Why is it necessary to use the average atomic mass of all isotopes, rather than the mass of the most commonly occurring isotope, when referring to the atomic mass of an element?
Why is it necessary to debit my account by
Why? Because accounting, and even more so chemistry, is a highly quantitative exercise. Mass is always conserved in a chemical reaction, and accurate masses, which are the weighted averages of the isotopic masses, are necessary to demonstrate this conservation of mass. For the lighter elements, hydrogen, carbon, and oxygen, this is not so important in that there is normally only the ONE isotope. But for the heavier elements, especially where the isotopic distribution is large, and we get fractional atomic masses, we must account for the isotopic distribution.
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It is necessary to use the average atomic mass of all isotopes because elements can have multiple isotopes with different masses. Using the average atomic mass accounts for the abundance of each isotope, providing a more accurate representation of the element's overall mass.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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