Which one of the following ionic species has | vedclass

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(A) Proton affinity is directly related to the basicity of the species. In a period,as electronegativity increases,the ability of the atom to hold its

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$NH_{2}^{-}$

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(A) Proton affinity is directly related to the basicity of the species. In a period,as electronegativity increases,the ability of the atom to hold its lone pair increases,thus decreasing basicity. Comparing $NH_{2}^{-}$ and $F^{-}$,nitrogen is less electronegative than fluorine,so $NH_{2}^{-}$ is a stronger base. In a group,as atomic size increases,the charge density decreases,which reduces the basicity. Comparing $F^{-}$ and $I^{-}$,$F^{-}$ is a stronger base. Comparing $F^{-}$ and $HS^{-}$,$F^{-}$ is a stronger base because oxygen (in $OH^{-}$) is more electronegative than sulfur (in $HS^{-}$),and $F^{-}$ is smaller than $HS^{-}$. Therefore,$NH_{2}^{-}$ has the highest proton affinity among the given species.

Which one of the following ionic species has the greatest proton affinity to form a stable compound?

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