Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: ²*, Pb**, ci ¯, s²- 2+ 4+ Mg
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: ²*, Pb**, ci ¯, s²- 2+ 4+ Mg
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Binary Ionic Compounds Formation
**Problem Statement:**
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions:
\[ \text{Mg}^{2+} \]
\[ \text{Pb}^{4+} \]
\[ \text{Cl}^{-} \]
\[ \text{S}^{2-} \]
### Explanation:
Binary ionic compounds consist of a metal and a non-metal ion. The empirical formula represents the simplest whole-number ratio of ions in the compound.
Given ions:
1. **Mg<sup>2+</sup>** (Magnesium ion)
2. **Pb<sup>4+</sup>** (Lead(IV) ion)
3. **Cl<sup>−</sup>** (Chloride ion)
4. **S<sup>2−</sup>** (Sulfide ion)
#### Possible Binary Ionic Compounds:
1. **Magnesium Chloride (MgCl<sub>2</sub>)**
- Combining Mg<sup>2+</sup> with Cl<sup>−</sup>.
- The formula is MgCl<sub>2</sub> because two Cl<sup>−</sup> ions are needed to balance the charge of one Mg<sup>2+</sup> ion.
2. **Magnesium Sulfide (MgS)**
- Combining Mg<sup>2+</sup> with S<sup>2−</sup>.
- The formula is MgS as one S<sup>2−</sup> ion balances one Mg<sup>2+</sup> ion.
3. **Lead(IV) Chloride (PbCl<sub>4</sub>)**
- Combining Pb<sup>4+</sup> with Cl<sup>−</sup>.
- The formula is PbCl<sub>4</sub> because four Cl<sup>−</sup> ions are needed to balance the charge of one Pb<sup>4+</sup> ion.
4. **Lead(IV) Sulfide (PbS<sub>2</sub>)**
- Combining Pb<sup>4+</sup> with S<sup>2−</sup>.
- The formula is PbS<sub>2</sub> because two S<sup>2−</sup> ions are needed to balance the charge of one Pb<sup>4+</](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F65e83490-1080-404e-b789-c63cb753ded3%2Fde40840f-e39c-46c4-af50-10352dc01f21%2Fiuguptl.png&w=3840&q=75)
Transcribed Image Text:### Binary Ionic Compounds Formation
**Problem Statement:**
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions:
\[ \text{Mg}^{2+} \]
\[ \text{Pb}^{4+} \]
\[ \text{Cl}^{-} \]
\[ \text{S}^{2-} \]
### Explanation:
Binary ionic compounds consist of a metal and a non-metal ion. The empirical formula represents the simplest whole-number ratio of ions in the compound.
Given ions:
1. **Mg<sup>2+</sup>** (Magnesium ion)
2. **Pb<sup>4+</sup>** (Lead(IV) ion)
3. **Cl<sup>−</sup>** (Chloride ion)
4. **S<sup>2−</sup>** (Sulfide ion)
#### Possible Binary Ionic Compounds:
1. **Magnesium Chloride (MgCl<sub>2</sub>)**
- Combining Mg<sup>2+</sup> with Cl<sup>−</sup>.
- The formula is MgCl<sub>2</sub> because two Cl<sup>−</sup> ions are needed to balance the charge of one Mg<sup>2+</sup> ion.
2. **Magnesium Sulfide (MgS)**
- Combining Mg<sup>2+</sup> with S<sup>2−</sup>.
- The formula is MgS as one S<sup>2−</sup> ion balances one Mg<sup>2+</sup> ion.
3. **Lead(IV) Chloride (PbCl<sub>4</sub>)**
- Combining Pb<sup>4+</sup> with Cl<sup>−</sup>.
- The formula is PbCl<sub>4</sub> because four Cl<sup>−</sup> ions are needed to balance the charge of one Pb<sup>4+</sup> ion.
4. **Lead(IV) Sulfide (PbS<sub>2</sub>)**
- Combining Pb<sup>4+</sup> with S<sup>2−</sup>.
- The formula is PbS<sub>2</sub> because two S<sup>2−</sup> ions are needed to balance the charge of one Pb<sup>4+</
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