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Among the statements (I – IV), the correct ones are : (I) Be has smaller atomic radius compared to Mg. (II) Be has higher ionization enthalpy then Al. (III) Charge/radius ratio of Be is greater than that of Al. (IV) Both Be and Al form mainly covalent compounds.

1. (1) (I), (II) and (III)
2. (2) (I), (II) and (IV)
3. (3) (I), (III) and (IV)
4. (4) (II), (III) and (IV)

Correct answer: (4) (II), (III) and (IV)

Solution

Statement II is correct because beryllium has a higher ionization enthalpy than aluminum due to its smaller atomic size and higher effective nuclear charge. Statement III is also true as the charge-to-radius ratio of Be is greater than that of Al, leading to stronger attraction in Be. Lastly, both Be and Al predominantly form covalent compounds, making statement IV accurate.

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