Two statements are given below.Statement I: N | vedclass

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(A) Statement $I$: Nitrogen $(Z=7)$ has a half-filled $2p^3$ configuration,which provides extra stability,leading to a higher ionization enthalpy comp

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Both statements $I$ and $II$ are correct

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(A) Statement $I$: Nitrogen $(Z=7)$ has a half-filled $2p^3$ configuration,which provides extra stability,leading to a higher ionization enthalpy compared to Beryllium $(Z=4)$. Also,electronegativity increases across a period,so Nitrogen $(3.04)$ is more electronegative than Beryllium $(1.57)$. Thus,statement $I$ is correct.Statement $II$: Non-metal oxides and high oxidation state metal oxides are generally acidic. $B_2O_3$ is a non-metal oxide (acidic),and $CrO_3$ (where $Cr$ is in $+6$ oxidation state) is an acidic oxide. Thus,statement $II$ is correct.

List-$I$ (Elements)	List-$II$ (Properties)
$A. Cl, S$	$I. \text{Elements with highest electronegativity}$
$B. Ge, As$	$II. \text{Elements with largest atomic size}$
$C. Fr, Ra$	$III. \text{Elements which show properties of both metals and non-metals}$
$D. F, O$	$IV. \text{Elements with highest negative electron gain enthalpy}$

Two statements are given below.
Statement $I$: Nitrogen has more ionization enthalpy and electronegativity than beryllium.
Statement $II$: $CrO_3$ and $B_2O_3$ are acidic oxides.
Correct answer is

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Two statements are given below.Statement $I$: Nitrogen has more ionization enthalpy and electronegativity than beryllium.Statement $II$: $CrO_3$ and $B_2O_3$ are acidic oxides.Correct answer is