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Chapter 7: Problem 26

Write formulas for ionic compounds composed of the following ions. aluminum and carbonate

Short Answer

Expert verified
The formula for the compound is \( \text{Al}_2(\text{CO}_3)_3 \).

Step by step solution

01

Identify the Ions and Their Charges

The first step is to identify the ions involved and their charges. Aluminum exists as the cation with a charge of +3, represented as \( \text{Al}^{3+} \). The carbonate ion is the anion with a charge of -2, represented as \( \text{CO}_3^{2-} \).
02

Determine the Least Common Multiple (LCM)

To balance the charges, we should find the least common multiple of the charges of both ions. The charge of aluminum is +3, and the charge of carbonate is -2. The least common multiple of 3 and 2 is 6.
03

Use the LCM to Balance the Charges

Determine the number of each ion needed to achieve a net charge of zero. Since the LCM is 6, and one aluminum ion has a +3 charge, we need 2 aluminum ions to achieve a total positive charge of +6. Similarly, one carbonate ion has a -2 charge, so we need 3 carbonate ions for a total negative charge of -6.
04

Write the Formula

Now that we have determined the ratio of ions (2 aluminum ions and 3 carbonate ions), we can write the formula for the compound: \( \text{Al}_2(\text{CO}_3)_3 \). This formula reflects the need for 2 \( \text{Al}^{3+} \) ions for every 3 \( \text{CO}_3^{2-} \) ions to balance the total charge to zero.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Aluminum Ion
The aluminum ion is a crucial component when forming ionic compounds. It is represented by the symbol \( \text{Al}^{3+} \), indicating that aluminum loses three electrons to achieve a stable positive charge. In chemistry, this ion is referred to as a cation, because it carries a positive charge. Understanding the nature of cations like the aluminum ion is important in the creation of compounds.
  • Aluminum has three electrons in its outer shell which it loses, resulting in a +3 charge.
  • The process of electron loss is known as oxidation.
  • In the context of forming compounds, this +3 charge plays a key role in balancing the total charge of the compound.
Carbonate Ion
The carbonate ion, \( \text{CO}_3^{2-} \), is a significant anion in chemistry, carrying a charge of -2. This negative charge results from the gain of two electrons, which forms a stable ion. The carbonate ion is part of many compounds found naturally, such as limestone and baking soda.
  • As a polyatomic ion, it is made up of one carbon atom and three oxygen atoms.
  • The presence of multiple atoms bonded together makes it different from simple ions.
  • Due to its -2 charge, it readily forms ionic bonds with positively charged cations, like aluminum, to balance out the charge.
Chemical Formulas
Chemical formulas are the scientific shorthand for representing chemical compounds. These formulas not only show the types of atoms and ions in a compound, but also the specific number to achieve charge neutrality. For example, in an ionic compound of aluminum and carbonate, the formula is \( \text{Al}_2(\text{CO}_3)_3 \). This notation provides significant information:
  • The subscripts indicate the number of each ion required to balance the overall charge.
  • In \( \text{Al}_2(\text{CO}_3)_3 \), the subscript 2 tells us there are two aluminum ions.
  • The subscript 3, outside the parentheses, denotes three carbonate ions, working together to make the compound electrically neutral.
Charge Balancing
Charge balancing is a fundamental principle when forming ionic compounds. It ensures the overall charge of the chemical compound is neutral, meaning the positive and negative charges must cancel out. Here's a simplified explanation:
  • Each ion contributes its charge to the compound's total charge.
  • For a balanced formula, the sum of the cations' positive charges equals the sum of the anions' negative charges.
  • In the \( \text{Al}_2(\text{CO}_3)_3 \) compound, two aluminum ions contribute \(+6\) (since each is \(+3\)) and three carbonate ions contribute \(-6\) (since each is \(-2\), resulting in \(-6\)).
Thus, the importance of charge balancing in creating stable ionic compounds cannot be overstated. Correctly balancing charges gives rise to stable, electrically neutral compounds.

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Most popular questions from this chapter

Ionic Compounds Chrysoberyl is a transparent or translucent mineral that is sometimes opalescent. It is composed of beryllium aluminum oxide, BeAl. \(\mathrm{O}_{4}\) . Identify the oxidation numbers of each of the ions found in this compound. Explain the formation of this ionic compound.

You are given a liquid of unknown density. The mass of a graduated cylinder containing 2.00 \(\mathrm{mL}\) of the liquid is 34.68 \(\mathrm{g} .\) The mass of the empty graduated cylinder is 30.00 \(\mathrm{g} .\) Given this information, determine the density of the liquid. (Chapter 2\()\)

Analyze What subscripts would you most likely use if the following substances formed an ionic compound? a. an alkali metal and a halogen b. an alkali metal and a nonmetal from group 16 c. an alkaline earth metal and a halogen d. an alkaline earth metal and a nonmetal from group 16

Observe and Infer Identify the mistakes in the incorrect formulas and formula names, and design a flowchart to prevent the mistakes. $$ \begin{array}{ll}{\text { a. copper acetate }} & {\text { d. disodium oxide }} \\\ {\text { b. } \operatorname{Mg}_{2} \mathrm{O}_{2}} & {\text { e. } \mathrm{Al}_{2} \mathrm{SO}_{43}} \\ {\text { c. } \mathrm{Pb}_{2} \mathrm{O}_{5}}\end{array} $$

Write the symbol and name of the element that fits each description. (Chapter 6\()\) a. the second-lightest of the halogens b. the metalloid with the lowest period number c. the only group 16 element that is a gas at room temperature d. the heaviest of the noble gases e. the group 15 nonmetal that is a solid at room temperature
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