![]() How does isotope abundance impact atomic weight?Ītomic mass depends on the composition of protons and neutrons in an element, with each weighing 1 atomic mass unit (amu). Carbon-14 is a naturally occurring carbon isotope that radioactively decays. One isotope of carbon, carbon-14, defies the normal reactivity of the stable element. Carbon is known to be a very stable element, often being involved in predictable reactions. In some instances, isotopes can have different reactivity, but in most cases, the defining difference is the number of neutrons.Ī common example of an isotope having reactivity that differs from what the element is known for is carbon. Though these two versions of the same element differ in the number of neutrons, it is important to note that they do not differ in the number of protons and electrons. Isotopes are very similar versions of the same element, only having one difference: the number of neutrons. ![]() Neutron: Neutrally charged subatomic particle located in the nucleus of an atom.Proton: Positively charged subatomic particle located in the nucleus of an atom.Isotope: when an element has a different form in which it contains the same number of protons, but differs in the number of neutrons.Quantifying Protons, Neutrons, and Electrons.In this tutorial, we will learn what isotope abundance is and how to use it to calculate the atomic weight of an element. If you look closely, it is clear that these values are almost never whole numbers. When looking at the periodic table, each element has a value displayed for the atomic mass.
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