introduction to radioactivity Flashcards
Atomic Structure
Subatomic particles
Smallest unit of electrical charge is the electron
= -1.6 x 10 -19 Coulombs (C)
Experience a force when placed in an Electromagnetic Field
Two types of electrical charge at an atomic level
Nucleons:Protons and Neutrons
Proton
U+U+D
2/3 + 2/3 + (-1/3) = 3/3 = 1 Proton = Positive Charge 1
Neutron
D+D+U
(-1/3) + (-1/3) + 2/3 = 0/3 = O Neutron = No Charge / Neutral
Up Quark = 2/3 electric charge
Down Quark = -1/3 electric charge
Strong Nuclear Force
What holds the nucleons together in the nucleus
Nucleons come close to each other
Results in exchange of particle called a meson
Behaves like a ping pong ball
Creates a strong nuclear force
Pulls the nucleons together
Range is 10-15m
Two Types of Nuclear Force
Strong Nuclear Force
Holds the nucleus together
Works at short distance of 10-15m
Weak Nuclear Force
Responsible for Radioactive Decay
Strong Nuclear Force (SNF)
What is holding the nucleons in the Nucleus?
Law of Electromagnetic force states ‘that like charges repel and opposite charges attract’
Protons are positively charged
Strong Nuclear Force works in the 10-15 m – 10-16 m range
How does it work?
Proton and Neutron are stable
Contain Quarks and Gluons
These exchange Kinetic Energy which allows energy to be exchanged between the particles.
As mass increases the SNF cannot hold all the nucleons on the nucleus leads to Radioactive Decay
What is an ISOTOPE
Every element in the periodic table has multiple variations
Same atomic number (protons) but different mass
Atomic number provides the chemical identity of the element
Some Isotopes are stable whilst others are unstable
C-12 P:6 C-13 P:6 C-14 P:6
n:6 n: 7 n: 8
Stable Stable Radioactive Half life
57000 years or 5.7 x 103 years
Different Isotopes of Carbon
Radioactive Decay
Also Known as:
Nuclear Decay
Radioactivity
Radioactive Disintegration
Nuclear disintegration
What is Radioactive Decay?
Process by which an unstable atom loses energy
Emission of particles – radiation
Decay occurs at a constant predictable rate
Known as the HALF LIFE (t1/2) or Decay Constant (λ)
Three types of Radioactive Decay
Alpha ( )
Beta ()
Gamma ()
The Decay Constant (λ) or Half Life (t1/2)
Time required for the activity of the radioisotope to reduce to half of the initial activity rate
Time taken to reduce by 50% of the initial rate
Means half of the initial quantity has become a different element
Units of Activity
SI unit for radioactivity is the Becquerel (Bq)
1 Bq = 1 disintegration per second
1 Bq is described as 1 radioactive decay per second
Specific Activity = activity of the Radionuclide per unit mass
BqKg-1
Radioactivity in Radiography
Radiopharmaceutical tracer
Radio-isotope is attached to a compound or chemical that cell or cells need
Inserted into the body - injection, ingested, inhaled
Radiation emitted is received and converted into a digital image
Radio-isotope Diagnostic Radiography
Isotope used – Technetium 99m (Tc99m) artificially produced
Starts with stable Molybdenum (Mo98) in a generator and bombarded with neutrons
Produces an Isotope Mo99 decays every 66 hours into Technetium 99m (Tc99m or 99mTc)
Tc99m bound to a carrier compound and is used to vector to the cell of interest
Often a glucose molecule
Tc99m or 99mTc has λ of 6 hours and decays with Gamma () rays at an energy level of 140.5 KeV which is constant
Radioisotope Iodine
Xenon (Xe124) is bombarded with protons to produce Iodine 123 (I123)
I123 decay rate is 13.22 hrs this achieved by emitting radiation until it reaches a steady state
I123 Decays to Tellurium 123 (Te123) half life = 9 x 1016 years so stable in our life time via a Gamma () at 159 KeV energy level
Used in the detection of Thyroid disease and cancer
Measuring the Gamma emission equates to uptake of isotope which equates to functionality of the organ
More Gamma greater emission rates greater the uptake of the organ
Radioactive Decay – Alpha
Large nucleus
Consists of 2 neutrons and 2 protons to from particle
Is a Helium particle
The element emits Energy and alpha particle to achieve stability
Radioactive Decay – Alpha
Large nucleus
Consists of 2 neutrons and 2 protons to from particle
Is a Helium particle
The element emits Energy and alpha particle to achieve stability
Alpha Decay Equation
Atomic mass (p + n)
Atomic number (p)
To find number of neutrons: atomic mass – protons
= 238 - 92=146
n: 146 n: 144 (lost 2 neutrons)
p: 92 p: 90 (lost 2 protons)
emits 2 protons + 2 neutrons that combine to form Helium
To find a tomic mass
= neutrons + protons
= 144+90=234
How dangerous is Decay
‘Least’ (used advisedly) dangerous of all radioactive particles
Heaviest of all decay process products
Travels a few centimetres through air
Cannot pass through a sheet of paper (0.09 mm) A4 (90GSM) is 5g in weight
Cannot penetrate epidermal tissue but can cause erythema(can burn skin)
If emitted inside the body it can cause organ and tissue damage
Alpha Particles - Clinical Practice
Cancer Treatment
Inserting sources into cancer masses
Alpha emissions destroy cancer cells
Lacks penetrating power so very localised area of effect
Development of Targeted Alpha Particle Therapy for Solid Tumors
https://www.ncbi.nlm.nih.gov/pmc/articles/PMC6930656/
Treatment Secondary Bone Cancer
https://www.macmillan.org.uk/cancer-information-and-support/bone-cancer-secondary/radiotherapy-for-secondary-bone-cancer
Click the link on the landing page for specific information
https://www.cancerresearchuk.org/about-cancer/cancer-in-general/treatment/radiotherapy/internal/radioactive-implant-treatment/what-is-brachytherapy
Beta Decay
Unstable atom with too many neutrons or protons
Protons and neutrons can transform into each other
Process to enable stability
Occurs at subatomic level of quarks
UP and DOWN quarks carry fractional charge of the electron
Results in the release of an electron
Electrons released from the nucleus are called Beta Particles
Two types
Positron +
Negatron -
Positron Decay +
Problem: Excess Protons
Solution: Protons transform into a Neutron
Result: Nucleus loses a proton however gains a Neutron
Change in Proton count = change in atomic number
Change in atomic number = change of the original element into another one
Positron Decay +
Proton consists of 2 up and 1 down quark
P = U+U+D (2/3)+(2/3)+(-1/3) = 1
Up quark changes to a Down quark
Releases a Positron and a Neutrino
Proton becomes a neutron
N=U+D+D (2/3)+(-1/3)+(-1/3)= 0
Energy is conserved so energy ‘lost’ = 1
Released as Positive Electron / Positron/ +
Remember:
p= UUD
n=UDD
Positron = +
Neutrino = energy particle (v)
Positron Decay +
Problem: too many protons
Solution: transform Proton into a Neutron
Result: Mass stays the same - + plus energy
Transforms into a different element
Negatron Decay -
Problem: Excess Neutrons
Solution: Neutron transform into a Proton
Result: Nucleus loses a neutron however gains a proton
Release of - Beta Minus
Change in Proton count = change in atomic number
Change in atomic number = change of the original element into another one
Negatron Decay -
Neutron consists of 1 up and 2 down quark
N= U+D+D (2/3)+(-1/3)+(-1/3) = 0
Down quark changes to an Up quark
Releases a -1 charge
Neutron becomes a proton
P=U+U+D (2/3)+(2/3)+(-1/3)= 1
Energy is conserved so energy ‘gained’ = -1
Released as negative Electron / negatron/ -
Remember:
p= UUD
n=UDD
Positron = +
Negatron = -
Neutrino = +ve energy particle ()
Anti Neutrino = -ve energy particle ()
n p + - +
