All Review II Notes AU10

All Review II Notes AU10 - 1 Midterm II Material/Topics...

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1 Midterm II Material/Topics Autumn 2010 Supplemental Material: Resonance Structures Ch 5.8 Molecular Geometry Ch 5.9 Electronegativity Ch 5.10 Bond Polarity Ch 5.11 Molecular Polarity Ch 5.12 Naming Binary Molecular Compounds Writing and Balancing Chemical Equations (Ch 6.6) A. Combination Reactions (Ch 9.1) B. Decomposition Reactions (Ch 9.1) C. Single-Replacement Reactions (Ch 9.1) D. Double-Replacement Reactions (Ch 9.1) with Solubility Rules (Ch 8.4) E. Combustion Reactions (Ch 9.1) F. Oxidation - Reduction Reactions (Ch. 9.2, 9.3) Supplemental Material: Comparing Strength of Agents H. Acid-Base Neutralization Reactions (Ch 10.1, 10.6 & 10.7) Ch 6.1 Formula Masses Supplemental material: Percent Composition Ch 6.2 The Mole & Avogadro's Number Ch 6.3 Molar Mass Ch 6.4 & 6.5 Chemical Formula & Mole Calculations Supplemental material & Lab Exp 8: Empirical & Molecular Formula Ch 6.6, 6.7, 6.8 Chemical Equations & Stoichiometric Calculations Supplemental material: Heat of Reaction Supplemental material: Percent Yield Supplemental material: Limiting Reagent
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2 Ch 7.1 & 7.2 The Kinetic Molecular Theory and States of Matter Ch 7.3 Gas Law Variables Ch 7.4 Boyle’s Law Ch 7.5 Charles’s Law Supplemental material: Amontons's Law Ch 7.6 The Combined Gas Law Ch 7.7 The Ideal Gas Law Supplemental material: Avogadro’s Hypothesis and the Molar Volume Ch 7.8 Dalton’s Law of Partial Pressures Ch 7.9 Changes of Physical State Ch 7.10 Evaporation of Liquids Ch 7.11Vapor Pressure of Liquids Ch. 7.12 Boiling and Boiling Point Supplemental material: Heat of Vaporization, Viscosity, and Surface Tension Ch 7.13 Intermolecular Forces in Liquids A. London Forces B. Dipole-Dipole Interactions C. Hydrogen Bonds Ch 8.1 Characteristics of Solutions Ch 8.2 Solubility Ch 8.3 Solution Formation Supplemental material: Entropy Ch 8.4 Solubility Rules
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3 Resonance Structures Resonance structures are two or more Lewis structures that represent the same ion or molecule equally well. Examples: nitrite ion NO 2 - ozone O 3 carbonate ion CO 3 2- benzene
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4 Ch 5.8 Molecular Geometry V alence S hell E lectron- P air R epulsion theory ( VSEPR theory) Electrons repel each other Electrons tend to be as far apart as possible Electron pairs control geometry 2 electron pairs or VSEPR groups 3 electron pairs or VSEPR groups 4 electron pairs or VSEPR groups Figure 5.8
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5 A. Two VSEPR groups = linear . . . . : O = C = O : 2 VSEPR groups around the central atom bond angle 180 o B. Three VSEPR groups = trigonal planar or angular : O : H C H 3 VSEPR groups Trigonal planar bond angle ~120 o . . . . . . - : O N O : 3 VSEPR groups around N 2 bonding, 1 nonbonding bent or angular shape bond angle ~120 o
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6 C. Four VSEPR groups: Tetrahedral (no nonbonding e pairs) Trigonal pyramidal (1 nonbonding e pair) Angular or bent (2 nonbonding e pairs) 109.5 o <109.5 o <109.5 o
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This note was uploaded on 06/03/2011 for the course CHM 123 taught by Professor Woodward during the Fall '08 term at Ohio State.

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All Review II Notes AU10 - 1 Midterm II Material/Topics...

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