   Chapter 2, Problem 20PS

Chapter
Section
Textbook Problem

Strontium has four stable isotopes. Strontium-84 has a very low natural abundance, but 86Sr, 87Sr, and 88Sr are all reasonably abundant. Knowing that the atomic weight of strontium is 87.62, which of the more abundant isotopes predominates?

Interpretation Introduction

Interpretation:

The most abundant isotope of Strontium has to be determined if the isotopes are 86Sr, 87Sr and 88Sr.

Concept Introduction:

The average weight (atomic weight) of Strontium is 87.62

Equation for average weight is,

average weight=(%abundanceisotop-1100)×(massofisotop-1) +(%abundanceisotop-2100)×(massofisotop-2)+etc

Explanation

There are three isotopes for Strontium atom.

The mass of isotope-1 (86Sr) is 86

The mass of isotope-2 is (87Sr) is 87.

The mass of isotope-3 is (88Sr) is 88

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