Calculating Relative Atomic Mass
Here's where maths meets chemistry in a really useful way. Relative atomic mass tells us the average mass of all an element's isotopes, weighted by how common each one is in nature.
Scientists use a clever formula: Relative atomic mass = Σ (isotope mass × isotope abundance). Don't worry about the Greek symbol - it just means "add up all the results". Let's see this in action with chlorine, which has two main isotopes.
Chlorine-35 makes up 75% of natural chlorine and has a mass of 34.97 amu. Chlorine-37 makes up 25% and weighs 36.97 amu. The calculation becomes: (34.97 × 0.75) + (36.97 × 0.25) = 35.47 amu.
This weighted average explains why the relative atomic mass on your periodic table rarely matches any single isotope's mass. You'll use these values constantly in stoichiometry - the calculations that help predict how much product you'll get from chemical reactions.
Remember: Relative atomic mass is always compared to carbon-12, which is exactly 12 amu by definition!