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Magazine Chapter 2: Problem 25
You have the mythical metal element " \(\mathrm{X}\) " that can exist as \(\mathrm{X}^{+}, \mathrm{X}^{2+}\), and \(\mathrm{X}^{5+}\) ions. a. What would be the chemical formula for compounds formed from the combination of each of the \(\mathrm{X}\) ions and \(\mathrm{SO}_{4}^{2-}\) ? b. If the name of the element \(X\) is exy, what would be the names of each of the compounds from part a of this problem?
Short Answer
Expert verified
a. \(\mathrm{X}_2(\mathrm{SO}_4)\), \(\mathrm{XSO}_4\), \(\mathrm{X}_2(\mathrm{SO}_4)_5\); b. exy(I) sulfate, exy(II) sulfate, exy(V) sulfate.
Step by step solution
01
Determine the Chemical Formula for X+ and SO4^2-
To form a neutral compound, the charges must balance. Here, we have \(\mathrm{X}^+\) and \(\mathrm{SO}_4^{2-}\). We need 2 \(\mathrm{X}^+\) ions to balance the \(\mathrm{SO}_4^{2-}\). Thus, the chemical formula is \(\mathrm{X}_2(\mathrm{SO}_4)\).
02
Determine the Chemical Formula for X2+ and SO4^2-
For \(\mathrm{X}^{2+}\) and \(\mathrm{SO}_4^{2-}\), the charges already balance, so we need one of each ion. The chemical formula is \(\mathrm{XSO}_4\).
03
Determine the Chemical Formula for X5+ and SO4^2-
To balance the charges between \(\mathrm{X}^{5+}\) and \(\mathrm{SO}_4^{2-}\), the least common multiple of charges is 10. We need 2 \(\mathrm{X}^{5+}\) ions and 5 \(\mathrm{SO}_4^{2-}\) ions. Thus, the chemical formula is \(\mathrm{X}_2(\mathrm{SO}_4)_5\).
04
Naming the Compound with X+
Since the metallic ion is \(\mathrm{X}^+\), the compound \(\mathrm{X}_2(\mathrm{SO}_4)\) is named exy(I) sulfate.
05
Naming the Compound with X2+
For the \(\mathrm{X}^{2+}\), the compound \(\mathrm{XSO}_4\) is named exy(II) sulfate.
06
Naming the Compound with X5+
The compound \(\mathrm{X}_2(\mathrm{SO}_4)_5\) formed with \(\mathrm{X}^{5+}\) is named exy(V) sulfate.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Cation and Anion Balancing
In chemistry, balancing cations and anions is crucial for forming stable ionic compounds. A cation is a positively charged ion, and an anion is a negatively charged ion. When they combine, their overall charges must equal zero for the compound to remain electrically neutral.
For example, if you have a cation \ \( \mathrm{X}^{+} \ \) and an anion \ \( \mathrm{SO}_{4}^{2-} \ \), you would need two \ \( \mathrm{X}^{+} \ \) ions to balance with one \ \( \mathrm{SO}_{4}^{2-} \ \) ion. This results in a compound with the formula \ \( \mathrm{X}_{2}(\mathrm{SO}_{4}) \ \).
For example, if you have a cation \ \( \mathrm{X}^{+} \ \) and an anion \ \( \mathrm{SO}_{4}^{2-} \ \), you would need two \ \( \mathrm{X}^{+} \ \) ions to balance with one \ \( \mathrm{SO}_{4}^{2-} \ \) ion. This results in a compound with the formula \ \( \mathrm{X}_{2}(\mathrm{SO}_{4}) \ \).
- For \ \( \mathrm{X}^{2+} \ \) or doubly charged cations, a single \ \( \mathrm{SO}_{4}^{2-} \ \) would suffice, resulting in the compound \ \( \mathrm{XSO}_{4} \ \).
- For a higher charge like \ \( \mathrm{X}^{5+} \ \), you must find the least common multiple of the charges (in this case, 10). Thus, you'd have \ \( 2 \ \mathrm{X}^{5+} \ \) ions with \ \( 5 \ \mathrm{SO}_{4}^{2-} \ \) ions to result in \ \( \mathrm{X}_{2}(\mathrm{SO}_{4})_{5} \ \).
Nomenclature of Ionic Compounds
Naming ionic compounds involves a few simple rules. First, the name of the cation is taken directly from the name of the element. If the metal can form multiple charges, a Roman numeral is included to denote its specific charge. This system is known as the Stock method.
In our example, if the hypothetical metal \ \( \mathrm{X} \ \) is named 'exy,' and it forms ions like \ \( \mathrm{X}^{+} \ \), \ \( \mathrm{X}^{2+} \ \), and \ \( \mathrm{X}^{5+} \ \), you would name the compounds as follows:
In our example, if the hypothetical metal \ \( \mathrm{X} \ \) is named 'exy,' and it forms ions like \ \( \mathrm{X}^{+} \ \), \ \( \mathrm{X}^{2+} \ \), and \ \( \mathrm{X}^{5+} \ \), you would name the compounds as follows:
- For \ \( \mathrm{X}^{+} \ \), the compound \ \( \mathrm{X}_{2}(\mathrm{SO}_{4}) \ \) is called exy(I) sulfate.
- For \ \( \mathrm{X}^{2+} \ \), the compound \ \( \mathrm{XSO}_{4} \ \) is exy(II) sulfate.
- For \ \( \mathrm{X}^{5+} \ \), the compound \ \( \mathrm{X}_{2}(\mathrm{SO}_{4})_{5} \ \) is named exy(V) sulfate.
Oxidation States
Oxidation states are numbers that represent the total number of electrons an atom either gains or loses to form a chemical bond. For metals like our mythical element \ \( \mathrm{X} \ \), these states vary depending on how many electrons are given up.
The element \ \( \mathrm{X} \ \) can exist in the oxidation states of +1, +2, and +5.
The element \ \( \mathrm{X} \ \) can exist in the oxidation states of +1, +2, and +5.
- An oxidation state of +1 corresponds to \ \( \mathrm{X}^{+} \ \), indicating the loss of one electron. This state results in a compound like \ \( \mathrm{X}_{2}(\mathrm{SO}_{4}) \ \).
- When \ \( \mathrm{X} \ \) is in the +2 state, it forms \ \( \mathrm{X}^{2+} \ \) ions, leading to \ \( \mathrm{XSO}_{4} \ \).
- The rare +5 oxidation state is seen in \ \( \mathrm{X}^{5+} \ \), forming a complex compound \ \( \mathrm{X}_{2}(\mathrm{SO}_{4})_{5} \ \).
Ionic Compounds
Ionic compounds are made up of cations and anions that are held together by strong electrostatic forces known as ionic bonds. These compounds usually consist of a metal and a non-metal. They arrange themselves in lattice structures which lead to high melting and boiling points.
An ionic compound forms when the positively charged ion (cation) and negatively charged ion (anion) combine in such a way that their charges cancel out each other. This results in a compound that is electrically neutral.
An ionic compound forms when the positively charged ion (cation) and negatively charged ion (anion) combine in such a way that their charges cancel out each other. This results in a compound that is electrically neutral.
- For example, \ \( \mathrm{X}_{2}(\mathrm{SO}_{4}) \ \) is an ionic compound where the balance of 2 \ \( \mathrm{X}^{+} \ \) ions balances the charge of one \ \( \mathrm{SO}_{4}^{2-} \ \) ion.
- Similarly, \ \( \mathrm{XSO}_{4} \ \) and \ \( \mathrm{X}_{2}(\mathrm{SO}_{4})_{5} \ \) follow these principles by balancing their respective cation and anion charges.
Sulfate Ion SO4^2-
The sulfate ion \ \( \mathrm{SO}_4^{2-} \ \) is a common polyatomic ion in chemistry. It consists of one sulfur atom surrounded by four oxygen atoms in a tetrahedral arrangement. The overall charge is -2, as it has two more electrons than protons.
This negative charge allows it to readily combine with positively charged ions, forming compounds such as sulfates.
This negative charge allows it to readily combine with positively charged ions, forming compounds such as sulfates.
- In compounds like \ \( \mathrm{X}_{2}(\mathrm{SO}_{4}) \ \), \ \( \mathrm{XSO}_{4} \ \), and \ \( \mathrm{X}_{2}(\mathrm{SO}_{4})_{5} \ \), the sulfate ion balances out the positive charges from the cations.
- The stability and presence of \ \( \mathrm{SO}_{4}^{2-} \ \) is pivotal for numerous biochemical processes and industrial applications.
- Sulfate ions are also prevalent in nature, contributing to mineral formation and nutrient cycles.
