What is the orientation of the two unhybridized p orbitals on be with respect to the two be−f bonds?

The two unhybridized orbitals are perpendicular to each other as well as to the hybridized orbitals.

As it is given that Be forms two Be-F bonds that means the molecule is .

VSEPR Theory is used to predict the geometry of the molecules from the number of electrons pairs that surround the central atom.

Formula used :

where, V = number of valence electrons present in central atom

N = number of monovalent atoms bonded to central atom

C = charge of cation

A = charge of anion

In the given molecule, Be is the central atom and F is the monovalent atom.

The number of electrons is 2 that means the hybridization will be sp and geometry of the molecule will be linear. Thus two p orbitals will be feft unhybridized and will be arranged perpendicularly to each other as well as to the hybrid orbitals.

thinking it would be d not too sure but i think it's right