Assertion (A): Beryllium compounds are covalent in nature.
Reason (R ): The size of `Be^(2+)`ion is larger in compariso to the radii of the other divalent ions of alkaline earth metals.

Options

A. If both `(A)` and `(R )` are correct and `(R )` is the correct explanation of `(A)`.
B. If both `(A)` and `(R )` are correct, but `(R )` is not the correct explanation of `(A)`.
C. If `(A)` is correct, but `(R )` is incorrect.
D. If `(A)` is incrrect, but `(R )` is correct.

Explanation

To analyze the assertion and reason provided in the question, let's break it down step by step:

### Step 1: Evaluate the Assertion
**Assertion (A): Beryllium compounds are covalent in nature.**
- This statement is **true**. Beryllium compounds tend to be covalent due to the high charge density of the beryllium ion (Be²⁺), which leads to significant polarization of the electron cloud of the anions it bonds with.

### Step 2: Evaluate the Reason
**Reason (R): The size of Be²⁺ ion is larger in comparison to the radii of the other divalent ions of alkaline earth metals.**
- This statement is **false**. The size of the Be²⁺ ion is actually smaller than that of other alkaline earth metal ions (like Mg²⁺, Ca²⁺, etc.). The small size of the Be²⁺ ion contributes to its high polarizing power, which is a key factor in forming covalent compounds.

### Step 3: Conclusion
- Since the assertion is true and the reason is false, we conclude that the correct relationship is that the assertion is correct, but the reason provided is incorrect.

### Final Answer:
- Assertion (A) is true, and Reason (R) is false. Therefore, the correct option is that A is correct, but R is incorrect.

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