This fifth in the series of Isotope Notations (iN 4.2) explains why it is essential to note specific isotopes in your laboratory instruments. The use of the correct lab notebook, reference book, or reference guide is critical for the successful handling of a number of laboratory studies.
Isotopes can be very unstable. They can become “super” or very unstable, causing an unstable chemical reaction. To avoid this, you must record in the laboratory journal your experiments and observations, with a special attention to observing how isotopes interact with each other and with one another’s isotopes.
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The two most commonly found isotopes, deuterium, and tritium, are unstable in nature. It takes a little more care in observing isotopic effects between these two types of radioactive elements and their isotopes.
Other isotopes, such as bromine and carbon 14, have very stable isotopes that do not interfere with each other. These isotopes, along with uranium and thorium, form the basis of a stable isotope mixture.
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Some of the stable isotopes are not radioactive and do not change their atoms to unstable ones. In these cases, they remain stable when they react with an isotope from another element or isotope of that element.
Isotopes can be easily detected when they are present in a sample. For example, boron and oxygen atoms will be found in nearly all compounds that have boron in them. Oxygen atoms are unstable, however, so when oxygen atoms attach to boron atoms, they form borate.
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Isotopes can also be measured on a chemistry laboratory worksheet. There are several examples where the measurement of isotopes can help in the proper evaluation and identification of a particular compound or element. The Isotope Handbook provides examples in this area.
Isotopes are vital for successful chemistry and medical studies. Knowing the meaning of these unstable atoms helps you keep better records, and gives you better confidence in your experimental results.
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Isotopes can affect the reactions of the molecules of different elements. As we age, our body chemistry changes, and certain types of molecules get larger while other types become smaller. These changes, together with changes in the atmosphere and the environment, cause us to react differently to the substances that we come in contact with. This is why isotopes are so important.
Isotopes are essential for keeping track of these chemical reactions. Without isotopes, it would be difficult to measure the stability of the different molecules, especially the molecular components of cells and DNA strands.
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Isotopes are particularly important for the proper analysis of biological samples, which are fragile, and must be treated with special care. These samples are made up of both living and non-living substances and they cannot be broken down into smaller components.
If the right techniques are used to deal with these samples, isotopes will provide much greater sensitivity than older methods. The Isotope Handbook explains how isotopes can be used in laboratory experiments.
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Isotopes can also be useful when studying the chemical properties of elements and in determining their atomic behavior. Their presence in natural substances, such as water and the atmosphere, is essential for many chemical reactions.
Isotopes can also be used in determining the composition of the Earth. By learning the relationship between the elements and the amounts of these isotopes present, you will be able to determine the composition of the Earth.
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