Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Atoms, Ions and Molecules: Predicting the Formula of Ionic Compounds with Common Ions**
**Task:**
Write the empirical formula for at least four ionic compounds that could be formed from the following ions:
\[ \text{Fe}^{2+}, \ \text{CN}^-, \ \text{NH}_4^+, \ \text{BrO}_3^- \]
[Interactive Box for Input]
**Instructions to Students:**
- Identify the possible combinations of cations and anions from the given ions.
- Ensure that the overall charge of the compound is neutral by balancing the charges of the ions correctly.
- Enter at least four different empirical formulas that represent the combinations of the provided ions.
**Example:**
If pairing \(\text{Fe}^{2+}\) with \(\text{BrO}_3^-\):
\[ (\text{Fe}^{2+})_{1}(\text{BrO}_3^-)_{2} = \text{Fe(BrO}_3\text{)}_2 \]
*Interactive Elements:*
- The empty box allows students to input their empirical formulas.
- The box on the right shows options that can be used to reset (\(\times\)), to undo an entry (curved arrow), or to get help (?).
**Note:**
Carefully check the oxidation states and ensure that the total charge of the resulting ionic compound is zero to validate the correctness of the formula.](https://content.bartleby.com/qna-images/question/19406573-6a1e-471a-ba9f-f1bcf97fa675/9a07b84d-1253-4f65-85f4-23e2da2cd0d0/2b6v8d.png)
Transcribed Image Text:**Atoms, Ions and Molecules: Predicting the Formula of Ionic Compounds with Common Ions**
**Task:**
Write the empirical formula for at least four ionic compounds that could be formed from the following ions:
\[ \text{Fe}^{2+}, \ \text{CN}^-, \ \text{NH}_4^+, \ \text{BrO}_3^- \]
[Interactive Box for Input]
**Instructions to Students:**
- Identify the possible combinations of cations and anions from the given ions.
- Ensure that the overall charge of the compound is neutral by balancing the charges of the ions correctly.
- Enter at least four different empirical formulas that represent the combinations of the provided ions.
**Example:**
If pairing \(\text{Fe}^{2+}\) with \(\text{BrO}_3^-\):
\[ (\text{Fe}^{2+})_{1}(\text{BrO}_3^-)_{2} = \text{Fe(BrO}_3\text{)}_2 \]
*Interactive Elements:*
- The empty box allows students to input their empirical formulas.
- The box on the right shows options that can be used to reset (\(\times\)), to undo an entry (curved arrow), or to get help (?).
**Note:**
Carefully check the oxidation states and ensure that the total charge of the resulting ionic compound is zero to validate the correctness of the formula.
Transcribed Image Text:### Predicting the Formula of Ionic Compounds with Common Ions
#### Understanding Charges and Ionic Compounds
When predicting the formula of ionic compounds, it's essential to consider the charges of the ions involved. For instance, Fe\(^{3+}\) represents an iron ion with a positive charge of +3, and MnO\(_4^{-}\) represents a permanganate ion with a negative charge of -1. To form a neutral compound, the total positive charge must balance the total negative charge. Therefore, the formula of the resulting compound can be predicted based on this balance.
#### Example: Predicting the Formula
Given:
- One MnO\(_4^{-}\) anion with charge \(-1\)
- Iron ion Fe\(^{3+}\) with charge \(+3\)
- Ammonium ion NH\(_4^{+}\) with charge \(+1\)
By balancing the charges to achieve a net charge of 0, we can predict the combinations of other ions to form neutral compounds.
#### Table of Ions Combinations
The table below shows the possible combinations of ions and the resulting compounds:
| | CH<sub>3</sub>CO<sub>2</sub><sup>−</sup> | MnO<sub>4</sub><sup>−</sup> |
|---------------|-----------------------------------------------|-----------------------------------|
| Fe<sup>3+</sup> | Fe(CH<sub>3</sub>CO<sub>2</sub>)<sub>3</sub> | Fe(MnO<sub>4</sub>)<sub>3</sub> |
| NH<sub>4</sub><sup>+</sup> | NH<sub>4</sub>CH<sub>3</sub>CO<sub>2</sub> | NH<sub>4</sub>MnO<sub>4</sub> |
**Explanation of the Table:**
- **Top Row:** Lists the anions (negatively charged ions) used in the combinations.
- **First Column:** Lists the cations (positively charged ions).
Each cell shows the empirical formula of the compound formed by combining the ions from the respective row and column.
#### Resulting Empirical Formulae
From the table, the empirical formulae of the four possible ionic compounds are:
- Fe(CH<sub>3</sub>CO<
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