Why this is the stabling order: $C H_{2}^{+} F < C H_{2}^{+} - O H < C H_{2}^{+} - N H_{2}$

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Solution

(1) $C H_{2}^{+} - . . N H_{2} ⟶$ This is more stable because lone pair of $e^{-}$ s on Nitrogen can stabilize the molecule.
(2) $C H_{2}^{+} - . . O . . H ⟶$ This is less stable than (1) because oxygen have lone pair of $e^{-}$ s but oxygen is highly electronegative than Nitrogen.
(3) $C H_{2}^{+} - F ⟶$ Fluorine does not have lone pair of $e^{-}$ s to stabilize the molecule.

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