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Must Know High School Chemistry By John Moore

Must Know High School Chemistry by John Moore

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Must Know High School Chemistry Summary

Must Know High School Chemistry by John Moore

Publisher's Note: Products purchased from Third Party sellers are not guaranteed by the publisher for quality, authenticity, or access to any online entitlements included with the product.

You know that moment when you feel as though a lightning bolt has hit you because you finally get something? That's how this book will make you react. (We hope!) Each chapter makes sure that what you really need to know is clear right off the bat and sees to it that you build on this knowledge. Where other books ask you to memorize stuff, we're going to show you the must know ideas that will guide you toward success in chemistry. You will start each chapter learning what the must know ideas behind a chemistry subject are, and these concepts will help you solve the chemistry problems that you find in your classwork and on exams.
Dive into this book and find:
* 250+ practice questions that mirror what you will find in your classwork and on exams* A bonus app with 100+ flashcards that will reinforce what you've learned* Extensive examples that drive home essential concepts* An easy-access setup that allows you to jump in and out of subjects* Chemistry topics aligned to national and state education standards* Special help for more challenging chemistry subjects, including the mole concept, stoichiometry, and solutions
We're confident that the must know ideas in this book will have you up and solving chemistry problems in no time-or at least in a reasonable amount of time!

About John Moore

McGraw-Hill authors represent the leading experts in their fields and are dedicated to improving the lives, careers, and interests of readers worldwide

Table of Contents

The Flashcard App
1 Getting Started in Chemical Calculations
How to Study Chemistry
The Macroscopic and Microscopic Levels of Chemistry
Units of Measurement (SI System)
Significant Figures
Problem Solving by the Unit Conversion Method
2 Atoms, Ions, and Molecules
The Subatomic Particles
The Periodic Table
Chemical Formulas: Ions and Molecules
Naming Compounds
3 Moles, Stoichiometry, and Equations
Balancing Chemical Equations
Avogadro's Number and Molar Mass
Moles and Stoichiometry
Limiting Reactant and Percent Yield
Percent Composition and Empirical Formulas
Confronting Mole Problems
4 Aqueous Solutions
Molarity (M)
Solubility and Precipitation
Acids, Bases, and Neutralization
Net Ionic Equations
5 Gases and Gas Laws
Gas Laws (P, V, n, and T)
Gas Stoichiometry
The Kinetic-Molecular Theory of Gases
Nonideal Gases
Working Gas Law Problems
6 Thermochemistry
Energy and Reactions
Enthalpy ( H)
Hess's Law
7 Electrons and Quantum Theory
Light and Matter
Bohr's Model
Quantum Mechanics
Quantum Numbers and Orbitals
Electron Configuration
Working Matter and Light Problems
8 Periodic Trends
Periodic Table Revisited
Ionization Energy
Electron Affinity
Periodic Trends
9 Lewis Structures and Chemical Bonding
Lewis Symbols
Ionic Bonds and Lattice Energy
Covalent Bonds
Bond Energy and Bond Length
More About Lewis Structures
10 Molecular Geometry and Hybridization
Molecular Geometry (VSEPR)
Valence Bond Theory (Hybridization)
Molecular Orbital (MO) Theory
Molecular Geometry Revisited
11 Solids, Liquids, and Intermolecular Forces
Types of Intermolecular Forces
Properties of Liquids
Phase Changes
12 Solutions
Concentration Units
Temperature and Pressure Effects on Solubility
Colligative Properties
Colligative Properties Problems
13 Kinetics
Reaction Rates
Rate Laws
Integrated Rate Laws (Time and Concentration)
Arrhenius and Activation Energy
More About Rate Law and Half-Life (t1/2)
14 Chemical Equilibria
Equilibrium Constants (K)
Le Chatelier's Principle
Additional Equilibria Problems
15 Acids and Bases
Bronsted-Lowry Acids and Bases
Strength of Acids and Bases
Kw-the Water Dissociation Constant
Acid-Base Equilibrium (Ka and Kb)
Acid-Base Properties of Salts and Oxides
Lewis Acids and Bases
Working Weak Acid and Base Problems
16 Buffers and Additional Equilibria
The Common Ion Effect
Buffers and pH
Titrations and Indicators
Solubility Equilibria (Ksp)
Kf-Complex Ion Equilibria
pH and Titrations Problems
17 Entropy and Free Energy
The Three Laws of Thermodynamics
Gibbs Free Energy
Free Energy and Reactions
Working Thermodynamic Problems
18 Electrochemistry
Redox Reactions
Galvanic (Voltaic) Cells
Standard Reduction Potentials (E Degrees)
Nernst Equation
Electrolytic Cells
19 Chemistry of the Elements
General Properties of Metals
Band Theory of Conductivity
Periodic Trends in Metallic Properties
General Properties of Nonmetals
Periodic Trends of Nonmetals
Properties of the Transition Metals
Coordination Compounds: Crystal Field Theory
Complex Ions
20 Nuclear Chemistry
Nuclear Reactions
Nuclear Stability
Half-Lives (t1/2)
Mass/Energy Conversions
Fission and Fusion
Nuclear Decay
21 Organic Chemistry, Biochemistry, and Polymers
Organic Compounds
Hydrocarbons and Nomenclature
Functional Groups
Nucleic Acids
Organic Reactions Problems
Answer Key
Periodic Table of the Elements

Additional information

Must Know High School Chemistry by John Moore
McGraw-Hill Education
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