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Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: 2+ Mg, Fe*, CI, s²-

Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: 2+ Mg, Fe*, CI, s²-

Living by Chemistry
Living by Chemistry
2nd Edition
ISBN:9781464142314
Author:Angelica M. Stacy
Publisher:Angelica M. Stacy
ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium
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### Determining Empirical Formulas of Binary Ionic Compounds **Problem Statement:** Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: - \(\text{Mg}^{2+}\) - \(\text{Fe}^{2+}\) - \(\text{Cl}^{-}\) - \(\text{S}^{2-}\) **Ions List:** 1. Magnesium ion: \(\text{Mg}^{2+}\) 2. Iron(II) ion: \(\text{Fe}^{2+}\) 3. Chloride ion: \(\text{Cl}^{-}\) 4. Sulfide ion: \(\text{S}^{2-}\) **Example Binary Ionic Compounds:** To form neutral ionic compounds, the total positive and negative charges must balance out. Here are at least four examples: 1. **Magnesium Chloride:** - Formula: \(\text{MgCl}_2\) - Magnesium ion (\(\text{Mg}^{2+}\)) combines with two Chloride ions (\(\text{Cl}^{-}\)) to form a neutral compound. 2. **Magnesium Sulfide:** - Formula: \(\text{MgS}\) - Magnesium ion (\(\text{Mg}^{2+}\)) combines with one Sulfide ion (\(\text{S}^{2-}\)) to form a neutral compound. 3. **Iron(II) Chloride:** - Formula: \(\text{FeCl}_2\) - Iron(II) ion (\(\text{Fe}^{2+}\)) combines with two Chloride ions (\(\text{Cl}^{-}\)) to form a neutral compound. 4. **Iron(II) Sulfide:** - Formula: \(\text{FeS}\) - Iron(II) ion (\(\text{Fe}^{2+}\)) combines with one Sulfide ion (\(\text{S}^{2-}\)) to form a neutral compound. **Note on the Image:** The image shows an online educational interface that prompts users to input the empirical formula for ionic compounds based on provided ions. It includes a text box to enter the answer and three buttons for additional functionalities: - One button appears to be for selecting or performing different actions (denoted by squares). - An 'X' button, possibly to
Transcribed Image Text:### Determining Empirical Formulas of Binary Ionic Compounds **Problem Statement:** Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: - \(\text{Mg}^{2+}\) - \(\text{Fe}^{2+}\) - \(\text{Cl}^{-}\) - \(\text{S}^{2-}\) **Ions List:** 1. Magnesium ion: \(\text{Mg}^{2+}\) 2. Iron(II) ion: \(\text{Fe}^{2+}\) 3. Chloride ion: \(\text{Cl}^{-}\) 4. Sulfide ion: \(\text{S}^{2-}\) **Example Binary Ionic Compounds:** To form neutral ionic compounds, the total positive and negative charges must balance out. Here are at least four examples: 1. **Magnesium Chloride:** - Formula: \(\text{MgCl}_2\) - Magnesium ion (\(\text{Mg}^{2+}\)) combines with two Chloride ions (\(\text{Cl}^{-}\)) to form a neutral compound. 2. **Magnesium Sulfide:** - Formula: \(\text{MgS}\) - Magnesium ion (\(\text{Mg}^{2+}\)) combines with one Sulfide ion (\(\text{S}^{2-}\)) to form a neutral compound. 3. **Iron(II) Chloride:** - Formula: \(\text{FeCl}_2\) - Iron(II) ion (\(\text{Fe}^{2+}\)) combines with two Chloride ions (\(\text{Cl}^{-}\)) to form a neutral compound. 4. **Iron(II) Sulfide:** - Formula: \(\text{FeS}\) - Iron(II) ion (\(\text{Fe}^{2+}\)) combines with one Sulfide ion (\(\text{S}^{2-}\)) to form a neutral compound. **Note on the Image:** The image shows an online educational interface that prompts users to input the empirical formula for ionic compounds based on provided ions. It includes a text box to enter the answer and three buttons for additional functionalities: - One button appears to be for selecting or performing different actions (denoted by squares). - An 'X' button, possibly to
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