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Chapter 7: Problem 89

For each of the following nonmetals, how many electrons will each atom of the nonmetal gain in reacting with a metal? a. oxygen b. fluorine c. nitrogen d. chlorine e. sulfur

Short Answer

Expert verified
a. Oxygen will gain 2 electrons. b. Fluorine will gain 1 electron. c. Nitrogen will gain 3 electrons. d. Chlorine will gain 1 electron. e. Sulfur will gain 2 electrons.

Step by step solution

01

Determine the group number for each nonmetal

Firstly, we need to find the group number of the given nonmetals in the periodic table. a. Oxygen is in Group 16. b. Fluorine is in Group 17. c. Nitrogen is in Group 15. d. Chlorine is in Group 17. e. Sulfur is in Group 16.
02

Calculate the number of electrons needed to achieve a stable electron configuration

After identifying the group number, we can now determine the number of electrons each nonmetal needs to gain to achieve a stable electron configuration. a. Oxygen (Group 16): Nonmetals in Group 16 need to gain 2 electrons to achieve a stable electron configuration, so oxygen will gain 2 electrons when reacting with a metal. b. Fluorine (Group 17): Nonmetals in Group 17 need to gain 1 electron to achieve a stable electron configuration, so fluorine will gain 1 electron when reacting with a metal. c. Nitrogen (Group 15): Nonmetals in Group 15 need to gain 3 electrons to achieve a stable electron configuration, so nitrogen will gain 3 electrons when reacting with a metal. d. Chlorine (Group 17): Nonmetals in Group 17 need to gain 1 electron to achieve a stable electron configuration, so chlorine will gain 1 electron when reacting with a metal. e. Sulfur (Group 16): Nonmetals in Group 16 need to gain 2 electrons to achieve a stable electron configuration, so sulfur will gain 2 electrons when reacting with a metal.

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Most popular questions from this chapter

What do we mean when we say that the transfer of electrons can be the "driving force" for a reaction? Give an example of a reaction where this happens.

If potassium atoms were to react with atoms of the nonmetal sulfur, how many electrons would each potassium atom lose? How many electrons would each sulfur atom gain? How many potassium atoms would have to react to provide enough electrons for one sulfur atom? What charges would the resulting potassium and sulfur ions have?

Many plants are poisonous because their stems and leaves contain oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) or sodium oxalate, \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4} ;\) when ingested, these substances cause swelling of the respiratory tract and suffocation. A standard analysis for determining the amount of oxalate ion, \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-},\) in a sample is to precipitate this species as calcium oxalate, which is insoluble in water. Write the net ionic equation for the reaction between sodium oxalate and calcium chloride, \(\mathrm{CaCl}_{2},\) in aqueous solution.

Most sulfide compounds of the transition metals are insoluble in water. Many of these metal sulfides have striking and characteristic colors by which we can identify them. Therefore, in the analysis of mixtures of metal ions, it is very common to precipitate the metal ions by using dihydrogen sulfide (commonly called hydrogen sulfide), \(\mathrm{H}_{2} \mathrm{S}\). Suppose you had a mixture of \(\mathrm{Fe}^{2+}, \mathrm{Cr}^{3+},\) and \(\mathrm{Ni}^{2+} .\) Write net ionic equations for the precipitation of these metal ions by the use of \(\mathrm{H}_{2} \mathrm{S}\).

On the basis of the general solubility rules given in Table \(7.1,\) predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply. a. sodium sulfate, \(\mathrm{Na}_{2} \mathrm{SO}_{4}\), and calcium chloride, \(\mathrm{CaCl}_{2}\) b. ammonium iodide, \(\mathrm{NH}_{4} \mathrm{I}\), and silver nitrate, \(\mathrm{AgNO}_{3}\) c. potassium phosphate, \(\mathrm{K}_{3} \mathrm{PO}_{4}\), and lead(II) nitrate, \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) d. sodium hydroxide, \(\mathrm{NaOH}\), and iron(III) chloride, \(\mathrm{FeCl}_{3}\) e. potassium sulfate, \(\mathrm{K}_{2} \mathrm{SO}_{4}\), and sodium nitrate, \(\mathrm{NaNO}_{3}\) f. sodium carbonate, \(\mathrm{Na}_{2} \mathrm{CO}_{3},\) and barium nitrate, \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\)
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