Which of the following compounds are water soluble ?

Options

A. `MgCI_(2)`
B. `CaCI_(2)`
C. `SrCI_(2)`
D. All of these

Explanation

To determine which of the given compounds are water soluble, we can follow these steps:

### Step 1: Identify the Compounds
First, we need to identify the specific compounds mentioned in the question. The question refers to chlorides and bromides of alkaline earth metals.

### Step 2: Understand Ionic Nature
Chlorides and bromides of alkaline earth metals (like magnesium, calcium, strontium, and barium) are ionic compounds. Ionic compounds tend to be soluble in water due to their ability to dissociate into ions.

### Step 3: Consider Lattice Enthalpy
Lattice enthalpy is the energy required to separate one mole of an ionic solid into its gaseous ions. For chlorides and bromides of alkaline earth metals, the lattice enthalpy is lower compared to that of fluorides. This lower lattice enthalpy means that less energy is required to break the ionic bonds, making these compounds more soluble in water.

### Step 4: Analyze Solubility Trends
As we move down the group in the periodic table, the atomic number of alkaline earth metals increases. Generally, the solubility of their chlorides and bromides increases with the atomic number. However, it is important to note that the solubility can decrease for some specific compounds, but for the common chlorides and bromides of alkaline earth metals, they are generally soluble.

### Step 5: Conclusion
Based on the ionic nature, lower lattice enthalpy, and solubility trends, we can conclude that all the chlorides and bromides of alkaline earth metals mentioned in the options are water soluble.

### Final Answer
All of the compounds (chlorides and bromides of alkaline earth metals) are water soluble.

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