Question
Asked Feb 16, 2020
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Almost all boron atoms are found in two forms: boron-10 and boron-11. Both isotopes behave alike chemically and are useful in fireworks (green color), in the antiseptic boric acid, and in heat-resistant glass. If the average atomic mass of boron is 10.81 amu, which boron isotope must be more abundant in nature? How do you know? 

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Expert Answer

Step 1

Given,

Boron atoms are found in two forms: boron-10 and boron-11

Average mass of B = 10.81 amu

 

 

Step 2

Since, the value 10.81 amu is a lot closer to 11 amu than it is to 10 amu, so there must be more of boron-11 than boron-10.

 

To confirm this, we can also do a simple calculation to find the natural abundance of boron-11 and boron-10.

Let us assume :

Atomic mass of 10B (isotope I) = 10 amu

Atomic mass of 11B (isotope II) = 11 amu

Natural abundance of 10B (isotope I) = A

Natural abundance of 11B (isotope II) = (1 – A)

 

The average mass of B is expressed as:

Chemistry homework question answer, step 2, image 1

Since natural abundance is expressed as percentage, ther...

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