Chemical Formulas & Balancing Chemical Equations
This video explains how to balance a chemical reaction: the same number of atoms of each element must be on both sides of the equation.
This video tutorial defines five simple steps to use when balancing chemical equations.
This video provides tips on how to balance more complicated chemical reactions. It also provides an example of balancing the combustion reaction of ethylene, C₂H₄.
This video uses different colors to relate a balanced chemical equation to the structural formulas of the reactants and products.
This video highlights the differences between empirical, molecular, and structural chemical formulas. Empirical formulas show the simplest whole-number ratio of atoms in a compound. Molecular formulasshow the number of each type of atom in a molecule. Structural formulas show the arrangement of the molecule.
This video defines oxidation and reduction using an example: NaCl. Oxidation is the gain of oxygen. Reduction is the loss of oxygen.
These videos explain how to balance redox reactions under acidic conditions. They also help to identify which half reaction is oxidation and reduction.
These videos explain how to balance redox reactions in basic solutions using the following steps: (1) separate the net reaction into two separate half reactions (oxidation and reduction), (2) balance the atoms first under acidic conditions using H+ and H2O, and (3) balance the charges by adding electrons to the side of the chemical equation with the highest oxidation state. Once the electrons in both half-reactions are equal, the two reactions may be combined together to form the net reaction. To neutralize the acid, OH- ions are added to both sides of the equation.