
Isotopes and Calculating Atomic Mass
Flashcard
•
Chemistry
•
10th Grade
•
Practice Problem
•
Hard
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1.
FLASHCARD QUESTION
Front
What is an isotope?
Back
Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons.
2.
FLASHCARD QUESTION
Front
How is atomic mass calculated?
Back
Average atomic mass is calculated by taking the sum of the products of the atomic mass of each isotope and its percent abundance.
3.
FLASHCARD QUESTION
Front
What does it mean for an atom to be electrically neutral?
Back
An atom is electrically neutral when the number of protons equals the number of electrons.
4.
FLASHCARD QUESTION
Front
What is the atomic mass of carbon-12?
Back
The atomic mass of carbon-12 is defined as exactly 12 atomic mass units (amu).
5.
FLASHCARD QUESTION
Front
What is the average atomic mass of an element with two isotopes: 10.013 amu (19.9% abundance) and 11.01 amu (80.1% abundance)?
Back
The average atomic mass is 10.812 amu.
6.
FLASHCARD QUESTION
Front
What is the difference between carbon-12 and carbon-14?
Back
Carbon-12 and carbon-14 differ in the number of neutrons; carbon-12 has 6 neutrons, while carbon-14 has 8 neutrons.
7.
FLASHCARD QUESTION
Front
What is percent abundance?
Back
Percent abundance is the relative amount of each isotope of an element in a natural sample, expressed as a percentage.
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