Key Concepts: Chemical Equations

A chemical equation represents a chemical reaction using the symbols of the elements involved. It details both the reactants (substances before the reaction) and the products (substances after the reaction).
The arrow in a chemical equation symbolises the direction of the reaction, from reactants to products. The reaction may be reversible, indicated by a two-sided arrow, meaning that it can proceed in both directions.
The law of conservation of mass states that no atoms are created or destroyed in a chemical reaction. Therefore, the number of each type of atom before a reaction equals the number after the reaction. This principle is reflected in balanced chemical equations.
Balancing chemical equations ensures that the same number of each type of atom is present on both sides of the equation. To do this, coefficients (whole numbers placed in front of the chemical symbols) may be modified.
Substances in a chemical equation are represented by their symbols or formulas. The states of matter are indicated as (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous (dissolved in water).
Certain conditions may be required for a reaction to take place such as heat, light or a catalyst. These are typically written above the reaction arrow.
Stoichiometry is the study of the quantitive relationships or ratios of amounts of reactants and products in a chemical reaction expressed by a balanced chemical equation. For example, if the equation reads 2H2 + O2 → 2H2O, this means for every two molecules of hydrogen gas, one molecule of oxygen gas is required to produce two molecules of water.
Some reactions may be exothermic (releasing heat) or endothermic (absorbing heat), which may be indicated in the chemical equation.
It is essential to understand how to interpret and write balanced equations accurately, as this allows prediction of the amounts of reactants needed or products made in a reaction. It also enables one to identify potential energy changes in reactions.
In terms of practical laboratory work, being able to write and balance equations can be crucial in preparing and carrying out experiments safely and effectively. For instance, knowing the exact quantities of reactants to use can prevent unwanted excesses that could potentially lead to hazardous situations.

Remember to practise balancing different types of equations, as this will help familiarise yourself with the process and develop your problem-solving skills.