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Chapter 5: Problem 141

Many acids can be thought of as anions that have an \(\mathrm{H}^{+}\) ion attached to them. Fill in the following table: \begin{tabular}{|l|l|l|l|} \hline Anion & Anion name & Acid formula & Acid name \\ \hline \(\mathrm{F}^{-}\) & & & \\ \hline \(\mathrm{NO}_{3}^{-}\) & & & \\ \hline \(\mathrm{Cl}^{-}\) & & & \\ \hline \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\) & & & \\ \hline \(\mathrm{NO}_{2}^{-}\) & & & \\ \hline \end{tabular}

Short Answer

Expert verified
Here is the completed table with the anion names, acid formulas, and acid names: \begin{tabular}{|l|l|l|l|} \hline Anion & Anion name & Acid formula & Acid name \\ \hline $\mathrm{F}^{-}$ & Fluoride & HF & Hydrofluoric Acid \\ \hline $\mathrm{NO}_{3}^{-}$ & Nitrate & HNO3 & Nitric Acid \\ \hline $\mathrm{Cl}^{-}$ & Chloride & HCl & Hydrochloric Acid \\ \hline $\mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}$ & Acetate & HC2H3O2 & Acetic Acid \\ \hline $\mathrm{NO}_{2}^{-}$ & Nitrite & HNO2 & Nitrous Acid \\ \hline \end{tabular}

Step by step solution

01

Identify the anion names

First, we will determine the names of the given anions: 1. F- : Fluoride 2. NO3- : Nitrate 3. Cl- : Chloride 4. C2H3O2- : Acetate 5. NO2- : Nitrite
02

Determine the acid formulas

To obtain the acid formula, we will add an H+ ion to each anion. The formulas for the acids are: 1. HF (F- + H+) 2. HNO3 (NO3- + H+) 3. HCl (Cl- + H+) 4. HC2H3O2 (C2H3O2- + H+) 5. HNO2 (NO2- + H+)
03

Identify the acid names

Now, we will name each of the acids based on their formulas: 1. HF: Hydrofluoric Acid 2. HNO3: Nitric Acid 3. HCl: Hydrochloric Acid 4. HC2H3O2: Acetic Acid 5. HNO2: Nitrous Acid With this information, we can now fill in the table: \begin{tabular}{|l|l|l|l|} \hline Anion & Anion name & Acid formula & Acid name \\ \hline F- & Fluoride & HF & Hydrofluoric Acid \\ \hline NO3- & Nitrate & HNO3 & Nitric Acid \\ \hline Cl- & Chloride & HCl & Hydrochloric Acid \\ \hline C2H3O2- & Acetate & HC2H3O2 & Acetic Acid \\ \hline NO2- & Nitrite & HNO2 & Nitrous Acid \\ \hline \end{tabular}

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Most popular questions from this chapter

Iodine atoms in \(\mathrm{I}_{2}\) should have a (a) \(1^{-}\) charge (b) \(\delta^{-}\) charge (c) \(\delta^{+}\) charge (d) No charge

Draw a dot diagram for \(\mathrm{BrF}_{5}\). (Hint: \(\mathrm{Br}\) is an expanded octet atom in this molecule. Don't be afraid to stick lone pairs of electrons on it if you have to.)

Draw a dot diagram for the \(\mathrm{NO}_{2}^{+}\) cation.

Draw a dot diagram for \(\mathrm{I}_{3^{\prime}}\). (Hint: Then central I atom is an expanded octet atom in this molecule. Don't be afraid to stick lone pairs of electrons on it if you have to.)

What is the most electronegative element in the periodic table? What is the least electronegative element? What kind of compound would form if these two elements were brought together?
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