High School

Magnesium has 3 naturally occurring isotopes:

- Magnesium-24 has a mass of 23.985 amu and an abundance of 78.99%.
- Magnesium-25 has a mass of 24.986 amu and an abundance of 10.00%.
- Magnesium-26 has a mass of 25.982 amu and an abundance of 11.01%.

What is the average atomic mass of magnesium?

Answer :

Final answer:

The average atomic mass of magnesium is calculated by taking a weighted average of the masses and abundances of its three isotopes (Magnesium-24, Magnesium-25, and Magnesium-26). The calculation results in an approximate atomic mass of 24.305 amu.

Explanation:

The average atomic mass of magnesium can be calculated by taking into account the different masses and abundances of its naturally occurring isotopes. Specifically, these three isotopes are Magnesium-24, Magnesium-25, and Magnesium-26. The weighted average of these isotopes can be calculated using the formula: (mass1 * abundance1) + (mass2 * abundance2) + (mass3 * abundance3). Abundance should be expressed as a decimal value in this formula.

So, for magnesium, it would be: (23.985 amu * 0.7899) + (24.986 amu * 0.1000) + (25.982 amu * 0.1101). Doing this calculation gives us an average atomic mass of approximately 24.305 amu for magnesium.

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