Introductory Chemistry: An Active Learning Approach
Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN: 9781305079250
Author: Mark S. Cracolice, Ed Peters
Publisher: Cengage Learning
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Chapter 5, Problem 40E
Interpretation Introduction

(a)

Interpretation:

The atomic mass of each element is to be calculated from the percentage abundances and atomic masses (u) of the natural isotopes of an element.

Concept introduction:

Elements which have same atomic number but different atomic mass are known as isotopes. The atomic mass of an element is defined as the total mass of one atom of an element. Its unit is atomic mass unit (a.m.u) and is denoted by the symbol u.

Expert Solution
Check Mark

Answer to Problem 40E

The atomic mass of the element is 58.73u.

Explanation of Solution

The percentage abundances and atomic masses (u) of the natural isotopes of an element are given as shown below.

67.88%57.935326.23%59.93321.19%60.93103.66%61.9283

1.08%63.9280

The contribution of the isotope to the atomic mass of element is calculated by the formula as shown below.

Atomicmassofisotope=(Massoftheisotope×Relativeabundanceoftheisotope)…(1)

Substitute the values of percentage abundance and atomic mass of the first isotope in equation (1).

Atomicmassofisotope=57.9353u×67.88%=(57.9353u×67.88100)u=39.32u

Substitute the values of percentage abundance and atomic mass of the second isotope in equation (1).

Atomicmassofisotope=135.907u×26.23%=(59.9332×26.23100)u=15.72u

Substitute the values of percentage abundance and atomic mass of the third isotope in equation (1).

Atomicmassofisotope=60.9310u×1.19%=(60.9310×1.19100)u=0.725u

Substitute the values of percentage abundance and atomic mass of the fourth isotope in equation (1).

Atomicmassofisotope=61.9283u×3.66%=(61.9283×3.66100)u=2.27u

Substitute the values of percentage abundance and atomic mass of the fifth isotope in equation (1).

Atomicmassofisotope=63.9280u×1.08%=(63.9280×1.08100)u=0.690u

The atomic mass of the element is equal to the sum of atomic masses of its five isotopes.

Therefore, the atomic mass of the element is calculated as shown below.

Atomicmass=39.32u+15.72u+0.725u+2.27u+0.690u=58.73u

Therefore, the atomic mass of the element is 58.73u.

Conclusion

The atomic mass of the element is 58.73u.

Interpretation Introduction

(b)

Interpretation:

The name of the element is to be identified.

Concept introduction:

Elements which have same atomic number but different atomic mass are known as isotopes. The atomic mass of an element is defined as the total mass of one atom of an element. Its unit is atomic mass unit (a.m.u) and is denoted by the symbol u.

Expert Solution
Check Mark

Answer to Problem 40E

The name of the element is cerium (Ni).

Explanation of Solution

The calculated atomic mass of the element is 58.73u.

In the periodic table, the element having atomic mass 58.73u is nickel.

Therefore, the name of the element is nickel (Ni).

Conclusion

The element having 58.73u atomic mass is nickel (Ni).

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Chapter 5 Solutions

Introductory Chemistry: An Active Learning Approach

Ch. 5 - Prob. 11ECh. 5 - What is meant by stating that the charge of an...Ch. 5 - How can we account for the fact that, in the...Ch. 5 - How can we account for the fact that most of the...Ch. 5 - What do we call the central part of an atom?Ch. 5 - What major conclusions were drawn from the...Ch. 5 - Describe the activity of electrons according to...Ch. 5 - The Rutherford experiment was performed and its...Ch. 5 - Compare the three major parts of an atom in charge...Ch. 5 - Prob. 20ECh. 5 - Can two different elements have the same atomic...Ch. 5 - Compare the number of protons and electrons in an...Ch. 5 - Explain why isotopes of different elements can...Ch. 5 - How many protons, neutrons and electrons are there...Ch. 5 - Prob. 25ECh. 5 - What advantage does the atomic mass unit have over...Ch. 5 - What is an atomic mass unit?Ch. 5 - The mass of an average atom of a certain element...Ch. 5 - The average mass of boron atoms is 10.81u. How...Ch. 5 - The atomic masses of the natural isotopes of neon...Ch. 5 - A certain element consists of two stable isotopes....Ch. 5 - The mass of 60.4 of the atoms of an element is...Ch. 5 - Isotopic data for boron allow the calculation of...Ch. 5 - Questions 31 through 36: Percentage abundances and...Ch. 5 - Questions 31 through 36: Percentage abundances and...Ch. 5 - Questions 31 through 36: Percentage abundances and...Ch. 5 - Questions 31 through 36: Percentage abundances and...Ch. 5 - Questions 31 through 36: Percentage abundances and...Ch. 5 - Prob. 40ECh. 5 - How many elements are in Period 5 of the periodic...Ch. 5 - Write the symbol of the element in each given...Ch. 5 - Prob. 43ECh. 5 - List the symbols of the elements of each of the...Ch. 5 - Using only a periodic table for reference, list...Ch. 5 - Prob. 46ECh. 5 - Write the atomic masses of helium and aluminum.Ch. 5 - Prob. 48ECh. 5 - Prob. 49ECh. 5 - Prob. 50ECh. 5 - Prob. 51ECh. 5 - Determine whether each statement that follows is...Ch. 5 - Prob. 53ECh. 5 - Sodium oxide and sodium peroxide are two compounds...Ch. 5 - Prob. 55ECh. 5 - The CRC Handbook, a large reference book of...Ch. 5 - The element lanthanum has two stable isotopes,...Ch. 5 - The atomic mass of lithium on a periodic table is...Ch. 5 - Prob. 59ECh. 5 - Prob. 60ECh. 5 - Prob. 61ECh. 5 - Prob. 62ECh. 5 - Prob. 5.1TCCh. 5 - Prob. 5.2TCCh. 5 - Prob. 5.3TCCh. 5 - Prob. 5.4TCCh. 5 - Prob. 5.5TCCh. 5 - Write a brief description of the relationships...Ch. 5 - Prob. 2CLECh. 5 - Prob. 3CLECh. 5 - Prob. 4CLECh. 5 - Prob. 5CLECh. 5 - Prob. 6CLECh. 5 - Prob. 7CLECh. 5 - What is the number of each type of subatomic...Ch. 5 - Naturally occurring lithium is composed of two...Ch. 5 - Prob. 3PECh. 5 - Prob. 4PECh. 5 - Prob. 5PE
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