1. Atomic Structure: The Quantum Mechanical Model

2. The Bohr Model of the Atom
I pictured the electrons orbiting the nucleus much like planets orbiting the sun.
However, electrons are found in specific circular paths around the nucleus, and can jump from one level to another.
Niels Bohr

3. Bohr’s model of the Atom
Energy level of an electron
analogous to the rungs of a ladder
The electron cannot exist between energy levels, just like you can’t stand between rungs on a ladder

4. The Quantum Mechanical Model of the Atom
Energy is “quantized” - It comes in chunks.
A quantum (quanta - plural) is the amount of energy needed to move from one energy level to another.
Since the energy of an atom is never “in between” there must be a quantum leap in energy.
In 1926, Erwin Schrodinger derived an equation that described the energy and position of the electrons in an atom.

5. Schrodinger’s Wave Equation
Erwin Schrodinger
Erwin Schrodinger

6. The Quantum Mechanical Model
Has energy levels for electrons.
Orbits are not circular.
It can only tell us the probability of finding an electron a certain distance from the nucleus.

7. The Quantum Mechanical Model
The electrons are found inside a blurry “electron cloud”
An area where there is a chance of finding an electron.
Think of fan blades
It’s within this area that we derive the electron configuration for an atom.

8. Principal Quantum Number
Generally symbolized by “n”, it denotes the shell (energy level/discrete energy level) in which the electron is located.
The lowest energy levels
fill up first…. :

9. Principal Quantum Number (n) = the energy level of the electron: 1, 2, 3, etc.
Within each energy level, the complex math of Schrodinger’s equation describes several shapes (s, p, d, f).
Within these “sublevels” (aka orbitals or suborbitals), there is a high probability (not certainty) of finding an electron.
These numbers and letters are the basis for writing electron configurations (which we’ll get to later)…

10. Summary 2 6 10 14 # of shapes (orbitals) Maximum electrons
Starts at energy level 2 s 1 1 p 3 6 2 10 d 5 3 7 14 4 f

11. It was actually the study of light that led to the development of the quantum mechanical model.
Matter can behave as particles and waves
The QM model treats an electron as a wave
So it was the study of light, a kind of electromagnetic radiation, that allowed scientists to “see” electrons and waves and particles.
Electromagnetic radiation includes many types: gamma rays, x-rays, radio waves…

12. Low Energy
High Energy
Radiowaves
Microwaves
Infrared .
Ultra-violet
X-Rays
GammaRays
Low Frequency
High Frequency
Long Wavelength
Short Wavelength
Visible Light

13. Parts of a wave
Crest
Wavelength
Amplitude
Origin
Trough

14. Wavelength and Frequency
Are inversely related
As one goes up the other goes down.
Different frequencies of light are different colors of light.

15. Energy and Frequency Are directly related
As one goes up the other goes up.

16. Long Wavelength = Low Frequency Low ENERGY Short Wavelength =
Wavelength Table
Long
Wavelength =
Low Frequency
Low ENERGY
Short
Wavelength =
High Frequency
High ENERGY

17. Atomic Spectrum Each element gives off its own characteristic colors.
Can be used to identify the atom.
This is how we know what stars are made of.

18. These are called the atomic emission spectrum
Unique to each element, like fingerprints!
Very useful for identifying elements

19. Explanation of atomic spectra
The energy level, and where the electron starts from, is called it’s ground state - the lowest energy level.

20. Changing the energy
Let’s look at a hydrogen atom, with only one electron, and in the first energy level.

21. Changing the energy
Heat, electricity, or light can move the electron up to different energy levels. The electron is now said to be “excited”

22. Changing the energy
As the electron falls back to the ground state, it gives the energy back as light

23. This is a simplified explanation!
Ultraviolet
Visible
Infrared
The further they fall, more energy is released and the higher the frequency.
This is a simplified explanation!
The orbitals also have different energies inside energy levels
All the electrons can move around.

24. Wave-Particle Duality
Like electrons, light can behave as both particles (packets called photons) and waves.

25. Wave-Particle Duality
J.J. Thomson won the Nobel prize for describing the electron as a particle.
His son, George Thomson won the Nobel prize for describing the wave-like nature of the electron.
The electron is a particle!
The electron is an energy wave!