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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?
Wiki User
∙ 7y ago
The abundance percentage of each isotope
Wiki User
∙ 7y ago
Wiki User
∙ 7y agoThe abundance percentage of each isotope or the mass of each isotope
benji
Emaya Williams
Wiki User
∙ 12y agoYou need to know how common each isotope is. You can the do a weighted average of each mass times the relative abundance of that isotope.
Please refer to the Wikipedia page for Atomic Mass: http://en.wikipedia.org/wiki/Atomic_mass
the abundance percentage of each isotope
Polo
The mass of each isotope (Apex 2021)
Dacieyion McGriff
Little Granger
The mass of each isotope
Anonymous
The abundance percentage of each isotope
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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 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.
The relative abundance of each isotope of an element determines its?
The relative abundance of each isotope of an element is used to determine its atomic mass. This is the weighted average of all naturally occurring isotopes.
How are isotopes placed in the periodic table?
Isotopes and their prevalence are not shown on the periodic table. Instead, the atomic weight shown for each element is an average of the atomic weights of all naturally-occurring isotopes (calculated from percentages occurring on Earth).
How are isotopes related to atomic masses not being whole numbers?
Atomic masses are the weighted average of all the isotopes of an element. The average is based on the relative abundance of each isotope. Let say we have an element with two isotopes, the first isotope has a mass of 6 and the second has a mass of 8. If we took a straight average of the atomic masses then the element would have a mass of 7. But a weighted average based on the abundance of each isotope would be different (unless both isotopes are found to be in equal amounts ie. both 50% abundance) If the isotope with a mass of 6 had a relative abundance of 75% (meaning that 3/4 of all atoms of that element had a mass of 6) then the other isotope would have a relative abundance of 25% (relative abundance must add up to 100%). The atomic mass of the elements would be calculated by multiplying each isotopes mass my the relative abundance and then adding the two results together. 75% (6) = 4.5 25% (8) = 2.0 4.5 + 2.0 = 6.5 The atomic mass for this element would have an atomic mass of 6.5 amu (atomic mass units)
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?
You still need to know the number of protons present in order to find the atomic mass.
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 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
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.
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.
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.
