Introduction to General Chemistry

by Muhammad Arif Malik

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The purpose of this book is to teach introductory concepts of chemistry to undergraduates in one semester, assuming no prior knowledge of chemistry. It is intended for health sciences, like pre-nursing, psychology, kinesiology, and non-science majors. This book will hopefully give enough knowledge to prepare the students to understand basic chemistry used in their professional subjects, take additional chemistry courses if needed and appreciate the impact of chemistry in everyday life.

Description from LibreTexts.

Publisher
Hampton University
Subjects
Chemistry, Introductory Chemistry
Licence
Public domain, as LibreTexts states it
Who can read
Tweens profiles and older, judged from its title and subjects

Contents

LibreTexts writes equations in TeX, and here they show as TeX; the PDF has them typeset.

  1. Front Matter
  2. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Dedicated to Mr. Frank Reidy, a philanthropist who brought the author to the US
  6. Licensing
  7. 1: Matter energy and their measurements
  8. 1.1: Matter and energy
  9. 1.2: What is chemistry?
  10. 1.3: Measurements
  11. 1.4: Significant Figures
  12. 1.5: Unit conversions
  13. 1.6: Equations and graphs
  14. 1.7: Density and specific gravity measurements
  15. 1.8: Heat and its measurements
  16. 1.9: Heat and changes in physical states of matter
  17. 2: Elements
  18. 2.1: Dalton’s atomic theory
  19. 2.2: Subatomic particles and a modern view of an atom
  20. 2.3: Atoms of elements
  21. 2.4: The periodic table
  22. 2.5: Electrons in atoms
  23. 2.6: The periodic trends in properties of the elements
  24. 3: Compounds
  25. 3.1: Bonding in compounds
  26. 3.2: Naming binary ionic compounds
  27. 3.3: Polyatomic ions and their compounds
  28. 3.4: Naming acids
  29. 3.5: Naming binary covalent compounds
  30. 3.6: Lewis structures of molecules
  31. 3.7: Molecular shapes –Valence shell electron pair repulsion (VSEPR) theory
  32. 3.8: Polarity of molecules
  33. 3.9: Intramolecular forces and intermolecular forces
  34. 4: Stoichiometry –the quantification of chemical reactions
  35. 4.1: Stoichiometry
  36. 4.2: The mole
  37. 4.3: Chemical reaction
  38. 4.4: Patterns of chemical reactions
  39. 4.5: Oxidation-reduction reactions
  40. 4.6: Energetics of chemical reactions
  41. 4.7: Stoichiometric calculations
  42. 5: Solutions
  43. 5.1: Introduction to solution
  44. 5.2: Solubility
  45. 5.3: Electrolytes
  46. 5.4: Concentration of solutions
  47. 5.5: Osmosis
  48. 6: Acids and bases
  49. 6.1: What is an Acid and a Base?
  50. 6.2: Brønsted–Lowry acids and bases
  51. 6.3: Strength of acids and bases
  52. 6.4: Acid-base equilibrium
  53. 6.5: Dissociation of water
  54. 6.6: The pH
  55. 6.7: Acid-base reactions
  56. 6.8: pH Buffers
  57. 7: Gases
  58. 7.1: Characteristics of gases
  59. 7.2: The pressure-volume relationship
  60. 7.3: The temperature-volume relationship
  61. 7.4: The pressure-temperature relationship
  62. 7.5: The combined gas law
  63. 7.6: The volume-amount relationship
  64. 7.7: Ideal gas law
  65. 7.8: Dalton’s law of partial pressure
  66. 8: Nuclear chemistry
  67. 8.1: Introduction to nuclear chemistry
  68. 8.2: Radioactivity
  69. 8.3: Half-life of radioisotopes
  70. 8.4: Radiation measurements
  71. 8.5: Ionizing radiation exposures
  72. 8.6: Medical uses of radioisotopes
  73. 8.7: Making radioisotopes for medical uses
  74. 8.8: Nuclear fusion and fission
  75. Back Matter
  76. Index
  77. Glossary
  78. Detailed Licensing