   Chapter 19, Problem 16QAP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
1 views

# . Although naturally occurring potassium consists mostly of the isotope of mass number 39(93.25%), isotopes of mass number 41(6.73%) and 40 (0.01%) also are present. Write the nuclear symbol for each of the isotopes of potassium. How many neutrons are present in each isotope? Is the average atomic mass of potassium (39.10 g) consistent with the relative abundances of the isotopes?

Interpretation Introduction

Interpretation:

To interpret the nuclear symbol of each of the isotopes of potassium and number of neutron along with average atomic mass of potassium with relative abundance of isotopes of potassium.

Concept Introduction:

The number of proton of the nuclide is equal to its atomic number and mass number is the sum of number of proton and neutron. The number of neutron is equal to the difference between the mass number to the number of proton. The elements having same atomic number and different mass number is known as isotopes.

The average atomic mass of an element is equal to the sum of the masses of its isotopes, each multiplied by its natural abundance.

Explanation

The general representation of atomic symbol is: A Z X

Where A is mass number, Z is atomic number, and X is the chemical symbol of the element.

Since, the atomic number of K is 19. So, the nuclear symbol of the K is represents as follows.

K-39, K-40 and K-41 are 39 1 9 K, 40 1 9 K and 41 1 9 K.

The subscript of is define the atomic number and super subscript denoted the atomic mass.

The number of neutron of an atom is equal to the difference between mass number and number of proton. The number of neutron is different in all the isotopes of K.

Number of neutron of K-39 = 39-19 = 20.

Number of neutron of K-40 = 40-19 = 21.

Number of neutron of K-41 = 41-19 = 22.

The average atomic mass of an element is equal to the sum of the masses of its isotopes, each multiplied by its natural abundance.

Average atomic mass of K =

Mass of K39 × Natural abundance of K39 + Mass of K

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