QUESTION IMAGE
Question
simple binary ionic compounds
please complete the following table:
| name of ionic compound | formula of ionic compound |
|---|---|
| 2. calcium chloride | cacl₂ |
| 3. magnesium sulfide | mgs |
| 4. aluminum oxide | al₂o₃ |
| 5. lithium phosphide | li₃p |
| 6. cesium nitride | cs₃n |
| 7. potassium iodide | ki |
| 8. barium fluoride | baf₂ |
| 9. rubidium nitride | |
| 10. barium oxide | |
| 11. | k₂o |
| 12. | mgi₂ |
Response
To complete the table for simple binary ionic compounds, we use the rules of ionic compound formation (criss - cross method for charges):
1. Sodium bromide
- Sodium ($\text{Na}$) has a charge of $+ 1$ ($\text{Na}^+$), and bromide ($\text{Br}$) has a charge of $-1$ ($\text{Br}^-$).
- Using the criss - cross method, the formula is $\text{NaBr}$.
2. Calcium chloride
- Calcium ($\text{Ca}$) has a charge of $+2$ ($\text{Ca}^{2 + }$), and chloride ($\text{Cl}$) has a charge of $-1$ ($\text{Cl}^-$).
- Cross - multiplying the charges, we get $1$ $\text{Ca}$ and $2$ $\text{Cl}$, so the formula is $\text{CaCl}_2$.
3. Magnesium sulfide
- Magnesium ($\text{Mg}$) has a charge of $+2$ ($\text{Mg}^{2+}$), and sulfide ($\text{S}$) has a charge of $-2$ ($\text{S}^{2 - }$).
- The formula is $\text{MgS}$ (since the charges cancel out: $+2$ and $-2$).
4. Aluminum oxide
- Aluminum ($\text{Al}$) has a charge of $+3$ ($\text{Al}^{3+}$), and oxide ($\text{O}$) has a charge of $-2$ ($\text{O}^{2 - }$).
- Cross - multiplying, we have $2$ $\text{Al}$ and $3$ $\text{O}$, so the formula is $\text{Al}_2\text{O}_3$.
5. Lithium phosphide
- Lithium ($\text{Li}$) has a charge of $+1$ ($\text{Li}^+$), and phosphide ($\text{P}$) has a charge of $-3$ ($\text{P}^{3 - }$).
- Cross - multiplying, we get $3$ $\text{Li}$ and $1$ $\text{P}$, so the formula is $\text{Li}_3\text{P}$.
6. Cesium nitride
- Cesium ($\text{Cs}$) has a charge of $+1$ ($\text{Cs}^+$), and nitride ($\text{N}$) has a charge of $-3$ ($\text{N}^{3 - }$).
- Cross - multiplying, we have $3$ $\text{Cs}$ and $1$ $\text{N}$, so the formula is $\text{Cs}_3\text{N}$.
7. Potassium iodide
- Potassium ($\text{K}$) has a charge of $+1$ ($\text{K}^+$), and iodide ($\text{I}$) has a charge of $-1$ ($\text{I}^-$).
- The formula is $\text{KI}$.
8. Barium fluoride
- Barium ($\text{Ba}$) has a charge of $+2$ ($\text{Ba}^{2+}$), and fluoride ($\text{F}$) has a charge of $-1$ ($\text{F}^-$).
- Cross - multiplying, we get $1$ $\text{Ba}$ and $2$ $\text{F}$, so the formula is $\text{BaF}_2$.
9. Rubidium nitride
- Rubidium ($\text{Rb}$) has a charge of $+1$ ($\text{Rb}^+$), and nitride ($\text{N}$) has a charge of $-3$ ($\text{N}^{3 - }$).
- Cross - multiplying, we have $3$ $\text{Rb}$ and $1$ $\text{N}$, so the formula is $\text{Rb}_3\text{N}$.
10. Barium oxide
- Barium ($\text{Ba}$) has a charge of $+2$ ($\text{Ba}^{2+}$), and oxide ($\text{O}$) has a charge of $-2$ ($\text{O}^{2 - }$).
- The formula is $\text{BaO}$.
11. For formula $\text{K}_2\text{O}$
- Potassium ($\text{K}$) has a charge of $+1$ ($\text{K}^+$), and oxide ($\text{O}$) has a charge of $-2$ ($\text{O}^{2 - }$).
- The name is Potassium oxide.
12. For formula $\text{MgI}_2$
- Magnesium ($\text{Mg}$) has a charge of $+2$ ($\text{Mg}^{2+}$), and iodide ($\text{I}$) has a charge of $-1$ ($\text{I}^-$).
- The name is Magnesium iodide.
| Name of Ionic Compound | Formula of Ionic Compound |
|---|---|
| 2. Calcium chloride | $\text{CaCl}_2$ |
| 3. Magnesium sulfide | $\text{MgS}$ |
| 4. Aluminum oxide | $\text{Al}_2\text{O}_3$ |
| 5. Lithium phosphide | $\text{Li}_3\text{P}$ |
| 6. Cesium nitride | $\text{Cs}_3\text{N}$ |
| 7. Potassium iodide | $\text{KI}$ |
| 8. Barium fluoride | $\text{BaF}_2$ |
| 9. Rubidium nitride | $\text{Rb}_3\text{N}$ |
| 10. Barium oxide | $\text{BaO}$ |
| 11. Potassium oxide | $\text{K}_2\text{O}$ |
| 12. Magnesium iodide | $\text{MgI}_2$ |
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To complete the table for simple binary ionic compounds, we use the rules of ionic compound formation (criss - cross method for charges):
1. Sodium bromide
- Sodium ($\text{Na}$) has a charge of $+ 1$ ($\text{Na}^+$), and bromide ($\text{Br}$) has a charge of $-1$ ($\text{Br}^-$).
- Using the criss - cross method, the formula is $\text{NaBr}$.
2. Calcium chloride
- Calcium ($\text{Ca}$) has a charge of $+2$ ($\text{Ca}^{2 + }$), and chloride ($\text{Cl}$) has a charge of $-1$ ($\text{Cl}^-$).
- Cross - multiplying the charges, we get $1$ $\text{Ca}$ and $2$ $\text{Cl}$, so the formula is $\text{CaCl}_2$.
3. Magnesium sulfide
- Magnesium ($\text{Mg}$) has a charge of $+2$ ($\text{Mg}^{2+}$), and sulfide ($\text{S}$) has a charge of $-2$ ($\text{S}^{2 - }$).
- The formula is $\text{MgS}$ (since the charges cancel out: $+2$ and $-2$).
4. Aluminum oxide
- Aluminum ($\text{Al}$) has a charge of $+3$ ($\text{Al}^{3+}$), and oxide ($\text{O}$) has a charge of $-2$ ($\text{O}^{2 - }$).
- Cross - multiplying, we have $2$ $\text{Al}$ and $3$ $\text{O}$, so the formula is $\text{Al}_2\text{O}_3$.
5. Lithium phosphide
- Lithium ($\text{Li}$) has a charge of $+1$ ($\text{Li}^+$), and phosphide ($\text{P}$) has a charge of $-3$ ($\text{P}^{3 - }$).
- Cross - multiplying, we get $3$ $\text{Li}$ and $1$ $\text{P}$, so the formula is $\text{Li}_3\text{P}$.
6. Cesium nitride
- Cesium ($\text{Cs}$) has a charge of $+1$ ($\text{Cs}^+$), and nitride ($\text{N}$) has a charge of $-3$ ($\text{N}^{3 - }$).
- Cross - multiplying, we have $3$ $\text{Cs}$ and $1$ $\text{N}$, so the formula is $\text{Cs}_3\text{N}$.
7. Potassium iodide
- Potassium ($\text{K}$) has a charge of $+1$ ($\text{K}^+$), and iodide ($\text{I}$) has a charge of $-1$ ($\text{I}^-$).
- The formula is $\text{KI}$.
8. Barium fluoride
- Barium ($\text{Ba}$) has a charge of $+2$ ($\text{Ba}^{2+}$), and fluoride ($\text{F}$) has a charge of $-1$ ($\text{F}^-$).
- Cross - multiplying, we get $1$ $\text{Ba}$ and $2$ $\text{F}$, so the formula is $\text{BaF}_2$.
9. Rubidium nitride
- Rubidium ($\text{Rb}$) has a charge of $+1$ ($\text{Rb}^+$), and nitride ($\text{N}$) has a charge of $-3$ ($\text{N}^{3 - }$).
- Cross - multiplying, we have $3$ $\text{Rb}$ and $1$ $\text{N}$, so the formula is $\text{Rb}_3\text{N}$.
10. Barium oxide
- Barium ($\text{Ba}$) has a charge of $+2$ ($\text{Ba}^{2+}$), and oxide ($\text{O}$) has a charge of $-2$ ($\text{O}^{2 - }$).
- The formula is $\text{BaO}$.
11. For formula $\text{K}_2\text{O}$
- Potassium ($\text{K}$) has a charge of $+1$ ($\text{K}^+$), and oxide ($\text{O}$) has a charge of $-2$ ($\text{O}^{2 - }$).
- The name is Potassium oxide.
12. For formula $\text{MgI}_2$
- Magnesium ($\text{Mg}$) has a charge of $+2$ ($\text{Mg}^{2+}$), and iodide ($\text{I}$) has a charge of $-1$ ($\text{I}^-$).
- The name is Magnesium iodide.
| Name of Ionic Compound | Formula of Ionic Compound |
|---|---|
| 2. Calcium chloride | $\text{CaCl}_2$ |
| 3. Magnesium sulfide | $\text{MgS}$ |
| 4. Aluminum oxide | $\text{Al}_2\text{O}_3$ |
| 5. Lithium phosphide | $\text{Li}_3\text{P}$ |
| 6. Cesium nitride | $\text{Cs}_3\text{N}$ |
| 7. Potassium iodide | $\text{KI}$ |
| 8. Barium fluoride | $\text{BaF}_2$ |
| 9. Rubidium nitride | $\text{Rb}_3\text{N}$ |
| 10. Barium oxide | $\text{BaO}$ |
| 11. Potassium oxide | $\text{K}_2\text{O}$ |
| 12. Magnesium iodide | $\text{MgI}_2$ |