Fluorine nitrate, $\mathrm{FONO}_{2}$, is an oxidizing agent used as a rocket propellant. A reference source lists the following data for $\mathrm{FO}_{\mathrm{a}} \mathrm{NO}_{2}$. (The subscript "a" shows that this O atom is different from the other two.)
Bond lengths: $\mathrm{N}-\mathrm{O}=129 \mathrm{pm}$
$\mathrm{N}-\mathrm{O}_{\mathrm{a}}=139 \mathrm{pm} ; \mathrm{O}_{\mathrm{a}}-\mathrm{F}=142 \mathrm{pm}$
Bond angles: $\mathrm{O}-\mathrm{N}-\mathrm{O}=125^{\circ}$
$\mathrm{F}-\mathrm{O}_{\mathrm{a}}-\mathrm{N}=105^{\circ}$
NO $_{\mathrm{a}} \mathrm{F}$ plane is perpendicular to the $\mathrm{O}_{2} \mathrm{NO}_{\mathrm{a}}$ plane
Use these data to construct a Lewis structure(s), a three-dimensional sketch of the molecule, and a plausible bonding scheme showing hybridization and orbital overlaps.