Topic 7: Atomic and nuclear physics Flashcards
Who discovered the electron and how?
JJ Thompson discovered the electron in 1897 by using a discharge tube.
Measurements of its charge to mass ratio showed that it was smaller than an atom.
How are electrons kept in orbit?
Electrons are kept in orbit around the nucleus as a result of the electrostatic attraction between the electrons and the nucleus.
Describe the Geiger-Marsden experiment
- Beam of alpha particles aimed at thin gold foil
- Passage through foil detected
- Expected that particles would pass straight through
- Some of the particles emerged at different angles and some reflected back
- It was realised that the positively charged alpha particles were being repelled and deflected by a tiny concentration of negative charge in the atom
- As a result, the plum pudding model was replaced by the nuclear model
- Rutherford concluded that the atom must have a tiny nucleus with electrons whizzing around it and that the nucleus had a positive charge to balance the negative charge of the electrons
- He thought that almost the whole mass of an atom was concentrated in the nucleus, so it must be incredibly dense
Outline one limitation of the simple model of the nuclear atom
Accelerating charges are known to lose energy. If the orbiting electrons were to lose energy they would spiral into the nucleus. The Rutherford model cannot explain how atoms are stable.
Outline evidence for the existence of atomic energy levels.
- Rutherford model was developed further by Niels Bohr who suggested that the electrons orbit the nucleus rather like a planet orbits the sun
- Radius of Bohr’s electrons depended on the energy they had
- He also suggested that they could only move in certain orbits: when the electrons moved from a high energy state to a lower energy state they emitted a photon of light and the frequency of the light depends on the difference between the energy levels
- As there are a fixed number of energy levels only a few wavelengths of light are given out, resulting in a line spectrum
- Each individual element has distinct energy levels and therefore the emission spectra can be used to identify them
Define: nuclide
An atom characterised by its proton number and atomic number:
AZX
Define: isotope
Nuclei with the same atomic number but different mass number (due to a different number of neutrons)
Define: nucleon
A proton or a neutron making up a nucleus
Define: nucleon/mass number, A
The number of nucleons in a nucleus
Define: proton/atomic number, Z
The number of protons in a nucleus.
Define: neutron number, N
The number of neutrons in a nucleus
Describe the interactions in a nucleus
- According to our knowledge of electrostatics a nucleus should not be stable; protons are positive charges so should repel each other and so there must be another force in the nucleus that overcomes the electrostatic repulsion and hold the nucleus together
- This force is called the strong nuclear force
- Strong nuclear forces must be very strong to overcome the electrostatic forces and must also have a very small range as they are not observed outside of the nucleus
- Neutrons have some involvement in strong nuclear forces: small nuclei have equal numbers of protons and neutrons, but larger nuclei, which are harder to hold together, have a greater ratio of neutrons to protons
Describe the phenomenon of alpha decay.
- Alpha decay is one process that unstable atoms can use to become more stable. During alpha decay, an atom’s nucleus sheds two protons and two neutrons in an alpha particle.
- Since an atom loses two protons during alpha decay, it changes from one element to another.
Describe the phenomenon of beta- decay.
Beta particles are electrons emitted from the nucleus. An electron and a proton are formed when a neutron decays. At the same time, another particle is emitted called an antineutrino.
Describe the phenomenon of gamma decay.
Gamma rays are unlike the other two radiations in that they are part of the electromagnetic spectrum. After their emission, the nucleus has less energy but its mass number and its atomic number have not changed. It is said to have changed from an excited state to a lower energy state.
Effect on photographic film of alpha, beta and gamma radiation
Alpha - yes
Beta - yes
Gamma - yes
Approximate number of ion pairs produced in air for alpha, beta and gamma radiation.
Alpha - 104 per mm travelled
Beta - 102 per mm travelled
Gamma - 1 per mm travelled
Typical material needed to absorb alpha, beta and gamma radiation.
Alpha - 10-2 mm aluminium; piece of paper
Beta - a few mm aluminium
Gamma - 10 cm lead
Penetration ability of alpha, beta and gamma radiation
Alpha - low
Beta - medium
Gamma - high
Typical path length in air of alpha, beta and gamma radiation
Alpha - a few cm
Beta - less than one m
Gamma - infinite
Speed of alpha, beta and gamma radiation
Alpha - about 107 m s-1
Beta - about 108 m s-1, very variable
Gamma - 3 X 108 m s-1
Outline the biological effects of ionising radiation.
At the molecular level, an ionisation could cause damage directly to a biologically important molecule such as DNA or RNA. This could cause it to cease functioning. Alternatively, an ionisation in the surrounding medium is enough to interfere with the complex chemical reactions called metabolic pathways taking place.
Molecular damage can result in a disruption to the functions that are taking place within the cells that make up the organism. As well as potentially causing the cell to die, this could just prevent cells from dividing and multiplying. On top of this, it could be the cause of the transformation of the cell into a malignant form.
As all body tissues are built up of cells, damage to these can result in damage to the body systems that have been affected. The non-functioning of these systems can result in death. If malignant cells continue to grow, then this is called cancer.
Explain why some nuclei are stable while others are unstable.
- The stability of a particular nuclide depends greatly on the numbers of neutrons present.
- For small nuclei, the number of neutrons tends to equal the number of protons.
- For large nuclei there are more neutrons than protons.
- Nuclides above the band of stability have too many neutrons and will decay with either alpha or beta decay.
- Nuclides below the band of stability have too few neutrons and will tend to emit positrons
Describe the process of radioactive decay
Radioactive decay is a random process and is not affected by external conditions. For example, increasing the temperature of a sample of radioactive material does not affect the rate of decay. This means that there is no way of knowing whether or not a particular nucleus is going to decay within a certain period of time. All we know is the chances of a decay happening in that time.
Although the process is random, the large numbers of atoms involved allows us to make some accurate predictions. If we start with a given number of atoms, then we can expect a certain number to decay within the next minute. If there were more atoms in the sample, we would expect the number decaying to be larger. On average, the rate of decay of a sample is proportional to the number of atoms in the sample. This proportionality means that radioactive decay is an exponential process. The number of atoms of a certain element, N, decreases exponentially over time.
Define: radioactive half life
The time taken for half the number of nuclides present in a sample to decay. The time taken for the rate of decay of a particular sample of nuclides to halve.
Define: artificial transmutation
The conversion of one isotope to another. This can be done through a nuclear reaction whereby a nucleus is bombarded with a nucleon, an alpha particle or another small nucleus.
Define: unified atomic mass unit
One-twelfth of the rest mass of a carbon-12 atom in its nuclear and electronic ground state.
Define: mass defect
The difference between the mass of a nucleus and the mass of its component nucleons
Define: binding energy
The amount of energy that is released when a nucleus is assembled from its component nucleons.
Define: binding energy per nucleon
Total binding energy for the nucleus divided by the total number of nucleons
What did JJ Thompon prove?
- electrons exist and are negative
- electrons come from atoms
- atoms are neutral
- atoms were not fundamental particles but must contain some sort of structure
What is the plum pudding model?
A ball of neutral mass with balls of positive or negative charge within.
or
A ball of positive charge with balls of negative charge (electrons) within.
What fundamental property do energy levels have?
They are quantized. This means that they must have discrete, finite values (they cannot just take any orbit/level).
What is an electron that is above the ground state said to be?
It is said to be excited. So energy level 2 is the first excited state, energy level 3 is the second excited state etc.
What does quantized energy level mean?
Electrons cannot be anywhere between the energy levels, i.e. cannot move from an energy level to the next without completely having the threshold energy required for that level.
What is the light spectrum for pure white light?
A continuous spectrum, i.e. all wavelengths are emitted/present
What is the light spectrum for a hot gas?
A hot gas emits light, so the atomic spectrum will be a dark spectrum with thin bars/lines of bright light of discrete wavelengths.
What is the light spectrum for a cold gas?
A cold gas absorbs light, so the atomic spectrum will be a light spectrum with thin bars/lines of dark light/black of discrete wavelengths.
How can you find which gases are present in a gaseous nebula?
Compare the emission lines to emission lines of certain gases such as hydrogen and helium.
How can electrons move between energy levels?
By absorbing or emitting energy in the form of quantum such as protons (light).
What is a packet of light called?
A quantum (in this case, photon).
How is the energy of a photon related to its frequency?
Ephoton = hf
where h is Planck’s constant is Js and f is the frequency in Hz
How is the energy of a photon related to its wavelength?
Ephoton = hc/λ
where h is Planck’s constant in Js, c is the speed of light in ms-1, λ is the wavelength in m.
Which colour has the most energy?
Violet as it has the highest frequency / shortest wavelength
Which colour has the least energy?
Red as it has the lowest frequency / longest wavelength
Which force keeps electrons in orbit?
Electrostatic
How are emission lines formed?
Electrons transition from higher energy levels to lower ones, which emit photons.
How are absorption lines formed?
Electrons absorb photons with the exact energy required to transition to a higher energy level. Therefore that frequency of light is absorbed.
What happens if an electron absorbs enough energy to reach a hypothetical level of 0eV?
The electron escapes as it overcomes the electrostatic force. The atom becomes ionised.
In what direction to electrons move on an energy level diagram if emitting?
Downwards
In what direction to electrons move on an energy level diagram if absorbing?
Upwards
How can you calculate the emitted photon energy?
Ephoton = Einital level - Efinal level
Einital level should always be the energy level that is higher and where the electron drops from. It should also have a lower value that the final energy level.
How can you calculate the energy of an absorbed photon?
It is like the emitting method as the energy emitted = energy required by absorption.
So Ephoton = Efinal level - Eintial level
where Efinal level is a higher level with less energy.
What is radioactive decay?
The spontaneous disintegration of an unstable nucleus, which is accompanied by the emission of an ionising particle.
How is the probability of decay affected by chemical or physical conditions (e.g. state)?
It is unaffected. The probability will be constant in all conditions.
What forces are contending during decay?
- electrostatic force which repels protons
- the strong nuclear force which binds nucleons together
Describe the phenomenon of beta+ decay.
Beta+ particles are positrons emitted from the nucleus. A positron and a neutron are formed when a proton decays. At the same time, another particle is emitted called a neutrino.
What is the number of decays per second measured in?
Becquerels (Bq)
What is the dose received from a source measured in?
Sieverts (Sv) or millisievert (mSv)
When does alpha decay occur?
In unstable isotopes with too many protons and neutrons.
When does beta - decay occur?
Beta - decay occurs when a nucleus contains too many neutrons to be stable.
When does beta + decay occur?
When a nucleus contains too many protons to be stable.