Estimating Nuclear Radius
- Nuclear radius can be measured experimentally using one of two methods
- Rutherford scattering - the closest approach method
- Electron scattering
Closest Approach Method
- In Rutherford scattering:
- Alpha particles were fired at a thin sheet of gold foil
- Some of the alpha particles were found to rebound from the gold foil by 180°
- Rutherford scattering indicates that there must be an electrostatic repulsion between the alpha particles and the gold nucleus
- The initial kinetic energy of an alpha particle is:
- At the point of closest approach, r, the repulsive force reduces the speed of the alpha particles to zero momentarily
- At this point, the initial kinetic energy of an alpha particle, Ek, is equal to electric potential energy, Ep
- The radius of the closest approach can be found be equating the initial kinetic energy to the electric potential energy
- Equating the two equations gives:
An alpha particle transfers its maximum kinetic energy to maximum potential energy at the distance of closest approach to a gold nucleus
Advantages of the Closest Approach Method
- Alpha scattering gives a good estimate of the upper limit for a nuclear radius
- The mathematics behind this approach are very simple
- The alpha particles are scattered only by the protons and not all the nucleons that make up the nucleus
Disadvantages of the Closest Approach Method
- Alpha scattering does not give an accurate value for nuclear radius as it will always be an overestimate
- This is because it measures the smallest separation between the alpha particle and the gold nucleus, not its radius
- Alpha particles contain hadrons which are affected by the strong nuclear force
- This affects high-energy alpha particles which get very close to the nucleus (0.5 to 3 fm)
- The mathematics in this method cannot account for the effects due to the strong nuclear force
- The gold nucleus will recoil as the alpha particle approaches
- Alpha particles have a finite size and mass whereas electrons can be treated as a point mass
- Very few alpha particles rebound at exactly 180°, so to detect these, a small collision region is required
- The alpha particles in the beam are assumed to have the same initial kinetic energy which may not be realistic
- The foil target must be extremely thin to prevent multiple scattering
Electron Scattering
- Electrons accelerated to close to the speed of light are found to have wave-like properties, such as the ability to diffract
- The de Broglie wavelength of an electron is equal to:
- Where:
- h = Planck's constant
- m = mass of an electron (kg)
- v = speed of the electrons (m s−1)
- The diffraction pattern forms a central bright spot with dimmer concentric circles around it
- From this pattern, a graph of intensity against diffraction angle can be used to find the diffraction angle of the first minimum
- Using this, the size of the atomic nucleus, R, can be determined from:
- Where:
- θ = angle of the first minimum (degrees)
- λ = de Broglie wavelength (m)
- R = radius of the nucleus (m)
The diffraction pattern produced by passing high-energy electrons through a target foil can be used to determine the nuclear radius
Pros & Cons of Electron Diffraction Method
Advantages
- Electron diffraction is much more accurate than the closest approach method
- This method gives a direct measurement of the radius of a nucleus
- Electrons are leptons; therefore, they will not interact with nucleons in the nucleus through the strong nuclear force as an alpha particle would
Disadvantages
- Electrons must be accelerated to very high speeds to minimise the de Broglie wavelength and increase resolution
- This is because significant diffraction takes place when the electron wavelength is similar in size to the nuclear diameter
- Electrons can be scattered by both protons and neutrons
- If there is an excessive amount of scattering, then the first minimum of the electron diffraction can be difficult to determine