Final answer:
The Lewis structure of XeF₂ has three lone pairs and two bonding pairs of electrons around the central Xe atom, due to xenon's ability to have more than eight valence electrons.
Step-by-step explanation:
The Lewis structure of XeF₂ reveals the electron arrangement around the central xenon (Xe) atom. For XeF₂, we start by calculating the total number of valence electrons, which is 8 (for Xe) + 2x7 (for each F), giving us 22 valence electrons in total.
After drawing the skeletal structure with Xe as the central atom and connecting it with single bonds to the two F atoms, we use the remaining electrons to complete the octets of the fluorine atoms, which each get three lone pairs. Considering xenon can accommodate more than eight electrons and possesses empty valence shell d orbitals, the leftover electrons—six in this case—will form three lone pairs around the central atom. This information leads us to conclude that the Lewis structure of XeF₂ has three lone pairs and two bonding pairs of electrons surrounding the central Xe atom.