What is the difference between stable isotopes and unstable isotopes?

A “stable isotope” is any of two or more forms of an element whos nuclei contains the same number of protons and electrons, but a different number of neutrons. Stable isotopes remain unchanged indefinitely, but “unstable” (radioactive) isotopes undergo spontaneous disintegration.Click to see full answer. Besides, what makes an isotope stable or unstable?An unstable isotope emits some kind of radiation, that is it is radioactive. A stable isotope is one that does not emit radiation, or, if it does its half-life is too long to have been measured. It is believed that the stability of the nucleus of an isotope is determined by the ratio of neutrons to protons.Additionally, what’s an unstable isotope? Explanation: Usually, what makes an isotope unstable is the large nucleus. If a nucleus becomes larger enough from the number of neutrons, since the neutron count is what makes isotopes, it will be unstable and will try to ‘shed’ its neutrons and/or protons in order to achieve stability. Also asked, what is the difference between stable isotopes and radioisotopes? These isotopes are known as radioisotopes. The key difference between stable isotopes and radioisotopes is that stable isotopes do not undergo radioactive decay whereas radioisotopes undergo radioactive decay.What is the difference between a stable and unstable nucleus?A stable atom is an atom that has enough binding energy to hold the nucleus together permanently. An unstable atom does not have enough binding energy to hold the nucleus together permanently and is called a radioactive atom.

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