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Chapter 2: Problem 58

What is the symbol of an ion with 16 protons, 18 neutrons, and 18 electrons? What is the symbol for an ion that has 16 protons, 16 neutrons, and 18 electrons?

Short Answer

Expert verified
The symbols for the two ions are \(\ce{^{34}_{16}S^{2-}}\) and \(\ce{^{32}_{16}S}\).

Step by step solution

01

Determine the element from the number of protons

The number of protons defines the element. In both cases, we have 16 protons, which corresponds to the element sulfur (S). The symbol for sulfur is \(S\).
02

Calculate the charge of the ion

The charge of an ion is the difference between the number of protons and electrons. 1. For the ion with 16 protons and 18 electrons: Charge = Number of protons - Number of electrons = 16 - 18 = -2 2. For the ion with 16 protons and 16 electrons: Charge = Number of protons - Number of electrons = 16 - 16 = 0
03

Determine the mass number

The mass number of an atom is the sum of its protons and neutrons. 1. For the ion with 16 protons and 18 neutrons: Mass number = Number of protons + Number of neutrons = 16 + 18 = 34 2. For the ion with 16 protons and 16 neutrons: Mass number = Number of protons + Number of neutrons = 16 + 16 = 32
04

Write the symbol for each ion

1. For the ion with 16 protons, 18 neutrons, and 18 electrons: The symbol is \(\ce{^{34}_{16}S^{2-}}\) 2. For the ion with 16 protons, 16 neutrons, and 18 electrons: Since the ion has no charge, it is not an ion but a neutral atom. The symbol is \(\ce{^{32}_{16}S}\)

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Most popular questions from this chapter

Would you expect each of the following atoms to gain or lose electrons when forming ions? What ion is the most likely in each case? a. \(\mathrm{Ra}\) c. \(\underline{P}\) e. \(\mathrm{Br}\) b. In d. Te f. \(\mathrm{Rb}\)

In an experiment it was found that the total charge on an oil drop was \(5.93 \times 10^{-18} \mathrm{C}\). How many negative charges does the drop contain?

You take three compounds, each consisting of two elements \((\mathrm{X}, \mathrm{Y}\), and \(/ \mathrm{or} \mathrm{Z})\), and decompose them to their respective elements. To determine the relative masses of \(\mathrm{X}, \mathrm{Y}\), and \(\mathrm{Z}\), you collect and weigh the elements, obtaining the following data: $$ \begin{array}{|ll|} \hline \text { Elements in Compound } & \text { Masses of Elements } \\ \hline \text { 1. } \mathrm{X} \text { and } \mathrm{Y} & \mathrm{X}=0.4 \mathrm{~g}, \mathrm{Y}=4.2 \mathrm{~g} \\ \text { 2. Y and } \mathrm{Z} & \mathrm{Y}=1.4 \mathrm{~g}, \mathrm{Z}=1.0 \mathrm{~g} \\ \text { 3. } \mathrm{X} \text { and } \mathrm{Y} & \mathrm{X}=2.0 \mathrm{~g}, \mathrm{Y}=7.0 \mathrm{~g} \\ \hline \end{array} $$ a. What are the assumptions needed to solve this problem? b. What are the relative masses of \(\mathrm{X}, \mathrm{Y}\), and \(\mathrm{Z} ?\) c. What are the chemical formulas of the three compounds? d. If you decompose \(21 \mathrm{~g}\) of compound \(\mathrm{XY}\), how much of each element is present?

What is the modern view of the structure of the atom?

A sample of chloroform is found to contain \(12.0 \mathrm{~g}\) of carbon, \(106.4 \mathrm{~g}\) of chlorine, and \(1.01 \mathrm{~g}\) of hydrogen. If a second sample of chloroform is found to contain \(30.0 \mathrm{~g}\) of carbon, what is the total mass of chloroform in the second sample?
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