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Test Bank for Chemistry The Science in Context, Fourth Edition

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This is completed downloadable of Test Bank for Chemistry The Science in Context, Fourth Edition

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ISBN-10 ‏ : ‎ 0393124185
ISBN-13 ‏ : ‎ 978-0393124187
Author: Thomas R. Gilbert (Author), Rein V. Kirss (Author), Natalie Foster (Author), Geoffrey Davies (Author)

All general chemistry students face similar challenges, but they use their textbook differently to meet those challenges. Some read chapters from beginning to end, some consult the book as a reference, and some look to the book for problem-solving help. Chemistry, Fourth Edition supports all kind of learners, regardless of how they use the book, by helping them connect chemistry to their world, see that world from a molecular point of view, and become expert problem solvers.

Table contents:

Chapter T: WebAssign Answer Templates and Tutorials
- T: WebAssign Answer Templates and Tutorials (3)
Chapter 1: Matter and Energy: The Origin of the Universe
- 1.1: Classes of Matter
- 1.2: Matter: An Atomic View
- 1.3: Mixtures and How to Separate Them
- 1.4: A Framework for Solving Problems
- 1.5: Properties of Matter
- 1.6: States of Matter (7)
- 1.7: The Scientific Method: Starting Off with a Bang
- 1.8: Making Measurements and Expressing the Results
- 1.9: Unit Conversions and Dimensional Analysis (17)
- 1.10: Testing a Theory: The Big Bang Revisited (7)
- 1: Visual Problems (2)
- 1: Additional Problems (5)
- 1: Extra Problems (13)
Chapter 2: Atoms, Ions, and Molecules: Matter Starts Here
- 2.1: The Nuclear Model of Atomic Structure
- 2.2: Isotopes
- 2.3: Average Atomic Mass (7)
- 2.4: The Periodic Table of the Elements (12)
- 2.5: Trends in Compound Formation (3)
- 2.6: Naming Compounds and Writing Formulas (17)
- 2.7: Nucleosynthesis (1)
- 2: Visual Problems
- 2: Additional Problems (5)
- 2: Extra Problems (3)
Chapter 3: Stoichiometry: Mass, Formulas, and Reactions
- 3.1: Chemical Reactions and Earth’s Early Atmosphere
- 3.2: The Mole (21)
- 3.3: Writing Balanced Chemical Equations (3)
- 3.4: Combustion Reactions
- 3.5: Stoichiometric Calculations and the Carbon Cycle (8)
- 3.6: Determining Empirical Formulas from Percent Composition
- 3.7: Empirical and Molecular Formulas Compared (4)
- 3.8: Combustion Analysis (2)
- 3.9: Limiting Reactants and Perfect Yield (7)
- 3: Visual Problems
- 3: Additional Problems (1)
- 3: Extra Problems (15)
Chapter 4: Solution Chemistry: The Hydrosphere
- 4.1: Solutions on Earth and Other Places
- 4.2: Concentration Units (12)
- 4.3: Dilutions (3)
- 4.4: Electrolytes and Nonelectrolytes (4)
- 4.5: Acid–Base Reactions: Proton Transfer (3)
- 4.6: Titrations (6)
- 4.7: Precipitation Reactions (7)
- 4.8: Ion Exchange
- 4.9: Oxidation–Reduction Reactions: Electron Transfer (7)
- 4: Visual Problems
- 4: Additional Problems
- 4: Calcium: In the Limelight
- 4: Extra Problems (14)
Chapter 5: Thermochemistry: Energy Changes in Reactions
- 5.1: Energy: Basic Concepts and Definitions
- 5.2: Systems, Surroundings, and Energy Transfer (8)
- 5.3: Enthalpy and Enthalpy Changes (4)
- 5.4: Heating Curves and Heat Capacity (8)
- 5.5: Calorimetry: Measuring Heat Capacity and Enthalpies of Reaction (6)
- 5.6: Hess’s Law
- 5.7: Standard Enthalpies of Formation and Reaction (8)
- 5.8: Fuel Values and Food Values (2)
- 5: Visual Problems (1)
- 5: Additional Problems (14)
- 5: Carbon: Diamonds, Graphite, and the Molecules of Life (1)
- 5: Extra Problems (9)
Chapter 6: Properties of Gases: The Air We Breathe
- 6.1: The Gas Phase
- 6.2: Atmospheric Pressure (4)
- 6.3: The Gas Laws (10)
- 6.4: The Ideal Gas Law
- 6.5: Gases in Chemical Reactions (10)
- 6.6: Gas Density (3)
- 6.7: Dalton’s Law and Mixtures of Gases (3)
- 6.8: The Kinetic Molecular Theory of Gases (7)
- 6.9: Real Gases (4)
- 6: Visual Problems
- 6: Additional Problems (9)
- 6: Nitrogen: Feeding Plants and Inflating Air Bags
- 6: Extra Problems (23)
Chapter 7: A Quantum Model of Atoms: Waves and Particles
- 7.1: Light Waves (5)
- 7.2: Atomic Spectra
- 7.3: Particles of Light and Quantum Theory (7)
- 7.4: The Hydrogen Spectrum and the Bohr Model (5)
- 7.5: Electron Waves (4)
- 7.6: Quantum Numbers and Electron Spin
- 7.7: The Sizes and Shapes of Atomic Orbitals (4)
- 7.8: The Periodic Table and Filling the Orbitals of Multielectron Atoms
- 7.9: Electron Configurations of Ions (10)
- 7.10: The Sizes of Atoms and Ions (1)
- 7.11: Ionization Energies
- 7.12: Electron Affinities
- 7: Visual Problems (3)
- 7: Additional Problems (2)
- 7: A Noble Family: Special Status for Special Behavior
- 7: Extra Problems (6)
Chapter 8: Chemical Bonds: What Makes a Gas a Greenhouse Gas?
- 8.1: Types of Chemical Bonds
- 8.2: Lewis Structures (6)
- 8.3: Polar Covalent Bonds (3)
- 8.4: Vibrating Bonds and the Greenhouse Effect
- 8.5: Resonance (2)
- 8.6: Formal Charge: Choosing among Lewis Structures (3)
- 8.7: Exceptions to the Octet Rule (3)
- 8.8: The Lengths and Strengths of Covalent Bonds (3)
- 8: Visual Problems
- 8: Additional Problems (4)
- 8: Fluorine and Oxygen: Location, Location, Location
- 8: Extra Problems (17)
Chapter 9: Molecular Geometry: Shape Determines Function
- 9.1: Molecular Shape
- 9.2: Valence-Shell Electron-Pair Repulsion Theory (VSEPR) (8)
- 9.3: Polar Bonds and Polar Molecules (4)
- 9.4: Valence Bond Theory (3)
- 9.5: Shape and Interactions with Large Molecules
- 9.6: Chirality and Molecular Recognition (1)
- 9.7: Molecular Orbital Theory (7)
- 9: Visual Problems
- 9: Additional Problems (8)
- 9: Chalcogens: From Alcohol to Asparagus, the Nose Knows (1)
- 9: Extra Problems (13)
Chapter 10: Intermolecular Forces: The Uniqueness of Water
- 10.1: Interactions between Ions (1)
- 10.2: Interactions Involving Polar Molecules (4)
- 10.3: Dispersion Forces (2)
- 10.4: Polarity and Solubility (2)
- 10.5: Vapor Pressure of Pure Liquids (2)
- 10.6: Phase Diagrams: Intermolecular Forces at Work (8)
- 10.7: Some Remarkable Properties of Water (2)
- 10: Visual Problems
- 10: Additional Problems (1)
- 10: The Halogens: The Salt of the Earth
- 10: Extra Problems (3)
Chapter 11: Solutions: Properties and Behavior
- 11.1: Vapor Pressure of Solutions (1)
- 11.2: Solubility of Gases in Water (3)
- 11.3: Energy Changes during Formation and Dissolution of Ionic Compounds (2)
- 11.4: Mixtures of Volatile Solutes (2)
- 11.5: Colligative Properties of Solutions (8)
- 11.6: Measuring the Molar Mass of a Solute Using Colligative Properties (1)
- 11: Visual Problems
- 11: Additional Problems (2)
- 11: Extra Problems (1)
Chapter 12: Solids: Structures and Applications
- 12.1: The Solid State
- 12.2: Structures of Metals (7)
- 12.3: Alloys (2)
- 12.4: Metallic Bonds and Conduction Bands (2)
- 12.5: Semiconductors (4)
- 12.6: Salt Crystals: Ionic Solids (4)
- 12.7: Structures of Nonmetals (1)
- 12.8: Ceramics: Insulators to Superconductors (1)
- 12.9: X-ray Diffraction: How We Know Crystal Structures (6)
- 12: Visual Problems (2)
- 12: Additional Problems (2)
- 12: Silicon, Silica, Silicates, Silicone: What’s in a Name?
- 12: Extra Problems (11)
Chapter 13: Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life
- 13.1: Carbon: The Scope of Organic Chemistry (3)
- 13.2: Alkanes (7)
- 13.3: Alkenes and Alkynes (4)
- 13.4: Aromatic Compounds (3)
- 13.5: Amines (1)
- 13.6: Alcohols, Ethers, and Reformulated Gasoline (3)
- 13.7: Carbonyl-Containing Compounds (8)
- 13.8: Chirality (5)
- 13: Visual Problems (6)
- 13: Additional Problems (2)
- 13: Extra Problems (2)
Chapter 14: Chemical Kinetics: Reactions in the Air We Breathe
- 14.1: Cars, Trucks, and Air Quality
- 14.2: Reaction Rates (4)
- 14.3: Effect of Concentration on Reaction Rate (16)
- 14.4: Reaction Rates, Temperature, and the Arrhenius Equation (3)
- 14.5: Reaction Mechanisms (3)
- 14.6: Catalysis (1)
- 14: Visual Problems (4)
- 14: Additional Problems (4)
- 14: Extra Problems (5)
Chapter 15: Chemical Equilibrium: How Much Product Does a Reaction Really Make?
- 15.1: The Dynamics of Chemical Equilibrium (2)
- 15.2: Writing Equilibrium Constant Expressions
- 15.3: Relationships between K_c and K_p Values (9)
- 15.4: Manipulating Equilibrium Constant Expressions (3)
- 15.5: Equilibrium Constants and Reaction Quotients (2)
- 15.6: Heterogeneous Equilibria
- 15.7: Le Châtelier’s Principle (2)
- 15.8: Calculations Based on K (12)
- 15: Visual Problems
- 15: Additional Problems
- 15: Extra Problems (7)
Chapter 16: Acid–Base and Solubility Equilibria: Reactions in Soil and Water
- 16.1: Acids and Bases: The Brønsted–Lowry Model (5)
- 16.2: pH and the Autoionization of Water (3)
- 16.3: Calculations Involving pH, K_a, and K_b (1)
- 16.4: Polyprotic Acids (7)
- 16.5: Acid Strength and Molecular Structure (1)
- 16.6: pH of Salt Solutions (3)
- 16.7: The Common-Ion Effect
- 16.8: pH Buffers (6)
- 16.9: Indicators and Acid–Base Titrations
- 16.10: Solubility Equilibria (5)
- 16: Visual Problems
- 16: Additional Problems (2)
- 16: The Chemistry of Two Strong Acids: Sulfuric and Nitric Acids (2)
- 16: Extra Problems (14)
Chapter 17: Metal Ions: Colorful and Essential
- 17.1: Lewis Acids and Bases (3)
- 17.2: Complex Ions (3)
- 17.3: Complex-Ion Equilibria (3)
- 17.4: Naming Complex Ions and Coordination Compounds (3)
- 17.5: Hydrated Metal Ions as Acids (5)
- 17.6: Polydentate Ligands
- 17.7: Ligand Strength and the Chelate Effect
- 17.8: Crystal Field Theory (2)
- 17.9: Magnetism and Spin States (2)
- 17.10: Isomerism in Coordination Compounds
- 17.11: Coordination Compounds in Biochemistry (2)
- 17: Visual Problems (3)
- 17: Additional Problems (3)
- 17: Extra Problems (6)
Chapter 18: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes
- 18.1: Spontaneous Processes
- 18.2: Thermodynamic Entropy (5)
- 18.3: Absolute Entropy and the Third Law of Thermodynamics (1)
- 18.4: Calculating Entropy Changes (1)
- 18.5: Free Energy (5)
- 18.6: Temperature and Spontaneity (1)
- 18.7: Free Energy and Chemical Equilibrium
- 18.8: Influence of Temperature on Equilibrium Constants (1)
- 18.9: Driving the Human Engine: Coupled Reactions
- 18.10: Microstates: A Quantized View of Entropy
- 18: Visual Problems (2)
- 18: Additional Problems (7)
- 18: Extra Problems (16)
Chapter 19: Electrochemistry: The Quest for Clean Energy
- 19.1: Redox Chemistry Revisited
- 19.2: Electrochemical Cells (2)
- 19.3: Standard Potentials (7)
- 19.4: Chemical Energy and Electrical Work (2)
- 19.5: A Reference Point: The Standard Hydrogen Electrode
- 19.6: The Effect of Concentration on E_cell (6)
- 19.7: Relating Battery Capacity to Quantities of Reactants (2)
- 19.8: Corrosion: Unwanted Electrochemical Reactions
- 19.9: Electrolytic Cells and Rechargeable Batteries (8)
- 19.10: Fuel Cells
- 19: Visual Problems (2)
- 19: Additional Problems (2)
- 19: Extra Problems (13)
Chapter 20: Biochemistry: The Compounds of Life
- 20.1: The Composition of Proteins (1)
- 20.2: Protein Structure and Function (2)
- 20.3: Carbohydrates (2)
- 20.4: Lipids (1)
- 20.5: Nucleotides and Nucleic Acids (1)
- 20.6: From Biomolecules to Living Cells
- 20: Visual Problems (2)
- 20: Additional Problems (1)
- 20: Extra Problems (6)
Chapter 21: Nuclear Chemistry: Applications to Energy and Medicine
- 21.1: Binding Energy and Nuclear Stability (2)
- 21.2: Unstable Nuclei and Radioactive Decay (2)
- 21.3: Rates of Radioactive Decay (2)
- 21.4: Radiometric Dating (3)
- 21.5: Measuring Radioactivity
- 21.6: Biological Effects of Radioactivity (2)
- 21.7: Medical Applications of Radionuclides (8)
- 21.8: Nuclear Fission (2)
- 21.9: Nuclear Fusion and the Quest for Clean Energy (1)
- 21: Visual Problems
- 21: Additional Problems (2)
- 21: Extra Problems (17)
Chapter 22: Life and the Periodic Table
- 22.1: The Periodic Table of Life (4)
- 22.2: Major Essential Elements (4)
- 22.3: Trace and Ultratrace Essential Elements (5)
- 22.4: Nonessential Elements
- 22.5: Elements for Diagnostics and Therapy (6)
- 22: Visual Problems (5)
- 22: Additional Problems
- 22: Extra Problems (5)