Question detail
Explain why the relative atomic mass of an element is often not a whole number, using isotopes as part of your answer.
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
Type
exam_style
Style
Topic
A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes
Question
Explain why the relative atomic mass of an element is often not a whole number, using isotopes as part of your answer.
Answer
The relative atomic mass of an element is often not a whole number because it is a weighted average of the masses of its isotopes, taking into account their relative abundances. Since isotopes of an element can have different masses and are present in varying amounts, the average will typically result in a non-integer value.
Explanation
This question assesses the student's understanding of the concept of relative atomic mass and the role of isotopes. It requires them to explain the relationship between isotopes and the calculation of relative atomic mass, demonstrating comprehension of the topic.
Common mistake
Misunderstanding Isotope Contributions
Students often think that the relative atomic mass is simply the average of the isotopes' mass numbers without considering their percentage abundances.
To fix this, students should remember to multiply each isotope's mass number by its percentage abundance, sum these values, and then divide by the total percentage (100) to find the relative atomic mass. Keep the correction anchored to Relative atomic mass and avoid mixing it with nearby Unit 4.1 ideas.
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