Sulphur HexaFluoride and its Hybridization according to VESPER Theory

Let's first discuss some properties of SF6:

1.       Its molar mass is 146.06 g/mol^-1.

2.      Its boiling point is -50.8◦C (-59.4F◦, 222.3K).

3.      It is non-flammable.

4.      It is a colorless, odorless, and tasteless gas.

5.      It is an un-reactive gas therefore it is called an inert gas.

6.      It is chemically stable and a highly electronegative gas.

7.      It has an excellent dielectric property of approximately 2.5 times more than air.

8.      SF6 is also a synthetic gas used in electricity industries to keep networks running safely.

9.      It is also a non-toxic gas.

10.   SF6 does not form any other compounds that alter its state of effectiveness.

11.    It is a hypervalent molecule.

12.   SF6 is a non-polar gas because it is quite soluble in non-polar organic solvents. It is poorly soluble in water.

13.   Its density is 6.12g/L at sea level.

14.   Its density is higher than air(1.225 g/L).

15.   Its non-toxic and non-flammable property makes it efficient for circuit breaking.

16.   SF6 is a stable gas and is thermally inert.

17.   SF6 has an excellent insulating property, which is its greatest advantage for circuit breakers.

18.   Its decomposing product is non-explosive so there is no fire risk.

19.   It is five times heavier than air. Therefore, it is one of the heaviest known gas.

20.  SF6 has a strong tendency to absorb free electrons. Therefore, it has high dielectric strength.

21.   SF6 is not a Lewis base.

22.  The molecular geometry of SF6 is octahedral.

23.  SF6 sublimes at -63.9◦C.

24.  Its dielectric constant is 1.00204.

25.  SF6 is an inorganic gas. It is made up of 1 sulphur atom and 6 fluorine atoms.

SF6:

Sulphur hexafluoride involves in AF₆ type( A= S, Te, and Se). In AF₆ type molecules have octahedral geometry which results in the formation of sp3d2 hybridization of the central atom. In SF6 sulphur is the central atom. In determining the type of hybridization sulfur and fluorine atoms are involved.

Let’s do the electronic configuration of the S-atom in the ground state.

S= 3s² 3px² 3py¹ 3pz¹                              

Excited state configuration: 3s¹ 3px¹ 3py¹ 3pz¹ 3pz₂¹ 3p_x2-y2¹

Diagram:

Explanation:

The diagram shows that S-atom is bounded to six F-atom by six S-F sigma bonds and the central atom has no lone pair of electrons on it. Thus in order to explain the formation of six S-F sigma bonds in the SF₆ molecule, 3s, and 3p electrons must be promoted to two 3d orbitals so that S-atom has six unpaired electrons. Now one 3s, three 3p, and two 3d orbitals each of which has one electron mix together and give rise to the formation of six sp³d² hybrid orbitals. These hybrid orbitals are directed toward the six corners of a regular octahedron. These singly filled hybrid orbitals overlap with each of the six singly filled 2px orbitals of F-atom and give six sigma bonds.

It is due to sp³d² hybridization and the absence of any lone pair of electrons on the S-atom that the SF₆ molecule has an octahedral shape. All the six atoms of sulphur will arrange themselves in an octahedral geometry forming a bond angle of 90◦.

Name of compound	Sulphur hexafluoride(SF6)
Electron Pair	6
Bond Pair	6
Lone Pair	0
Geometry	Octahedral
Bond Angle	90◦
Hybridization	Sp3d2

Also, read about the following:

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