The isotopes of an element are like different versions of an element – they have the same number of protons but different number of neutrons. In turn, we can also say that isotopes of an element have the same atomic numbers but different atomic mass.Click to see full answer. In this manner, what is an example of a pair of isotopes? Isotope Examples Carbon 12 and Carbon 14 are both isotopes of carbon, one with 6 neutrons and one with 8 neutrons (both with 6 protons). Carbon-12 is a stable isotope, while carbon-14 is a radioactive isotope (radioisotope). Uranium-234 forms as a decay product.Secondly, how isotopes are formed? Long story short, isotopes are simply atoms with more neutrons — they were either formed that way, enriched with neutrons sometime during their life, or are originated from nuclear processes that alter atomic nuclei. So, they form like all other atoms. Simply so, how do you know the charge of an isotope? The number of electrons in neutral atoms and isotopes equals the number of protons. In ions, the number of electrons equals the number of protons plus or minus the opposite of the charge on the ion. An ion with a plus two (+2) charge has two less electrons than protons.How do you tell if an atom is an isotope?Look up at the atom on the periodic table of elements and find out what its atomic mass is. Subtract the number of protons from the atomic mass. This is the number of neutrons that the regular version of the atom has. If the number of neutrons in the given atom is different, than it is an isotope.
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