Isotopes in Chemistry
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Objective
I can calculate the average atomic mass of an element using the relative abundances of its isotopes.
Part 1 of 3
Warm-up video
Unknown Channel · 5:00
We don't generate video — this one is by Unknown Channel on YouTube. The practice questions and exit ticket below were drafted by AI for this objective, and every question is editable in the teacher guide.
Part 2 of 3
Practice
9 questions
Define isotopes and explain how they differ from one another.
Given that carbon has two isotopes, carbon-12 and carbon-14, explain how the number of neutrons affects the mass of an isotope.
Part 3 of 3
Exit ticket
Quick comprehension check
“A sample of magnesium contains two stable isotopes: magnesium-24 (abundance 78.99%) and magnesium-26 (abundance 21.01%). Calculate the average atomic mass of magnesium to one decimal place. Show all work. An element has three isotopes: isotope P with a mass of 30 amu and an abundance of 50%, isotope Q with a mass of 31 amu and an abundance of 30%, and isotope R with a mass of 32 amu and an abundance of 20%. Calculate the average atomic mass of this element to one decimal place. Show all work.”
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