Why does SF6 exist but SH6 does not?

Fluorine is most electronegative and Sulfur is electropositive in this particular case so it forms SF6. But SH6 doesn’t exist because hydrogen is electropositive and Sulfur is electronegative.

Why are sf4 and SF6 known but OF4 and OF6 are not?

There are two reasons that you can have SF6 but not OF6: Electronegativity. There’s a large amount of positive charge on sulfur in SF6, and this is possible because of the large electronegativity difference between sulfur and fluorine. There isn’t enough room around an oxygen atom for six fluorine atoms.

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 can a molecule with the structure of OF6 not exist?

Not much electronegativity difference between O and F. The atomic size of Oxygen is not sufficient for it to hold 6 atoms.

Why SF6 is known but sncl4 is not known?

Explanation: Flourine being smaller in size accommodate its six atoms in given space of sulphur while chlorine being bigger in size is not able to accommodate itself due to repulsion between its six atoms. That’s why SF6 is known but SCL6 is not known.

Why SF6 is not easily hydrolysed?

SF6 is not easily hydrolysis because here S atom is surrounded by 6 F atom so it’s complected for H2O to attack SF6 but in case of SF4 here S atom is surrounded by 4F atom so it’s to attack by H2O.

Why can SF4 exist but not OF4?

This clearly indicates that oxygen is small in size and does not possess vacant orbitals to accommodate extra electrons. It can only accept two more electrons. Sulphur, on the other hand is large in size and possesses vacant d-orbitals in its valence shell.

Why is scl4 the highest chloride of sulphur but with fluorine SF6 is formed?

This is due to the difference in size of flourine and chlorine. Flourine being smaller in size accommodate its six atoms in given space of sulphur while chlorine being bigger in size is not able to accommodate itself due to repulsion between its six atoms. That’s why SF6 is known but SCL6 is not known.

Is SF4 possible?

A molecule which can’t exist theoretically is: (A) SF4 (B) OF2 (C) OF4 (D) O2F2? But, Oxygen cannot exhibit valency of 4. Hence, the molecule OF4 is theoretically not possible.

Why is SF6 much less reactive than SF4?

SF4 is asymmetrical and has a lone pair of electrons on the sulphur atom, which can react further. In SF6, all of the electrons are paired, giving great stability to the molecule and reducing its reactivity.

Which of the following does not exist SF4 OF6?

oxygen does not form OF4 or OF6 whereas S forms SF4, SF6.

Which is more stable SF6 or SCL6 Why?

Due to small size of fluorine six F– ion can be accomodated around sulphur whereas chloride ion is comparatively larger in size, therefore, there will be interionic repulsion.

Why SF6 exists but SH6 does not?

SF6 exists but SH6 doesnt , why? 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.

Why does sulfur in SF6 and SF4 have a high oxidation number?

Because sulfur in SF6 and SF4 has a high oxidation number (+6 and +4). This is possible because fluorine is very electronegative and almost exclusively forms compounds in which it has an oxidation number of -1. Hydrogen seldom forms compounds in which it has Ox= -1. It fact it only does that with strongly electropositive elements like Na or K.

Why SH6 does not exist in the periodic table?

Fluorine is most electronegative and Sulfur is electropositive in this particular case so it forms SF6. But SH6 doesn’t exist because hydrogen is electropositive and Sulfur is electronegative.

Is a Lewis dot structure of SF6 possible?

Even OF4 is impossible; there are 2 electrons we can’t account for when trying a Lewis dot structure. This is the actual reason SF6 is possible. I see there’s already an answer invoking d-orbitals. That’s a common misconception, but it is a misconception. Electronegativity.