Anomalous ConfigurationsChromium, copper do not follow patternsCr= 1s2, 2s2 2p6 3s2 sp6 3s5 4s1Cu=1s2 2s2 2p6 3s2 3p6 4s1 3d10Anomalies arise from stability associated with half-filled and completely filled d-subshellsPeriodic table arranged based on electron configurationsCh, Mo, Cu, Ag, AuEverything else follows the same pattern(http://hyperphysics.phy-astr.gsu.edu/hbase/pertab/cr.html)Electron Configuration of IonsFormation of Ions:Gain/loss of valence electron to achieve stable electron configuration (filled shell)Gain an electron-Loose and electron-Cations: positive (loosing electrons)The more electrons you remove, the smaller its going to getAnions: negative (gaining electrons)Electrons will form ions that will allow them to get to the closest noble gas configurationIsoelectronic Atoms/IonsWhen you have the same electron configurations for two speciesMain group elements:Form ions by gain/loss of e- to obtain noble gas configurationsIsoelectronic: describes atoms/ions having identical electron configurationsBased on the row of the main group element, we can figure out what kind of ions they’re going to form (with a few exceptions)Cations of Transition MetalsTransition metal cations:Loss of valence electron (s) and, in some cases, d electronsFe: [Ar]3d 6 4s 2Fe 2+ : [Ar]3d64s2= [Ar]3d6 (loss of valence e-Fe 3+ : [Ar]3d6 = [Ar]3d5 (loss of one 3d= half filled d subshell)Sizes of Atoms/IonsAtomic radius- half the distance btw identical nuclear centers in a molecule (i.e. covalent radius)Metallic Radius- half the distance between nuclear centers in the crystal of a metalIonic Radius- derived from the distance between nuclear centers in ionic crystalsHow big is this element and what happens to the size of this element when we add and subtract electronsAtomic Radius TrendsAtomic Radii:Increase going down a family“Shielding” by inner shell electrons decreases effective nuclear (Zeff)Decrease going across a rowIncreased nuclear charge (z) moving across rowIncreased attraction for electrons in inner orbitals  atomic size decreasesCHEM 111 1nd Edition Lecture 11 Outline of Last Lecture I. Energy Level DiagramII. Bohr’s Atomic ModelIII. The Wavea. Linear Wavesb. Electrons as wavesc. de Broglie Wavelengthi. Particle Nature of PhotonsIV. Heisenberg’s uncertain principalOutline of Current Lecture II. Anomalous Configurationsa. Electron Configuration of IonsIII. Isoelectronic Atoms/IonsIV. Cations of Transitional Metals V. Sizes of Atoms/Ionsa. Atomic Radius TrendsCurrent LectureThese 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.Anomalous Configurations-Chromium, copper do not follow patternso Cr= 1s2, 2s2 2p6 3s2 sp6 3s5 4s1o Cu=1s2 2s2 2p6 3s2 3p6 4s1 3d10o Anomalies arise from stability associated with half-filled and completely filled d-subshells-Periodic table arranged based on electron configurations-Ch, Mo, Cu, Ag, AuEverything else follows the same pattern(http://hyperphysics.phy-astr.gsu.edu/hbase/pertab/cr.html)Electron Configuration of Ions-Formation of Ions:o Gain/loss of valence electron to achieve stable electron configuration (filled shell)Gain an electron- Loose and electron- o Cations: positive (loosing electrons) The more electrons you remove, the smaller its going togeto Anions: negative (gaining electrons)o Electrons will form ions that will allow them to get to the closest noble gas configurationIsoelectronic Atoms/IonsWhen you have the same electron configurations for two species-Main group elements:o Form ions by gain/loss of e- to obtain noble gas configurations-Isoelectronic: describes atoms/ions having identical electron configurationsBased on the row of the main group element, we can figure out what kind of ions they’re going to form (with a few exceptions)Cations of Transition Metals-Transition metal cations:o Loss of valence electron (s) and, in some cases, d electronso Fe: [Ar]3d 6 4s 2o Fe 2+ : [Ar]3d64s2= [Ar]3d6 (loss of valence e-o Fe 3+ : [Ar]3d6 = [Ar]3d5 (loss of one 3d= half filled d subshell)Sizes of Atoms/Ions-Atomic radius- half the distance btw identical nuclear centers in a molecule (i.e. covalent radius)-Metallic Radius- half the distance between nuclear centers in the crystal of a metal-Ionic Radius- derived from the distance between nuclear centers in ionic crystalsHow big is this element and what happens to the size of this element when we add and subtract electronsAtomic Radius Trends-Atomic Radii:o Increase going down a family“Shielding” by inner shell electrons decreases effective nuclear (Zeff)o Decrease going across a rowIncreased nuclear charge (z) moving across rowIncreased attraction for electrons in inner orbitals  atomic size