1. Quantum Model of the Atom

2. Do Now
What do we know about the atom based on Bohr’s model?

3. Bohr’s Model Central nucleus Electrons revolved in circular orbits
However, only worked for hydrogen

4. The Quantum Model 1926- proposed by Schrödinger
Treated the electron like a wave
Heisenberg’s Uncertainty Principle
it is impossible to know the velocity and position of a particle at the same time
Therefore it is nearly impossible to know the exact location of an electron at any exact moment.

5. Like Bohr’s model, there are different energy levels
As electrons travel away from the nucleus, they require more energy
Like climbing a ladder
The high your climb, the more energy you use

6. Orbital Shapes
Inside each energy level there are different shaped orbitals s p d f
(in order of increasing energy)

7. First Energy Level 1 sublevel s-shaped orbitals Has one sub-orbital
Holds 2 electrons

8. Second Energy Level 2 sublevels s-shaped p shaped 1 sub-orbital
Holds 2 electrons
p shaped
3 sub-orbitals
Holds total of 6 electrons (2 per sub-orbital)

10. Third Energy Level 3 sublevels s-shaped p-shaped d-shaped
1 sub-orbital
Holds 2 electron
p-shaped
3 sub-orbitals
Holds 6 electrons
d-shaped
5 sub-orbitals
Holds 10 electrons (2 per sub-orbital)

11. Fourth Energy Level 4 sublevels s-shaped p-shaped d-shaped f-shaped
1 sub-orbital
Holds 2 electrons
p-shaped
3 sub-orbitals
Holds 6 electrons
d-shaped
5 sub-orbitals
Holds 10 electrons
f-shaped
7 sub-orbitals
Holds 14 electrons

13. Each energy level acquires a sublevel
Each sublevel is a different shaped orbital

14. Aufbau’s Principle
Electrons will occupy the lowest available energy level first
Energy levels closest to the nucleus have less energy
Like climbing a ladder

15. Pauli’s Exclusion Principle
Hund’s Rule
Electrons will occupy each sub-orbital before pairing up
School bus
Pauli’s Exclusion Principle
When electrons are paired together, they will spin in opposite directions