1. FRCR I – Basic Physics Nick Harding Clinical Scientist
Radiotherapy Department
Castle Hill Hospital
Hull & East Yorkshire Hospitals NHS Trust

2. FRCR LECTURES Lecture I – 13/09/2016: Lecture II – 13/09/2016:
Structure of Matter: the Atom and the Nucleus
Lecture II – 13/09/2016:
Radioactivity
Lecture III – 15/09/2016:
Interactions of EM Radiation with Matter
Lecture IV – 15/09/2016:
Interactions of Electrons with Matter

3. BIBLIOGRAPHY Radiological Physics
P. Dendy, B. Heaton – Physics for Radiologists
Medical Imaging
J. Bushberg et al – The Essential Physics of Medical Imaging
S. Webb – The Physics of Medical Imaging
P. Allisy-Roberts, J. Williams – Farr’s Physics for Medical Imaging
Nuclear Medicine
S. Cherry – Physics in Nuclear Medicine
P. Sharp et al – Practical Nuclear Medicine
Radiotherapy
F Khan – The Physics of Radiation Physics

4. Atoms & Nuclei

5. WHAT IS AN ATOM? Definition:
Άτομο {átomo} – something that cannot be divided any further
The smallest division of an element in which the physical and chemical properties of the element are maintained

6. STRUCTURE OF THE ATOM
Electron e-
Neutron n0 - - -
Proton p+ + -

7. Protons + Neutrons + Electrons
STRUCTURE OF THE ATOM
Particle
Charge
Mass (kg)
Mass (amu)
Proton +
1.6726×10-27 kg
Neutron
Neutral
1.6749×10−27 kg
Electron -
9.1094×10−31 kg
Mass of atom
Protons + Neutrons + Electrons
The atom is electrically neutral
Protons = Electrons
1amu = mass of 1/12th of C-12 =1.661x10-27 kg

8. NUCLEAR FORCES Two main forces in the nucleus:
Coulombic (electrical) forces – between protons
Repulsive
Strong nuclear forces – between all nucleons
Attractive
Strong forces operate over short nuclear distances

9. SIZE OF THE ATOM Radius of an atom is: Radius of the nucleus is:
Thus, size of atom is 104=10,000 times more than that of nucleus
Football vs 2km

10. Li 7 3 ATOMIC NOTATION Α = 7 Z = 3 Ν = 4 Z = 3 Mass Number
Atomic Number
Z = 3
Neutron Number
Ν = 4
Atomic Number
Z = 3

11. The Periodic Table Li 7 3

12. ELEMENTS Elements are groups of atoms with the same
number of protons (Z)
physical properties
e.g. density, melting and boiling point, electrical conductivity
chemical properties
e.g. reactions with water, oxygen, acids
There are more than 120 chemical ELEMENTS
92 naturally occurring

13. ELEMENTS

14. ISOTOPES
Isotopes are atoms of the same element but with different mass number (A)
same atomic number (Z)
different neutron number
they have the same physical and chemical properties
but different nuclear properties

15. ISOBARS / ISOTONES / ISOMERS
Nuclides with the same mass number (A) are called ISOBARS eg. Mo-99 and Tc-99
Nuclides with the same number of neutrons (A – Z) are called ISOTONES eg. I-131 and Xe-132
Nuclides with the same atomic (Z) and mass numbers (A) but different nuclear energy states are called ISOMERS eg. Tc-99 and Tc-99m

16. ISOTOPES

17. BOHR’S ATOMIC MODEL The Bohr model
Electrons orbit around the nucleus at fixed distances;
Electron shells designated letters K,L,M… and quantum numbers 1,2,3… respectively.
Max number of electrons in each shell is 2n2 where n is the quantum number;
Outer shell is referred to as the valence shell;
The Bohr model

18. ELECTRONIC STRUCTURE

19. ELECTRONIC STRUCTURE Hydrogen Z=1
Each orbit is associated with a discrete energy state called binding energy (or orbital binding energy);
It is the energy required to remove an electron completely from the atom
The atom is then ionised;
K orbital has largest energy;
Binding energy increases with Z;
NB the eV is a unit of energy.
ionisation
excitation
Hydrogen Z=1

20. ELECTRONIC STRUCTURE

21. EXCITATION & IONISATION
Excitation of the atom
energy transferred to an orbiting electron
electron “jumps” from lower to higher energy levels
the atom is “excited”
Ionisation of the atom
electron removed from the electric field of nucleus
the atom is “ionised”

22. EXCITATION & IONISATION

23. ELECTRON CASCADE Electron removed from its shell (i.e. ionisation) by
an X-Ray photon
a γ-Ray photon
a charged particle (e.g. electron, proton)
Vacancy created in shell
usually filled by an electron from outer shell
Secondary vacancy in outer shell
filled by an electron transition from a more outer shell
The phenomenon is called Electron Cascade

24. CHARACTERISTIC X-RAYS
Electron transitions emission of radiation
Characteristic X-rays
Characteristic of the atom itself

25. CHARACTERISTIC X-RAYS
De-excitation of a tungsten atom

26. CHARACTERISTIC X-RAYS
Characteristic X-Rays named according to:
the orbital in which the vacancy occurs
Radiation resulting from a vacancy in the:
K-shell  K-characteristic X-Ray
L-shell  L-characteristic X-Ray
Vacancy filled by an electron from:
the adjacent shell  Ka-characteristic X-ray
a non-adjacent shell  Kb-characteristic X-Ray

27. X-RAY TUBE

28. PRODUCTION OF X-RAYS

29. X-RAY SPECTRUM

30. AUGER ELECTRONS Energy not always released as a photon;
Predominant in low-Z elements is Auger electron emission;
Energy released  an orbital electron
Ejected Auger electron has a kinetic energy equal to:
the difference between the transition energy and the binding energy of the ejected electron
(69.5 – 2.5) – 2.5 = 64.5 keV

31. AUGER ELECTRONS

32. FLUORESCENT YIELD Fluorescent yield (ω) is the probability
characteristic X-Rays emitted
Auger emission predominates in
low-Z elements
in electron transitions of the outer shells
K-shell fluorescent yield is essentially
<1% for elements with Z<10 (i.e. majority of soft tissue)
15% for Calcium (Z=20)
65% for Iodine (Z=53)
~ 80% for elements with Z>60

33. NUCLEAR ENERGY LEVELS The nucleus has energy levels
analogous to orbital electron shells
often of much higher in energy
The lowest energy state is called the ground state
Nuclei in excess energy are in an excited state
Excited states (100s years>t>10-12 sec) referred to as
metastable or isomeric states (e.g. 99Tcm)

34. NUCLEAR STABILITY Nuclear line of stability For Z up to 10 ~N=Z
is a plot of N against Z
For Z up to 10
~N=Z
For Z>10
more neutrons than protons (increases to ~1.5N per Z)
Unstable nuclei above the curve
-> Neutron-rich
Unstable nuclei below the curve
-> Neutron-poor
Z=83 (Bismuth) is last element with stable isotopes 1

35. UNSTABLE NUCLEI Combinations of unstable nuclei DO exist
over time  decay to stable nuclei
Two kinds of instability
neutron excess
neutron deficiency (proton excess)
Such nuclei have excess internal energy
Stability achieved through conversion of
a neutron to a proton
a proton to a neutron
Emission of energy

36. RADIOACTIVITY Nuclides (isotopes) decaying to more stable nuclei are
Radioactive
The process is called
Radioactive Decay or Radioactivity
A nucleus undergoes a series of radioactive decays until it reaches a stable configuration

37. GAMMA RAYS
Analogous to the emission of characteristic X-Rays but generally much more energetic;
Nucleus in excited state (often from nuclear decay);
Nucleus decays to a lower (more stable) energy state
Electromagnetic radiation emitted
This electromagnetic radiation is called a
γ-ray
Gamma rays stem from the nucleus;

38. Internal Conversion Electrons
Analogous to Auger electrons;
Nuclear de-excitation energy completely transferred to orbital electron;
Electron kinetic energy equals de-excitation energy – binding energy of electron;
Electron cascade will then occur as described earlier;

39. Atomic and Nuclear Binding Energy
Nuclear binding energy is energy required to completely separate nucleus into constituent parts;
>>> electron binding energy;
Atomic binding energy is the sum of the two i.e. energy required to completely separate an atom into constituent parts;
Bringing two subatomic particles together their total energy decreases due to strong nuclear force;
∴ bound sub-atomic particles have less energy than free particles

40. Mass Defect E=mc2 where c is speed of light = 3.00x108 m/s;
(1amu = MeV)
As above, energy of bound particles is less than free particles -> mass of bound particles less than sum of mass of free particles;
E.g. N-14 atom mass is amu;
Mass of 7 p + 7 n + 7e is amu;
Mass defect = – = amu = 104.5MeV = atomic binding energy

41. Average Binding Energy

42. Nuclear Fission Splitting of a large nucleus into two smaller parts;
Separate parts have a higher average binding energy;
Overall total nuclear binding energy increases;
This energy released as radiation and kinetic energy of the fragments;
Typically also releases energetic neutrons -> more fission;
Eg. U n -> U-236 -> Sn Mo n + energy
Process used in nuclear power plants and atom bombs;

43. Nuclear Fusion Joining of two small nucleus atoms;
Eg. H-2 + H-2 -> He-3 + n
Overall nuclear binding energy (greatly) increases;
Needs a large amount of (heat/kinetic) energy to initiate fusion;
Eg. The sun, H-bomb (triggered by an atom bomb);

44. Any questions ?
With thanks to Manos Papadopoulos for the original slides.