Atomic Mass: How to Calculate Isotope Abundance

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How do you determine and calculate isotope abundance when you know the relative atomic mass (also known as atomic weight), as measured in amu or atomic mass numbers? Here we will go through the algebra and reasoning to figure out the amount of abundances of the isotopes, in percentages and in decimals.

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Atomic mass and atomic weight are the same thing--they are both the average mass of atoms of an element. It's mass number (not to be confused with atomic mass) that is the mass of a specific isotope.

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What if there are 3 isotopes? how can we tackle that problem?

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Hamza Ali tThere is not a question like that,unless they give u one of istope’s percentage

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devid them by ther pirsent and then add them

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@GT Talks True, finding the percentage is legit the purpose of the problem -_-

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good question, i’m trying to figure that out right now too😅 my question is asking to find the abundance for 2 isotopes while i have the abundance of 1 and the atomic mass

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@@valentinacastanoo that's super easy. It is done in the Same manner. But the third we be called different

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I would appreciate your assistance in solving this. Silicon has three stable isotopes, 28Si, 29Si and 30Si. The heaviest isotope has a percentage abundance of 3.1%. using the relative atomic mass from the periodic table, calculate the percentage abundance of the lightest isotope to one decimal place

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Hi Tyler, first thank u for the great explanation! I have a Q which is how can I calculate 3 isotopes abundance. For example, calculate the three isotopes S-32, S-33 & S-34 and tell which of them is more abundant. Regards

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Thank you so much, now I know how to solve for the % abundance. 💯

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This is the most amazing explanation in the world. Thank you so much.

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Thank YOU! I’m glad you like it!

[@brittneywilson3369]

Hi Tyler, How do you know which isotope to set to x and which one to set to (1-x) when solving for the abundance?

[@tdewitt451]

it doesn't matter. you can do either one.

[@CR1257]

Tyler DeWitt Hi Tyler, What if you have 3 isotopes instead of 2. What does the third isotope become if we already have an (X) and a (1-X) attached to the first two isotopes?!?

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[@vishu1334]

If the question, for example asks, "A sample of Chlorine gas the same atomic mass stated on the periodic table. There are two known stable isotopes of Chlorine: Chlorine-35 and Chlorine-37. Calculate the percent abundance of each isotopes in the sample." How would I answer this question if it doesn't tell the atomic mass of Chlorine 35 and 37?

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Very good explanation

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what if you have 3 or 4 isotopes and there are no percent abundance given. the only given value is the average mass of the isotopes how will I solve it?

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I'm completely stuck when it comes to finding the abundances of more than two isotopes. (Magnesium in this case) :( cant find any videos showing those

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[@robboyko3712]

This works very well when looking at an element that only has two isotopes. I have been trying to figure out how to use this with an element that has more than two isotopes. Do tou have a trick for this type of problem?

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Hi Tyler, what should the variable and the "in terms of x" be to calculate the isotope abundance of three or four isotopes? You make this so easy, thanks a lot!

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thank you so much for this video!! had no clue what i was doing until i watched it- great explanations :)

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