Question

what is the f-xe-f angle in the molecule xef₂ (xe has three lone pairs of electrons)? enter the answer!

Explanation:

Step1: Determine the electron - pair geometry

For \(XeF_2\), the central atom \(Xe\) has 8 valence electrons. It forms 2 bonds with \(F\) atoms (each \(F\) contributes 1 electron for bonding). So the number of bonding pairs \(= 2\). There are 3 lone pairs (\(8-(2\times1)=6\) non - bonding electrons, \(6\div2 = 3\) lone pairs). The electron - pair geometry (VSEPR theory) for \(AX_2E_3\) (where \(A\) is the central atom, \(X\) is the bonded atom, \(E\) is the lone pair) is trigonal bipyramidal.

Step2: Determine the molecular geometry

In a trigonal bipyramidal electron - pair geometry with 3 lone pairs, the lone pairs occupy the equatorial positions (to minimize repulsions). The molecular geometry (which only considers the positions of the bonded atoms) is linear. For a linear molecule, the bond angle \(F - Xe - F\) is \(180^{\circ}\).

Answer:

\(180\)