Nguồn ngoài
CHEM 113: Human Chemistry I
This text provides a general background on the factual basis and principles of chemistry. These first year chemistry courses explore chemical phenomena and principles with emphasis on developing an understanding of chemistry and an appreciation of what chemists do. You must commit yourself to learning the basic vocabulary of chemistry. You will acquire skills in dealing with chemical phenomena and principles and in manipulating mathematical expressions that describe chemical behavior.
- Tác giả
- Pedro Muíño
- Nhà xuất bản
- Saint Francis University
- Nguồn
- LibreTexts
- Ngôn ngữ
- EN
- Danh mục
- Khoa học cơ bản
Mục lục· 130 mục
- 01: Matter and Measurements
- 1.01: Chemistry - The Central Science
- 1.02: States of Matter
- 1.03: Classification of Matter
- 1.04: Chemical Elements and Symbols
- 1.05: Chemical Reactions- Examples of Chemical Change
- 1.06: Physical Quantities- Units and Scientific Notation
- 1.07: Measuring Mass Length and Volume
- 1.08: Measurement and Significant Figures
- 1.09: Rounding Off Numbers
- 1.10: Problem Solving - Unit Conversions and Estimating Answers
- 1.11: Temperature Heat and Energy
- 1.12: Density and Specific Gravity
- 02: Atoms and the Periodic Table
- 2.01: Atomic Theory and the Structure of Atoms
- 2.02: Elements and Atomic Number
- 2.03: Isotopes and Atomic Weight
- 2.04: The Periodic Table
- 2.05: Some Characteristics of Different Groups
- 2.06: Electronic Structure of Atoms
- 2.07: Electron Configurations
- 2.08: Electron Configurations and the Periodic Table
- 2.09: Electron-Dot Symbols
- 03: Ionic Compounds
- 3.01: Ions
- 3.02: Ions and the Octet Rule
- 3.03: Ions of Some Common Elements
- 3.04: Periodic Properties and Ion Formation
- 3.05: Naming Monoatomic Ions
- 3.06: Polyatomic Ions
- 3.07: Ionic Bonds
- 3.08: Formulas of Ionic Compounds
- 3.09: Naming Ionic Compounds
- 3.10: Some Properties of Ionic Compounds
- 3.11: H and OH Ions - An Introduction to Acids and Bases
- 04: Molecular Compounds
- 4.01: Covalent Bonds
- 4.02: Covalent Bonds and the Periodic Table
- 4.03: Multiple Covalent Bonds
- 4.04: Coordinate Covalent Bonds
- 4.05: Characteristics of Molecular Compounds
- 4.06: Molecular Formulas and Lewis Structures
- 4.07: Drawing Lewis Structures
- 4.08: The Shapes of Molecules
- 4.09: Polar Covalent Bonds and Electronegativity
- 4.10: Polar Molecules
- 4.11: Naming Binary Molecular Compounds
- 05: Classification and Balancing of Chemical Reactions
- 5.01: Chemical Equations
- 5.02: Balancing Chemical Equations
- 5.03: Precipitation Reactions and Solubility Guidelines
- 5.04: Acids Bases and Neutralization Reactions
- 5.05: Redox Reactions
- 5.06: Recognizing Redox Reactions
- 5.07: Net Ionic Equations
- 06: Chemical Reactions - Mole and Mass Relationships
- 6.01: The Mole and Avogadros Number
- 6.02: Gram-Mole Conversions
- 6.03: Mole Relationships and Chemical Equations
- 6.04: Mass Relationships and Chemical Equations
- 6.05: Limiting Reagent and Percent Yield
- 07: Chemical Reactions - Energy Rates and Equilibrium
- 7.01: Energy and Chemical Bonds
- 7.02: Heat Changes during Chemical Reactions
- 7.03: Exothermic and Endothermic Reactions
- 7.04: Why Do Chemical Reactions Occur Free Energy
- 7.05: How Do Chemical Reactions Occur Reaction Rates
- 7.06: Effects of Temperature Concentration and Catalysts on Reaction Rates
- 7.07: Reversible Reactions and Chemical Equilibrium
- 7.08: Le Chateliers Principle- The Effect of Changing Conditions on Equilibria
- 08: Gases Liquids and Solids
- 8.01: States of Matter and Their Changes
- 8.02: Intermolecular Forces
- 8.03: Gases and the Kinetic-Molecular Theory
- 8.04: Gas Pressure
- 8.05: Boyles Law - The Relation between Volume and Pressure
- 8.06: Charless Law- The Relation between Volume and Temperature
- 8.07: Gay-Lussac's Law- The Relationship Between Pressure and Temperature
- 8.08: The Combined Gas Law
- 8.09: Avogadros Law - The Relation between Volume and Molar Amount
- 8.10: The Ideal Gas Law
- 8.11: Partial Pressures and Dalton's Law
- 8.12: Liquids
- 8.13: Solids
- 8.14: Changes of State Calculations
- 09: Solutions
- 9.01: Mixtures and Solutions
- 9.02: The Solution Process
- 9.03: Solubility
- 9.04: The Effect of Temperature on Solubility
- 9.05: The Effect of Pressure on Solubility - Henrys Law
- 9.06: Units of Concentration
- 9.07: Dilution
- 9.08: Ions in Solution - Electrolytes
- 9.09: Properties of Solutions
- 9.10: Osmosis and Osmotic Pressure
- 9.11: Dialysis
- 10: Acids and Bases
- 10.01: Acids and Bases Definitions
- 10.02: Acid and Base Strength
- 10.03: Acid Dissociation Constants
- 10.04: Water as Both an Acid and a Base
- 10.05: Measuring Acidity in Aqueous Solutions- The pH Scale
- 10.06: Working with pH
- 10.07: Acid and Base Equivalents
- 10.08: Some Common Acid-Base Reactions
- 10.09: Acidity and Basicity of Salt Solutions
- 10.10: Buffer Solutions
- 10.11: Titration
- 12: Introduction to Organic Chemistry - Alkanes
- 12.01: The Nature of Organic Molecules
- 12.02: Families of Organic Molecules - Functional Groups
- 12.03: The Structure of Organic Molecules - Alkanes and Their Isomers
- 12.04: Drawing Organic Structures
- 12.05: The Shapes of Organic Molecules
- 12.06: Naming Alkanes
- 12.07: Properties of Alkanes
- 12.08: Reactions of Alkanes
- 12.09: Cycloalkanes
- 12.10: Drawing and Naming Cycloalkanes
- 13: Nuclear Chemistry12
- 11.06: Ionizing Radiation
- 11.07: Measuring Radiation
- 11.08: Artificial Transmutation
- 11.09: Nuclear Fission and Nuclear Fusion
- 13.01: Nuclear Reactions
- 13.02: The Discovery and Nature of Radioactivity
- 13.03: Stable and Unstable Isotopes
- 13.04: Nuclear Decay
- 13.05: Radioactive Half-Life