- The relative atomic mass is defined as follows : The weighted average of all the element's natural isotopes on a scale where the mass of Carbon-12 is exactly 12.
- The relative atomic mass of an element or the relative formula mass of a compound is always equal to the mass of one mole of the substance in grams.
- A mole of a substance is defined as being 6.02*10^23 atoms/molecules of that substance.
- The molar volume of any gas is always the same and one mole of gas occupies 24dm^3 or 24000cm^3.
- Empirical formulae are the most simple ratio of atoms of each element in a compound, while the molecular formula gives the actual numbers of each element in a compound. For instance, the molecular formula for Hydrogen Peroxide is H2-O2, while its empirical formula is H-O.
- To work out the relative molecular mass of compund, simple add the relative atomic mass of its constituent elements. For instance, the Mr of H2-O is the 2 lots of the Ar of Hydrogen (1*2=2) plus 1 lot of the Ar of Oxygen (1*1=1).

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