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If an element has 3 isotopes with known natural abundance percentages what other information is needed to find the average atomic mass of the element?
Wiki User
∙ 7y ago
You still need to know the number of protons present in order to find the Atomic Mass.
Wiki User
∙ 7y ago
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What is the average mass of an element with isotopes a b and c?
a*% abundace + b*%abundance + c*%abundance
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)
How much effect do high percent abundance isotopes have on the average atomic mass of an element?
This entirely depends on the percentage of the different isotopes present. This is typically determined through mass spectrometry. After the percentages of the different isotopes are known, one times the percentage of each isotope by its relative atomic mass, then add this all together. After dividing this by 100, you will have attained the average atomic mass of a naturally ocurring element.
How the atomic mass of an element is affected by the distribution of its isotopes in nature?
The atomic mass of an element is the average of its isotopes, weighted by abundance in nature.
Europium has a mass of 150.9196amu and a mass of m152.9209amu the average atomic mass of Eu is 151.96amu calculate the relative abundance of the two europium isotopes?
Europium 150.9196 has relative abundance of 51.99%, while Europium 152.9209 has a relative abundance of 48.04% (Assuming that these are the only 2 isotopes of Europium
What is the average mass of an element with isotopes a b and c?
a*% abundace + b*%abundance + c*%abundance
If an element has three isotopes with known masses what information is needed to find the average atomic mass of the element?
The abundance percentage of each isotope
If an element has three isotopes with known natural abundance percentages what other information is needed to find the average atomic mass of the element?
The abundance percentage of each isotope
If an element had three isotopes with known masses what other information is needed to find the average atomic mass of the element?
The abundance percentage of each isotope
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)
How is the atomic mass for chlorine related to isotopes for that atom?
The average atomic mass is weighted by the most common isotopes and their relative abundance.
How is the atomic mass of an element affected by the distribution of its isotopes in nature?
The atomic mass of an element is the average of its isotopes, weighted by abundance in nature.
How the atomic mass of an element is affected by the distribution of its isotopes in nature?
The atomic mass of an element is the average of its isotopes, weighted by abundance in nature.
How much effect do high percent abundance isotopes have on the average atomic mass of an element?
This entirely depends on the percentage of the different isotopes present. This is typically determined through mass spectrometry. After the percentages of the different isotopes are known, one times the percentage of each isotope by its relative atomic mass, then add this all together. After dividing this by 100, you will have attained the average atomic mass of a naturally ocurring element.
If an element has 3 isotopes with known masses what other information is needed to find the average atomic mass of the element?
You would also need to know the abundance of each of the isotopes, i.e., how much percent of each you will typically encounter.
Why don't we use normal mean to average all of the isotopes of each element?
Because their abundance is not the same.
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.
