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What is the relative atomic mass of boron?

10.8 is the relative atomic mass of boron. Notice the effect of the "weighted" average. A simple average of 10 and 11 is, of course, 10.5. Our answer of 10.8 allows for the fact that there are a lot more of the heavier isotope of boron - and so the "weighted" average ought to be closer to that.

Why is boron in a decimal form?

or, for the more commonly occurring boron isotope (approx. 80% of all boron): The atomic mass shown on the periodic table is in a decimal form because it is the average atomic mass of boron’s isotopes and their relative abundance.

What is the percentage composition of boron?

A sample of boron was found to have the following percentage composition by mass: boron-10 (18.7%) boron-11 (81.3%). What is the value for the relative atomic mass of boron?

How do you find the relative atomic mass of an element?

Working out the relative atomic mass. The relative atomic mass of an element is the weighted average of the masses of the isotopes on a scale on which a carbon-12 atom has a mass of exactly 12 units. A "weighted average" allows for the fact that there won't be equal amounts of the various isotopes.


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