Higher tier only

Chemists maybe calculating how much of substance A to add to substance B to get the reaction
to go as expected, or calculating how much of a certain product they will be able to make if they
start with X grams of substance A. One of the essential skills you must have as a good chemist is
to be able to calculate how much of a particular reactant or product you will need or make.
The problem is that atoms are by themselves far too small to weigh or count so counting atoms
is a complete non-starter. What is needed is a quantity or number that will let them compare
equal numbers of particles.

Chemists are not the only people faced with this problem, consider
paper! You don't buy individual sheets of paper, you buy paper in reams. A ream contains 500
sheets of paper. A ream of A3 paper will be bigger than a ream of A4 paper because A3 paper is
bigger than A4 paper- obviously! But a ream of A3 paper still contains 500 sheets of paper.
The ream is a unit used by paper suppliers because it contains a standard number of sheets,
500 sheets. So if an order comes in for 10 000 sheets of paper would you rather count out
10 000 sheets of paper or quickly count out 20 reams?

Chemists like paper suppliers need a standard unit which they can use to measure out equal
numbers of atoms/ions/molecules or particles. They don't use reams instead they use a unit
called the mole. The word mole may seem an odd choice of a word, since most people think of
moles as furry little gritters that dig up your lawn! The word mole is actually derived from a
Latin word meaning mass or pile. 1 mole of a substance contains 6 x 10^{23} particles.
So like the example above with paper, would you rather measure out 1 mole of a substance
or count out 6 x 10^{23} atoms?

Chemists use a relative atomic mass scale when we measure the mass of atoms
(relative simply means compared to). In 1961 the isotope of carbon, ^{12}C, was picked
as the standard from which the masses of all other atoms would be compared. On the carbon-12 scale
the ^{12}C isotope is given an atomic mass of exactly 12. This means that 12 grams of ^{12}C
contains 1 mole of carbon atoms. That is 6 x10^{23} atoms.

On this scale the mass of magnesium is 24, since magnesium atoms are twice as "heavy" as carbon atoms.
So we would say the relative atomic mass of magnesium
is 24. This means that magnesium atoms have twice the mass of carbon atoms. The relative atomic
mass of magnesium is therefore 24, we use the symbol A_{r} for relative atomic mass. So if
we weigh
out 24g of magnesium we will have the same number of atoms as we have in 12g of ^{12}C, that
is
1 mole of magnesium atoms. The only difference is the magnesium atoms are twice as massive as
carbon atoms.

Similarly carbon atoms are 12 times as heavy as hydrogen atoms, so it follows that 12g of carbon and 1g of hydrogen contain the same number of atoms, that is 1 mole of atoms. The relative atomic mass in grams of all elements will contain 1 mole of atoms.

1 mole of carbon or 12 grams of carbon is
quite a large pile of carbon and obviously atoms are very small, so there is going to be
quite a large number of atoms in that pile of carbon. In fact it's an unbelievable huge
number of carbon atoms, there are : 600 000 000 000 000 000 000 000 atoms of carbon in the
charcoal block opposite! That is 6 x 10^{23} atoms. That's a lot! This number is often called Avagadro's number,
after the Italian scientist Amedeo Avagadro. Imagine having to
count them! Well that is why we don't, we weigh them. That is the beauty of the mole. By simply
weighing out 12g of carbon we know exactly how many atoms we have. If you weigh out 1.2g of carbon,
that is 1/10th of a mole or 0.1 moles then you can easily work out how many atoms of carbon you have:

It follows then that 24g of magnesium, also contains 6 x 10^{23} atoms of magnesium

or

32g of sulfur also contains 6 x 10^{23} atoms of sulfur
or

48g of titanium also contains 6 x 10^{23} atoms of titanium.

So by weighing out masses in grams or kilograms chemists have a way of counting atoms which
is quick and also accurate.

- Chemists need to know how many atoms are reacting in order to calculate amounts of products they can make. However atoms are too small to count so chemists weigh them instead.
- All measurements have a standard or reference point, whether it is the kiolgram or the metre. The standard
chemists use to measure the masses of atoms against is the carbon-12 isotope,
^{12}C. It is assumed to have a mass of exactly 12 units. The masses of all other atoms are obtained by comparing their mass against^{12}C - 1 mole of any substance contains Avagadro's number of particles, that is 6x10
^{23}particles.