The electronic geometry of XeO3F2 is trigonal bipyramidal. This means that there are five electron pairs around the central xenon atom, with three of them bonding to oxygen atoms and two of them being lone pairs.
The molecular geometry of XeO3F2 is also trigonal bipyramidal. This is because the lone pairs on the central atom do not significantly affect the molecular shape, which is determined by the positions of the bonded atoms.
The hybridization of XeO3F2 is sp3d. This means that the central xenon atom has five hybrid orbitals formed by mixing its s, p, and d orbitals, in order to accommodate the five electron pairs around it in the trigonal bipyramidal geometry.
There are three sigma bonds and two pi bonds in XeO3F2. The three sigma bonds are formed between the central xenon atom and the three oxygen atoms, while the two pi bonds are formed between the central xenon atom and the two fluorine atoms.
XeO3F2 is a polar molecule. This is because the lone pairs on the central xenon atom create an uneven distribution of charge, with a slightly negative end and a slightly positive end. Additionally, the polar bonds between xenon and oxygen and between xenon and fluorine also contribute to the overall polarity of the molecule.