Chemistry

Give students a robust conceptual foundation while building critical problem-solving skills Robinson/McMurry/Fay's Chemistry, known for a concise and united author voice, conceptual focus, extensive worked examples, and thoroughly constructed connections between organic, biological, and general...

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Detalles Bibliográficos
Autor principal: Jill Kirsten Robinson (-)
Otros Autores: Robinson, Jill K., author (author), McMurry, John, author, Fay, Robert C., 1936- author
Formato: Libro electrónico
Idioma:Inglés
Publicado: Harlow, England : Pearson [2021]
Edición:Eighth edition, Global edition
Materias:
Ver en Biblioteca Universitat Ramon Llull:https://discovery.url.edu/permalink/34CSUC_URL/1im36ta/alma991009767117006719
Tabla de Contenidos:
  • Front Cover
  • Periodic Table of the Elements
  • Title Page
  • Copyright Page
  • Brief Contents
  • Content
  • Preface
  • For Instructors
  • 1 Chemical Tools: Experimentation and Measurement
  • 1.1 The Scientific Method: Nanoparticle Catalysts for Fuel Cells
  • 1.2 Measurements: SI Units and Scientific Notation
  • 1.3 Mass and Its Measurement
  • 1.4 Length and Its Measurement
  • 1.5 Temperature and Its Measurement
  • 1.6 Derived Units: Volume and Its Measurement
  • 1.7 Derived Units: Density and Its Measurement
  • 1.8 Derived Units: Energy and Its Measurement
  • 1.9 Accuracy, Precision, and Significant Figures in Measurement
  • 1.10 Significant Figures in Calculations
  • 1.11 Converting from One Unit to Another
  • INQUIRY? What are the unique properties of nanoscale materials?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 2 Atoms, Molecules, and Ions
  • 2.1 Chemistry and the Elements
  • 2.2 Elements and the Periodic Table
  • 2.3 Some Common Groups of Elements and Their Properties
  • 2.4 Observations Supporting Atomic Theory: The Conservation of Mass and the Law of Definite Proportions
  • 2.5 The Law of Multiple Proportions and Dalton's Atomic Theory
  • 2.6 Atomic Structure: Electrons
  • 2.7 Atomic Structure: Protons and Neutrons
  • 2.8 Atomic Numbers
  • 2.9 Atomic Weights and the Mole
  • 2.10 Measuring Atomic Weight: Mass Spectrometry
  • 2.11 Mixtures and Chemical Compounds
  • Molecules and Covalent Bonds
  • 2.12 Ions and Ionic Bonds
  • 2.13 Naming Chemical Compounds
  • INQUIRY? How can measurements of oxygen and hydrogen isotopes in ice cores determine past climates?
  • Study Guide
  • Key Terms
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 3 Mass Relationships in Chemical Reactions.
  • 3.1 Representing Chemistry on Different Levels
  • 3.2 Balancing Chemical Equations
  • 3.3 Molecular Weight and Molar Mass
  • 3.4 Stoichiometry: Relating Amounts of Reactants and Products
  • 3.5 Yields of Chemical Reactions
  • 3.6 Reactions with Limiting Amounts of Reactants
  • 3.7 Percent Composition and Empirical Formulas
  • 3.8 Determining Empirical Formulas: Elemental Analysis
  • 3.9 Determining Molecular Weights: Mass Spectrometry
  • INQUIRY? How is the principle of atom economy used to minimize waste in a chemical synthesis?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 4 Reactions in Aqueous Solution
  • 4.1 Solution Concentration: Molarity
  • 4.2 Diluting Concentrated Solutions
  • 4.3 Electrolytes in Aqueous Solution
  • 4.4 Types of Chemical Reactions in Aqueous Solution
  • 4.5 Aqueous Reactions and Net Ionic Equations
  • 4.6 Precipitation Reactions and Solubility Guidelines
  • 4.7 Acids, Bases, and Neutralization Reactions
  • 4.8 Solution Stoichiometry
  • 4.9 Measuring the Concentration of a Solution: Titration
  • 4.10 Oxidation-Reduction (Redox) Reactions
  • 4.11 Identifying Redox Reactions
  • 4.12 The Activity Series of the Elements
  • 4.13 Redox Titrations
  • 4.14 Some Applications of Redox Reactions
  • INQUIRY? How do sports drinks replenish the substances lost in sweat?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 5 Periodicity and the Electronic Structure of Atoms
  • 5.1 Wave Properties of Radiant Energy and the Electromagnetic Spectrum
  • 5.2 Particlelike Properties of Radiant Energy: The Photoelectric Effect and Planck's Postulate
  • 5.3 Atomic Line Spectra and Quantized Energy
  • 5.4 Wavelike Properties of Matter: de Broglie's Hypothesis.
  • 5.5 The Quantum Mechanical Model of the Atom: Heisenberg's Uncertainty Principle
  • 5.6 The Quantum Mechanical Model of the Atom: Orbitals and Quantum Numbers
  • 5.7 The Shapes of Orbitals
  • 5.8 Electron Spin and the Pauli Exclusion Principle
  • 5.9 Orbital Energy Levels in Multielectron Atoms
  • 5.10 Electron Configurations of Multielectron Atoms
  • 5.11 Anomalous Electron Configurations
  • 5.12 Electron Configurations and the Periodic Table
  • 5.13 Electron Configurations and Periodic Properties: Atomic Radii
  • INQUIRY? How does knowledge of atomic emission spectra help us build more efficient light bulbs?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 6 Ionic Compounds: Periodic Trends and Bonding Theory
  • 6.1 Electron Configurations of Ions
  • 6.2 Ionic Radii
  • 6.3 Ionization Energy
  • 6.4 Higher Ionization Energies
  • 6.5 Electron Affinity
  • 6.6 The Octet Rule
  • 6.7 Ionic Bonds and the Formation of Ionic Solids
  • 6.8 Lattice Energies in Ionic Solids
  • INQUIRY? How do ionic liquids lead to more environmentally friendly processes?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 7 Covalent Bonding and Electron-Dot Structures
  • 7.1 Covalent Bonding in Molecules
  • 7.2 Strengths of Covalent Bonds
  • 7.3 Polar Covalent Bonds: Electronegativity
  • 7.4 A Comparison of Ionic and Covalent Compounds
  • 7.5 Electron-Dot Structures: The Octet Rule
  • 7.6 Procedure for Drawing Electron-Dot Structures
  • 7.7 Drawing Electron-Dot Structures for Radicals
  • 7.8 Electron-Dot Structures of Compounds Containing Only Hydrogen and Second-Row Elements
  • 7.9 Electron-Dot Structures and Resonance
  • 7.10 Formal Charges.
  • INQUIRY? How does bond polarity affect the toxicity of organophosphate insecticides?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 8 Covalent Compounds: Bonding Theories and Molecular Structure
  • 8.1 Molecular Shapes: The VSEPR Model
  • 8.2 Valence Bond Theory
  • 8.3 Hybridization and sp3 Hybrid Orbitals
  • 8.4 Other Kinds of Hybrid Orbitals
  • 8.5 Polar Covalent Bonds and Dipole Moments
  • 8.6 Intermolecular Forces
  • 8.7 Molecular Orbital Theory: The Hydrogen Molecule
  • 8.8 Molecular Orbital Theory: Other Diatomic Molecules
  • 8.9 Combining Valence Bond Theory and Molecular Orbital Theory
  • INQUIRY? Which is better for human health, natural or synthetic vitamins?
  • Study Guide
  • Key Terms
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 9 Thermochemistry: Chemical Energy
  • 9.1 Energy and Its Conservation
  • 9.2 Internal Energy and State Functions
  • 9.3 Expansion Work
  • 9.4 Energy and Enthalpy
  • 9.5 Thermochemical Equations and the Thermodynamic Standard State
  • 9.6 Enthalpies of Chemical and Physical Changes
  • 9.7 Calorimetry and Heat Capacity
  • 9.8 Hess's Law
  • 9.9 Standard Heats of Formation
  • 9.10 Bond Dissociation Energies
  • 9.11 An Introduction to Entropy
  • 9.12 An Introduction to Free Energy
  • INQUIRY? How do we determine the energy content of biofuels?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 10 Gases: Their Properties and Behavior
  • 10.1 Gases and Gas Pressure
  • 10.2 The Gas Laws
  • 10.3 The Ideal Gas Law
  • 10.4 Stoichiometric Relationships with Gases
  • 10.5 Mixtures of Gases: Partial Pressure and Dalton's Law
  • 10.6 The Kinetic-Molecular Theory of Gases
  • 10.7 Gas Diffusion and Effusion: Graham's Law.
  • 10.8 The Behavior of Real Gases
  • 10.9 The Earth's Atmosphere and the Greenhouse Effect
  • 10.10 Greenhouse Gases
  • 10.11 Climate Change
  • INQUIRY? How do inhaled anesthetics work?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 11 Liquids and Phase Changes
  • 11.1 Properties of Liquids
  • 11.2 Vapor Pressure and Boiling Point
  • 11.3 Phase Changes between Solids, Liquids, and Gases
  • 11.4 Energy Changes during Phase Transitions
  • 11.5 Phase Diagrams
  • 11.6 Liquid Crystals
  • INQUIRY? How is caffeine removed from coffee?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 12 Solids and Solid-State Materials
  • 12.1 Types of Solids
  • 12.2 Probing the Structure of Solids: X-Ray Crystallography
  • 12.3 The Packing of Spheres in Crystalline Solids: Unit Cells
  • 12.4 Structures of Some Ionic Solids
  • 12.5 Structures of Some Covalent Network Solids
  • 12.6 Bonding in Metals
  • 12.7 Semiconductors
  • 12.8 Semiconductor Applications
  • 12.9 Superconductors
  • 12.10 Ceramics and Composites
  • INQUIRY? What are quantum dots, and what controls their color?
  • Study Guide
  • Key Terms
  • Key Equations
  • Practice Test
  • Conceptual Problems
  • Section Problems
  • Multiconcept Problems
  • 13 Solutions and Their Properties
  • 13.1 Solutions
  • 13.2 Enthalpy Changes and the Solution Process
  • 13.3 Predicting Solubility
  • 13.4 Concentration Units for Solutions
  • 13.5 Some Factors That Affect Solubility
  • 13.6 Physical Behavior of Solutions: Colligative Properties
  • 13.7 Vapor-Pressure Lowering of Solutions: Raoult's Law
  • 13.8 Boiling-Point Elevation and Freezing-Point Depression of Solutions
  • 13.9 Osmosis and Osmotic Pressure.
  • INQUIRY? How does hemodialysis cleanse the blood of patients with kidney failure?.