Steps

1. Write reactants as they occur naturally if the reactants are elements of atoms
2. If there are bonding involved in the reactants, ensure they are bonded correctly
3. Bond the products correctly
4. Note that subscript numbers are used during bonding
5. Once all bonding are correct, balance the equation by ensuring all the number or reacting atoms is equal to the number of atoms in the product. Note that Integers/large numbers are used in front of the compound being balanced
6. Include state Symbols

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Rules

N.B. : in order to balance a chemical equation, you must 1st have all the correct reactants and products. The reactants and Products must be bonded correctly.

1. If there is an ionic compound in the chemical eqn. balance the atom which forms that compound 1st.
2. Balance the most complex covalent substances 2nd
3. If there are any group of atoms bonded together in the same way in the products and reactants then you can treat that group of atoms as an individual atom and balance the group as a whole. For eg. if there is a SO4 group then you balance the entire SO4 group by saying there is SO4 in the product and 1 SO4 in the reactants.
4. If there are reactants or products which are made up of the same type of atoms, balance the reoccurring atom last, For eg. if there are 2 reactants and hydrogen exists in both reactants then hydrogen should be balanced last.

N.B. when balancing, normal numbers are used and when bonding, subscripts are used.

Hydrogen normally bonds covalently however it will bond basically when it is bonding with a metal. When hydrogen is bonding covalently the charge is 1+ and when it is bonding ionically it it 1+.

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Examples

Na + H2SO4 → NaSO4 + H2

Na - 1 | 2

H - 2 | 2

SO4 - 1 | 1

Na - 2

H - 2

SO4 - 1

2Na + H2 SO4 → Na2 SO4 + H2

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