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An in-depth understanding of electronic configurations in atoms through two different methods: spdf notation and orbital diagrams. the principles of filling electrons, the first three rows of the periodic table, rules for writing electron configurations, exceptions, and solved problems. Key concepts include Pauli's exclusion principle, Hund's rule, and Aufbau principle.
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Dr. Sapna Gupta
H 1 s 1 He 1s^2 Li 1s^2 2s^1 Be 1s^2 2s^2 B 1s 2 2s 2 2p 1 C 1s 2 2s 2 2p 2 N 1s^2 2s^2 2p^3 O 1s^2 2s^2 2p^4 F 1s^2 2s^2 2p^5 Ne 1s 2 2s 2 2p 6 Na 1s^2 2s^2 2p^6 3 s^1 Mg 1s 2 2s 2 2p 6 3 s 2 Al 1s 2 2s 2 2p 6 3 s 2 3 p 1 Si 1s^2 2s^2 2p^6 3 s^2 3 p^2 P 1s^2 2s^2 2p^6 3 s^2 3 p^3 S 1s^2 2s^2 2p^6 3 s^2 3 p^4 Cl 1s 2 2s 2 2p 6 3 s 2 3 p 5 Ar 1s 2 2s 2 2p 6 3 s 2 3 p 6 Row 1 Row 2 Row 3
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5 1s 2 2s 2 3 s 2 2p 6 4 s 2 5 s 2 3d 10 4 d 10 3 p 6 4 p 6 5p 5
A paramagnetic substance is one that is weakly attracted by a magnetic field, usually as the result of unpaired electrons. A diamagnetic substance is not attracted by a magnetic field generally because it has only paired electrons. Visit UC Davis ChemWiki for more information.