1. Quantum Theory Schroedinger’s Cat Place a cat in a box
Also place a radioactive isotope and a vial of poison
The isotope decays once per hour
If the particle triggers a Geiger counter, the cat dies
If the Geiger counter is not triggered, the cat lives
Seal the box and wait an hour
What happened to the cat?

2. Electromagnetic Spectrum
The speed of light© is 3.00 x 108 m/s

4. Photoelectric Effect
The emission of _________ from a metal when ______________ on the metal
Light had to be a certain ______________ ____for electrons to be emitted
Wave theory of light said that _____________ of light should have worked
This led to the concept of light as a ___________

5. Light as a particle Max Planck (1900)
Hot objects emit light and other forms of electromagnetic radiation, but not continuously, as expected
Instead, it is emitted in small, specific amounts called quanta.
E=hv
H=6.626 x J*s
This number is called Planck’s constant

7. Dual Nature of Light Albert Einstein (1905)
Light behaves as a ________ when it travels through space
Light behaves as a _________ when interacting with matter
Even though it isn’t quite right to do so, you can think of light as a __________________ that travels as a wave
A _________ is a massless bundle of light
E photon=hv
Some metals hold electrons more tightly than others and require ____________________ to move electrons

8. Emission Spectra Ground State ___________ energy state of an electron
Excited State
___________ energy state
Energy is absorbed to move from ___________ ___________ states and is released as ___________ ___________ when returning to the ground state
___________ ___________ of light are emitted for any given element
___________ spectrum- ___________ range of em light(rainbow)
(Bright) Line emission spectrum-Only ___________ ___________ of light are seen

9. The Bohr Model Niels Bohr (1913)
Allowed for electrons to have ___________
Electrons have ___________ energies
Lower energy- ___________ to nucleus
Higher energy- ___________ from nucleus
Electrons can ___________ energy to raise to the next energy level and ___________ the same energy when falling to the ground state
This model works well for ___________ but not for other elements

10. Electrons as Waves Louis de Broglie (1924)
Suggested that electrons could be considered as ___________ confined to the space around a nucleus
___________ - bending of light around edges
Wave Interference- when waves ___________

11. Quantum Theory Werner Heisenberg (1927) The Uncertainty Principle
One cannot simultaneously know the ___________ and ___________ of an electron

12. Quantum Theory Erwin Schroedinger (1926)
Wave Equation- The quantization of an electron’s energies is an outcome
Quantum Theory-mathematically describes wave properties of ___________ and other ___________ ___________

13. Atomic Orbitals and Quantum Numbers
Quantum Numbers- properties of ___________ ___________ and properties of ___________ in orbitals
Like the address of an electron or a seat in a stadium or theater

14. Principal Quantum Number
1,2,3
K,L,M
This would be like the section on a ticket for a stadium seat

15. Angular Momentum Quantum Number
___________ of an orbital
0,1,2,3
s,p,d,f
Like the row in a stadium or theater

16. Magnetic Quantum Number
___________ of an orbital around the nucleus
+1 to -1
Like finding your seat in a stadium or theater

17. Spin Quantum Number Ms Fundamental ___________ of an electron
+1/2 or -1/2
A single orbital can hold up to a maximum of ___________ of ___________ spin
This would be which direction you are facing in a theater or stadium seat

19. Some Quantum Theory Rules
Pauli Exclusion Principle- No two electrons have the same set of ______________________ .
Or An orbital within a sublevel can contain up to ___________ of opposite spin
Hund’s Rule- Each orbital within a ___________ receives an electron of ___________ spin before any can receive an electron of ___________ spin