Two p-block elements $$X$$ and $$Y$$ form fluorides of the type $$EF_{3}$$. The fluoride compound $$XF_{3}$$ is a Lewis acid and $$YF_{3}$$ is a Lewis base. The hybridizations of the central atoms of $$XF_{3}$$ and $$YF_{3}$$ respectively are

Two p-block elements X and Y form trifluorides $$XF_3$$ and $$YF_3$$. $$XF_3$$ is a Lewis acid and $$YF_3$$ is a Lewis base. Find their hybridizations.

A trifluoride that is a Lewis acid must be electron-deficient. The classic example is $$BF_3$$ (boron trifluoride), where boron has only 6 electrons in its valence shell and can accept a lone pair.

A trifluoride that is a Lewis base must have a lone pair to donate. The classic example is $$NF_3$$ (nitrogen trifluoride), where nitrogen has a lone pair it can donate.

Boron in $$BF_3$$: 3 bond pairs, 0 lone pairs. Geometry: trigonal planar.

Hybridization: $$sp^2$$

Nitrogen in $$NF_3$$: 3 bond pairs, 1 lone pair. Geometry: trigonal pyramidal.

Hybridization: $$sp^3$$

The hybridizations are $$sp^2$$ and $$sp^3$$ respectively.

The correct answer is Option 2: $$sp^2$$ and $$sp^3$$.