CHEM 1061 1nd Edition Lecture 23Outline of Last Lecture II. Electron Configuration for Cl, Br, and IIII. Transition ElementsIV. Periodic Trendsa. Atomic Size (Radius)b. Ionization Energyc. Electron Affinity Outline of Current Lecture V. Transition ElementsVI. Ionization Energya. Ionization Energy for Boron and Oxygenb. Successive Ionization EnergyVII. Electron AffinityVIII. Metallic BehaviorCurrent LectureTransition ElementsStay about the same size (radius doesn't really grow or shrink)Place the following in order of:A) Increasing atomic size of Ca, Rb, and KCa < K < RbB) Decreasing atomic size of Ca, O, and SeCa > Se > OIonization Energy (IE1) <-- important for laterAtom(g)--> ion+(g) + e-(Delta)H = IE1 <-- first ionization energyH is positive because reaction is endothermicEnergy is required to remove outermost e- 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.Ex: place in order of increasing IE1 Ca Rb KRb < K < Ca Why do B and O families fall out of trend?Electron configurations Li: [He]2s1Be: [He]2s2B: [He]2s22p1C: [He]2s22p2N: [He]2s22p3O: [He]2s22p4F: [He]2s22p5Removing on electron makes it have full or half filled sub shells which are more stable and thus easier to remove. B and O trend go down periodic table (B and O family easier to remove electron)Successive Ionization Energy (IE2, IE3, ETC)Atom(g) ion+(g) + e- (IE1)ion+(g) ion2+(g) + e- (IE2)ion2+(g) ion3+(g) + e- (IE3)ETC…IE1 < IE2 < IE3 (for increase in ionization energy or delta H)Table 8.5 Delta H for Li, Be, and BIE1 IE2 IE3 IE4Li 0.52 7.30 11.80 -Be 0.90 1.76 14.85 -B 0.80 2.46 3.66 25.02Li: 1s(2)2s(1)2s(1) = IE1 (valence electrons)1s(2) = IE2 and IE3 (core electrons)!! Big jumps in IE means you are starting to remove core electrons !!Be: 1s(2)2s(2)2s(2)= IE1 + IE2 (valence)1s(2) = IE3 + IE4 (core)B: 1s(2)2s(2)2p(1)2s(2)2p(1) = IE1 + IE2 + IE3 (valence)1S(2) = IE4 + IE5 (core)Electron Affinity (EA1)“opposite from ionization”Atom(g) + e- ion-(g) Delta H is necagtive (generally exothermic with some exceptions)The more northeast on the periodic table, the easier it is to add e-Metallic BehaviorMetals:low IE1 (easier to remove e-)lower (smaller, less negative) EA1 (harder to add e-)metals like to form cationsNonmetals:high IE1 (hard to remove e-)higher (larger, more negative) EA1 (easier to add e-)Metal vs. Nonmetal OxidesMetal Oxides:CaO(s) + H2O(l) Ca(OH2)(aq) baseThe more metallic the elementthe more basic the oxideNon Metal Oxides:CO2(g) + H2O(l) H2CO3(aq)More
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