Electron affinity is maximum when
O changes into $\mathrm{O}^{-}$
Cl changes into $\mathrm{Cl}^{-}$
F changes into $\mathrm{F}^{-}$
N changes into $\mathrm{N}^{-}$
The bond dissociation energies of $A_2, B_2$ and $A B$ are in the ratio $1: 4: 2$. If $\Delta H$ for formation of $A B$ from $A_2$ and $B_2$ is $-100 \mathrm{~kJ} / \mathrm{mol}$, calculate the bond dissociation energy of $B_2$.
$-400 \mathrm{~kJ} / \mathrm{mol}$
$-800 \mathrm{~kJ} / \mathrm{mol}$
$300 \mathrm{~kJ} / \mathrm{mol}$
$100 \mathrm{~kJ} / \mathrm{mol}$
Among aqueous 1 N solutions, the pH of HCl , $\mathrm{HNO}_2$ and $\mathrm{CH}_3 \mathrm{COOH}$ follows the order
$\mathrm{HCl}<\mathrm{HNO}_2<\mathrm{CH}_3 \mathrm{COOH}$
$\mathrm{CH}_3 \mathrm{COOH}<\mathrm{HNO}_2<\mathrm{HCl}$
$\mathrm{HNO}_2<\mathrm{CH}_3 \mathrm{COOH}<\mathrm{HCl}$
$\mathrm{HCl}<\mathrm{CH}_3 \mathrm{COOH}<\mathrm{HNO}_2$
The ionic radii of $\mathrm{N}^{3-}, \mathrm{O}^{2-}$ and $\mathrm{F}^{-}$follow the trend
$\mathrm{N}^{3-}>\mathrm{O}^{2-}>\mathrm{F}^{-}$
$\mathrm{F}^{-}>\mathrm{N}^{3-}>\mathrm{O}^{2-}$
$\mathrm{O}^{2-}>\mathrm{F}^{-}>\mathrm{N}^{3-}$
$\mathrm{F}^{-}>\mathrm{O}^{2-}>\mathrm{N}^{3-}$
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