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The fundamental particle responsible for isotopes is the neutron. As such, different isotopes of the same element have the same atomic number (since the protons never change), but have a different atomic weight/mass dependent on the differing number of neutrons in the atom's nucleus.

For instance, the element carbon has 6 protons (a different number of protons would yield a different element); therefore, carbon has an atomic number of 6. However, there are 15 known isotopes of carbon that all have a different number of neutrons and thus a different atomic weight. Of those 15 isotopes, only three occur naturally, so let's use these in the example. These three naturally-occurring isotopes are carbon 12, carbon 13 and carbon 14 (the numbers represent the isotope's atomic weight). These isotopes have 6, 7 and 8 neutrons, respectively, paired with the 6 protons in the nucleus.

protons: 6

+

neutrons: 6

------------------------------

Carbon 12 (6 + 6 = 12)

protons: 6

+

neutrons: 7

------------------------------

Carbon 13 (6 + 7 = 13)

protons: 6

+

neutrons: 8

------------------------------

Carbon 14 (6 + 8 = 14)

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