Answer:
\[B{{F}_{3}}\]has
a planar structure as boron is in \[sp\] -hybridized state. It has one empty
p-orbital. F atom has lone pairs. On account of small size, a lone pair of F
atom is transferred to B atom and thus forms a\[p\pi -p\pi \] back bonding, i.e.,
double bond character comes and due to resonance in the molecule, the bond length
is shorter.
In \[BF_{4}^{-}\] ion, B atom is \[s{{p}^{3}}\] -hybridized
and it has no p-orbital, i.e., back bonding or \[p\pi -p\pi \] bonding is not
possible. Thus, the bond length, B-F is larger as the bond is purely a single
bond.
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