Isotopes are variants of a chemical element that have the same number of protons in their atomic nuclei, but a different number of neutrons. This means that isotopes of a given element have the same atomic number, but a different atomic mass.
Definition:
Isotopes are atoms of the same element that have the same number of protons but a different number of neutrons.
History:
Isotopes were first discovered by Frederick Soddy in 1913. He noticed that the atomic weight of an element did not always match its atomic number and suggested that this was due to the presence of isotopes. In the following years, other scientists confirmed the existence of isotopes and began to study their properties.
Properties:
Isotopes have the same chemical properties as their parent element because they have the same number of protons and electrons. However, their physical properties may be different due to their different atomic masses. For example, isotopes of an element may have different melting and boiling points, densities, and radioactivity.
Explanation:
Isotopes are formed when the number of neutrons in the nucleus of an atom is different from the number of protons. This can happen naturally or through artificial means, such as nuclear reactions. Isotopes can be stable or radioactive, depending on the number of neutrons in their nuclei.
Examples:
- Carbon has three stable isotopes: carbon-12, carbon-13, and carbon-14.
- Hydrogen has three isotopes: protium, deuterium, and tritium.
- Oxygen has three isotopes: oxygen-16, oxygen-17, and oxygen-18.
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| Isotopes of hydrogen |
In general, isotopes are formed due to the number of neutrons in the nucleus of an atom. In nature, isotopes of an element can be found in different proportions, and these proportions can vary depending on the source of the element. Some isotopes are stable, while others are radioactive and can be used for various purposes such as medical, industrial, or scientific research.
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