Anhydrous aluminium chloride `(Al_(2)Cl_(6))` is covalent compound and soluble in water giving:

Options

A. `Al^(3+) and Cl^(-)` ions.
B. `[Cl(H_(2)O)_(6)]^(3+) and Cl^(-)` ions
C. `[AlCl_(2)(H_(2)O)_(4)] and [AlCl_(4)(H_(2)O)_(2)]^(-)` ions
D. none of the above

Explanation

To solve the question regarding the solubility of anhydrous aluminum chloride `(Al_(2)Cl_(6))` in water, we will follow these steps:

### Step 1: Understand the nature of anhydrous aluminum chloride
Anhydrous aluminum chloride `(AlCl3)` is a covalent compound. It does not dissolve in water in its original form but reacts with water to form a hydrated complex.

**Hint:** Remember that covalent compounds often require a reaction to form ions in solution.

### Step 2: Write the reaction of anhydrous aluminum chloride with water
When anhydrous aluminum chloride is added to water, it reacts to form aluminum chloride hexahydrate `(AlCl3·6H2O)`. The reaction can be represented as:
\[ AlCl3 + 6H2O \rightarrow AlCl3 \cdot 6H2O \]

**Hint:** Look for the formation of hydrated compounds when covalent substances interact with water.

### Step 3: Dissociation of aluminum chloride hexahydrate
The hydrated form `(AlCl3·6H2O)` can dissociate in solution to produce aluminum ions and chloride ions. The dissociation is represented as:
\[ AlCl3 \cdot 6H2O \rightarrow Al^{3+} + 3Cl^{-} + 6H2O \]

**Hint:** Focus on how the hydrated compound breaks down into its constituent ions.

### Step 4: Identify the ions produced
From the dissociation reaction, we can see that the ions produced are:
- Aluminum ion: \( Al^{3+} \)
- Chloride ions: \( 3Cl^{-} \)

**Hint:** Count the number of each type of ion produced in the dissociation.

### Conclusion
Thus, when anhydrous aluminum chloride is dissolved in water, it produces aluminum ions and chloride ions.

**Final Answer:** The solution of anhydrous aluminum chloride in water gives \( Al^{3+} \) and \( 3Cl^{-} \) ions.