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CHEM 111 (69)
Lecture

Orbital energies, electron configuration, Aufbau principle, Hund's rule

4 Pages
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Department
Chemistry
Course Code
CHEM 111
Professor
Dana Johnson

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20 September Announcements More ch. 7 problems 39, 41, 48, 49, 51, 55, 57, 59, 63, 69 Exam 1 High score: 96.6 Median: 62.6 Keys are now on RamCT Scantrons and cover sheets are available From Friday Which statement is TRUE regarding multi – electron atoms? A. Z effs up as the electron is further from the nucleus B. As Z increases, the amount of energy to remove an electron goes down C. Shielding is due to electron – electron repulsion Solution C. A – Zeffes down as the electron is further from the nucleus B – As Z increases, the amount of energy to remove an electron goes up D – Only 3 quantum numbers are necessary to specify the exact location of each electron Orbital energies Shielding and Z contribute to a more complicated picture of orbital energies eff Each orbital has its own energy level, even within a shell (n value) Within a given n value, the lower the l value, the lower the energy Orbital energy: S < p < d < f Electron configuration Arrangement of electrons within an atom Explains periodic characteristics of the elements Written using shorthand: Energy shell number: n Subshell letters: s, p, d, f, grouped together Number of electrons as exponents 1s , 2p , 4d5 Not read as exponents: “one – ess – one” Orbital diagrams: Lines for orbitals Arrows for electrons Aufbau principle From the German “to build up” Electrons fill the lowest energy orbitals first Hydrogen 1s 1 Helium 1s 2 2 1 Lithium 1s 2s Note tha
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