1. Quantum Warmup #1
1) What is the difference between an electron orbit as described by Bohr and orbital described by modern quantum theory?
Answer:
orbit = precisely defined path
orbital = region of space around nucleus in there is a high (90% probability of finding an electron)

2. Orbital: a region of space (3D) where there is a high (90%) probability of locating an electron.
Orbital ≠ Orbit

3. Warmup #1
2a) Describe what is observed when salts of Li, Na, Cu, Sr and K are heated strongly in a flame.
2b) Write an essay using the word bank below and draw a labeled diagram to support your answer that explains what is happening inside the atom that produces the different colors of light.
Word Bank: Atoms, Heat Energy, Electrons, Quantized Energy Levels, Absorb Energy, Ground State, Quantum Leap, Excited State, Emits Light Energy, Different colors of light

4. Link to flame tests
Fireworks
Lithium Copper Strontium

5. Sample answer
Each atom contains electrons with quantized energy levels, meaning only certain specific energy values are allowed. When heat energy from the flame is added to the atoms, the electrons absorb the energy. Electrons in the ground state (lowest energy quantum level) absorb the energy and make a quantum leap to higher energy excited states. The electrons are only able to remain in the excited state for a very brief time. When electrons make a quantum leap from a higher energy excited state to a lower state, they emit (release) the exact difference in energy between the excited state and ground state in the form of light. The different colors of light emitted are the result of different energies between excited and ground states.

6. Diagram of Quantum Leaps
Absorption of Heat Energy
Emission of Light Energy e-
EXCITED STATE e-
GROUND STATE