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apKotzChp8WS - AP Chemistry Practice Atomic Electron...

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AP Chemistry Practice Atomic Electron Configurations and Chemical Periodicity Name: ____________________________ Date: __________________ Period: ____ 1. Must all atoms having an odd atomic number be paramagnetic? Must all atoms having an even atomic number be diamagnetic? Explain. 2. Which of the following orbital diagrams are possible for a ground-state electron configuration and which are not? If the orbital diagram is not allowed state why it is not. a) ↑↓ ↑↓ ↑↓ ↑↑ ↑↓ 1s 2s 2p b) ↑↓ ↑↓ ↑↓ ↑↓↑ 1s 2s 2p c) ↑↓ ↑↓ 1s 2s 2p d) ↑↓ ↑↓ 1s 2s 2p e) ↑↓ ↑↓ 1s 2s 2p 3. What principle(s) or rule(s) does each of the following electron configurations violate? a) 1s 2 2s 6 3s 2 b) 1s 2 2s 2 2p 7 3s 1 c) 1s 2 2s 2 2p 6 2d 3 4. Use orbital box diagrams to represent the electron configurations of a) Br - b) Ni 2+ c) Sb 3+ d) Te 2- (Part of your diagram may be a noble gas core abbreviation) 5. Use the relationship between electron configurations
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This note was uploaded on 12/07/2011 for the course CHEM 100 taught by Professor Feebeck during the Fall '10 term at Purdue.

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apKotzChp8WS - AP Chemistry Practice Atomic Electron...

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