What is the hybridization the central atom in the structure shown below? The image displays a Lewis structure diagram of the molecule Krypton Difluoride Dioxide (\(\text{KrF}_2\text{O}_2\)).### Diagram Description:- **Central Atom:** - **Krypton (Kr):** Positioned in the center. - **Surrounding Atoms:** - **Fluorine (F) Atoms:** Two fluorine atoms are bonded to the krypton atom. Each fluorine atom shares a single bond with krypton and has three lone pairs of electrons, shown as dots around the F symbol. - **Oxygen (O) Atoms:** Two oxygen atoms are bonded to the krypton atom. Each oxygen atom shares a double bond with krypton and has two lone pairs of electrons, shown as dots around the O symbol.### Electron Representation:- **Bonds:** - Two single bonds between krypton and each of the fluorine atoms. - Two double bonds between krypton and each of the oxygen atoms.- **Lone Pairs:** - Each fluorine atom has six electrons (three lone pairs). - Each oxygen atom has four electrons (two lone pairs).### Overall Structure:The diagram visually represents the electron sharing and distribution around the krypton atom, illustrating the molecular geometry of the \(\text{KrF}_2\text{O}_2\) molecule.

The structure of the molecule given is as shown below. From the above structure we can see that the central atom is Kr with 1 lone pair electrons remaining on it. And the central atom Kr is making 4 sigma and 2 pi bonds (double bond is 1 sigma and 1 pi bond) Hence number of hybridised orbitals in Kr = Number of sigma bonds + Number of lone pair electrons = 4 + 1 = 5 Hence the hybridisation of Kr will be sp3d.