Chem 1061 1st Edition Lecture 21 Outline of Last Lecture 1 Energy Levels in H atom 2 Ionization Energy 3 Conversions 4 Energy Levels in H Atom 5 Absorbance 6 Wave Particle Duality Outline of Current Lecture 7 Energy Splitting with Multiple Electrons a Electrostatic Effects i Nuclear Charge ii Electron Repulsions b Inner Orbitals c Penetration 8 Electron Configuration Current Lecture Energy Splitting with Multiple Electrons M l and m l describe the orbital M s describes the electron No two electrons in the same orbital can have the same four quantum numbers QNs exclusion principle Electrostatic Effects a nuclear charge How does the number of protons Z in nucleus affect electron energy Z 1 H 1s electron Z 2 He 1s electron Z 3 Li2 1s electron All are one electron specie but have a different Z These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute Compare Ionization Energy Ionization energy is a measure of how strongly an electron is attracted to the nucleus H 1311 KJ He 5250 KJ Li2 11615 KJ More protons higher nuclear charge stronger attraction It is more difficult to remove electron requires more energy b Electron Repulsions same orbital He vs He He to remove 2372 KJ mol He to remove 5250 KJ mol Higher ratio of protons to electrons make it easier to remove Example mom and dad has divided attention with two kids e in comparison to undivided with one kid e 2 Inner Orbitals shielding net nuclear charge Z eff Li vs Li2 Li to remove 520 KJ mol Li2 to remove 2954 KJ mol Example older children bigger can get away from mom and dad have more freedom because the mom and dad are focused on the small child e but when it is only the older child they focus more on you e no screening of other electrons on outer Greater shielding by inner electrons Easier to take e from Li atom because of repulsion from 2e in 1s orbital shield effective nuclear charge reducing Z eff 3 Penetration How do we know e in 2s is lower in energy than 2p 2s spends more time closer to nucleus than 2p Energy within a given shell S P D F Filling in orbitals with elow high E fill periodic table Electron Configuration Ls 1 l n value s l value 1 how many e in orbital described
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