Relative Atomic Mass Takes All Stable Isotopes into Account Flashcards
1
Q
What is relative atomic mass (A) just a way of saying?
A
How heavy different atoms are compared with the mass of an atom of carbon-14
2
Q
What is relative atomic mass?
A
The average mass of all the isotopes of an element
3
Q
What does it have to allow?
A
For the relative atomic mass of each isotope and its relative abundance
4
Q
What does relative abundance mean?
A
How much there is of each isotope compared to the total amount of the element in the world - ratio, fraction or percentage
5
Q
How can you find the relative atomic mass of any element?
A
Using the periodic table
6
Q
How do relative atomic masses usually come out?
A
Not usually as whole numbers of easy decimals, but often rounded to nearest 0.5
7
Q
How do you use relative atomic mass?
Step by step -
A
- Multiply mass of each isotope by its relative abundance
- add them together
- divide by sum of relative abundances
8
Q
Check example on page 17
A
Ok
