1. ELECTRONS IN ATOMS

2. Electrons in Atoms
The chemical properties of atoms, ions, and molecules are related to the arrangement of the ELECTRONS within them.

3. Quantum Numbers: Where is the electron??
In Schrodinger’s model, there are four quantum “numbers” that tell us where an electron is likely to be located.
Principal (n), 1-7, gives the energy level
Sublevel (l), s-p-d-f, gives the shape of region
Orbital (m), gives the orientation in space of the shapes
Spin (s), clockwise or counterclockwise
No two electrons have the same 4 quantum numbers.

4. Principal Quantum Number (n)
Designates the energy level
Tells how far away from the nucleus an electron is likely to be.
Assigned values in order of increasing energy: n = 1, 2, 3, 4, 5, 6, or 7
Corresponds to the period (row)on the periodic table.

5. Principal Quantum Number (n)
Lower value of n means the electron is closer to nucleus and has less energy. +
n = 1
n = 2
n = 3

6. Sublevels (l), s-p-d-f (Shapes)
Within each principal energy level there are a certain number of sublevels
Energy level 1 has 1 sublevel; energy level 2 has 2 sublevels; energy level 3 has 3 sublevels, etc.
These sublevels are called s, p, d, or f.
Each sublevel has a unique shape
These shapes describe the region of space where the electron is likely to be located s p d

7. Principal Energy Level
Subshell, (l), s-p-d-f
Principal Energy Level
Number of Subshells
Type of Subshell
n = 1 1 1s
n = 2 2
2s, 2p
n = 3 3
3s, 3p, 3d
How many sublevels will principal energy level 4 have, and what shapes will they be?

8. Orbitals (m) Each orbital can only hold 2 electrons.
(The orbital names s, p, d, and f stand for names given to groups of lines in the spectra of the alkali metals. These line groups are called sharp, principal, diffuse, and fundamental—This is not important.)
Within each sublevel there are a certain number of orbitals.
s sublevel—1 orbital
p sublevel—3 orbitals
d sublevel—5 orbitals
f sublevel—7 orbitals
Orbitals within each sublevel have similar shapes, but are oriented differently in space.
Each orbital can only hold 2 electrons.

9. s - orbitals Spherical shape Hold a maximum of 2 electrons
First found in the 1st energy level

10. p-orbitals Pear or dumbbell shaped 3 different orientations
Each orientation holds a max of 2 e-
The p sublevel as a whole holds a maximum of 6 e-
First found in the 2nd energy level
p-orbitals

11. d - orbital 5 different orientations Each holds 2 e-’s
The sublevel as a whole holds a maximum of 10 e-
First found in the 3rd energy level

12. "f" Atomic Orbitals
Do not appear until the 4th shell (energy level) and higher.

13. Maximum eֿs Allowed
The maximum # of electrons that can occupy a principal energy level is given by the formula 2n².
How many eֿs are allowed in energy level 3? 18

14. Let’s Review How many orbitals are in the following sublevels? 3p 2s 33d 3 1 7 3 5

15. Electron Configuration:
How are the electrons in any given element arranged?
In an atom, electrons are positioned around the nucleus in the most stable arrangement possible.
This is the arrangement that has the lowest energy.
There are 3 important rules to help us find the configuration of electrons in atoms.

16. Aufbau’s Principle
Electrons will occupy orbitals having the lowest energy FIRST and then in order of increasing energy.
The "Ground State" of an atom is when every electron is in its lowest energy orbital.

17. Pauli’s Exclusion Principle
An orbital can be empty, have one electron, or AT MOST have two electrons.
Electrons occupying the same orbital must have opposite spins!
One clockwise, and one counter clockwise

18. Hund’s Rule
When electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins.