Isotopes are different forms of an element that have the same number of protons but different numbers of neutrons in the nucleus. This means that isotopes have the same atomic number, which determines the element's identity, but different atomic mass due to the varying number of neutrons.
For example, let's consider the element carbon. Its atomic number is 6, which indicates that it has 6 protons in its nucleus. Carbon typically has 6 neutrons, giving it an atomic mass of 12.01 (since the mass number is the sum of protons and neutrons).
However, carbon can have isotopes with different numbers of neutrons. One of the isotopes of carbon is carbon-13 (13C), which has 6 protons and 7 neutrons. This isotope has a slightly higher atomic mass of approximately 13 (again, by summing protons and neutrons).
Another isotope of carbon is carbon-14 (14C), which has 6 protons and 8 neutrons. This isotope is radioactive and is used in carbon dating to determine the age of ancient artifacts.
So, isotopes provide us with different forms of an element that share similar chemical properties but have different physical properties due to differences in atomic mass.
Explain the concept of isotopes and provide an example.
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