Question

Fill in the blanks in the table. \begin{tabular}{|c|c|c|c|} \hline Cation & Anion & Formula & \multicolumn{1}{|c|} { Name } \\ \hline & & & Magnesium bicarbonate \\ \hline & & \(\mathrm{Sr} \mathrm{Cl}_{2}\) & \\ \hline \(\mathrm{Fe}^{3+}\) & \(\mathrm{NO}_{2}^{-}\) & & \\ \hline & & & Manganese(II) chlorate \\ \hline & & \(\mathrm{SnBr}_{4}\) & \\ \hline \(\mathrm{Co}^{2+}\) & \(\mathrm{PO}_{4}^{3-}\) & & \\ \hline \(\mathrm{Hg}_{2}^{2+}\) & \(\mathrm{I}^{-}\) & & \\ \hline & & \(\mathrm{Cu}_{2} \mathrm{CO}_{3}\) & \\ \hline & & & Lithium nitride \\ \hline \(\mathrm{Al}^{3+}\) & \(\mathrm{S}^{2-}\) & & \\ \hline \end{tabular}

Short answer

The formulas and names are: 1. \( \mathrm{Mg(HCO}_{3})_{2} \), 2. Strontium chloride, 3. \( \mathrm{Fe(NO}_{2})_{3} \), 4. \( \mathrm{Mn(ClO}_{3})_{2} \), 5. Tin(IV) bromide, 6. \( \mathrm{Co}_{3}(\mathrm{PO}_{4})_{2} \), 7. \( \mathrm{Hg}_{2}\mathrm{I}_{2} \), 8. Copper(I) carbonate, 9. \( \mathrm{Li}_{3}\mathrm{N} \), 10. \( \mathrm{Al}_{2}\mathrm{S}_{3} \).

Step-by-step solution

Determine the Formula for Magnesium Bicarbonate

Magnesium has a charge of \( \mathrm{Mg}^{2+} \) and bicarbonate has a charge of \( \mathrm{HCO}_{3}^{-} \). To balance the charges, we need two bicarbonate ions for each magnesium ion. So, the formula is \( \mathrm{Mg(HCO}_{3})_{2} \).

Name the Compound \( \mathrm{SrCl}_{2} \)

\( \mathrm{SrCl}_{2} \) consists of strontium and chlorine. Strontium forms a \( \mathrm{Sr}^{2+} \) cation and chlorine forms \( \mathrm{Cl}^{-} \). The name of \( \mathrm{SrCl}_{2} \) is strontium chloride.

Determine the Formula for Iron and Nitrite

Iron has a charge of \( \mathrm{Fe}^{3+} \) and nitrite \( \mathrm{NO}_2^{-} \). We need three nitrite ions to balance one iron ion. The formula is \( \mathrm{Fe(NO}_{2})_{3} \).

Determine the Formula for Manganese(II) Chlorate

Manganese(II) indicates \( \mathrm{Mn}^{2+} \), and chlorate is \( \mathrm{ClO}_{3}^{-} \). We need two chlorate ions to balance one manganese ion. The formula is \( \mathrm{Mn(ClO}_{3})_{2} \).

Name the Compound \( \mathrm{SnBr}_{4} \)

\( \mathrm{SnBr}_{4} \) is composed of tin and bromine. Tin can have multiple oxidation states, but here it is \( \mathrm{Sn}^{4+} \). Thus, the name is tin(IV) bromide.

Determine the Formula for Cobalt and Phosphate

Cobalt has a charge of \( \mathrm{Co}^{2+} \) and phosphate \( \mathrm{PO}_4^{3-} \). To balance the charges, two cobalt and three phosphate ions combine to form \( \mathrm{Co}_{3}(\mathrm{PO}_{4})_{2} \).

Determine the Formula for Mercury(I) Iodide

Mercury(I) is \( \mathrm{Hg}_{2}^{2+} \), which means it acts as a diatomic ion. Iodide is \( \mathrm{I}^{-} \). The formula is \( \mathrm{Hg}_2\mathrm{I}_2 \).

Name the Compound \( \mathrm{Cu}_{2} \mathrm{CO}_{3} \)

\( \mathrm{Cu}_{2} \mathrm{CO}_{3} \) consists of copper, which here is copper(I) due to the formula, and carbonate. The compound is called copper(I) carbonate.

Determine the Formula for Lithium Nitride

Lithium forms \( \mathrm{Li}^{+} \) and nitride is \( \mathrm{N}^{3-} \). To balance, three lithium ions are needed for one nitride ion, giving \( \mathrm{Li}_{3} ext{N} \).

Determine the Formula for Aluminum Sulfide

Aluminum is \( \mathrm{Al}^{3+} \) and sulfide is \( \mathrm{S}^{2-} \). To balance the charges, two aluminum ions and three sulfide ions form \( \mathrm{Al}_{2}\mathrm{S}_{3} \).

Key concepts

Cation and Anion Identification

In chemistry, identifying cations and anions is crucial for understanding how compounds are formed. A **cation** is a positively charged ion that has lost one or more electrons. Common examples include metal ions like magnesium (\( \mathrm{Mg}^{2+} \)) or tin (\( \mathrm{Sn}^{4+} \)). An **anion** is a negatively charged ion that has gained electrons, such as chloride (\( \mathrm{Cl}^{-} \)) or sulfate (\( \mathrm{SO}_{4}^{2-} \)). Understanding the charge on each ion helps in determining the ratio in which these ions combine to form neutral compounds. For instance:

• In magnesium bicarbonate, the magnesium ion is \( \mathrm{Mg}^{2+} \), and the bicarbonate ion is \( \mathrm{HCO}_{3}^{-} \).
• Tin(IV) bromide involves a tin ion with a \( \mathrm{Sn}^{4+} \) charge and bromide ions \( \mathrm{Br}^{-} \).

Identifying these charges is the first step toward balancing chemical formulas effectively.

Balancing Chemical Formulas

Balancing a chemical formula involves ensuring that the total positive charge of the cations equals the total negative charge of the anions, resulting in a neutral compound. To do this, we adjust the ratio of ions to balance the overall charge. For example, in the compound formula for iron and nitrite, iron forms \( \mathrm{Fe}^{3+} \) and nitrite is \( \mathrm{NO}_2^{-} \). To balance these, three nitrite ions are needed for each iron ion, resulting in the formula \( \mathrm{Fe(NO}_{2})_{3} \).

• Magnesium bicarbonate: Two \( \mathrm{HCO}_{3}^{-} \) are needed to balance one \( \mathrm{Mg}^{2+} \), giving \( \mathrm{Mg(HCO}_{3})_{2} \).
• For cobalt and phosphate, \( \mathrm{Co}^{2+} \) requires two cations of cobalt and three anions \( \mathrm{PO}_{4}^{3-} \) giving \( \mathrm{Co}_{3}(\mathrm{PO}_{4})_{2} \).

Balancing ensures the compound is stable and accurately represents the proportions of ions present.

Compound Naming Rules

Naming chemical compounds involves understanding the rules to accurately describe the compound's makeup. Compounds are named based on the cation and the anion they contain. **Basic Steps to Follow:**

• Identify the cation and the anion. For example, in \( \mathrm{SrCl}_{2} \), the cation is strontium \( \mathrm{Sr}^{2+} \), and the anion is chloride \( \mathrm{Cl}^{-} \).
• When naming, start with the cation name followed by the anion. In this case, it becomes "strontium chloride."
• For multivalent metals (metals that can have multiple charges), include the charge in Roman numerals in parentheses. For instance, \( \mathrm{SnBr}_{4} \) is named as "tin(IV) bromide" because tin has a \( \mathrm{Sn}^{4+} \) charge.

These naming conventions not only aid in communication but also provide insight into the molecular structure and composition of the compound.