The average atomic mass of an element that has multiple isotopes is calculated by multiplying the mass of each isotope by its relative abundance (expressed as a decimal), and then adding those values together.

In the case of bromine, we have two isotopes. Let's assume the isotopes are bromine-79 and bromine-81, which are the two stable isotopes of bromine.

1. Convert the relative abundances into decimal form:
- For bromine-79: 49.7% = 0.497
- For bromine-81: 50.3% = 0.503

2. Multiply the mass of each isotope by its relative abundance:
- For bromine-79: 79 amu * 0.497 = 39.263 amu
- For bromine-81: 81 amu * 0.503 = 40.743 amu

3. Add these values together to find the average atomic mass:
- 39.263 amu + 40.743 amu = 80.006 amu

So, the average atomic mass of bromine, given these relative abundances, is approximately 80.006 amu.

Question

The average atomic mass of an element that has multiple isotopes is calculated by multiplying the mass of each isotope by its relative abundance (expressed as a decimal), and then adding those values together.

In the case of bromine, we have two isotopes. Let's assume the isotopes are bromine-79 and bromine-81, which are the two stable isotopes of bromine.

1. Convert the relative abundances into decimal form: 
   - For bromine-79: 49.7% = 0.497
   - For bromine-81: 50.3% = 0.503

2. Multiply the mass of each isotope by its relative abundance:
   - For bromine-79: 79 amu * 0.497 = 39.263 amu
   - For bromine-81: 81 amu * 0.503 = 40.743 amu

3. Add these values together to find the average atomic mass:
   - 39.263 amu + 40.743 amu = 80.006 amu

So, the average atomic mass of bromine, given these relative abundances, is approximately 80.006 amu.

Knowee AI · Accepted Answer

The average atomic mass of an element that has multiple isotopes is calculated by multiplying the mass of each isotope by its relative abundance (expressed as a decimal), and then adding those values together.

In the case of bromine, we have two isotopes. Let's assume the isotopes are bromine-79 and bromine-81, which are the two stable isotopes of bromine.

1. Convert the relative abundances into decimal form: 
   - For bromine-79: 49.7% = 0.497
   - For bromine-81: 50.3% = 0.503

2. Multiply the mass of each isotope by its relative abundance:
   - For bromine-79: 79 amu * 0.497 = 39.263 amu
   - For bromine-81: 81 amu * 0.503 = 40.743 amu

3. Add these values together to find the average atomic mass:
   - 39.263 amu + 40.743 amu = 80.006 amu

So, the average atomic mass of bromine, given these relative abundances, is approximately 80.006 amu.

If bromine atom is available in the form of, say, two isotopesStructure of Atom(49.7%) andStructure of Atom(50.3%), calculate the average atomic mass of bromine atom.

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