Question
For the following pairs of ions, use the concept that a chemical compound must have a net charge of zero to predict the simplest compound that the ions are most likely to form.a. $\mathrm{Co}^{2+}$ and $\mathrm{O}^{2-}$b. $C o^{3+}$ and $S^{2-}$c. $A l^{3+}$ and $C l^{-}$d. $\mathrm{Ba}^{2+}$ and $\mathrm{N}^{3-}$e. $C a^{2+}$ and $C^{4-}$f. $K^{+}$ and $N^{3-}$
Step 1
The charge on an ion is the number of electrons it has gained or lost. A positive charge means the ion has lost electrons, while a negative charge means it has gained electrons. Show more…
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Use the concept that a chemical compound must have a net charge of zero to predict the formula of the simplest compound that the following pairs of ions are most likely to form. a. $\mathrm{Fe}^{3+}$ and $\mathrm{P}^{3-}$ b. $\mathrm{Fe}^{3+}$ and $\mathrm{S}^{2-}$ c. $\mathrm{Fe}^{3+}$ and $\mathrm{Cl}^{-}$ d. $\mathrm{Mg}^{2+}$ and $\mathrm{Cl}^{-}$ e. $\mathrm{Mg}^{2}+$ and $\mathrm{O}^{2-}$ $\mathrm{f} . \mathrm{Mg}^{2+}$ and $\mathrm{N}^{3-}$ g. $\mathrm{Na}^{+}$ and $\mathrm{P}^{3-}$ h. $\mathrm{Na}^{+}$ and $\mathrm{S}^{2-}$
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For each of the following positive ions, use the concept that a chemical compound must have a net charge of zero to predict the formula of the simple compounds that the positive ions would form with the $\mathrm{Cl}^{-}, \mathrm{S}^{2-},$ and $\mathrm{N}^{3-}$ ions. a. $\mathrm{K}^{+}$ b. $\mathrm{Mg}^{2+}$ c. $\mathrm{Al}^{3+}$ d. $\mathrm{Ca}^{2+}$ e. $\mathrm{Li}^{+}$
For each of the following positive ions, use the concept that a chemical compound must have a net charge of zero to predict the formula of the simple compounds that the positive ions would form with the $\mathrm{Cl}^{-}, \mathrm{S}^{2-},$ and $\mathrm{N}^{3-}$ ions. $\begin{array}{ll}{\text { a. } \mathrm{K}^{+}} & {\text { C. } \mathrm{Al}^{3+}} & {\text { e. } \mathrm{Li}^{+}} \\ {\text { b. } \mathrm{Mg}^{2+}} & {\text { d. } \mathrm{Ca}^{2+}}\end{array}$
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