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Introductory Chemistry: A Foundati...

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

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. Naturally occurring magnesium consists primarily of three isotopes. of mass numbers 24, 25, and 26. How many protons does each of these nuclides contain? How many neutrons does each of these nuclides contain? Write nuclear symbols for each of these isotopes.

Interpretation Introduction

Interpretation:

To interpret the number of proton of the given nuclide of Mg having mass number 24, 25 and 26 respectively along with number of neutron of the given nuclide of Mg having mass number 24, 25 and 26 respectively and write the symbol of each of the nuclides of Mg.

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 are known as isotopes.

Explanation

The number of proton in the isotopes of Mg is same for all isotopes because the number of proton is equal to the atomic number and for the isotopes means same atomic number so, number of proton is same. Atomic number is 12 so, number of proton is 12.

The number of neutron of all the isotopes is as:

Number of neutron = Mass number − Number of proton

Mg-24.

Number of neutron = 24-12 = 12.

Mg-25...

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