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In chemical reactions, electrons in atoms are responsible for
bonds forming and being destroyed.
The identity of the atoms involved does not change
This is not true for nuclear processes because;
These reactions involve the protons and neutrons in the
nucleus – too large or too small of a ratio between protons and
neutrons
Fission Reactions
• Involve a nucleus collapsing to form a smaller nucleus
• Usually involve atoms with large nucleii such as the Lathanides and Actinides
• They produce , and emissions.
Fusion Reactions
• These involve nuclei joining together to make larger ones.
• These type of reactions are what go on inside stars and provide the energy that causes them to shine.
The particle
• Consists of 2 protons and 2 neutrons
• Is emitted from a nucleus during radio active decay
• Is the most destructive radiation because it ionizes atoms it bumps into
The particle
• Has a relative mass of 4 amu• Low penetration ability (stopped by paper
or skin)• Harmful if ingested or inhaled (can’t get
out)• Decreases atomic number by 2 • Decreases mass by 4
The particle
• The particle is the same as a Helium atom with the electrons removed.
• It is often written as He 4
2 in nuclear equations
An decay reaction
The Uranium atom U23892 decays by particle emission
U 238
92 He 42 + ? 234
90
What is represented by ?
An decay reaction
The Uranium atom U23892 decays by particle emission
U 238
92 He 42 + Th 234
90
Th is thorium – we can work it out by using the periodic table and looking up the atom with atomic number 90. The mass number does not matter – it is simply an isotope of Th.
More decay reactions
The Thorium atom Th22790 decays by particle emission
Th 227
90Complete the equation
More decay reactions
The Actinium atom Ac22589 decays by 3 particle emissions
Ac 225
89Complete the equation
Particle emissions
Particles are electrons but they do not come from the electron shells which surround the nucleus – they come from the nucleus itself.
The electron is emitted when a neutron sheds its negative chargeand becomes a proton.
N10 p1
1 0-1
Particle emissions
The effect of Particle emission is to increase the proton count by 1 whilst leaving the overall mass unchanged.
Th231
90 0
-1 + ?What is ?
Pa231
91
Decay Series
When a radioactive nucleus such as U23892 decays it
often produces another radioactive isotope which goes on to decay further.
We are going to construct a decay series on graph paper for the element U238
92 to show how it eventually forms a stable isotope of lead Pb206
82
GET A PIECE OF GRAPH PAPER
• Draw a vertical axis representing atomic mass. It will need to run from 200 to 240
• Draw a horizontal axis representing atomic number. It will need to run from 78 to 93.
• Position the isotope U23892 on your graph
and mark it clearly.
Plotting an decay
• The nucleus gives off an alpha particle first to form a new nucleus
• Work out what the new nucleus is• Find the nucleus on your graph and add it in• Join the points with an arrow
Plotting a beta emission
• The Thorium next loses a Beta particle• Work out what would be formed• Add the nucleus onto your chart
Building up the decay series
Continue to build up the series using the following emissions. Each alpha emission is shown as a diagonal to the left and each beta emission is a horizontal line to the right.
If you are successful you should end up with Pb20682
Good Luck !
Emission sequence (including the first two example emissions)
1. 2. 3. 4. 5. 6. 7.
8. 9. 10. 11. 12. 13. 14.
Electron Capture
• Some times a nucleus will capture an electron and a proton converts to a neutron.
• This decreases the atomic number but does not change the mass
• 201Hg80 + 0-1e 201Au79 + γ0
0
Positron Emission
• A positron has the mass of an electron and the charge of a proton – it’s kind of like a “positive electron”
• It may be emitted when a proton turns into a neutron
• Atomic number decreases and mass stays the same.
• 22Na11 0+1e + 22Ne10