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Contents - Lessons & Practice

Science

Chemistry: Atoms First 2e

OpenStax book

OpenStax

Chemistry: Atoms First 2e

21 lessons

One lesson for each chapter of Chemistry: Atoms First 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. 3Electronic Structure and Periodic Properties of ElementsOther important wave phenomena include standing waves, periodic oscillations, and vibrations.
  4. 4Chemical Bonding and Molecular GeometryIn pure covalent bonds, the electrons are shared equally.
  5. 5Advanced Theories of 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.
  6. 6Composition of Substances and SolutionsThe empirical formula mass of a covalent compound may be compared to the compound’s molecular or molar mass to derive a molecular formula
  7. 7Stoichiometry 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
  8. 8GasesAtmospheric pressure is measured using a barometer; other gas pressures can be measured using one of several types of manometers
  9. 9ThermochemistryKinetic energy (KE) is the energy of motion; potential energy is energy due to relative position, composition, or condition.
  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. 12ThermodynamicsEntropy ( 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.
  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. 16ElectrochemistryElectrons 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…
  17. 17KineticsRelations between different rate expressions for a given reaction are derived directly from the stoichiometric coefficients of the equation representing the reaction
  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. 20Nuclear 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 .
  21. 21Organic ChemistryThe alkanes are saturated hydrocarbons—that is, hydrocarbons that contain only single bonds.