Thư viện Trường Đại học Phú Xuân
|
PXU E-LIB
Đăng nhập
CHEM 114: Introductory Chemistry

Nguồn ngoài

CHEM 114: Introductory Chemistry

This is a lecture and laboratory course that covers the fundamental concepts of chemistry. This course assumes no previous knowledge of chemistry, presenting both chemical problem solving and laboratory skills. This course is intended primarily to prepare students for CHEM 131.

Chemistry
Nhà xuất bản
LibreTexts
Nguồn
LibreTexts
Giấy phép
CC BY-NC-SA
Ngôn ngữ
EN
Danh mục
Khoa học cơ bản
Đọc trực tuyến Tải PDF (nguồn mở)
Mục lục· 147 mục
  1. 01: The Chemical World
  2. 1.01: The Scope of Chemistry
  3. 1.02: Chemicals Compose Ordinary Things
  4. 1.03: Hypothesis, Theories, and Laws
  5. 1.04: The Scientific Method- How Chemists Think
  6. 1.05: A Beginning Chemist- How to Succeed
  7. 02: Measurement and Problem Solving
  8. 2.01: Taking Measurements
  9. 2.02: Scientific Notation- Writing Large and Small Numbers
  10. 2.03: Significant Figures- Writing Numbers to Reflect Precision
  11. 2.04: Significant Figures in Calculations
  12. 2.05: The Basic Units of Measurement
  13. 2.06: Problem Solving and Unit Conversions
  14. 2.07: Solving Multistep Conversion Problems
  15. 2.08: Units Raised to a Power
  16. 2.09: Density
  17. 2.10: Numerical Problem-Solving Strategies and the Solution Map
  18. 2.11: Taking Measurements
  19. 2.E: Measurement and Problem Solving (Exercises)
  20. 03: Matter and Energy
  21. 3.01: In Your Room
  22. 3.02: What is Matter?
  23. 3.03: Classifying Matter According to Its State- Solid, Liquid, and Gas
  24. 3.04: Classifying Matter According to Its Composition
  25. 3.05: Differences in Matter- Physical and Chemical Properties
  26. 3.06: Changes in Matter- Physical and Chemical Changes
  27. 3.07: Conservation of Mass- There is No New Matter
  28. 3.08: Energy
  29. 3.09: Energy and Chemical and Physical Change
  30. 3.10: Temperature- Random Motion of Molecules and Atoms
  31. 3.11: Temperature Changes- Heat Capacity
  32. 3.12: Energy and Heat Capacity Calculations
  33. 3.E: Exercises
  34. 04: Atoms and Elements
  35. 4.01: Experiencing Atoms at Tiburon
  36. 4.02: Indivisible- The Atomic Theory
  37. 4.03: The Nuclear Atom
  38. 4.04: The Properties of Protons, Neutrons, and Electrons
  39. 4.05: Elements- Defined by Their Numbers of Protons
  40. 4.06: Looking for Patterns- The Periodic Law and the Periodic Table
  41. 4.07: Ions- Losing and Gaining Electrons
  42. 4.08: Isotopes- When the Number of Neutrons Varies
  43. 4.09: Atomic Mass- The Average Mass of an Element’s Atoms
  44. 05: Molecules and Compounds
  45. 5.01: Sugar and Salt
  46. 5.02: Compounds Display Constant Composition
  47. 5.03: Chemical Formulas- How to Represent Compounds
  48. 5.04: A Molecular View of Elements and Compounds
  49. 5.05: Writing Formulas for Ionic Compounds
  50. 5.06: Nomenclature- Naming Compounds
  51. 5.07: Naming Ionic Compounds
  52. 5.08: Naming Molecular Compounds
  53. 5.09: Naming Acids
  54. 5.10: Nomenclature Summary
  55. 5.11: Formula Mass- The Mass of a Molecule or Formula Unit
  56. 06: Chemical Composition
  57. 6.01: How Much Sodium?
  58. 6.02: Counting Nails by the Pound
  59. 6.03: Counting Atoms by the Gram
  60. 6.04: Counting Molecules by the Gram
  61. 6.05: Chemical Formulas as Conversion Factors
  62. 6.06: Mass Percent Composition of Compounds
  63. 6.07: Mass Percent Composition from a Chemical Formula
  64. 6.08: Calculating Empirical Formulas for Compounds
  65. 6.09: Calculating Molecular Formulas for Compounds
  66. 07: Chemical Reactions
  67. 7.01: Grade School Volcanoes, Automobiles, and Laundry Detergents
  68. 7.02: Evidence of a Chemical Reaction
  69. 7.03: The Chemical Equation
  70. 7.04: How to Write Balanced Chemical Equations
  71. 7.05: Aqueous Solutions and Solubility- Compounds Dissolved in Water
  72. 7.06: Precipitation Reactions- Reactions in Aqueous Solution That Form a Solid
  73. 7.07: Writing Chemical Equations for Reactions in Solution- Molecular, Complete Ionic, and Net Ionic Equations
  74. 7.08: Acid–Base and Gas Evolution Reactions
  75. 7.09: Oxidation–Reduction Reactions
  76. 7.10: Classifying Chemical Reactions
  77. 7.11: The Activity Series
  78. 08: Quantities in Chemical Reactions
  79. 8.01: Climate Change- Too Much Carbon Dioxide
  80. 8.02: Stoichiometry
  81. 8.03: Making Molecules- Mole-to-Mole Conversions
  82. 8.04: Making Molecules- Mass-to-Mass Conversions
  83. 8.05: Limiting Reactant, Theoretical Yield, and Percent Yield
  84. 8.06: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
  85. 8.07: Enthalpy- A Measure of the Heat Evolved or Absorbed in a Reaction
  86. 09: Electrons in Atoms and the Periodic Table
  87. 9.01: Blimps, Balloons, and Models of the Atom
  88. 9.02: Light- Electromagnetic Radiation
  89. 9.03: The Electromagnetic Spectrum
  90. 9.04: The Bohr Model- Atoms with Orbits
  91. 9.05: The Quantum-Mechanical Model- Atoms with Orbitals
  92. 9.06: Quantum-Mechanical Orbitals and Electron Configurations
  93. 9.07: Electron Configurations and the Periodic Table
  94. 9.08: The Explanatory Power of the Quantum-Mechanical Model
  95. 9.09: Periodic Trends- Atomic Size, Ionization Energy, and Metallic Character
  96. 10: Chemical Bonding
  97. 10.01: Bonding Models and AIDS Drugs
  98. 10.02: Representing Valence Electrons with Dots
  99. 10.03: Lewis Structures of Ionic Compounds- Electrons Transferred
  100. 10.04: Covalent Lewis Structures- Electrons Shared
  101. 10.05: Writing Lewis Structures for Covalent Compounds
  102. 10.06: Resonance- Equivalent Lewis Structures for the Same Molecule
  103. 10.07: Predicting the Shapes of Molecules
  104. 10.08: Electronegativity and Polarity - Why Oil and Water Don’t Mix
  105. 11: Gases
  106. 11.01: Extra-Long Straws
  107. 11.02: Kinetic Molecular Theory- A Model for Gases
  108. 11.03: Pressure- The Result of Constant Molecular Collisions
  109. 11.04: Boyle’s Law- Pressure and Volume
  110. 11.05: Charles’s Law- Volume and Temperature
  111. 11.06: Gay-Lussac's Law- Temperature and Pressure
  112. 11.07: The Combined Gas Law- Pressure, Volume, and Temperature
  113. 11.08: Avogadro’s Law- Volume and Moles
  114. 11.09: The Ideal Gas Law- Pressure, Volume, Temperature, and Moles
  115. 11.10: Mixtures of Gases- Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
  116. 11.11: Gases in Chemical Reactions
  117. 12: Liquids, Solids, and Intermolecular Forces
  118. 12.01: Interactions between Molecules
  119. 12.02: Properties of Liquids and Solids
  120. 12.03: Intermolecular Forces in Action- Surface Tension and Viscosity
  121. 12.04: Evaporation and Condensation
  122. 12.05: Melting, Freezing, and Sublimation
  123. 12.06: Types of Intermolecular Forces- Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole
  124. 12.07: Types of Crystalline Solids- Molecular, Ionic, and Atomic
  125. 12.08: Water- A Remarkable Molecule
  126. 13: Solutions
  127. 13.01: Prelude - Tragedy in Cameroon
  128. 13.02: Solutions- Homogeneous Mixtures
  129. 13.03: Solutions of Solids Dissolved in Water- How to Make Rock Candy
  130. 13.04: Solutions of Gases in Water- How Soda Pop Gets Its Fizz
  131. 13.05: Solution Concentration- Mass Percent
  132. 13.06: Solution Concentration- Molarity
  133. 13.07: Solution Dilution
  134. 13.08: Solution Stoichiometry
  135. 13.09: Freezing Point Depression and Boiling Point Elevation- Making Water Freeze Colder and Boil Hotter
  136. 13.10: Osmosis- Why Drinking Salt Water Causes Dehydration
  137. 14: Acids and Bases
  138. 14.01: Sour Patch Kids and International Spy Movies
  139. 14.02: Acids- Properties and Examples
  140. 14.03: Bases- Properties and Examples
  141. 14.04: Molecular Definitions of Acids and Bases
  142. 14.05: Reactions of Acids and Bases
  143. 14.06: Acid–Base Titration- A Way to Quantify the Amount of Acid or Base in a Solution
  144. 14.07: Strong and Weak Acids and Bases
  145. 14.08: Water- Acid and Base in One
  146. 14.09: The pH and pOH Scales- Ways to Express Acidity and Basicity
  147. 14.10: Buffers- Solutions That Resist pH Change