Problem: Magnesium has three naturally occurring isotopes with masses of 23.99 amu, 24.99 amu, and 25.98 amu and natural abundances of 78.99 %, 10.00 %, and 11.01 %, respectively. Calculate the atomic mass of magnesium.

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FREE Expert Solution

We’re being asked to calculate the atomic mass of magnesium. We can use the following equation:


Atomic Mass = [mass×f.a.]isotope 1 + [mass×f.a.]isotope 2


where atomic mass = average atomic mass of the element and f.a. = fractional abundance of the isotope. To get f.a., we simply need to divide the given percent abundance by 100.



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Problem Details

Magnesium has three naturally occurring isotopes with masses of 23.99 amu, 24.99 amu, and 25.98 amu and natural abundances of 78.99 %, 10.00 %, and 11.01 %, respectively. Calculate the atomic mass of magnesium.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Isotopes concept. You can view video lessons to learn Isotopes. Or if you need more Isotopes practice, you can also practice Isotopes practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Azimi's class at TCC.