   # Calculating Atomic Mass Magnesium has three naturally occurring isotopes with masses 23 .99,24 .99, and 25 .98 amu and natural abundances 78 .99, 10 .00, and 11 .01% . Calculate the atomic mass of magnesium. ### Chemistry In Focus

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

#### Solutions

Chapter
Section ### Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 3, Problem 3.4YT
Textbook Problem
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## Calculating Atomic MassMagnesium has three naturally occurring isotopes with masses 23 .99,24 .99, and 25 .98 amu and natural abundances 78 .99, 10 .00, and 11 .01% . Calculate the atomic mass of magnesium.

Interpretation Introduction

Interpretation:

The atomic mass of magnesium is to be calculated.

Concept Introduction:

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

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

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

### Explanation of Solution

Given information: Magnesium has three naturally occurring isotopes with masses 23.99, 24.99, 25.98 amu, respectively, and natural abundances 78.99, 10.00 and 11.01%, respectively.

The atomic mass of an element is calculated by adding the mass of isotopes and multiplying the sum by their natural abundance. The product is further divided by hundred. The atomic mass of magnesium, calculated using isotopes, is as follows:

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

Atomic mass of Mg=(23.99 amu×78.99)+(24

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