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Chapter 2: Problem 27

How many protons, neutrons, and electrons are in the following atoms? (a) \(^{40} \mathrm{Ar},(\mathbf{b})^{65} \mathrm{Zn},(\mathbf{c})^{70} \mathrm{Ga},(\mathbf{d})^{80} \mathrm{Br},(\mathbf{e})^{184} \mathrm{W}\) \((\mathbf{f})^{243} \mathrm{Am} .\)

Short Answer

Expert verified
(a) \(^{40}Ar\): 18 protons, 22 neutrons, 18 electrons; (b) \(^{65}Zn\): 30 protons, 35 neutrons, 30 electrons; (c) \(^{70}Ga\): 31 protons, 39 neutrons, 31 electrons; (d) \(^{80}Br\): 35 protons, 45 neutrons, 35 electrons; (e) \(^{184}W\): 74 protons, 110 neutrons, 74 electrons; (f) \(^{243}Am\): 95 protons, 148 neutrons, 95 electrons.

Step by step solution

01

Identifying Atomic Numbers and Mass Numbers

The given isotopes are expressed by the element symbols and mass numbers. \(^{A}X\), where A is the mass number and X is the element symbol. We can find the atomic number, Z, by looking at the periodic table.
02

(a) \(^{40}Ar\)

For Argon (Ar), the atomic number is Z = 18. We are given the mass number A = 40. Use the following relationships to determine the number of protons, neutrons, and electrons. Protons: Z = 18 Neutrons: A - Z = 40 - 18 = 22 Electrons: Z = 18 (neutral atom)
03

(b) \(^{65}Zn\)

For Zinc (Zn), the atomic number is Z = 30. We are given the mass number A = 65. Apply the same relationships as in (a) to determine the number of protons, neutrons, and electrons. Protons: Z = 30 Neutrons: A - Z = 65 - 30 = 35 Electrons: Z = 30 (neutral atom)
04

(c) \(^{70}Ga\)

For Gallium (Ga), the atomic number is Z = 31. We are given the mass number A = 70. Apply the same relationships as in (a) and (b) to find the number of protons, neutrons, and electrons. Protons: Z = 31 Neutrons: A - Z = 70 - 31 = 39 Electrons: Z = 31 (neutral atom)
05

(d) \(^{80}Br\)

For Bromine (Br), the atomic number is Z = 35. We are given the mass number A = 80. Apply the relationships again to find the number of protons, neutrons, and electrons. Protons: Z = 35 Neutrons: A - Z = 80 - 35 = 45 Electrons: Z = 35 (neutral atom)
06

(e) \(^{184}W\)

For Tungsten (W), the atomic number is Z = 74. We are given the mass number A = 184. Apply the relationships again to find the number of protons, neutrons, and electrons. Protons: Z = 74 Neutrons: A - Z = 184 - 74 = 110 Electrons: Z = 74 (neutral atom)
07

(f) \(^{243}Am\)

For Americium (Am), the atomic number is Z = 95. We are given the mass number A = 243. Apply the relationships again to find the number of protons, neutrons, and electrons. Protons: Z = 95 Neutrons: A - Z = 243 - 95 = 148 Electrons: Z = 95 (neutral atom)

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Most popular questions from this chapter

The diameter of a rubidium atom is 4.95 A. We will consider two different ways of placing the atoms on a surface. In arrangement \(A,\) all the atoms are lined up with one another to form a square grid. Arrangement B is called a close-packed arrangement because the atoms sit in the "depressions" formed by the previous row of atoms:(a) Using arrangement A, how many Rb atoms could be placed on a square surface that is 1.0 \(\mathrm{cm}\) on a side? ( b) How many Rb atoms could be placed on a square surface that is 1.0 \(\mathrm{cm}\) on a side, using arrangement \(\mathrm{B} ?(\mathbf{c})\) By what factor has the number of atoms on the surface increased in going to arrangement \(\mathrm{B}\) from arrangement A? If extended to three dimensions, which arrangement would lead to a greater density for Rb metal?

(a) What is a hydrocarbon? (b) Pentane is the alkane with a chain of five carbon atoms. Write a structural formula for this compound and determine its molecular and empirical formulas.

The oxides of nitrogen are very important components in urban air pollution. Name each of the following compounds: (a) \(\mathrm{N}_{2} \mathrm{O},(\mathbf{b}) \mathrm{NO},(\mathbf{c}) \mathrm{NO}_{2},(\mathbf{d}) \mathrm{N}_{2} \mathrm{O}_{5},(\mathbf{e}) \mathrm{N}_{2} \mathrm{O}_{4}\)

Predict whether each of the following compounds is molecular or ionic: (a) \(\mathrm{B}_{2} \mathrm{H}_{6},(\mathbf{b}) \mathrm{CH}_{3} \mathrm{OH},(\mathbf{c}) \mathrm{LiNO}_{3},(\mathbf{d}) \mathrm{Sc}_{2} \mathrm{O}_{3}\) (e) \(\mathrm{CsBr},(\mathbf{f}) \mathrm{NOCl},(\mathbf{g}) \mathrm{NF}_{3},(\mathbf{h}) \mathrm{Ag}_{2} \mathrm{SO}_{4}\)

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound:(a) Calculate the mass of fluorine per gram of iodine in each compound. (b) How do the numbers in part (a) support the atomic theory?
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