Hence, Sulfur Hexafluoride has sp3d2 hybridization. These six orbitals are in the six directions of the octahedron shape. These orbitals overlap with the 2p orbitals of the fluorine atom when Sulfur and Fluorine atoms form bonds. These hybrid orbitals are the ones that accommodate the shared electrons. As a result, six hybrid orbitals are formed ( one of 3s, three of 3p, and two 3d). These electrons move to fill the higher vacant 3d orbitals. But when it shares electrons and is in the excited state the electron pairs in both 3s and 3p orbitals get unpaired. The electronic configuration of SF6 in its ground state is 3s23p4. Here as Sulphur is sharing its electrons with the Fluorine atoms, we will look at its hybridization. Now that we know the Lewis Structure of SF6, we can now determine the atoms’ hybridization in the molecule. Hence, this is the right Lewis structure of SF6. This is because it is an exception to the octet role and can expand its orbital to accommodate more electrons. Once you do that, you will see valence electrons in the outer shells of all Fluorine atoms, but Sulphur has more than 8 electrons in its outer shell. Place all the remaining valence electrons around the Fluorine atoms and check if the octets of all the fluorine atoms are complete. So all these bonds will take up 12 valence electrons out of 48. In Lewis Structure, we show the bonds in the structure by drawing a straight line between two atoms. Thus, Sulphur will share six of its valence electrons with all the fluorine atoms that result in forming six single bonds between S and F. As every atom follows the octet rule to attain a stable structure, the Fluorine atom will share one valence electron of the Sulphur atom. So place it in the centre and all Fluorine atoms around it like this:įluorine atom needs only one valence electron to complete its octet. Sulphur atom will take the central position as it is less electronegative than Fluorine. This structure helps us know the bond formations in the molecule and the arrangement of electrons in it. The Lewis Dot structure of any molecule is a pictorial representation of the atoms involved in forming the structure and its individual valence electrons. Thus SF6 has 48 valence electrons that will help us draw the Lewis Dot Structure of SF6. Total number of valence electrons in SF6 – Valence electrons of Sulfur + Valence electrons of Fluorineįluorine has seven valence electrons, but as there are six Fluorine atoms in this molecule, we will multiply this number by 6. Here we will find out the total number of valence electrons for SF6 by adding the valence electrons for both Sulfur and Fluorine atoms. To determine the Lewis Structure of any molecule, we first need to know the total number of valence electrons. Is SF6 polar or nonpolar? SF6 Valence Electrons.
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