U Can: Chemistry I For Dummies
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Оглавление
Hren Chris. U Can: Chemistry I For Dummies
Introduction
About This Book
Foolish Assumptions
Beyond the Book
Where to Go from Here
Part I
Chapter 1. Looking at Numbers Scientifically
Using Exponential and Scientific Notation to Report Measurements
Multiplying and Dividing in Scientific Notation
Using Scientific Notation to Add and Subtract
Distinguishing between Accuracy and Precision
Identifying Significant Figures
Doing Arithmetic with Significant Figures
Chapter 2. Using and Converting Units
Familiarizing Yourself with Base Units and Metric System Prefixes
Looking at Density
Using Conversion Factors
Working with the Factor Label Method
Chapter 3. Breaking Down Atoms into Their Subatomic Particles
The Atom: Protons, Electrons, and Neutrons
A Brief History of the Atom
Deciphering Chemical Symbols: Atomic and Mass Numbers
Accounting for Isotopes Using Atomic Masses
Chapter 4. Surveying the Periodic Table of the Elements
Organizing the Periodic Table
Putting Electrons in Their Places: Electron Configurations
Predicting Properties and Valence Electrons from Periodic Trends
Forming Ions
Measuring the Amount of Energy (or Light) an Excited Electron Emits
Part II
Chapter 5. Building Bonds
Pairing Charges with Ionic Bonds
Forming Sodium Chloride
Ionic Salts
Sharing Electrons with Covalent Bonds
Drawing the Structural Formulas of Molecules
Occupying and Overlapping Molecular Orbitals
Polarity: Sharing Electrons Unevenly
Shaping Molecules: VSEPR Theory and Hybridization
Wondering About Water and Intermolecular Forces
Chapter 6. Naming Compounds and Writing Formulas
Labeling Ionic Compounds and Writing Their Formulas
Getting a Grip on Ionic Compounds with Polyatomic Ions
Naming Covalent Compounds and Writing Their Formulas
Addressing Acids
Mixing the Rules for Naming and Formula Writing
Beyond the Basics: Naming Organic Carbon Chains
Chapter 7. Understanding the Many Uses of the Mole
The Mole Conversion Factor: Avogadro’s Number
Doing Mass and Volume Mole Conversions
Determining Percent Composition
Calculating Empirical Formulas
Using Empirical Formulas to Find Molecular Formulas
Chapter 8. Getting a Grip on Chemical Equations
Translating Chemistry into Equations and Symbols
Understanding How Reactions Occur
Balancing Chemical Equations
Recognizing Reactions and Predicting Products
Canceling Spectator Ions: Net Ionic Equations
Chapter 9. Putting Stoichiometry to Work
Using Mole-Mole Conversions from Balanced Equations
Putting Moles at the Center: Conversions Involving Particles, Volumes, and Masses
Limiting Your Reagents
Counting Your Chickens after They’ve Hatched: Percent Yield Calculations
Part III
Chapter 10. Understanding States of Matter in Terms of Energy
Describing States of Matter and Their Phase Changes
Changing States of Matter
Classifying Pure Substances and Mixtures
Nice Properties You’ve Got There
Taking a Look at Energy and Temperature
Measuring Energy
Figuring Out Phase Diagrams
Chapter 11. Warming Up to Thermochemistry
Understanding the Basics of Thermodynamics
Working with Specific Heat Capacity and Calorimetry
Absorbing and Releasing Heat: Endothermic and Exothermic Reactions
Summing Heats with Hess’s Law
Chapter 12. Obeying Gas Laws
Working with the Kinetic Molecular Theory
Measuring and Converting Pressure
Boyle’s Law: Playing with Pressure and Volume
Charles’s Law and Absolute Zero: Looking at Volume and Temperature
Gay-Lussac’s Law: Examining Pressure and Temperature
Combining Pressure, Temperature, and Volume into One Law
Dealing with Amounts: Avogadro’s Law and the Ideal Gas Law
Mixing It Up with Dalton’s Law of Partial Pressures
Diffusing and Effusing with Graham’s Law
Chapter 13. Dissolving into Solutions
Seeing Different Forces at Work in Solubility
Concentrating on Molarity and Percent Solutions
Changing Concentrations by Making Dilutions
Altering Solubility with Temperature
Chapter 14. Playing Hot and Cold: Colligative Properties
Portioning Particles: Molality and Mole Fractions
Too Hot to Handle: Elevating and Calculating Boiling Points
How Low Can You Go? Depressing and Calculating Freezing Points
Determining Molecular Masses with Boiling and Freezing Points
Chapter 15. Working with Acids and Bases
Getting to Know Acids and Bases
Acids and Bases at the Atomic Level
Measuring Acidity and Basicity: pH, pOH, and KW
Dissociating with Strong and Weak Acids
Chapter 16. Achieving Neutrality with Titrations and Buffers
Using Indicators and Titration to Figure Out Molarity
Maintaining Your pH with Buffers
Measuring Salt Solubility with Ksp
Part IV
Chapter 17. Exploring Rates and Equilibrium
Measuring Rates
Focusing on Factors that Affect Rates
Measuring Equilibrium
Chapter 18. Accounting for Electrons in Redox
Oxidation Numbers: Keeping Tabs on Electrons
Balancing Redox Reactions under Acidic Conditions
Balancing Redox Reactions under Basic Conditions
Chapter 19. Galvanizing Yourself to Do Electrochemistry
Identifying Anodes and Cathodes
Calculating Electromotive Force and Standard Reduction Potentials
Coupling Current to Chemistry: Electrolytic Cells
Chapter 20. Doing Chemistry with Atomic Nuclei
Decaying Nuclei in Different Ways
Measuring Rates of Decay: Half-Lives
Making and Breaking Nuclei: Fusion and Fission
Part V
Chapter 21. Ten Tips for Acing a Chemistry Test
Don’t Cram
Figure Out What Is Probably on the Test
Allocate Your Study Time Wisely
Know the Basics
Do Example Problems
Be Confident
Spend Time with the Numbers
Know Your Resources
Eat and Sleep
Don’t Get Discouraged
Chapter 22. Ten Chemistry Formulas You Should Remember
The Combined Gas Law
Dalton’s Law of Partial Pressures
The Dilution Equation
Rate Laws
The Equilibrium Constant
Free Energy Change
Constant-Pressure Calorimetry
Hess’s Law
pH, pOH, and KW
KA and KB
Chapter 23. Ten Annoying Exceptions to Chemistry Rules
Hydrogen Isn’t an Alkali Metal
The Octet Rule Isn’t Always an Option
Some Electron Configurations Ignore the Orbital Rules
One Partner in a Coordinate Covalent Bond Giveth Electrons; the Other Taketh
All Hybridized Orbitals Are Created Equal
Use Caution When Naming Compounds with Transition Metals
You Must Memorize Polyatomic Ions
Liquid Water Is Denser Than Ice
No Gas Is Truly Ideal
Common Names for Organic Compounds Hearken Back to the Old Days
Chapter 24. Ten (Or So) Great Chemists
Amedeo Avogadro
Niels Bohr
Marie Curie
John Dalton
Michael Faraday
Antoine Lavoisier
Dmitri Mendeleev
Linus Pauling
Ernest Rutherford
Glenn Seaborg
That Third-Grader Experimenting with Vinegar and Baking Soda
Chapter 25. Ten Serendipitous Discoveries in Chemistry
Taking the Measure of Volume
Keeping Rubber Solid
Right- and Left-Handed Molecules
Finding a Shortcut to Color: Artificial Dye
Dreaming Up the Ring Structure
Discovering Radioactivity
Finding Really Slick Stuff: Teflon
Stick ’Em Up! Sticky Notes
Growing Hair
Speaking of Sweet Somethings
Glossary
About the Authors
Отрывок из книги
In many cases, when students think back to their time in high school or college chemistry, they don’t think of the class fondly (unless perhaps they’re science majors). A lot of people think chemistry is too abstract, too mathematical, too removed from their real lives.
One of the biggest challenges you encounter with chemistry is that you’re forced to work with numbers that have meaning behind them, maybe for the first time. You’re no longer simply doing a math problem with abstract values. Instead, these numbers represent physical quantities, so they’re associated with things like units, measurements, and chemical formulas.
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✔ Precision: Precision, which we discuss more in the next section, describes how close repeated measurements are to one another, regardless of how close those measurements are to the actual value. The bigger the difference between the largest and smallest values of a repeated measurement, the less precision you have.
The two most common measurements related to accuracy are error and percent error:
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