How does SF6 exist?

Sulfur hexafluorideIn the SF6 molecule, the central sulfur atom is bonded to six fluorine atoms, so sulfur has 12 bonding electrons around it. For atoms in the fourth period and beyond, higher d orbitals can be used to accommodate additional shared pairs beyond the octet.

Why SF6 is known and SH6 is not known?

sf6 exist because electronegativity of fluorine is most high, it is of small size and high polarising power but it is not possible in SH6.

Why SH4 is not possible?

The reason that they do not exist (or at least are not the most stable form) is because the decomposition reaction is exothermic.

Why OF6 does not exist but SF6 exist?

(i) SF6 exists but OF6 does not because oxygen does not has vacant d-orbitals in the valence shell. Electrons are oxygen cannot be excited to higher levels to six unpaired electrons. In ‘S’ it is possible to do so as it has vacant d-orbital.

Which of the following do not exist SH6?

Answer: In this question, does not exist because when bonding with 6 Hydrogen’s, the oxidation number of S would be -6, which is impossible for the Sulfur atom.

Why does SF4 exist but not OF4?

Unfortunately, valence shell of oxygen is 2nd shell where there is no d orbital. So, oxygen can’t extend its covalency to 4. Hence, it can’t form OF4. But SF4 exists, as S has 3d orbitals.

Does SH4 exist?

Thus SH4 does not exist but SF4 does. As sulfur belongs to group 16 in periodic table, its electronic configuration is ns²np⁴, it can show +2,+4 , +6 and -2 oxidation state.

Which of the following does not exist SH6?

Which of the following does not exist OF6?

SF6 exist not OF6.

Which of the following species does not exist SF6 SH6?

Hydrogen is a very weak oxidizing agent as compared to fluorine this means that hydrogen is not able to oxidise sulphur to its maximum oxidation state. Hence, $S{{H}_{6}}$ does not exist.

Why bf6 3 does not exist?

Boron does not have d orbital in its valence shell. Hence, Maximum covalency of boron can not exceed 4.

Why SH6 does not exist in nature?

Expert Answer: Fluorine is the strongest oxidising agent and hydrogen is a weakest oxidising agent. Therefore, fluorine oxidises sulphur to its maximum oxidation state of +6 whereas hydrogen cannot oxidise S to its maximum oxidation state of +6. Hence SH6 does not exist.

Why is excitation not possible in SF6 and SH6?

In SF6, Oxidation state of ‘S’ is +6 hence its size is small and terminal atoms are more electro-negative So, excitation of electrones to ‘d-orbital’ is possible. But in ‘SH6’, Oxidation state of ‘S’ is -6. So,its size is large and terminal atoms are also not more electronegative. So, excitation is not possible. Hence,It do not exist.

Why do compounds like SF6 and SF4 not exist?

There are other reasons why compounds do not exist. The shapes of SF6 and SF4 are explained by invoking use of d orbitals on sulfur (d2sp3 orbital hybridization gives the octahedral shape of SF6 and explains the square planar shape of SF4, with two lone pairs occupying axial positions).

What is the hybridisation of hydrogen in SH6?

This hybridisation is brought up by high electronegative surrounding atoms such as chlorine and flourine. In SH6, hydrogen is not a high electronegative element and thus hybridisation is not possible. Thus Hydrogen can’t combine with sulphur to form SH6 and this compound is non existent.