1. Relative Atomic Mass and the Mole
Chapter 4 of Hienemann Textbook

2. Relative Isotopic Mass
Knowing the mass of an individual atom is not very useful because we usually work with large quantities of atoms.
The International Union of Physics and Chemistry decided that the relative atomic weights of elements would be calculated relative to the most common isotope of carbon: 12C.
Element
Isotopes
Relative Isotopic Mass
Abundance (%)
Hydrogen 1H
1.008
99.986 2H
2.014
0.014 3H
3.016
0.0001
Carbon
12C
12 EXACTLY
98.888
13C
13.003
1.112
14C
14.003
Approx

3. Relative Atomic Mass
A naturally occurring sample of an element contains the same isotopes in the same proportions, regardless of the source.
Therefore we use an average of the relative isotopic masses of the isotopes that make up an element  the relative atomic mass.
Relative atomic mass has the symbol Ar

4. Example Imagine taking 100 atoms from a sample of chlorine.
There will be:
75.80 atoms of 35Cl
24.20 atoms of 37Cl
Average relative mass of one chlorine atom:
= x x 24.20
100 =
The relative atomic mass of chlorine is 35.45
Ar (Cl) = 35.45

5. Relative Molecular Mass
The relative molecular mass (Mr) of a compound is the mass of one molecule of that substance relative to the mass of a 12C atom.
e.g. Oxygen
Mr(O2) = 2 x Ar (O)
= 2 x 16.0
= 32.0
Have a go!
Find the relative molecular mass of CO2
Mr(CO2) = Ar (C) + 2 x Ar (0)
= x 16.0
= 44.0

6. What is a mole?
Since atoms are so small it is impossible to measure out how many individual atoms of a particular element is needed in reactions.
Therefore, a unit called the mole was established which allows us to measure out an exact number of atoms.

7. (entities can be atoms, molecules etc.)
One mole contains:
6.02 x 1023 entities
(entities can be atoms, molecules etc.)
One mole of sodium ions contains 6.02 x 1023 sodium ions
One mole of water contains 6.02 x 1023 water molecules
One mole of doughnuts
contains 6.02 x 1023
doughnuts

8. e.g. What is the weight of 1 mole of Magnesium?
The weight of a mole depends on what substance is being measured.
e.g x 1023 peas weighs less than 6.02 x 1023 watermelons
The weight of 1 mole of atoms of an element is defined as the relative atomic mass of that element in grams.
e.g. What is the weight of 1 mole of Magnesium?
M(Mg) = 24g mol-1
Atomic mass
M means molar mass
(mass of 1 mole)
mol-1 means per mole

9. Give it a go!
How much will 1 mole of Helium weigh?
M(He) = 4g mol-1

10. Molar Mass
One mole of any substance (an element or a compound) will have a mass in grams equal to the sum of the relative atomic masses of all the atoms in the formula.
This is called the molar mass (M).
e.g. one mole of chlorine gas (Cl2) weighs:
M(Cl2) = 2 x Ar(Cl)
= 2 x 35.5
= 71.0g

11. Give it a go! Calculate the Molar mass of hydrogen chloride (HCl).
M(HCl) = Ar (H) + Ar (Cl) =
= 36.5g

12. Solving Problems with the Mole
The number of moles of a substance =
Mass of substance
Molar mass of the substance
Using symbols this can be written as……
m is the symbol for mass (of the sample
n = m M
n is the symbol for number of moles
M is the symbol for molar mass

13. An easy way to remember this equation…..
Cover up the corner of the triangle that symbolises the value you are looking for. n M
e.g. if you need to calculate the mass of a sample and you know the number of moles and the molar mass of the sample
Cover the m
equation: m = n x M
Give it a go! What is the equation if you’re looking for Molar mass?
M = m/n

14. Give it a go! How much does 0.024 mole of Chlorine gas (Cl2) weigh?
Work out what you’re calculating: mass
Equation to use: m = n x M
Substitute in the values that you have been given:
m = x (2 x Ar (Cl))
m = x (2 x 35)
m = x 70
m = 1.68
4. Remember the units: 1.68g