Lecture 20 - Energy of orbitals in a single electron atom Energy only depends on principal quantum number n n=3 n=2 En =-RH 1 n2 n=1 7.7 Energy of

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Energy of orbitals in a single electron atom Energy only depends on principal quantum number n E n = -R H ( ) 1 n 2 n=1 n=2 n=3 7.7
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Energy of orbitals in a multi -electron atom Energy depends on n and l n=1 l = 0 n=2 l = 0 n=2 l = 1 n=3 l = 0 n=3 l = 1 n=3 l = 2 7.7
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“Fill up” electrons in lowest energy orbitals ( Aufbau principle ) H 1 electron H 1s 1 He 2 electrons He 1s 2 Li 3 electrons Li 1s 2 2s 1 Be 4 electrons Be 1s 2 2s 2 B 5 electrons B 1s 2 2s 2 2p 1 C 6 electrons ? ? 7.7
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C 6 electrons The most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins ( Hund’s rule ) . C 1s 2 2s 2 2p 2 N 7 electrons N 3 O 8 electrons O 1s 2 2s 2 2p 4 F 9 electrons F 1s 2 2p 5 Ne 10 electrons Ne 1s 2 2s 2 2p 6 7.7
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Electron Configuration & the Periodic Table the Group number corresponds to the number of valence electrons the length of each “block” is the maximum number of electrons the sublevel can hold the Period number corresponds to the principal energy level of the valence electrons
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This note was uploaded on 05/20/2008 for the course CHEM 115 taught by Professor Larkin during the Spring '08 term at Bloomsburg.

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Lecture 20 - Energy of orbitals in a single electron atom Energy only depends on principal quantum number n n=3 n=2 En =-RH 1 n2 n=1 7.7 Energy of

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