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Why is a weighted average required for calculating atomic mass?
Wiki User
∙ 9y ago
Isotopes - that same element with a different atomic weight.
Wiki User
∙ 9y ago
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Weighted average atomic mass?
What is weighted average atomic number
What is the weighted average atomic mass of bromine?
79.9173125
An average of the masses of all the naturallly occurring isotopes of an element?
The weighted average for all isotopes that occur in nature for an element is its atomic weight listed on the Periodic Table of the elements.
Weighted average mass of the mixture of its isotopes?
Average atomic mass I think.
The average atomic mass of an element is the average of the atomic masses of its?
The average atomic mass of an element is the average of the atomic masses of its isotopes (that is a weighted average). You have to take into account the abundance of each isotope when they do your averaging.
What is the weighted average of the atomic masses of an element's naturally occurring isotopes is called the?
The atomic weight that is listed on the periodic table for each element is the weighted average of the atomic masses of an element's naturally occurring isotopes. So you are describing atomic weight as it is used on the periodic table.
Is the mass and atomic mass the same?
No. The atomic weight is the number on the Periodic Table and is a weighted average of the atomic masses.
How do the decimal places on the atomic masses of elements realate to isotopes?
The atomic mass of an element is the weighted average of masses of the isotopes of the element, weighted in proportion to their abundance.
What is the average atomic mass compared to atomic mass?
Atomic mass is the number of protons and neutrons in an atom.
The atomic mass of an element is defined as the weighted average mass of that element's?
For the chemical elements the correct expression is atomic weight.This value is the weighted average mass of the natural isotopes of this element.
Why do elements which exists as isotopes have fractional atomic mass?
Each isotope of an element has a different Atomic Mass, so an average is taken of all the isotopes, but the average is weighted because the natural abundance (%) of each isotope is factored in. If hydrogen-1 is much more abundant than deuterium and tritium, then the weighted average will be closer to 1 than 2 or 3 but not a whole number. The following equation shows how percent abundance factors into the weighted average. (atomic mass A)(X% abundance) + (atomic mass B)(Y% abundance)...=(weighted average of all isotopes of the element)(100% abundance)
Why is the atomic mass of sulfur listed on the periodic table not a whole number?
The atomic mass given on the periodic table is a weighted average of all the isotopes, weighted by abundance of each isotope
