Mass Number & Isotopes (Oxford AQA International A Level Chemistry)
Revision Note
Written by: Alexandra Brennan
Reviewed by: Stewart Hird
The Composition of an Atom
Atomic number
Atoms consist of protons, neutrons and electrons
The atomic number (or proton number) is the number of protons in the nucleus of an atom
The symbol for this number is Z
It is also the number of electrons present in an atom and determines the position of the element on the Periodic Table
The proton number is unique to each element, so no two elements have the same number of protons
Electrons can be lost, gained, or shared during chemical processes but the proton number of an atom does not change in a chemical reaction
Mass number
The mass number (or nucleon number) is the total number of protons and neutrons in the nucleus of an atom
The symbol for this number is A
The atomic number and mass number for every element is on the periodic table
Atomic number & Mass number diagram
Determining the number of protons, neutrons and electrons
To calculate the number of protons, neutrons and electrons in an atom:
Number of protons= the atomic number
Number of neutrons= mass number - atomic number
Number of electrons= the atomic number
To calculate the number of protons, neutrons and electrons in an ion:
Number of protons= the atomic number
Number of neutrons= mass number - atomic number
Number of electrons
The charge on the ion indicates the number of electrons that have been lost or gained
E.g. If the charge of an ion is 2+, two electrons have been lost but if it is 1- it has gained one
Worked Example
Using a Periodic Table, identify the number of protons, neutrons and electrons in:
Mg
O2-
Al3+
Answer:
Magnesium has 12 protons, 12 neutrons and 12 electrons
Atomic number = 12 so there are 12 protons and 12 electrons
Mass number = 24 so 24-12 = 12 neutrons
An oxide ion has 8 protons, 8 neutrons and 10 electrons
Atomic number = 8 so there are 8 protons
Mass number = 16 so there are 16 - 8 = 8 neutrons
The charge on the ion is 2-, so oxygen has gained two electrons
An oxygen atom has 8 electrons so an oxide ion has 8 + 2 = 10 electrons
An aluminium ion has 13 protons, 14 neutrons and 10 electrons
Atomic number = 13 so there are 13 protons
Mass number = 27 so there are 27-13 = 14 neutrons
The charge on the ion is 3+, so aluminium has lost 3 electrons
An aluminium atom has 13 electrons so an aluminium ion has 13-3 = 10 electrons
What are isotopes?
Isotopes are atoms of the same element that contain the same number of protons and electrons but a different number of neutrons
The symbol for an isotope is the chemical symbol (or word) followed by a dash and then the mass number
E.g. carbon-12 and carbon-14 are isotopes of carbon containing 6 and 8 neutrons respectively
Isotopes of hydrogen
Time of Flight Mass Spectrometry
Mass spectrometry is a powerful analytical technique
It is used to determine the relative atomic mass, Ar, of an element, based on the abundance and mass of each of its isotopes
Knowing the relative atomic mass allows the element to be identified
It is also used to find the relative molecular mass of molecules
There are several types of mass spectrometer but they all work in the same way
The sample is ionised
It is then accelerated through the mass spectrum
The ions are separated based on the ratio of their charge to their mass
How does TOF mass spectrometry work?
Time of flight mass spectrometry is a common form of mass spectrometry
There are 4 key stages:
Ionisation
Acceleration
Ion drift
Detection
Ionisation
The sample is dissolved in a volatile solvent
The solvent is injected into the mass spectrometer using a fine hollow needle to create a mist
The needle is attached to a high voltage power supply, so as the sample is injected, the particles are ionised by losing electrons
X (g) → X+ (g) + e-
Most of the positive ions will have a 1+ charge as it is difficult to remove further electrons
The solvent evaporates until the mist contains only positively charged ions
Ionisation diagram
Acceleration
The positively charged ions are attracted towards a negatively charged plate
They accelerate towards it using an electric field
This ensures all of the positive ions have the same kinetic energy
Since all the positive ions will have the same kinetic energy, their velocity will depend on their mass
Lighter ions will move faster and heavier ions will move slower
Ion Drift
The positively charged ions will pass through a hole in the negatively charged plate and move into a flight tube
This is where the name 'Time of Flight' comes from
The time of flight of each ion in this tube depends on their velocity
Detection
When the ions have passed through the flight tube they hit a negatively charged 'detector' plate
As they hit this electric plate, they gain an electron
This gaining of an electron causes a current to be produced
The size of the current is proportional to the abundance of those ions hitting the plate and gaining an electron
Lighter ions will reach the detector first followed by heavier ions
The signal from the detector is transferred to a computer, which produces the mass spectrum
TOF spectrometry process
Examiner Tips and Tricks
Remember: All particles in the mass spectrometer are accelerated to the same kinetic energy.
This allows them to separate based on their mass.
The heavier the ion, the slower it will travel and the longer it will take to hit the detector.
Interpreting Mass Spectra
Mass spectroscopy can be used to find the relative abundance of isotopes experimentally
The relative abundance of an isotope is the proportion of one particular isotope in a mixture of isotopes found in nature
For example, the relative abundance of Cl-35 and Cl-37 is 75% and 25% respectively
This means that in nature, 75% of the chlorine atoms is the Cl-35 isotope and 25% is the Cl-37 isotope
The heights of the peaks in mass spectroscopy show the abundance of each isotope present
The horizontal axis gives the mass to charge ratio, m/z
For ions with a single charge, the m/z ratio and mass number are the same
The mass spectrum of boron
Looking at the mass spectrum of boron:
There are two peaks so there are two isotopes of boron
One isotope has a mass number of 10, and the other 11
The relative abundance of B-10 is 19.9%
The relative abundance of B-11 is 80.1 %
The data from mass spectrometry can be used to determine the relative atomic mass of an element
For each isotope multiply the relative abundance by the m/z ratio
Add these values together and divide by 100
Worked Example
Calculate the relative atomic mass of boron.
Answer:
RAM= = 10.8
Examiner Tips and Tricks
The type of spectrometry described here is called low resolution mass spectrometry, and is used to calculate relative atomic mass. High resolution mass spectrometry can be used to find the relative molecular mass of a compound.
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