QUESTION IMAGE
Question
fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table.
some ionic compounds
cation | anion | empirical formula | name of compound
mg²⁺ | p³⁻ | |
mg²⁺ | s²⁻ | |
mg²⁺ | o²⁻ | |
mg²⁺ | n³⁻ | |
To determine the empirical formula and name of each ionic compound formed from \( \text{Mg}^{2+} \) (cation) and the given anions, we use the crisscross method (also called the "swap and drop" method) for balancing the charges of cations and anions. The goal is to make the total positive charge equal to the total negative charge in the compound.
Step 1: Compound with \( \text{Mg}^{2+} \) and \( \text{P}^{3-} \)
- Charge Balance: \( \text{Mg}^{2+} \) (charge = +2) and \( \text{P}^{3-} \) (charge = -3).
- Swap the absolute values of the charges: \( \text{Mg} \) takes the charge of \( \text{P} \) (3) and \( \text{P} \) takes the charge of \( \text{Mg} \) (2).
- Formula: \( \text{Mg}_3\text{P}_2 \) (since \( 3 \times (+2) + 2 \times (-3) = 0 \), the compound is neutral).
- Name: Magnesium phosphide (cation name + anion name, where \( \text{P}^{3-} \) is "phosphide").
Step 2: Compound with \( \text{Mg}^{2+} \) and \( \text{S}^{2-} \)
- Charge Balance: \( \text{Mg}^{2+} \) (charge = +2) and \( \text{S}^{2-} \) (charge = -2).
- Swap the absolute values of the charges: Both have a charge magnitude of 2, so the ratio is 1:1.
- Formula: \( \text{MgS} \) (since \( 1 \times (+2) + 1 \times (-2) = 0 \), the compound is neutral).
- Name: Magnesium sulfide (cation name + anion name, where \( \text{S}^{2-} \) is "sulfide").
Step 3: Compound with \( \text{Mg}^{2+} \) and \( \text{O}^{2-} \)
- Charge Balance: \( \text{Mg}^{2+} \) (charge = +2) and \( \text{O}^{2-} \) (charge = -2).
- Swap the absolute values of the charges: Both have a charge magnitude of 2, so the ratio is 1:1.
- Formula: \( \text{MgO} \) (since \( 1 \times (+2) + 1 \times (-2) = 0 \), the compound is neutral).
- Name: Magnesium oxide (cation name + anion name, where \( \text{O}^{2-} \) is "oxide").
Step 4: Compound with \( \text{Mg}^{2+} \) and \( \text{N}^{3-} \)
- Charge Balance: \( \text{Mg}^{2+} \) (charge = +2) and \( \text{N}^{3-} \) (charge = -3).
- Swap the absolute values of the charges: \( \text{Mg} \) takes the charge of \( \text{N} \) (3) and \( \text{N} \) takes the charge of \( \text{Mg} \) (2).
- Formula: \( \text{Mg}_3\text{N}_2 \) (since \( 3 \times (+2) + 2 \times (-3) = 0 \), the compound is neutral).
- Name: Magnesium nitride (cation name + anion name, where \( \text{N}^{3-} \) is "nitride").
Summary Table
| Cation | Anion | Empirical Formula | Name of Compound |
|---|---|---|---|
| \( \text{Mg}^{2+} \) | \( \text{S}^{2-} \) | \( \text{MgS} \) | Magnesium sulfide |
| \( \text{Mg}^{2+} \) | \( \text{O}^{2-} \) | \( \text{MgO} \) | Magnesium oxide |
| \( \text{Mg}^{2+} \) | \( \text{N}^{3-} \) | \( \text{Mg}_3\text{N}_2 \) | Magnesium nitride |
These formulas and names follow the rules of ionic compound nomenclature (cation name + anion name, with anions ending in "-ide") and charge balancing.
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To determine the empirical formula and name of each ionic compound formed from \( \text{Mg}^{2+} \) (cation) and the given anions, we use the crisscross method (also called the "swap and drop" method) for balancing the charges of cations and anions. The goal is to make the total positive charge equal to the total negative charge in the compound.
Step 1: Compound with \( \text{Mg}^{2+} \) and \( \text{P}^{3-} \)
- Charge Balance: \( \text{Mg}^{2+} \) (charge = +2) and \( \text{P}^{3-} \) (charge = -3).
- Swap the absolute values of the charges: \( \text{Mg} \) takes the charge of \( \text{P} \) (3) and \( \text{P} \) takes the charge of \( \text{Mg} \) (2).
- Formula: \( \text{Mg}_3\text{P}_2 \) (since \( 3 \times (+2) + 2 \times (-3) = 0 \), the compound is neutral).
- Name: Magnesium phosphide (cation name + anion name, where \( \text{P}^{3-} \) is "phosphide").
Step 2: Compound with \( \text{Mg}^{2+} \) and \( \text{S}^{2-} \)
- Charge Balance: \( \text{Mg}^{2+} \) (charge = +2) and \( \text{S}^{2-} \) (charge = -2).
- Swap the absolute values of the charges: Both have a charge magnitude of 2, so the ratio is 1:1.
- Formula: \( \text{MgS} \) (since \( 1 \times (+2) + 1 \times (-2) = 0 \), the compound is neutral).
- Name: Magnesium sulfide (cation name + anion name, where \( \text{S}^{2-} \) is "sulfide").
Step 3: Compound with \( \text{Mg}^{2+} \) and \( \text{O}^{2-} \)
- Charge Balance: \( \text{Mg}^{2+} \) (charge = +2) and \( \text{O}^{2-} \) (charge = -2).
- Swap the absolute values of the charges: Both have a charge magnitude of 2, so the ratio is 1:1.
- Formula: \( \text{MgO} \) (since \( 1 \times (+2) + 1 \times (-2) = 0 \), the compound is neutral).
- Name: Magnesium oxide (cation name + anion name, where \( \text{O}^{2-} \) is "oxide").
Step 4: Compound with \( \text{Mg}^{2+} \) and \( \text{N}^{3-} \)
- Charge Balance: \( \text{Mg}^{2+} \) (charge = +2) and \( \text{N}^{3-} \) (charge = -3).
- Swap the absolute values of the charges: \( \text{Mg} \) takes the charge of \( \text{N} \) (3) and \( \text{N} \) takes the charge of \( \text{Mg} \) (2).
- Formula: \( \text{Mg}_3\text{N}_2 \) (since \( 3 \times (+2) + 2 \times (-3) = 0 \), the compound is neutral).
- Name: Magnesium nitride (cation name + anion name, where \( \text{N}^{3-} \) is "nitride").
Summary Table
| Cation | Anion | Empirical Formula | Name of Compound |
|---|---|---|---|
| \( \text{Mg}^{2+} \) | \( \text{S}^{2-} \) | \( \text{MgS} \) | Magnesium sulfide |
| \( \text{Mg}^{2+} \) | \( \text{O}^{2-} \) | \( \text{MgO} \) | Magnesium oxide |
| \( \text{Mg}^{2+} \) | \( \text{N}^{3-} \) | \( \text{Mg}_3\text{N}_2 \) | Magnesium nitride |
These formulas and names follow the rules of ionic compound nomenclature (cation name + anion name, with anions ending in "-ide") and charge balancing.