Sulfur hexafluoride or SF6 is an inorganic, greenhouse gas. The is non-flammable, odourless, and colourless, and is an excellent insulator. That is a hypervalent octahedral molecule that has actually been an amazing topic that conversation amongst chemistry enthusiasts.
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Henri Moissan found the presence of SF6. Incidentally, he is also the discoverer the fluorine. The standard means of manufacturing SF6 is to disclose S8 to F2. This an approach causes the formation of a few sulfur fluorides, but those deserve to be eliminated through heating and then making use of NaOH to eliminate any additional SF4 molecules.
SF6 can not be used instantly after synthesis. It needs to it is in purified to get rid of all reactive fluorides. After ~ that, it requirements to go with pyrolysis.
Here in this blog post, us will learn the Lewis structure of SF6 and also its link angles, molecular geometry and shape that can aid us recognize the physical properties the this molecule.
|Name the molecule||Sulphur Hexafluoride ( SF6)|
|No that Valence electrons in the molecule||48|
|Hybridization that SF6||sp3d2 hybridization|
|Bond Angles||90 degrees|
|Molecular Geometry that SF6||Octahedral|
SF6 Valence Electrons
To determine the Lewis structure of any type of molecule, we an initial need to understand the total number of valence electrons. Below we will find out the total number of valence electrons because that SF6 by adding the valence electrons for both Sulfur and Fluorine atoms.
Total variety of valence electrons in SF6 – Valence electron of Sulfur + Valence electron of Fluorine
Sulfur has actually six valence electrons.
Fluorine has actually seven valence electrons, yet as over there are six Fluorine atoms in this molecule, we will multiply this number by 6.
= 6 + 7*6
= 6 + 42
= 48 valence electrons
Thus SF6 has 48 valence electrons that will aid us draw the Lewis Dot structure of SF6.
SF6 Lewis Structure
The Lewis Dot framework of any type of molecule is a photographic representation that the atoms connected in forming the structure and also its individual valence electrons. This structure helps us know the shortcut formations in the molecule and the arrangement of electron in it.
Sulphur atom will certainly take the central position as it is less electronegative 보다 Fluorine. So ar it in the centre and also all Fluorine atoms about it favor this:
Fluorine atom requirements only one valence electron to finish its octet. Together every atom complies with the octet ascendancy to achieve a secure structure, the Fluorine atom will share one valence electron that the Sulphur atom. Thus, Sulphur will certainly share 6 of the valence electrons through all the fluorine atoms that an outcome in developing six single bonds in between S and also F.
In Lewis Structure, we show the bonds in the framework by drawing a directly line in between two atoms. So every these bonds will certainly take increase 12 valence electrons out of 48.
Place all the continuing to be valence electrons around the Fluorine atoms and check if the octets of every the fluorine atoms room complete.
Once you carry out that, you will see valence electrons in the external shells of every Fluorine atoms, yet Sulphur has an ext than 8 electrons in its external shell. This is due to the fact that it is an exemption to the octet function and can expand its orbital to accommodate more electrons.
Hence, this is the appropriate Lewis framework of SF6.
Now the we understand the Lewis framework of SF6, we can now determine the atoms’ hybridization in the molecule. Here as Sulphur is sharing its electrons through the Fluorine atoms, we will certainly look in ~ its hybridization.
The digital configuration the SF6 in its ground state is 3s23p4. Yet when it share electrons and is in the excited state the electron pairs in both 3s and 3p orbitals gain unpaired. These electrons move to fill the higher vacant 3d orbitals. As a result, six hybrid orbitals are created ( one of 3s, three of 3p, and also two 3d). These hybrid orbitals are the ones that accommodate the mutual electrons. These orbitals overlap with the 2p orbitals the the fluorine atom when Sulfur and Fluorine atoms form bonds. These six orbitals are in the 6 directions the the octahedron shape.
Hence, Sulfur Hexafluoride has sp3d2 hybridization.
SF6 shortcut angle
As Sulphur shares its valence electrons v 6 Fluorine atoms, we have the right to see that all six electrons that the Sulphur atom are common to type bonds. The bond edge of F-S-F is 90 degrees.
SF6 molecule Geometry
When we look at Sulphur Hexafluoride molecule, Sulphur is in the central position through the fluorine atom arranged symmetrically about it. The atom are inserted in the octahedral pattern, which makes the molecule geometry of SF6 is octahedral.
Looking in ~ the molecule geometry of the molecule, we deserve to say that the SF6 molecule has actually an octahedral shape as it has actually eight sides. However, the central atom binding with 6 Fluorine atoms, the shape of SF6 is octahedral.
Is SF6 polar or nonpolar?
SF6 is a nonpolar molecule. This is due to the fact that the VSEPR theory states that once six fluorine atoms are arranged symmetrically approximately the sulfur atom, the link dipoles room cancelled. Together a result, that is a nonpolar molecule.
It also has the same properties together non-polar molecule such together being non-soluble in water and also being soluble in non-polar essential solvents.
To summarize this write-up we have the right to say that in the Lewis dot framework of SF6, all the valence electrons are used up which outcomes in forming six single bonds in between S-F through no lone pairs of electrons.
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The hybridization of Sulphur in this molecule is sp3d2 with the bond angle of 90 degrees.