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Unit 2: Chemical Compositions & Reactions an overview of the key ideas…

- - - - Mass of a sample (g) = (moles of sample) * (molar mass of compound)
    - - Mass percent =
        (mass of a given element in 1 mol of a compound) / (mass of 1 mol of compound)
        x 100%
- - - - Color change
      - Solid formation
      - Bubble formation
      - Heat
      - Flame
  - - - 1) Write the formulas of the reactants and products to give the unbalanced chemical equation
      - 2) Balance by trial and error, starting with the most complicated molecules
      - 3) Check to be sure the equation is balanced (same numbers of all types of atoms on the reactant and product sides)
- - - - percent yield = (actual yield (g)) / (theoretical yield (g)) x 100%
- - - - formation of a solid
      - formation of water
      - transfer of electrons
      - formation of a gas
    - - Molecular formula equation which shows the complete formulas of all reactants and products
      - Complete ionic equations in which all strong electrolytes are shown as ions
      - Net ionic equation which includes only those components of the solution that undergo a change
  - - - A synthesis reaction is one in which a compound forms from simpler substances, such as elements
      - A decomposition reaction occurs when a compound is broken down into simpler substances
      - A combustion reaction is an oxidation-reduction reaction that involves O2
      - A precipitation reaction can also be classified as a double displacement reaction