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  • Empirical Formula

    The simplest whole-number ratio of atoms in a compound, derived from mass percentages using moles.

  • Molecular Formula

    Gives the actual number of atoms of each element in a compound, which may be a multiple of the empirical formula.

  • Steps to Calculate Empirical Formula
    1. Write down mass or mass % of elements.
    2. Convert masses to moles.
    3. Divide by smallest mole value.
    4. Adjust to whole numbers.
  • Determining Molecular Formula

    Calculate empirical formula mass, then divide molar mass by empirical mass to find n-factor. Multiply empirical formula by n-factor.

  • Combustion Analysis Purpose

    Used to determine the empirical formula of compounds by burning them and measuring CO2 and H2O produced.

  • Combustion Products of Hydrocarbons

    Hydrocarbons react with O2 to produce CO2 and H2O.

  • Polyatomic Ions

    Tightly bound groups of atoms with an overall charge, often oxyanions ending with oxygen.

  • Naming Ionic Compounds
    1. Cation (metal) name first, use Roman numeral if multiple charges.
    2. Anion (nonmetal) base name with suffix -ide.
    3. Polyatomic ions keep their names.
  • Naming Ionic Hydrates

    Name ionic compound first, then add numerical prefix + 'hydrate' to indicate water molecules.

  • Binary Acids Naming Rules
    1. Prefix 'hydro-' for H+ ion.
    2. Base name of nonmetal.
    3. Suffix '-ic' for acid.
  • Oxyacids Naming Rules
    1. Polyatomic ion ending '-ate' changes to '-ic'.
    2. Polyatomic ion ending '-ite' changes to '-ous'.
  • Naming Molecular (Covalent) Compounds
    1. First nonmetal named normally, no 'mono' prefix.
    2. Second nonmetal uses numerical prefix and suffix '-ide'.
    3. Drop 'a' in prefixes before vowels.
  • Balancing Chemical Equations

    Ensure equal number of atoms on both sides using coefficients called stoichiometric coefficients.

  • Stoichiometry

    Calculates amounts of reactants and products using mole ratios from balanced equations.

  • Functional Group

    Part of a molecule responsible for its chemical properties; includes groups with or without carbonyls.

  • Mass Percent

    Percentage by mass of an element in a compound:
    \(\text{Mass Percent} = \frac{\text{mass of element}}{\text{mass of compound}} \times 100\%\)

  • Common Functional Groups without Carbonyl

    Include hydroxyl (-OH), amine (-NH2), halides (X = F, Cl, Br, I), thiol (-SH).

  • Common Functional Groups with Carbonyl

    Include aldehydes, ketones, carboxylic acids, esters, and amides, all containing C=O.