Atoms differ from one another suggesting that the arrangement of sub-atomic particles is different from atom to atom. One way that they differ is in terms of mass.
Syllabus reference S1.2.2Structure 1.2.2 - Isotopes are atoms of the same element with different numbers of neutrons.
- Perform calculations involving non-integer relative atomic masses and abundance of isotopes from given data.
Guidance
- Differences in the physical properties of isotopes should be understood.
- Specific examples of isotopes need not be learned.
Tools and links
- Nature of science, Reactivity 3.4 - How can isotope tracers provide evidence for a reaction mechanism?
Isotope definition
Isotopes are atoms of a specific element that have a definite number of neutrons and consequently a different mass. In effect all atoms are isotopes of one element or another.
Most elements have several isotopes, some of which are stable, and others that spontaneously break apart releasing radioactivity.
For example, the element hydrogen has three isotopes, 1H, 2H and 3H. 1H is the most common of the isotopes and makes up 99.99% of any sample of hydrogen. 2H is also called deuterium and comprises the other 0.01% of naturally occurring hydrogen. The third isotope is called tritium and is not very common.
Tritium is radioactive and breaks apart spontaneously releasing radioactivity, in this case, a fast moving electron.
Note that the product of this radioactive process is helium. Effectively, one of the neutrons in the tritium nucleus has emitted an electron (called a beta particle) and turned into a proton.
Summary of the hydrogen isotopes
Relative abundance
The 'relative abundance' of an isotope means the percentage of that particular isotope that occurs in nature. Most elements are made up of a mixture of isotopes. Clearly the sum of the percentages of the specific isotopes must add up to 100%.
Example:Chlorine has two isotopes 35Cl and 37Cl, with relative abundance of 75% and 25% respectively.
This means that in any naturally occurring sample of chlorine 75% of the atoms are Cl-35 atoms and 25% of the atoms are chlorine-37 atoms.
Properties of isotopes
Isotopes differ only in their number of neutrons. This means that they have identical electronic configurations and identical chemical properties. The masses of the isotopes affects any characteristic that depends on mobility or mass of the particles.
Density is defined as mass/volume therefore isotopes have different densities.
Diffusion is a process that is dependent on the density of the diffusing species. According to Graham's law, the rate of diffusion is proportional to the square root of the reciprocal density and hence the reciprocal relative mass (of a gas):
Example:How does the rate of diffusion of hydrogen differ from the rate of diffusion of deuterium?
- Hydrogen, H2, relative mass = 2
- Deuterium, D2, relative mass = 4
Applying Graham's law, relative rates of diffusion = 1/√2 : 1/√4
Therefore 1/1.414 : 1/2 = 0.71 to 0.5
Hydrogen diffuses 1.4 x faster than deuterium
This principle is put to use in the purification of uranium 235 for use in the atomic energy industry. The uranium occurs naturally as two isotopes 235U and 238U with relative abundances of approximately 0.28% to 99.71% with the remainder due to other isotopes.
Only the uranium 235 can be used for atomic energy and so needs to be concentrated in the sample. This is done by reacting the uranium with hydrogen fluoride to form uranium hexafluoride UF6, which is a volatile solid that can be converted to a gas at easily attainable temperatures.
- 235UF6
- 238UF6
Once in the gaseous form, use is made of the different diffusion rates of the two compounds. The relative masses of the two hexafluorides are so similar, the gases must be diffused using a series of centrifuges, each one increasing the percentage of the required uranium isotope in the mixture.
The uranium hexafluoride is then turned into uranium dioxide for use in fuel pellets.
Uses of isotopes
Isotopes are used in medicine, industry, and in many other applications. The danger of radioisotopes revolves around their ability to cause cell damage by ionising the atoms that are involved in molecules and hence, breaking bonds.
Radioisotopes may emit three different common types of radiation, alpha, beta and gamma radiation, depending on the specific atom.
- Alpha radiation consists of particles containing two protons and two neutrons (equivalent to a helium nucleus); is highly destructive to living tissue, but has very low penetration power and is stopped by a few centimetres of air. It is only seriously dangerous if ingested in some way.
- Beta radiation consists of highly energetic electrons. It has poorer ionising characteristics than alpha radiation, but has greater penetrating power.
- Gamma radiation is electromagnetic in nature and has the lowest ionising ability, but extremely great penetrating power.
14C - radiocarbon dating
Living organisms respire. Plants breathe in carbon dioxide and animals eat plants (and other animals!). The consequence is that all living things take up carbon throughout their lives.
The percentage of the isotope carbon 14 remains fairly constant in our atmosphere, as it is produced in the upper atmosphere by cosmic bombardment of naturally occurring carbon-12 in the form of carbon dioxide. At the same time the carbon 14 nuclei are decaying. There is an equilibrium between these two processes:
carbon-12 ⇋ carbon-14
This means that the proportion of carbon-14 compared to carbon-12 found in all living organisms is also constant. However, when a living organism dies it stops taking up both forms of carbon.
The carbon -14 isotope decays naturally with a half life of about 5,600 years. So, a simple procedure involving counting the radioemissions due to carbon-14 from a sample of material that was once alive, can be used to estimate how long ago it died.
Therapeutic applications
Cobalt-60 is used in hospitals as a beta emission source in the treatment of cancer
Beta rays are fast moving electrons. They can be focussed onto cancerous tissue to destroy it using a cobalt 60 source. This form of treatment is known as radiotherapy.
Iodine-131 and Iodine-125 are used as medical tracers and for treating certain cancers.
In several conditions the body can be scanned for problems using iodine, which is easily taken up by the body and transported through the lymphatic system. The isotopes 131I and 125I are easy to detect and short lived in the body.
Use is made of the destructive effect on cellular tissue to destroy cancer cells in treatment with radioisotopes. Radioactive sources are used that have a short lifetime in the body, but which can be focussed in their effects on tissues.
Technetium-99, for example is used in gammagraphy, a technique where a sample of the radioisotope is injected into the body. After a few hours the technetium circulates around the body and binds to areas of bone damage. By detection of areas of unusually high concentration of radiation, it is possible to identify bone injuries that do not show up on X-rays.
The bone scans of radiation emissions are called gammagrams.
Industrial applications
Detection of leaks in gas pipes by injection of a radioisotope into the pipeline and detecting where the radiation emerges. Beta emitters are used in measurement of thickness in the paper industry.
Nuclear energy generation
Both uranium-235 and plutonium-239 are neutron emitting radioactive isotopes. The neutrons emitted cause further events in neighbouring nuclei leading to chain reactions, which release large amounts of energy as the nuclei break apart (fission). This energy is used to heat up water into steam to drive turbines for electricity production.
Nuclear energy remains controvertial and there are strong arguments both for and against its use.
Other applications
Americium-241 is a man-made isotope used in smoke detectors.
