Chapter 9: Problem 16

Give the empirical formulas and names of the compounds formed from the following pairs of ions: (a) \(\mathrm{Rb}^{+}\) and \(\mathrm{I}^{-},\) (b) \(\mathrm{Cs}^{+}\) and \(\mathrm{SO}_{4}^{2-},\) (c) \(\mathrm{Sr}^{2+}\) and \(\mathrm{N}^{3-}\) (d) \(\mathrm{Al}^{3+}\) and \(\mathrm{S}^{2-}\)

Short Answer

Expert verified

The empirical formulas and names of the compounds are: (a) \(RbI\): Rubidium iodide, (b) \(Cs_2SO_4\): Cesium sulfate, (c) \(Sr_3N_2\): Strontium nitride, (d) \(Al_2S_3\): Aluminum sulfide.

Step by step solution

Balancing Charges and Writing the Formula for Rb+ and I-

Here we have Rb+ which has a charge of +1, and I- which has a charge of -1. This means we can combine one Rb atom with one I atom to neutralise the charges. Therefore, the empirical formula for this compound is \(RbI\).

Naming the Compound RbI

The name of the compound is derived from the names of the ions. The cation is rubidium (Rb), the anion is iodide(I). Iodine becomes iodide when it gains an electron and becomes an ion. As a result, the name of the compound is Rubidium iodide.

Balancing Charges and Writing the Formula for Cs+ and \(SO_{4}^{2-}\)

Here we have Cs+ which has a charge of +1, and \(SO_{4}^{2-}\) which has a charge of -2. To balance these charges, we need two Cs+ for every \(SO_{4}^{2-}\). Therefore, the empirical formula for this compound is \(Cs_2SO_4\).

Naming the Compound \(Cs_2SO_4\)

The name of the compound is derived from the names of the ions. The cation is cesium (Cs), the anion is sulfate(\(SO_{4}^{2-}\)). That follows, the name of the compound is Cesium sulfate.

Balancing Charges and Writing the Formula for Sr2+ and N3-

Here we have Sr2+ with a charge of +2, and N3- with a charge of -3. To balance these charges, three Sr2+ ions are needed for every two N3- ions. So the empirical formula for this compound is \(Sr_3N_2\).

Naming the Compound \(Sr_3N_2\)

The name of the compound is derived from the names of the ions. The cation is strontium (Sr), the anion is nitride(N). Nitrogen becomes nitride when it gains three electrons and becomes an ion. So the name of the compound is Strontium nitride.

Balancing Charges and Writing the Formula for Al3+ and S2-

Here we have Al3+ with a charge of +3, and S2- with a charge of -2. To balance these charges, two Al3+ ions are needed for every three S2- ions. So the empirical formula for this compound is \(Al_2S_3\).

Naming the Compound \(Al_2S_3\)

The name of the compound is derived from the names of the ions. The cation is aluminum (Al), the anion is sulfide(S). Sulfur becomes sulfide when it gains two electrons and becomes an ion. So the name of the compound is Aluminum sulfide.

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Give the empirical formulas and names of the compounds formed from the following pairs of ions: (a) \(\mathrm{Rb}^{+}\) and \(\mathrm{I}^{-},\) (b) \(\mathrm{Cs}^{+}\) and \(\mathrm{SO}_{4}^{2-},\) (c) \(\mathrm{Sr}^{2+}\) and \(\mathrm{N}^{3-}\) (d) \(\mathrm{Al}^{3+}\) and \(\mathrm{S}^{2-}\)

Short Answer

Step by step solution

Balancing Charges and Writing the Formula for Rb+ and I-

Naming the Compound RbI

Balancing Charges and Writing the Formula for Cs+ and \(SO_{4}^{2-}\)

Naming the Compound \(Cs_2SO_4\)

Balancing Charges and Writing the Formula for Sr2+ and N3-

Naming the Compound \(Sr_3N_2\)

Balancing Charges and Writing the Formula for Al3+ and S2-

Naming the Compound \(Al_2S_3\)

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