erage Atomic Mass Calculations Format Tools Add-ons Help Last edit was 8 minutes ago 三 Element: Magnesium Number of Protons Name of isotope Number of Abundance Abundance Mass (amu) Neutrons (%) (decimal) Magnesium-24 23.985 78.99% Magnesium-25 24.986 10.00% Magnesium-26 25.983 11.01% Isotope Mass Abundance
erage Atomic Mass Calculations Format Tools Add-ons Help Last edit was 8 minutes ago 三 Element: Magnesium Number of Protons Name of isotope Number of Abundance Abundance Mass (amu) Neutrons (%) (decimal) Magnesium-24 23.985 78.99% Magnesium-25 24.986 10.00% Magnesium-26 25.983 11.01% Isotope Mass Abundance
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:**Element: Magnesium**
| Name of isotope | Number of Protons | Number of Neutrons | Mass (amu) | Abundance (%) | Abundance (decimal) |
|-----------------|-------------------|--------------------|------------|---------------|---------------------|
| Magnesium-24 | | | 23.985 | 78.99% | |
| Magnesium-25 | | | 24.986 | 10.00% | |
| Magnesium-26 | | | 25.983 | 11.01% | |
**Isotope — Mass Abundance Table**
*No data provided.*
**Explanation:**
In this table, isotopes of Magnesium are listed with their respective atomic mass (in atomic mass units, amu) and their natural abundance percentages. The isotopes shown are Magnesium-24, Magnesium-25, and Magnesium-26. The table appears to be part of a section on average atomic mass calculations where the abundance as a decimal might be used, although those values are not filled in here.
Expert Solution
Step 1
Average atomic mass:
The average atomic mass of an element is the sum of the masses of its isotopes, each multiplied by its natural abundance. The average atomic mass of an element can be calculated as follows:
- Change each percent abundance of the isotope into decimal form by dividing by 100.
- Multiply this value by the atomic mass of that isotope.
- And finally, add together for each isotope to get the average atomic mass.
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