The ions `Mg^(2+)` and `PO_4^(3-)` combines to form

Options

A. `Mg_3(PO_4)_2`
B. `Mg_2(PO_4)_2`
C. `Mg_2(PO_4)_3`
D. `Mg_3(PO_4)_3`

Explanation

To determine the compound formed by the combination of the ions \( \text{Mg}^{2+} \) and \( \text{PO}_4^{3-} \), we can follow these steps:

### Step 1: Identify the charges of the ions
- The magnesium ion \( \text{Mg}^{2+} \) has a charge of +2.
- The phosphate ion \( \text{PO}_4^{3-} \) has a charge of -3.

### Step 2: Determine the ratio of the ions needed to balance the charges
To form a neutral compound, the total positive charge must equal the total negative charge. We can find the least common multiple (LCM) of the charges:
- The LCM of 2 (from \( \text{Mg}^{2+} \)) and 3 (from \( \text{PO}_4^{3-} \)) is 6.

### Step 3: Calculate the number of each ion required
- To achieve a total positive charge of +6, we need 3 magnesium ions:
\[ 3 \times (+2) = +6 \]
- To achieve a total negative charge of -6, we need 2 phosphate ions:
\[ 2 \times (-3) = -6 \]

### Step 4: Write the chemical formula
Now that we have determined the number of each ion required, we can write the formula for the compound:
- The formula will be \( \text{Mg}_3(\text{PO}_4)_2 \).

### Final Answer
The compound formed by combining \( \text{Mg}^{2+} \) and \( \text{PO}_4^{3-} \) is \( \text{Mg}_3(\text{PO}_4)_2 \).

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