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Chapter 2: Problem 58

How do \({ }_{35}^{79} \mathrm{Br}^{-}\)and \({ }_{35}^{81} \mathrm{Br}\) differ in their numbers of subatomic particles? Which should have the greater mass?

Short Answer

Expert verified
\({ }_{35}^{79} \mathrm{Br}^{-}\) has 35 protons, 44 neutrons, and 36 electrons, while \({ }_{35}^{81} \mathrm{Br}\) has 35 protons, 46 neutrons, and 35 electrons. \({ }_{35}^{81} \mathrm{Br}\) has the greater mass because it has more neutrons.

Step by step solution

01

Interpret Isotope Notation

Using the isotopic notation \(_{Z}^{A}\mathrm{X}\^{Q}, where \(Z\) is the atomic number, indicating the number of protons and \(A\) is the atomic mass number, standing for the total of protons and neutrons, and \(Q\) the charge of the species, indicative of the number of electrons. For the isotopes given in the exercise, \({ }_{35}^{79} \mathrm{Br}^{-}\) and \({ }_{35}^{81} \mathrm{Br}\), \(Z=35\), so each isotope has 35 protons. \(A\) varies, with 79 and 81 for the respective isotopes, and the charges of the isotopes are -1 and 0 respectively, thus electrons vary from 36 to 35.
02

Calculate Number of Neutrons

The number of neutrons in an isotope is given by the equation \[Number of neutrons = A - Z\], For \({ }_{35}^{79} \mathrm{Br}^{-}\), there are \(79 - 35 = 44\) neutrons, and for \({ }_{35}^{81} \mathrm{Br}\), there are \(81 - 35 = 46\) neutrons.
03

Determine Greater Mass

The atomic mass is primarily determined by the combined number of protons and neutrons. Since \({ }_{35}^{81} \mathrm{Br}\) has more neutrons than \({ }_{35}^{79} \mathrm{Br}^{-}\), it should also have a greater mass.

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