Calculating Average Atomic Mass
Flashcard
•
Chemistry
•
10th Grade
•
Practice Problem
•
Hard
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1.
FLASHCARD QUESTION
Front
What is average atomic mass?
Back
Average atomic mass is the weighted average of the masses of an element's isotopes, taking into account their relative abundances.
2.
FLASHCARD QUESTION
Front
How do you calculate average atomic mass from isotopic abundances?
Back
To calculate average atomic mass, multiply the mass of each isotope by its relative abundance (as a decimal), then sum these values.
3.
FLASHCARD QUESTION
Front
What is the formula for calculating average atomic mass?
Back
Average Atomic Mass = (mass1 * abundance1) + (mass2 * abundance2) + ... + (massN * abundanceN)
4.
FLASHCARD QUESTION
Front
What is the significance of atomic mass units (amu)?
Back
Atomic mass units (amu) are a standard unit of mass used to express atomic and molecular weights, where 1 amu is defined as one twelfth of the mass of a carbon-12 atom.
5.
FLASHCARD QUESTION
Front
What does it mean if an isotope is more abundant?
Back
If an isotope is more abundant, it contributes more significantly to the average atomic mass of the element.
6.
FLASHCARD QUESTION
Front
How do you convert percentage abundance to decimal form?
Back
To convert percentage abundance to decimal form, divide the percentage by 100.
7.
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.
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