CHEM 1061 1nd Edition Lecture 24Outline of Last Lecture 1. Transition Elements2. Ionization Energya. Ionization Energy for Boron and Oxygenb. Successive Ionization Energy3. Electron Affinity4. Metallic BehaviorOutline of Current Lecture 5. Monoatomic Ions6. Pseudo Noble Gas Configurations7. Transition Elements8. Trends in Ionic Size9. Isoelectronic IonsCurrent LectureMonoatomic IonsMain Group: Why does an ion have a particular charge?11p+/11e- Na:1s(2)2s(2)2p(6)3s(1) [Lose e-, low IE]11p+/10e- Na:1s(2)2s(2)2p(6)Isoelectronic: same number of electronsNa+, Ne, Mg2+ are isoelectronic (all have 10 electrons)82e- Pb: [Xe]6s(2)4f(14)5d(10)6p(2)80e- Pb2+: [Xe]6s(2)4f(14)5d(10)Pseudo Noble Gas Configurations: Fill subshells; stable78 e- Pb4+ : [Xe]4f(14)5d(10)!!Remove electrons from the outermost shell!!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.Transition ElementsRemove e- with the highest n value first (ex: remove 4s before 3d)23e- V : [Ar]4s(2)3d(2)20e- V3+: [Ar]3d(2)Diamagnetic: no unpaired electrons (not attracted to magnetic field [can be slightly repelled]_ex: [Ar]3d(10)Paramagnetic: has unpaired electrons [are attracted to a magnetic field]ex: Mn2+ : [Ar]3d(5)more unpaired=more magneticTrends in Ionic Sizecations = smaller than parent atomshigher charge pulls electrons in p+>e-Anions = larger than parent atom increase shielding and e-/e- repulsions, lower Z(eff)Ex: place the following in order of increasing size. I-, Li+, F-Li+, I-, F-Isoelectronic IonsSame number of electronsCompare the number of protonsLargest proton number, smallest sizeEx: O2-, F-, Na+,
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