#Chem 161-2007 recitation 11th week

#Chem 161-2007 recitation 11th week - CHEMISTRY 161-2007...

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CHEMISTRY 161-2007 11 th WEEK RECITATION ANNOUNCEMENTS ATTENDANCE QUIZZES Pick up new and old quizzes after class. EXAMS Wednesday, Nov. 28 th , 9:40 – 11:00 PM, H&P Ch. 7-9, Chem 161 Exam III Review two days, 8-10 PM; choice of Sun 11/18, Mon 11/19, Tue  11/20, Mon 11/26. RESCHEDULING Tuesday, Nov. 20 th , Thursday classes. Wednesday, Nov. 21 st , Friday classes Thursday and Friday, Nov. 22 nd  and 23 rd , no classes Section 23: Next week no class. Section 25 & 29: Next week’s class Tues. Nov. 20 th . Office hours: Next week Tues., Nov. 20 th , H ck 206? 8:00-9:00 AM THANKSGIVING Have a horrible Thanksgiving :>) Study! Vacation during winter break. Chem 161-2007 11 th week recitation 1
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PLAN FOR TODAY : CHAPTER 9 • PERIODIC TABLE AND PERIODIC PROPERTIES -- Electronegativity • BOND POLARITY AND DIPOLE MOMENTS -- Ions and ionic bonding BOND ENERGIES OF IONIC BOND FORMATION -- Lattice energies (Born-Haber cycle) LEWIS STRUCTURES FORMAL CHARGE RESONANCE STRUCTURES BOND ENERGY/LENGTH • ALKANES, ALKENES, ALKYNES AND POLYMERS (Orgo this week only for sect 23) Chem 161-2007 11 th week recitation 2
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AUFBAU PRINCIPLE -- ORDER OF SUBSHELLS ET: “Aufbau” meams “building up” in German ( He) 14 8s 8p 8d 8f 14 Chem 161-2007 11 th week recitation 3
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Chem 161-2007 11 th week recitation 4 SMALLER ATOM SMALLER ION HIGHER FIRST IONIZATION ENERGY ELECTRON AFFINITY HIGHER ELECTRONEGATIVITY LESS METALLIC PROPERTY POOR REDUCING AGENT GOOD OXIDIZING ACIDIC OXIDES PERIODIC TABLE AND PERIODIC PROPERTIES
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FACTORS GOVERNING PE RIODIC TABLE TRENDS (1) Increasing valence principle shell number → less attraction of valence electrons to nucleus (2) Increasing effective nuclear charge (with same number of principal shells) → Greater attraction of valence electrons to nucleus. (3) Increasing electrons in valence shell (with same number of principal shells and same effective nuclear charge) → Greater electron repulsion (4) Exceptions: Nearest neighbor atoms ionization energies and electron affinities, due mainly to subshell influences. Ionization energies: , e.g., B vs Be [p vs s], O vs N [filled p orbital vs half-filled p orbital Electron affinities: e.g., formation of C - vs N - ; also electron repulsion in smaller atoms, e.g., O vs. S. Chem 161-2007 11 th week recitation 5 INCREASING PRIORITY
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ELECTRONEGATIVITY PERIODIC TABLE 1A 2A 3B 4B 5B 6B 7B 8B 8B 8B 1B 2B 3A 4A 5A 6A 7A 8A H 2. 1 He Li 1.0 Be 1.5 B 2.0 C 2.5 N 3.0 O 3.5 F 4.0 Ne Na 0.9 Mg 1.2 Al 1.5 Si 1.8 P 2.1 S 2.5 Cl 3.0 Ar K 0.8 Ca 1.0 Sc 1. 3 Ti 1. 5 V 1. 6 Cr 1.6 Mn 1.5 Fe 1.8 Co 1. 8 Ni 1. 8 Cu 1. 9 Zn 1. 7 Ga 1.6 Ge 1.8 As 2.0 Se 2.4 Br 2.8 Kr Rb 0.8 Sr 1.0 Y 1. 2 Zr 1. 4 Nb 1. 5 Mo 1.8 Tc 1.9 Ru 2.2 Rh 2. 2 Pd 2. 2 Ag 1. 9 Cd 1. 7 In 1.7 Sn 1.8 Sb 1.9 Te 2.1 I 2.5 Xe Cs 0.7 Ba 0.9 La 1. 1 Ce Pr Nd Pm Sm Eu Gd Tb Tl 81 204.3 8 Pb 82 207.
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#Chem 161-2007 recitation 11th week - CHEMISTRY 161-2007...

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