This increased reactivity of the cis-isomer can be readily
explained. In both $\ce{N2F2}$ isomers, each nitrogen atom
possesses a sterically active free valence electron pair.
The transformation of $\ce{N2F2}$ to $\ce{N2F+}$ requires the conversion
of the $\ce{N=N}$ double bond into a $\ce{N#N}$ triple bond
by an overlap of electrons from these two free valence electron pairs. Obviously, this overlap is greatly facilitated
in cis-$\ce{N2F2}$, where these free pairs are on the same
side of the molecule.
This increased reactivity of the cis-isomer can be readily explained. In both $\ce{N2F2}$ isomers, each nitrogen atom possesses a sterically active free valence electron pair. The transformation of $\ce{N2F2}$ to $\ce{N2F+}$ requires the conversion of the $\ce{N=N}$ double bond into a $\ce{N#N}$ triple bond by an overlap of electrons from these two free valence electron pairs. Obviously, this overlap is greatly facilitated in cis-$\ce{N2F2}$, where these free pairs are on the same side of the molecule.
According to Dinitrogen Difluoride Chemistry Inorg. Chem., 2010, 49 (15), pp 6823–6833:
According to Dinitrogen Difluoride Chemistry Inorg. Chem., 2010, 49 (15), pp 6823–6833:
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