Why atoms of the same element can weigh different amounts
In short: This video breaks down the fundamental chemistry of isotopes and how they determine an element's relative atomic mass. It explains why chemical properties remain stable even when the internal weight of an atom shifts.
Atoms are defined by their proton number, which determines their identity on the Periodic Table. However, isotopes occur when atoms of the same element possess the same number of protons but different numbers of neutrons. For example, Carbon-12 and Carbon-13 are isotopes; they behave similarly in chemical reactions but differ in mass.
The Relative Atomic Mass (Ar) of an element is not a simple average of its isotopes. Instead, it is a weighted average based on the relative abundance of each isotope found in nature. The video demonstrates how to calculate this value using specific isotopic masses and their percentage abundances, using copper as a practical example.
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Sources
- Summary by Intellect · source: GCSE Chemistry - Elements, Isotopes & Relative Atomic Mass (2027/28 exams)
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