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

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2
Q

What is relative atomic mass?

A

The average mass of all the isotopes of an element

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3
Q

What does it have to allow?

A

For the relative atomic mass of each isotope and its relative abundance

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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

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5
Q

How can you find the relative atomic mass of any element?

A

Using the periodic table

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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

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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
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8
Q

Check example on page 17

A

Ok

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