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Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

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BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 3, Problem 39E
Textbook Problem
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Calculate the atomic mass of neon ( Ne ) , which is composed of three naturally occurring isotopes with the following natural abundances and masses:

a . 90 .51% Ne-20  ( mass = 19 .992 amu ) b . 0 .27% Ne-21  ( mass = 20 .993 amu ) c . 9 .22% Ne-22  ( mass = 21 .991 amu )

Interpretation Introduction

Interpretation:

The atomic mass of neon is to be calculated which is composed of three given naturally occurring isotopes.

Concept Introduction:

 The mass of an atom is defined as its atomic mass. It is a characteristic of an element which can be a whole number or fractional and its unit is amu.

 An element can have more than one form of atoms. These forms have a different number of neutrons in the nucleus while the number of protons remains the same. These are termed as isotopes.

 As these isotopes are the atoms of the same element so the actual atomic mass is dependent on the natural abundance of the isotopes of that element.

Explanation of Solution

Given information: Three natural occurring isotopes of neon with the following natural abundances and masses are as follows:

90.51% Ne20(mass=19.992 amu)  0.27% Ne21(mass=20.993 amu)  9.22% Ne22(mass=21.991 amu)

The atomic mass of an element is calculated by adding the mass of its isotopes multiplied with its natural abundance which is further divided by hundred.

The atomic mass of neon using isotopes is calculated as follows:

Atomic mass=Mass of isotope×Natural abundance(%)100

Atomic mass of Ne=(19

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Chemistry In Focus
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