QQuestionChemistry
QuestionChemistry
Naturally occurring Bromine has a relative atomic mass of 80 and consists entirely of two isotopes of relative atomic masses 79 and 81. What can be deduced about naturally occurring Bromine from this information only?
A) Bromine contains the two isotopes in equal proportions
B) Bromine has different oxidation states
C) Bromine isotopes have different numbers of protons
D) Bromine is radioactive
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Answer
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Step 1:Let's solve this step by step:
Step 2:: Understand the given information
- Bromine's relative atomic mass is 80 - Bromine consists of two isotopes - These isotopes have relative atomic masses of 79 and 81
Step 3:: Calculate the proportions of isotopes
79x + 81(1-x) = 80
Let x be the fraction of the 79 isotope and (1 -x) be the fraction of the 81 isotope. The weighted average of the isotope masses must equal the overall atomic mass:
Step 4:: Solve the equation
x = \frac{1}{2}
79x - 81x = 80 - 81
Step 5:: Interpret the result
This means the two isotopes are present in equal proportions (50% each).
Step 6:: Analyze the options
A) Bromine contains the two isotopes in equal proportions ✓ (This matches our calculation) B) Oxidation states are unrelated to isotope composition C) Isotopes have the same number of protons (by definition) D) Not all isotopes are radioactive
Final Answer
Key Insight: The equal proportions of isotopes explain why the weighted average of their masses (79 and 81) precisely equals the observed atomic mass of 80.
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