Average Atomic Mass Practice Problems
Authored by Emily Schaefer
Chemistry
9th - 12th Grade
Used 1K+ times
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About
This quiz focuses on average atomic mass calculations in chemistry, specifically targeting the concept of isotopes and their relative abundances. The content is appropriate for high school chemistry students in grades 9-12, as it requires understanding of atomic structure, isotopes, and weighted average calculations. Students need to master several core concepts to successfully solve these problems: the relationship between isotope abundance and average atomic mass, the mathematical process of calculating weighted averages using percentage abundance and atomic mass units, and the ability to interpret data about isotopic composition. The problems progress from straightforward calculations where students must apply the formula (abundance × mass) for each isotope and sum the results, to more complex analysis questions that require students to determine which isotope is most abundant based on how the average atomic mass compares to individual isotope masses. Created by Emily Schaefer, a Chemistry teacher in the US who teaches grades 9-12. This quiz serves as an excellent tool for practicing one of the fundamental quantitative concepts in atomic theory and can be effectively used as homework practice, formative assessment during instruction, or review material before summative assessments on atomic structure. The variety of question types—from direct calculations to conceptual analysis—allows teachers to gauge both computational skills and deeper understanding of the relationship between isotopic abundance and average atomic mass. Students benefit from working through multiple scenarios with different numbers of isotopes and varying abundance percentages, building confidence in their problem-solving approach. This quiz aligns with NGSS HS-PS1-1, which requires students to use the periodic table as a model to predict properties of elements, and supports Common Core mathematical practices in problem-solving and mathematical modeling within the chemistry context.
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6 questions
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1.
MULTIPLE CHOICE QUESTION
15 mins • 1 pt
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
2.
MULTIPLE CHOICE QUESTION
2 mins • 1 pt
Calcium has three different isotopes. One has a mass of 35.00 amu; another has a mass of 41.00 amu; and another has a mass of 40.00 amu. Which isotope is the most abundant of the three?
3.
MULTIPLE CHOICE QUESTION
15 mins • 1 pt
Calculate the average atomic mass of an element with the follow isotope information: 4.35% have a mass of 49.9461 amu, 83.79% have amass of 51.9405 amu, 9.50% have a mass of 52.9407 amu, and 2.36% have a mass of 53.9389 amu.
51.99 amu
52.19 amu
53.45 amu
17.33 amu
4.
MULTIPLE CHOICE QUESTION
15 mins • 1 pt
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
5.
MULTIPLE CHOICE QUESTION
15 mins • 1 pt
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
6.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
Nitrogen has three occurring isotopes: Nitrogen-13, Nitrogen-14, Nitrogen-15. Which isotope is the most abundant?
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