Among the statements (I-IV),the correct ones | vedclass

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(A) $I$. Atomic radius: $Be

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$(I), (II)$ and $(IV)$

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(A) $I$. Atomic radius: $Be $II$. Ionization Enthalpy $(IE)$: $Be$ $(9.32 \ eV) > Al$ $(5.98 \ eV)$. This statement is correct.$III$. Charge/radius ratio (ionic potential): $Be^{2+}$ $(r \approx 0.31 \ \mathring{A})$ has a higher charge/radius ratio than $Al^{3+}$ $(r \approx 0.54 \ \mathring{A})$. This statement is correct.$IV$. Both $Be$ and $Al$ show diagonal relationship and form mainly covalent compounds due to high polarizing power. This statement is correct.All statements $(I, II, III, IV)$ are correct. Based on the provided options,the most appropriate set is $(I, II, IV)$.

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

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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 than $Al$.$(III)$ Charge/radius ratio of $Be$ is greater than that of $Al$.$(IV)$ Both $Be$ and $Al$ form mainly covalent compounds.