When `MgCl_(2).6H_(2)O` is strongly heated, then if forms `:`

Options

A. `MgO`
B. `Mg(OH)_(2)`
C. `Mg(OH)Cl`
D. `MgCl_(2)`

Explanation

To determine the product formed when `MgCl2.6H2O` is strongly heated, we can follow these steps:

### Step 1: Identify the compound and its components
The compound in question is magnesium chloride hexahydrate, represented as `MgCl2.6H2O`. This indicates that there are 6 water molecules associated with each formula unit of magnesium chloride.

**Hint:** Recognize the significance of the water of crystallization in the compound.

### Step 2: Heating the compound
When `MgCl2.6H2O` is subjected to strong heating, the water of crystallization will begin to evaporate. The first step in the thermal decomposition will lead to the loss of 4 water molecules, resulting in the formation of `MgCl2.2H2O`.

**Hint:** Remember that heating causes the release of water molecules from hydrated compounds.

### Step 3: Further heating
If the heating continues, `MgCl2.2H2O` will also lose its remaining water molecules. The magnesium chloride will then undergo a reaction with the water that is lost and will form magnesium oxide (`MgO`), hydrochloric acid (`HCl`), and additional water.

**Hint:** Consider the possible reactions that can occur when magnesium chloride is heated in the presence of water.

### Step 4: Write the balanced chemical equation
The balanced equation for the reaction can be represented as follows:
\[ MgCl2.2H2O \rightarrow MgO + 2HCl + H2O \]

This indicates that from `MgCl2.2H2O`, we obtain magnesium oxide, hydrochloric acid, and water.

**Hint:** Ensure that the equation is balanced with respect to both mass and charge.

### Step 5: Identify the final product
The final product formed after the complete heating of `MgCl2.6H2O` is magnesium oxide (`MgO`).

**Hint:** Focus on the end product of the thermal decomposition process.

### Final Answer
When `MgCl2.6H2O` is strongly heated, it ultimately forms magnesium oxide (`MgO`).

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