Mass Number & Isotopes (Oxford AQA International A Level Chemistry)

Revision Note

Alexandra Brennan

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

Periodic Table Symbols - AQA
The atomic number and mass number are found on the Periodic Table for each element

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

The atomic structure of hydrogen isotopes
Isotopes of the same element have different numbers of neutrons

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

Ionisation in mass spectrometry
The sample is injected to produce a mist of positively charged ions

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

TOF-mass-spectometry
Lighter ions arrive at the detector first as they have higher velocities than heavier ions

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

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

    1. For each isotope multiply the relative abundance by the m/z ratio

    2. Add these values together and divide by 100

Worked Example

Calculate the relative atomic mass of boron.

Mass spectrum of boron

Answer:

  • RAM= fraction numerator left parenthesis 19.9 space straight x space 10 right parenthesis space plus space left parenthesis 80.1 space straight x space 11 right parenthesis over denominator 100 end fraction = 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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Alexandra Brennan

Author: Alexandra Brennan

Expertise: Chemistry

Alex studied Biochemistry at Newcastle University before embarking upon a career in teaching. With nearly 10 years of teaching experience, Alex has had several roles including Chemistry/Science Teacher, Head of Science and Examiner for AQA and Edexcel. Alex’s passion for creating engaging content that enables students to succeed in exams drove her to pursue a career outside of the classroom at SME.

Stewart Hird

Author: Stewart Hird

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.