   Chapter 2.8, Problem 1.2ACP

Chapter
Section
Textbook Problem

There are three stable isotopes of oxygen (16O, mass 15.9949 u, 99.763%, l7O, mass 16.9991 u, 0.0375%, and 18O, 17.9991 u, 0.1995%). Use these data to calculate the atomic weight of oxygen.

Interpretation Introduction

Interpretation: The atomic weight of oxygen should be determined using the given conditions that the isotopes 16O has a mass of 15.9949u in an abundance 99.763%, 17O has a mass of 16.9991u in an abundance 0.0375% and 18O has a mass of 17.9991u in an abundance of 0.1995%.

Concept introduction:

Equation for average weight is,

average weight=(%abundanceisotope-1100)×(massofisotope-1) +(%abundanceisotope-2100)×(massofisotope-2)+etc

Two species are said to be isotopes if both have same atomic number but different mass number.

Explanation

There are three isotopes for oxygen atom.

The mass of isotope-1 (16O) is 15.9949u and its abundance is 99.763%.

The mass of isotope-2 (17O) is 16.9991u and its abundance is 0.0375%.

The mass of isotope-3 (18O) is 17.9991u and its abundance is 0.1995%.

Equation for average weight is,

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

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