Details

Subject(s)

• Chemistry—Problems, exercises, etc [Browse]
• Chemical equations [Browse]
• Chemical reactions [Browse]

Summary note

"Chemistry in Quantitative Language provides students with a concise summary of important concepts in chemistry and a detailed guide to understanding every type of calculation likely to arise in a general chemistry course. Problem-solving is one of the most challenging aspects of general chemistry courses. This book's primary goal is to prevent frustration by providing students with innovative, intuitive, and systematic strategies to master problem-solving in chemistry. To achieve this goal, the text offers several sample problems with carefully explained, step-by-step solutions for each concept. Key concepts, basic theories, and equations are provided, and worked examples are selected to reflect possible ways problems could be presented to students."--Jacket.

Notes

Includes index.

Action note

Committed to retain in perpetuity — ReCAP Shared Collection (HUL)

Contents

• Essential Mathematics
• 1.1 Significant Figures
• 1.2 Significant Figures and Mathematical Operations
• 1.3 Scientific Notation and Exponents
• 1.4 Logarithms
• 1.5 Algebraic Equations
• 1.6 Problems
• Systems of Measurements
• 2.1 Measurements in Chemistry
• 2.2 Measurement of Mass, Length, and Time
• 2.3 Temperature
• 2.4 Derived Units
• 2.5 Density and Specific Gravity
• 2.6 Dimensional Analysis and Conversion Factors
• 2.7 Problems
• Atomic Structure and Isotope
• 3.1 Atomic Theory
• 3.2 The Structure of Atoms
• 3.3 Isotopes
• 3.4 Relative Atomic Mass
• 3.5 Problems
• Formula and Molecular Mass
• 4.1 Formula Mass
• 4.2 Molecular Mass
• 4.3 Molar Mass
• 4.4 Problems
• The Mole Concept and Avogadro's Number
• 5.1 The Mole and Avogadro's Number (NA)
• 5.2 The Mole and Molar Mass
• 5.3 Calculating the Number of Moles
• 5.4 Problems
• Formulas of Compounds and Percent Composition
• 6.1 Percent Composition
• 6.2 Empirical Formula
• 6.3 Molecular Formula
• 6.4 Problems
• Chemical Formula and Nomenclature
• 7.1 General Background
• 7.2 Chemical Formula
• 7.3 Oxidation Numbers
• 7.4 Writing The Formulas of Compounds
• 7.5 Nomenclature of Inorganic Compounds
• 7.6 Problems
• Chemical Equations
• 8.1 Writing Chemical Equations
• 8.2 Balancing Chemical Equations
• 8.3 Types of Chemical Reactions
• 8.4 Problems
• Stoichiometry.
• 9.1 Reaction Stoichiometry
• 9.2 Information From a Balanced Equation
• 9.3 Types of Stoichiometric Problems
• 9.4 Limiting Reagents
• 9.5 Reaction Yields: Theoretical, Actual, and Percent Yields
• 9.6 Problems
• The Structure of the Atom
• 10.1 Electronic Structure of the Atom
• 10.2 Electromagnetic Radiation
• 10.3 The Nature of Matter and Quantum Theory
• 10.4 The Hydrogen Atom
• 10.5 The Quantum-Mechanical Description of the Hydrogen Atom
• 10.6 Quantum Mechanics and Atomic Orbitals
• 10.7 Electronic Configuration of Multielectron Atoms
• 10.8 Problems
• Gas Laws
• 11.1 Boyle's Law: Pressure vs. Volume Relationship
• 11.2 Charles's Law: Temperature vs. Volume Relationship
• 11.3 The Combined Gas Law
• 11.4 Gay-Lussac's Law and Reactions Involving Gases
• 11.5 Avogadro's Law
• 11.6 The Ideal Gas Law
• 11.7 Density and Molecular Mass of a Gas
• 11.8 Molar Volume of an Ideal Gas
• 11.9 Dalton's Law of Partial Pressures
• 11.10 Partial Pressure and Mole Fraction
• 11.11 Real Gases and Deviation from the Gas Laws
• 11.12 Graham's Law of Diffusion
• 11.13 Problems
• Liquid and Solids.
• 12.1 The Liquid State
• 12.2 Calculations Involving Liquids
• 12.3 Application of The Clausius-Clapeyron Equation
• 12.4 The Solid State
• 12.5 The Crystal System
• 12.6 Calculation Involving Unit Cell Dimensions
• 12.7 Ionic Crystal Structure
• 12.8 Radius Ratio Rule for Ionic Compounds
• 12.9 Determination of Crystal Structure by X-Ray Diffraction
• 12.10 Problems
• Solution Chemistry
• 13.1 Concentration of Solutions
• 13.2 Solution and Solubility
• 13.3 Solving Solubility Problems
• 13.4 Effect of Temperature on Solubility
• 13.5 Solubility Curves
• 13.6 Effect of Pressure on Solubility
• 13.7 Problems
• Volumetric Analysis
• Introduction
• Application of Titration
• Acid-Base Titrations
• Calculations Involving Acid-Base Titration
• Back Titrations
• Problems
• Ideal Solutions and Colligative Properties.
• 15.1 Colligative Properties
• 15.2 Vapor Pressure
• 15.3 Raoult's Law
• 15.4 Elevation of Boiling Point
• 15.5 Depression of Freezing Point
• 15.6 Osmosis and Osmotic Pressure
• 15.7 Problems
• Chemical Kinetics
• Rates of Reaction
• Measurement of Reaction Rates
• Reaction Rates and Stoichiometry
• Collision Theory of Reaction Rates
• Rate Laws and The Order of Reactions
• Experimental Determination of Rate Law Using Initial Rates
• The Integrated Rate Equation and the Half-life of A Reactant
• Reaction Rates and Temperature: The Arrhenius Equation
• Chemical Equilibrium.
• 17.1 Reversible and Irreversible Reactions
• 17.2 The Equilibrium Constant
• 17.3 The Reaction Quotient
• 17.4 Predicting The Direction of Reaction
• 17.5 Position of Equilibrium
• 17.6 Homogeneous vs Heterogeneous Equilibra
• 17.7 Calculating Equilibrium Constants
• 17.8 Qualititative Treatment of Equilibrium: Le Chatelier's Principle
• 17.9 Problems
• Ionic Equilibra and pH
• The Ionization of Water
• Definition of Acidity and Basicity
• The pH of a Solution
• The pOH of a Solution
• The Acid Ionization Constant, Ka
• Calculating pH and Equilibrium Concentrations in Solutions of Weak Acids
• Percent Dissociation of Weak Acids
• The Base Dissociation Constant, Kb
• Relationship Between Ka and Kb
• Salt Hydrolysis: Acid-Basis Properties of Salts
• The Common Ion Effect
• Buffers and pH of Buffer Solutions
• Polyprotic Acids and Bases
• Acid: Base Titration pH Titration Curves
• Solubility & Complex-Ion Equilibra
• 19.1 Solubility Equilibria
• 19.2 The Solubility Product Principle
• 19.3 Determing Ksp from Molar Solubility
• 19.4 Calculating Molar Solubility from Ksp
• 19.5 Ksp and Precipitation
• 19.6 Complex-Ion Equilibra
• 19.7 Problems
• Thermochemistry.
• 20.1 Introduction
• 20.2 Calorimetry and Heat Capacity
• 20.3 Calculating of Reaction
• 20.4 Hess's Law of Heat Summation
• 20.5 Bond Energies and Enthalpy
• 20.6 Problems
• Chemical Thermodynamics
• 21.1 Definition of Terms
• 21.2 The First Law of Thermodynamics
• 21.3 Expansion Work
• 21.4 Entropy
• 21.5 The Second Law of Thermodynamics
• 21.6 Calculation of Entropy Changes in Chemical Reactions
• 21.7 Enthalpy and Entropy Changes During a Phase Change
• 21.8 Free Energy
• 21.9 The Standard Free Energy Change
• 21.10 Free Energy and the Constant
• 21.11 Variation of and Equilibrium Constant with Temperature
• 21.12 Problems
• Oxidation and Reduction Reactions
• 22.1 Introduction
• 22.2 Oxidation and Reduction in Terms of Electron Transfer
• 22.3 Oxidation Numbers
• 22.4 Oxidation and Reduction in Terms of Oxidation Number
• 22.5 Disproportionation
• 22.6 Oxidizing and Reducing Agents
• 22.7 Half-Cell Reactions
• 22.8 Balancing Redox Equations
• 22.9 Oxidation-Reduction Titration
• 22.10 Problems
• Fundamentals of Electrochemistry.
• 23.1 Galvanic Cells
• 23.2 The Cell Potential
• 23.3 Standard Electrode Potential
• 23.4 The Electrochemical Series (ECS)
• 23.5 Applications of Electrode Potential
• 23.6 Cell Diagrams
• 23.7 Calculating from Electrode Potential
• 23.8 Relationship of the Standard Electrode Potential, the Gibbs Free Energy, and the
• Equilibrium Constant
• 23.9 Dependence of Cell Potential on Concentration (the Nernst equation)
• 23.10 Electrolysis
• 23.11 Faraday's Law of Electrolysis
• 23.12 Problems
• Radioactivity and Nuclear Reactions
• 24.1 Definition of Terms
• 24.2 Radioactive Decay and Nuclear Equations
• 24.3 Nuclear Transmutations
• 24.4 Rates of Radioactive Decay and Half-Life
• 24.5 Energy of Nuclear Reactions
• 24.6 Problems.

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ISBN

• 9780195367997 (cloth : alk. paper)
• 0195367995 (cloth : alk. paper)

LCCN

^^2008040392

OCLC

255015656

RCP

H - S

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