January 2018 NY Regents Chemistry Exam
33 The table below gives the atomic mass and the abundance of the two naturally occurring isotopes of boron.
![](https://static.wixstatic.com/media/d261a6_bd177d851e034c538c6ea9c8688648b5~mv2.png/v1/fill/w_49,h_23,al_c,q_85,usm_0.66_1.00_0.01,blur_2,enc_auto/d261a6_bd177d851e034c538c6ea9c8688648b5~mv2.png)
Which numerical setup can be used to determine the atomic mass of the element boron?
![](https://static.wixstatic.com/media/d261a6_ae9a26f7fd0a4e66aa0764834ff66d28~mv2.png/v1/fill/w_49,h_36,al_c,q_85,usm_0.66_1.00_0.01,blur_2,enc_auto/d261a6_ae9a26f7fd0a4e66aa0764834ff66d28~mv2.png)
Solution: To calculate the average atomic mass of an element, we take the atomic mass of each isotope and multiply by percent abundance in the decimal form ( divide by 100).
Answer: 1
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