# Chemical Formulas & Balancing Chemical Equations

## ⚛ 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.

## ⚛ How to Balance Chemical Equations in 5 Steps 📺

• This video tutorial defines five simple steps to use when balancing chemical equations.

## ⚛ Balancing Complex 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.

## ⚛ Visually Understanding Balancing Chemical Equations 📺

• This video uses different colors to relate a balanced chemical equation to the structural formulas of the reactants and products.

## ⚛ The Difference Between Empirical, Molecular, and Structural Formulas 📺

• 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.

## ⚛ Oxidation and Reduction 📺

• This video defines oxidation and reduction using an example: NaCl. Oxidation is the gain of oxygen. Reduction is the loss of oxygen.

## ⚛ Balancing Redox Reactions in Acidic Solution 📺

• These videos explain how to balance redox reactions under acidic conditions. They also help to identify which half reaction is oxidation and reduction.

## ⚛ Balancing Redox Reactions in Basic Solution 📺

• 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.