QQuestionChemistry
QuestionChemistry
Fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table:
| Some ionic compounds | anion | empirical formula | name of compound |
| --- | --- | --- | --- |
| S^12 + | S^2 - | | |
| S^12 + | O^2 - | | |
| S^12 + | N^3 - | | |
| S^12 + | P^3 - | | |
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Answer
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Step 1:: Identify the cation and anion in the first ionic compound.
The cation is S^{12 +} and the anion is S^{2 -}.
Step 2:: Write the empirical formula for the ionic compound.
Since both ions have a charge of - 12 and + 12 respectively, they will combine in a 1:1 ratio. Therefore, the empirical formula for this compound is SS or S_2.
Step 3:: Name the ionic compound.
Since the cation is sulfur (S) and the anion is sulfide (S^{2 -}), the name of the compound is sulfur sulfide.
Step 4:: Repeat steps 1 - 3 for the remaining ionic compounds.
Step 5:: Ionic compound S^{12 +} and O^{2 -}
Step 6:: Identify the cation and anion in the ionic compound.
The cation is S^{12 +} and the anion is O^{2 -}.
Step 7:: Write the empirical formula for the ionic compound.
Since the charge of the cation and anion do not balance each other, we need to find the smallest ratio of ions that will balance the charges. To do this, we divide the charge of each ion by its absolute value and find the least common multiple (LCM) of the two numbers. Charge of S^{12 +} / |charge| = 12 / 12 = 1 Charge of O^{2 -} / |charge| = 2 / 2 = 1 The LCM of 1 and 1 is 1. Therefore, the empirical formula for this compound is SO or S_1 O_1.
Step 8:: Name the ionic compound.
Since the cation is sulfur (S) and the anion is oxide (O^{2 -}), the name of the compound is sulfur oxide.
Step 9:: Ionic compound S^{12 +} and N^{3 -}
Step 10:: Identify the cation and anion in the ionic compound.
The cation is S^{12 +} and the anion is N^{3 -}.
Step 11:: Write the empirical formula for the ionic compound.
Since the charge of the cation and anion do not balance each other, we need to find the smallest ratio of ions that will balance the charges. To do this, we divide the charge of each ion by its absolute value and find the least common multiple (LCM) of the two numbers. Charge of S^{12 +} / |charge| = 12 / 12 = 1 Charge of N^{3 -} / |charge| = 3 / 3 = 1 The LCM of 1 and 1 is 1. Therefore, the empirical formula for this compound is SN or S_1 N_1.
Step 12:: Name the ionic compound.
Since the cation is sulfur (S) and the anion is nitride (N^{3 -}), the name of the compound is sulfur nitride.
Step 13:: Ionic compound S^{12 +} and P^{3 -}
Step 14:: Identify the cation and anion in the ionic compound.
The cation is S^{12 +} and the anion is P^{3 -}.
Step 15:: Write the empirical formula for the ionic compound.
Since the charge of the cation and anion do not balance each other, we need to find the smallest ratio of ions that will balance the charges. To do this, we divide the charge of each ion by its absolute value and find the least common multiple (LCM) of the two numbers. Charge of S^{12 +} / |charge| = 12 / 12 = 1 Charge of P^{3 -} / |charge| = 3 / 3 = 1 The LCM of 1 and 1 is 1. Therefore, the empirical formula for this compound is SP or S_1 P_1.
Step 16:: Name the ionic compound.
Since the cation is sulfur (S) and the anion is phosphide (P^{3 -}), the name of the compound is sulfur phosphide.
Final Answer
| Some ionic compounds | anion | empirical formula | name of compound | | --- | --- | --- | --- | | S^12 + | S^2 - | S^2 | sulfur sulfide | | S^12 + | O^2 - | SO | sulfur oxide | | S^12 + | N^3 - | SN | sulfur nitride | | S^12 + | P^3 - | SP | sulfur phosphide |
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