Acid and Base Nomenclature

Acid and Base Naming

• There are five questions on acid and base naming on the exam.

• Binary acids contain hydrogen and one other element.

• Oxy acids contain hydrogen and an oxyanion.

• Oxyanions are negatively charged polyatomics that include oxygen.

• All acids contain hydrogen at the beginning of the compound.

• To name a binary acid:

  • Start the first word with "hydro-."

  • End the first word with "-ic."

  • The middle part of the first word is the stem of the second element.

    • Example: HF is hydrofluoric acid.

• For oxy acids, pay attention to the polyatomic ion in the formula.

  • If the polyatomic ending is "-ite", the acid ends in "-ous".

  • If the polyatomic ending is "-ate", the acid ends in "-ic".

    • Example: ClO3- is chlorate

      • Chlorate (ends in "-ate") becomes chloric acid.

      • Carbonate (ends in "-ate") becomes carbonic acid.

      • Sulfite (ends in "-ite") becomes sulfurous acid.

      • Nitrate (ends in "-ate") becomes nitric acid.

• For bases, follow these naming rules:

  • Name the cation.
  • Name the anion.
  • Make sure to crisscross the charges when writing formulas.
    • Example: Magnesium hydroxide is Mg(OH)2. Transition metals require Roman numerals to indicate their charge.
    • Example: Iron(III) hydroxide is Fe(OH)3.

Types of Chemical Reactions

• There are five types of chemical reactions: synthesis, combustion, decomposition, single replacement, and double replacement.

• Synthesis reactions contain only two reactants (elements) and one product.

  • To predict the product, crisscross the charges of the reactants.
  • Example: Aluminum and oxygen combine to form aluminum oxide (Al2O3).

• Combustion reactions contain oxygen (O2) as a reactant.

  • Hydrocarbon + O2 → H2O + CO2
  • Element + O2 → Oxide (same as synthesis)

• The exam will ask you to:

  • Predict products
  • Identify reactions
  • Write complete and net ionics

• Decomposition reactions have one compound as the reactant.

  • Binary decomposition: A compound breaks down into its elements.

    • For example: Cao breaks down into calcium and oxygen.

  • Metal hydroxide decomposition: Metal hydroxide → Metal oxide + Water

    • For example: LiOH decomposes into Li2O and H2O.

  • Metal carbonate decomposition: Metal carbonate → Metal oxide + CO2 Metal chlorate decomposition: Metal chlorate → Metal chloride + O2

• Single replacement reactions have one element and one compound as reactants.

  • Use the activity series to determine if the replacement will occur.

  • Three types:

    • Metal replaces a metal: needs activity series to solve
    • Metal replaces hydrogen in water/acid: needs activity series to solve
    • Nonmetal replaces nonmetal: needs activity series to solve

• Double replacement reactions have two ionic compounds as reactants.

  • Anions swap places between the two reactants.

• For all reaction types, ensure the chemical equation is balanced.

Aqueous Solutions and Solubility

• Solubility is the ability of a solute to dissolve in a solvent to form a solution.

• Aqueous solutions have a solute dissolved in a solvent, where water is the solvent.

  • Not every aqueous solutions contains dissolved particles
    • Instead, water can have a precipitate at the bottom

• The solubility chart is used to determine if a compound is soluble (aq) or insoluble (s).

  • Alkali metals (Group 1) are always soluble.
  • Ammonium (NH4+) and nitrate (NO3-) are also always soluble.

Complete and Net Ionic Equations

• Complete ionic equations show all soluble ionic compounds written as ions.
  • Only aqueous compounds can be separated into ion form.
  • Each ion must have a charge, state of matter, and coefficient.
• Solids, liquids, and gases cannot be separated into ions.
• Net ionic equations do not show spectator ions.
• Spectator ions appear on both sides of the reaction and do not participate.
• Short cut to solve net ionic - Net ionic equations will always equal the solid

Mole Conversions

• Conversions between grams, moles, and particles of the same substance.

• Known conversion factors include:

  • Avogadro's number: 6.022 x 10^23 representative particles/mol (atoms, molecules, formula units)
  • Molar mass: grams/mole (obtained from the periodic table)

•   Significance figures matter 
  

Empirical and Molecular Formulas

• Empirical Formula: The lowest whole number ratio of the elements in the compound

  • To find follow steps,
    • If given percent compositions, assume the % as grams
    • Convert grams to moles
    • Divide by the smallest amount
    • If don't have whole number, multiply a number by a whole number
    • Cannot round numbers

• Molecular Formula: The exact number of atoms in the compound that may or not be be reduced.

  • To find follow steps,
    • To find the molecular formula of a compound with and empirical, divide the molecular formula by the empirical formula
    • Multiply all the subscripts if atoms by this factor

Percent Composition

• Percent composition is the mass of each element in a compound divided by the total mass of the compound, multiplied by 100.

Stoichiometry

• Conversions between grams/moles of different substances and a reaction.
• Stoichiometry Problem vs. Limiting Reactant
  • One # in problem - Stoichiometry (Grams & Moles can mix to make new compounds)
  • Two reactants w/ masses = Limiting Reactant

Limiting and Excess Reactant

• Limiting reactant: The reactant that runs out first.
• Excess reactant: The reactant that has leftovers.
• To solve a typical three part LRA Problem, follow these basic steps: - What are we given (grams reactant, and what are we trying to find? (grams product) - Convert from grams to moles for both reactants (A & B) using conversion factor - Convert the moles in reactants into a "ratio" using coefficients - You will solve the first questions: (limiting and excess Reactant) - Percent Yield: Actual yield / theoretical yield * 100

Cheat sheet notes

• Cheat sheet:
  • Definitions for binary and oxy acids
  • Rules for naming binary and oxy acids + examples
  • Rules for naming bases + examples
  • All types of reactions with general formulas (A+B→AB, etc.)
  • Solubility table
  • Metal oxides are solid
  • Brinklehoff elements + states
  • Definition of solubility
  • Definition of spectator ion
  • Example of complete ionic equation
  • Grams to mole particle map
  • Conversion factors (Avogadro's number, molar mass)
  • Examples of empirical and molecular formula calculations
  • Percent composition formula
  • Stoichiometry map
  • Example of a gram to gram stoichiometry problem
  • Limiting Reactant + one completed example.
  • A's Birthday