Thư viện Trường Đại học Phú Xuân
|
PXU E-LIB
Đăng nhập
Chem 121 OER Textbook

Nguồn ngoài

Chem 121 OER Textbook

Introductory Chemistry for Allied Health: This OER text was created by the faculty of South Puget Sound Community College, Exceptional Faculty Grant 2022.

Chemistry
Tác giả
Morgan Stock, Sidnee-Marie Dunn, Travis Knowles, Alaka Pradhan, Priyanka Thakral
Nhà xuất bản
South Puget Sound Community College
Nguồn
LibreTexts
Ngôn ngữ
EN
Danh mục
Khoa học cơ bản
Đọc trực tuyến Tải PDF (nguồn mở)
Mục lục· 124 mục
  1. 01: Chapter 1 - Matter
  2. 1.01: What is chemistry
  3. 1.02: States of matter
  4. 1.03: Classification of Matter
  5. 1.04: Physical and Chemical Properties
  6. 1.05: Chemical Elements and Symbols
  7. 1.06: Chemical Equations
  8. 02: Chapter 2 - Measurements
  9. 2.01: Units in Measurements
  10. 2.1.01: Systems of measurment (Metric system and SI system)
  11. 2.1.02: Prefixes
  12. 2.1.03: Measurement and Scale - The Mole Concept
  13. 2.1.3.01: Avogadro's Number and the Mole
  14. 2.1.04: Quantities and associated units
  15. 2.1.4.01: Instruments used to measure mass length and volume
  16. 2.02: Numbers in measurement (scientific notation)
  17. 2.2.01: Scientific notation
  18. 2.2.02: Calculator skills
  19. 2.2.03: Significant Figures
  20. 2.2.04: Error in measurement
  21. 2.2.05: Rounding off
  22. 2.2.5.01: Expressing Numbers
  23. 2.03: Unit conversions
  24. 2.3.01: Unit Conversion with the Metric System
  25. 2.3.02: Temperature conversions
  26. 2.3.03: Unit analysis (conversion factors equivalencies and proportionalities)
  27. 2.3.3.01: Dosage Calculations
  28. 2.3.3.02: Mole and Avogadro's number conversions
  29. 2.04: Density (definition and formula)
  30. 2.4.01: Density as a conversion factor
  31. 2.4.02: Graphing Density Under Construction
  32. 03: Chapter 3 - Atomic Structure
  33. 3.01: Atomic Theory
  34. 3.02: Elements and Atomic Number
  35. 3.03: Isotopes and Atomic Weights
  36. 3.04: Masses of Atoms and Molecules
  37. 3.05: Moles and Molar Masses
  38. 3.06: Periodic Table
  39. 3.07: Electrons and Valence Shells
  40. 04: Chapter 4 - Ionic Bonding
  41. 4.01: What is a Chemical Bond
  42. 4.1.01: Overview of Ionic and Covalent Compounds
  43. 4.1.02: Why Do Atoms Form Bonds
  44. 4.02: Ionic Compounds
  45. 4.2.01: Oxidation and Reduction
  46. 4.2.02: Electron Dot Structures of Ions
  47. 4.2.03: Ionic Charge Patterns
  48. 4.2.04: Formation of Ionic Compounds
  49. 4.03: Writing Formulas for Ionic Compounds
  50. 4.3.01: Naming Binary Ionic Compounds
  51. 4.04: Polyatomic and Ternary Ionic Compounds
  52. 4.05: Formula Mass and the Mole Concept
  53. 05: Chapter 5A - Covalent Bonding
  54. 5.01: Covalent Bonding- Introduction
  55. 5.02: Covalent (Molecular) Compounds
  56. 5.2.01: Lewis (Electron-Dot) Symbols
  57. 5.03: Covalent Bonds- Shared Electron Pairs
  58. 5.3.01: The Octet Rule
  59. 5.3.02: Electronegativity and Bond Polarity
  60. 5.04: Covalent Compounds - Formulas and Names
  61. 5.05: Lewis Structures
  62. 06: Chapter 5B - Intermolecular Forces and Molecular Models
  63. 6.01: The VSEPR Model
  64. 6.02: Molecular Polarity
  65. 6.03: Intermolecular Forces
  66. 6.3.01: Dipole-Dipole and Dispersion Forces
  67. 6.3.02: Hydrogen Bonding
  68. 07: Chapter 6 - Chemical Reactions and Stoichiometry
  69. 7.01: Prelude to Chemical Reactions
  70. 7.1.01: Reactants products states of matter and the Chemical Equation
  71. 7.1.02: Balancing of Chemical Equations
  72. 7.02: Types of Chemical Reactions
  73. 7.2.01: Combination Reactions
  74. 7.2.02: Decomposition Reactions
  75. 7.2.03: Combustion Reactions
  76. 7.2.04: Single Replacement Reactions
  77. 7.2.05: Double Replacement Reactions
  78. 7.2.06: OxidationReduction Reactions
  79. 7.03: Stoichiometry
  80. 7.3.01: Molar interpretation of balanced Chemical Reactions
  81. 7.3.02: Mole-Mass and Mass-Mass Calculations
  82. 7.3.03: Yields
  83. 7.3.04: Limiting Reagents
  84. 08: Chapter 7 - Solutions
  85. 8.01: Homogenous Mixtures
  86. 8.02: Solubility and Saturation
  87. 8.03: Gas Solubility
  88. 8.04: Mass Percents
  89. 8.05: Molarity
  90. 8.06: Dilutions
  91. 8.6.01: Serial Dilutions Under Construction
  92. 8.07: Solution Stoichiometry (Titration)
  93. 09: Chapter 8A - Acids bases and pH
  94. 9.01: Strong and Weak Acids and Bases (Conceptual Introduction)
  95. 9.1.01: Ionization of Acids in Solution (Ka values and Comparative strengths)
  96. 9.02: The pH Scale (Acidic Basic Neutral solutions)
  97. 9.2.01: Autoionization of Water (Ionic constant) and Calculator skills
  98. 9.2.02: Hydroniun ion concentration
  99. 9.2.2.01: The pH and pOH Scales - Ways to Express Acidity and Basicity
  100. 9.2.2.02: Finding the H3O and pH of Strong and Weak Acid Solutions
  101. 9.03: AcidBase Titration
  102. 9.04: Definition and Properties of Acids and Bases
  103. 9.4.01: Arrhenius Acids and Bases
  104. 9.4.1.01: Properties of acids and bases
  105. 9.4.1.02: 8.1.1.1 Nomenclature of acids and bases
  106. 9.4.1.03: Naming Acids and Bases Under Construction
  107. 9.4.02: Brnsted-Lowry Acids and Bases
  108. 9.4.2.01: Amphoteric nature of water
  109. 10: Chapter 8B - Acid-Base Buffers
  110. 10.01: What is a buffer
  111. 10.02: Buffer capacity
  112. 10.03: Henderson-Hasselbalch Approximation
  113. 10.04: Biological Buffers
  114. 11: Chapter 9 - Gases
  115. 11.01: Pressure and units
  116. 11.02: Combined gas law
  117. 11.03: Ideal Gas Law
  118. 11.04: Partial pressure
  119. 11.05: Gas collection by water displacement
  120. 12: Chapter 10 - Nuclear Chemistry
  121. 12.01: Radioactivity and Decay Types
  122. 12.02: Half-Life
  123. 12.03: Units of Radioactivity
  124. 12.04: Applications of Radioactivity