, -1, 0 , 1, 2, 3
Ex. If n = 5, then l = 0, 1, 2, 3, 4,
then m = -4, -3, -2, -1, 0, 1, 2, 3, 4

8. Spin Quantum Number –
Indicate the two fundamental spin states of an electron in an orbital.
Can only be + ½ or – ½

9. Quantum Number Relationships in Atomic Structure
Principle
Quantum
Number (Main Energy Level)
Sublevels
In Main Energy Level
Number of Orbital’s per Sublevel
Number of Orbital’s per Main Energy Level
Number of Electrons per Sublevel
Number of Electrons per Main Energy Level 1 s 2 4 8 p 3 6 9 18 d 5 10 16 32 f 7 14

10. Electron Configuration –
The arrangement of electron’s in an atom.
Aufbau Principle –
An electron occupies the lowest energy orbital that can receive it.
Pauli Exclusion Principle –
No two electrons in the same atom can have the same set of four quantum numbers.
Hunds Rule –
Orbital’s of equal energy are each occupied by one electron before any orbital is occupied by a second electron.

11. 1s2
2s2
2p6
3s2
3p6
4s2
3d10
4p6
5s2
4d10
5p6
6s2
4f14
5d10
6p6
7s2
5f14
6d10

12. Orbital Sample 1
The electron configuration of boron is 1s22s22p1. How many electrons are present in an atom of boron? What is the atomic number of boron? Write the orbital notation for boron.

13. Number of electrons =
super scripts added together
Number of electrons =
Number of electrons = 5
Atomic Number = look on PT
Atomic Number = 5

14. Orbital Notation = ___ ___ ___ ___ ___
1s 2s 2px 2py 2pz
Start with the first orbital…
___ ___ ___ ___ ___
Move onto the next orbital…
According to Hunds rule, we have to fill each orbital of the 2p level with one electron first, then go back and fill with the second electron…

15. Orbital Sample 2
The electron configuration of nitrogen is 1s22s22p3. How many electrons are present in a nitrogen atom? What is the atomic number of nitrogen? Write the orbital notation for nitrogen.

16. Number of electrons =
super scripts added together
Number of electrons =
Number of electrons = 7
Atomic Number = look on PT
Atomic Number = 7

17. Orbital Notation = ___ ___ ___ ___ ___
1s 2s 2px 2py 2pz
Start with the first orbital…
___ ___ ___ ___ ___
Move onto the next orbital…
According to Hunds rule, we have to fill each orbital of the 2p level with one electron first, then go back and fill with the second electron…

18. Orbital Sample 3
The electron configuration of fluorine is 1s22s22p5. What is the atomic number of fluorine? How many of its p orbital’s are filled? How many unpaired electrons does a fluorine atom contain?

19. Atomic Number = look on PT
How many of its p orbital’ are filled =
___ ___ ___ ___ ___
1s 2s 2px 2py 2pz
How many of its p orbital’s are filled = 2
How many unpaired electrons does a fluorine atom contain = 1

20. When the s and p orbital’s are filled. s orbital = 2 + p orbital = 6
Octet of Electrons –
When the s and p orbital’s are filled.
Octet = 8
s orbital = 2 + p orbital = 6
2 + 6 = 8
Nobel Gas –
The group 18 elements. No unpaired electrons and all orbital’s of the energy level are full.

21. E- Config. Sample 1
Write both the complete electron-configuration notation and the noble-gas notation for iron, Fe.

22. Write the complete electron-configuration notation…
Figure out number of electrons
In a stable atom, number of protons = number of electrons
Fe = 26
Start writing electron configuration till number of electrons is reached
1s2 2s2 2p6 3s2 3p6 4s2 3d6

23. Write the noble-gas notation…
Find the highest filled p orbital and its Noble gas
3p6 = Ar
Write the noble gas in brackets and then the remainder of the full electron configuration
[Ar] 4s23d6

24. E- Config. Sample 2
Write both the complete electron configuration notation and the noble-gas notation for iodine, I.

25. Write the complete electron-configuration notation…
Figure out number of electrons
In a stable atom, number of protons = number of electrons
I = 53
Start writing electron configuration till number of electrons is reached
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5

26. Write the noble-gas notation…
Find the highest filled p orbital and its Noble gas
4p6 = Kr
Write the noble gas in brackets and then the remainder of the full electron configuration
[Kr] 5s24d105p5

27. E- Config. Sample 3
Without consulting the periodic table or a table in this chapter, write the complete electron configuration for the element with atomic number 25.

28. Write the complete electron-configuration notation…
Figure out number of electrons
Given 25
Start writing electron configuration till number of electrons is reached
1s2 2s2 2p6 3s2 3p6 4s2 3d5