BLUE QUESTIONS

BLUE QUESTIONS - B LUE QUESTIONS: Well, UV is a higher...

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Well, UV is a higher energy wave than visible light, so the electron can be excited up many energy levels by a single UV photon. Then it will spontaneously drop down these energy levels one at a time at a later time, emitting lower energy photons i.e. in the visible. 1. Purple line: 410 Light Purple line:440 Green:485 Red:655 2. Case 1:Higher-Lower (Energy is emitted) Case 2: Lower to Higher (Energy is absorbed) Case 3: Higher to Lower (Energy is emitted) 3. ASK TEACHER! 4. This is not possible because n must be a whole number. Either the electron gains the energy and jumps one full shell or it does not jump at all. GREEN QUESTIONS! 1. Bohr’s model was a success because it was able to describe why the light spectrum looked as it did. He gave us the idea of orbitals. 2. His significant problem was that his ideology only worked for Hydrogen gas spectrum. 3. The new area was quantum physics. He used the principal of quantized energy in the atom and played with it. ORANGE QUESTIONS
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This note was uploaded on 05/31/2011 for the course CHEM 4U taught by Professor Jargin during the Spring '11 term at York University.

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BLUE QUESTIONS - B LUE QUESTIONS: Well, UV is a higher...

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