Chem 1211 1st Edition Lecture 19Outline of Last Lecture I. Quantum numbersII. Energy of OrbitalsOutline of Current Lecture I. Electron Configuration: TransitionII. Atomic Properties: Atomic SizeIII. Atomic Properties: Ionization EnergyIV. Atomic Properties: Ion SizeCurrent LectureI. Electron Configuration: Transition a. Special stability: one e- in each of five 3d orbitals and again for two e- in each of five 3d orbitalsb. ConcepTest: Which transition metal has the electron configuration [Kr]4d55s1?i. Vii. Criii. Nbiv. Mov. Tc1. ANSWER: Mo2. REASONING: Because of the d5, it has to be under Cr in the periodic tablec. Ion (Cations) Reversei. Na: [Ne] 3s1ii. Na+: [Ne]d. ConcepTest: Which transition metal has the electron configuration [Ar]4d5?i. Mn+ii. Mn2+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.iii. Cr+iv. Cr2+1. ANSWER: Mn2+ or C+e. Cationsi. Electrons removed first from highest nii. Within a shell, electrons of maximum/removed1. Na: [1s22s22p63s1] Na+ [1s22s22p6] (=Ne)iii. Transition metals: ns (4s) electrons lost before n-1 (3d) electronsII. Atomic Properties: Atomic Sizea. Periodic properties related to valence shell electron configurationsi. Units pm= 10-12 mb. ConcepTest: Which pair of atoms is NOT listed in order of INCREASING atomic radius?i. K, Rbii. Mg, Caiii. O, Siv. Sr, Inv. Sr, Rb1. ANSWER: Sr, In2. REASONING: Atomic radius increases as you move from the top to the bottom of the periodic tablea. Atomic radius decreases as you move left to right across the periodic tablec. ConcepTest: Which pair of atoms would be expected to have the longest interatomic distance in a molecule having such a bond? i. C-Cii. C-Niii. C-Oiv. C-Sv. C-Br1. ANSWER: C-Br2. Reasoning: Bromium is the largest in the listd. ConcepTest: Which pair of atoms in a single period would be expected to have the smallest and the largest ionization energies, respectively?i. Li, Naii. Li, Neiii. Ne, Liiv. Li, Bev. F, Ne1. ANSWER: Li, Ne2. REASONING: Ionization energy: atom (g) atom + (g) + e-III. Atomic Properties: Ionization Energya. 1st IE: atom (g) atom+ (g) + e-b. 2nd IE: atom (g) atom2+ (g) + 2e-c. 3rd IE: atom (g) atom3+ (g) + 3e-d. ConcepTest: Which pair of atoms in a single period would be expected to have the smallest and the largest electron attachment enthalpies, respectively?i. Li, Naii. Li, Fiii. F, Liiv. Li, Bev. O, F1. ANSWER: Li, F2. REASONING: Largest range covered (there is a lot of incentive to gain an electron from a halogen) a. Electron attachment enthalpies given as a negative numberIV. Atomic Properties: Ion Sizesa. Trends for ions are the same as atomsb. Cations shrink, anions expand i. + charge: smaller than corresponding atomii. – charge: larger than their corresponding
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