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Contents - Lessons & Practice

Science

Chemistry 2e

OpenStax book

OpenStax

Chemistry 2e

21 lessons

One lesson for each chapter of Chemistry 2e, in the book’s order. The lesson teaches what that chapter says you need to know, then checks it.

  1. 1Essential IdeasThe basic building block of matter is the atom, the smallest unit of an element that can enter into combinations with atoms of the same or other elements.
  2. 2Atoms, Molecules, and IonsSamples of a particular compound all have the same elemental proportions by mass.
  3. 3Composition of Substances and SolutionsDue to the use of the same reference substance in defining the atomic mass unit and the mole, the formula mass (amu) and molar mass (g/mol) for any substance are numerically equivalent (for example, one H 2 O molecule…
  4. 4Stoichiometry of Chemical ReactionsChemical reactions in aqueous solution that involve ionic reactants or products may be represented more realistically by complete ionic equations and, more succinctly, by net ionic equations
  5. 5ThermochemistryKinetic energy (KE) is the energy of motion; potential energy is energy due to relative position, composition, or condition.
  6. 6Electronic Structure and Periodic Properties of ElementsElectromagnetic radiation that passes through two closely spaced narrow slits having dimensions roughly similar to the wavelength will show an interference pattern that is a result of constructive and destructive…
  7. 7Chemical Bonding and Molecular GeometryIn pure covalent bonds, the electrons are shared equally.
  8. 8Advanced Theories of Covalent BondingValence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms.
  9. 9GasesAtmospheric pressure is measured using a barometer; other gas pressures can be measured using one of several types of manometers
  10. 10Liquids and SolidsIntermolecular attractive forces, collectively referred to as van der Waals forces, are responsible for the behavior of liquids and solids and are electrostatic in nature.
  11. 11Solutions and ColloidsThe solutes are the other components typically present at concentrations less than that of the solvent.
  12. 12KineticsRelations between different rate expressions for a given reaction are derived directly from the stoichiometric coefficients of the equation representing the reaction
  13. 13Fundamental Equilibrium ConceptsThe system’s response to these disturbances is described by Le Châtelier’s principle: An equilibrium system subjected to a disturbance will shift in a way that counters the disturbance and re-establishes equilibrium.
  14. 14Acid-Base EquilibriaThe species formed when a Brønsted-Lowry base gains a proton is the conjugate acid of the base.
  15. 15Equilibria of Other Reaction ClassesComplex ions are examples of Lewis acid-base adducts and comprise central metal atoms or ions acting as Lewis acids bonded to molecules or ions called ligands that act as Lewis bases.
  16. 16ThermodynamicsEntropy ( S ) is a state function that can be related to the number of microstates for a system (the number of ways the system can be arranged) and to the ratio of reversible heat to kelvin temperature.
  17. 17ElectrochemistryElectrons are transferred from the reductant (in the anode half-cell) to the oxidant (in the cathode half-cell) through an external circuit, and inert solution phase ions are transferred between half-cells, through a…
  18. 18Representative Metals, Metalloids, and NonmetalsThese elements are representative metals, metalloids, and nonmetals.
  19. 19Transition Metals and Coordination ChemistryThe transition metals are elements with partially filled d orbitals, located in the d -block of the periodic table.
  20. 20Organic ChemistryThe alkanes are saturated hydrocarbons—that is, hydrocarbons that contain only single bonds.
  21. 21Nuclear ChemistryThis “missing” mass is the mass defect, which has been converted into the binding energy that holds the nucleus together according to Einstein’s mass-energy equivalence equation, E = mc 2 .