1. Objectives
To learn about the shapes of the s, p and d orbitals
To review the energy levels and orbitals of the wave mechanical model of the atom
To learn about electron spin

2. A. The Hydrogen Orbitals
Orbitals do not have sharp boundaries.
90% boundary

3. A. The Hydrogen Orbitals
Hydrogen Energy Levels
Hydrogen has discrete energy levels.
Called principal energy levels (electron shells)
Labeled with whole numbers
Energy is related to 1/n2
En = E1/n2
Energy levels are closer together the further they are from the nucleus

4. A. The Hydrogen Orbitals
Hydrogen Energy Levels
Each principal energy level is divided into sublevels.
Labeled with numbers and letters
Indicate the shape of the orbital

5. Orbital Designations

6. Orbitals Define the Periodic Table

7. A. The Hydrogen Orbitals
Hydrogen Energy Levels
The s and p types of sublevel

8. Representation of s, p, d atomic orbitals

9. A. The Hydrogen Orbitals
Why does an H atom have so many orbitals and only 1 electron?
An orbital is a potential space for an electron.
Atoms can have many potential orbitals.
s, p, d, f orbitals named for sharp, principal, diffuse and fundamental lines on spectra. Further orbitals designated alphabetically

10. s p d d f f f g g g g

11. B. The Wave Mechanical Model: Further Development
Electron Spin
Close examination of spectra revealed doublets
Need one more property to determine how electrons are arranged
Spin – electron modeled as a spinning like a top
Spin is the basis of magnetism

12. B. The Wave Mechanical Model: Further Development
Pauli Exclusion Principle
Pauli Exclusion Principle (Wolfgang Pauli 1925) - an atomic orbital can hold a maximum of 2 electrons and those 2 electrons must have opposite spins
When an orbital contains two electrons (of opposite spin) it is said to be full
What are the four descriptors that define an energy level / electron’s position in an atom?