Full and Ionic Equations for Chemical Reactions

Full molecular equations show all reactants and products involved in a chemical reaction. The substances are represented using their full chemical symbols, denoting their states of matter.
Ionic equations, on the other hand, only show the ions participating in the reaction. Spectator ions, ions that do not change in the reaction, are not included.
For example, consider the reaction between sodium chloride and silver nitrate. The full equation is NaCl(aq) + AgNO3(aq) –> NaNO3(aq) + AgCl(s).
In the ionic form, this would be written: Ag+(aq) + Cl-(aq) –> AgCl(s). The sodium and nitrate ions are spectators in this reaction.
Balancing equations: Ensure there are equal numbers of each type of atom on each side of the equation.
The state of matter is typically denoted next to the formula. (s) for solid, (l) for liquid, (g) for gas, and (aq) for an aqueous, or water-based, solution.
Remember that in a neutral compound, the total charges should cancel out. So if an ion is missing in the products, you may need to infer its presence based on charge balancing.
Acids and bases also participate in similar reactions. For example, hydrochloric acid reacts with sodium hydroxide to produce water and sodium chloride. The ionic equation, omitting the spectator ions, can be represented as: H+(aq) + OH-(aq) –> H2O(l).
Redox reactions involve changes in oxidation states of ions. The oxidation state is typically represented as a Roman numeral after the element symbol. Consider an example where Iron (II) reacts with Copper (II) sulphate to form Iron (III) sulphate and Copper. In the ionic form, Fe2+(aq) + Cu2+(aq) = Fe3+(aq) + Cu(s).
Consider solubility rules when writing ionic equations. Some compounds do not dissolve in water, and are thus represented in their solid form in the equations.
When writing ionic equations, taking note of the acidic or basic nature of the reactants may help determine their ionisation in solution. Some substances, like strong acids, fully ionise in water, whereas others, like weak acids, only partially do so.