Linked Questions

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Why is Sulfur Trioxide has SP² hybridization? [duplicate]

When I google what is the type of hybridization in SO₃ it gives me "SP² hybridization". The problem I have is why does it has the above hybridization when it has 3 double bonds with the ...
donthababakka's user avatar
61 votes
2 answers

Striking examples where Kohn-Sham orbitals clearly have no physical meaning

In Density Functional Theory courses, one is often reminded that Kohn-Sham orbitals are often said to bear no any physical meaning. They only represent a noninteracting reference system which has the ...
F'x's user avatar
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28 votes
3 answers

What is Y-aromaticity? Is the trinitromethanide anion aromatic?

The wikipedia article on trinitromethane claims that: There is some evidence that the anion (which obeys the $4n+2$ Hückel rule) is aromatic. Unfortunately the citation is behind a paywall so I ...
bon's user avatar
  • 15.4k
16 votes
3 answers

Is the S–O bond strength in sulfur trioxide or sulfite anion larger?

Can you please explain the difference between the bond enthalpies in sulfurtrioxide $\ce{SO3}$ and the sulfite anion $\ce{SO3^{2-}}$?
sanja's user avatar
  • 169
34 votes
2 answers

Hypervalency and the octet rule

I realize that the octet rule is more a suggestion than a rule, and that it applies mainly to non-transition metal compounds. Still, compounds that don't have an octet, like $\ce{BH3}$, tend to ...
ron's user avatar
  • 85k
19 votes
1 answer

What is the hybridization of the carbonyl oxygen in a carboxylic acid?

My professor sent out a review guide. One of the questions on this guide is The carboxylic acid carbonyl oxygen is: 1. $\ce{sp^2}$ 2. $\ce{sp^3}$ 3. $\ce{H}$-bond donor 4. rapidly ...
user15750's user avatar
  • 191
14 votes
1 answer

Delocalization of π-electrons in nitrate ion

Benzene and nitrate ion are given in my textbook as examples for the delocalization of π-electrons. Benzene, due to symmetry of its resonating structures, is simple enough. We assume that σ-electrons ...
Gerard's user avatar
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8 votes
3 answers

Why is there a need for resonance?

Why are we able to show structures of compounds with different position of electron, but with same position of them? Shouldn't the structure become unstable due to this? Let's take benzene for the ...
pcforgeek's user avatar
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4 votes
3 answers

How is sulphur trioxide formed and why is it stable? [duplicate]

Structure of $\ce{SO3}$ (sulfur trioxide): In the molecule, if each oxygen atom shares two electrons with sulfur atom then how does the sulfur atom remain stable? It already has 6 valence electrons ...
Hark's user avatar
  • 239
7 votes
1 answer

Which d orbitals of sulfur take part in the pi bonds of SO3?

In $\ce{SO3}$, 2 $p\pi-d\pi$ bonds are present. But which $d$ orbitals of sulfur take part in these $\pi$ bonds? The answer says $d_{xy}$ and $d_{yz}$. Someone also told me that crystal field ...
user avatar
3 votes
1 answer

Reason for shorter bond between sulphur and oxygen?

I recently came across this sentence in my textbook: the bonds between sulphur and oxygen in oxides of sulphur ($\ce{SO2}$ and $\ce{SO3}$) are much shorter than might be expected for a single bond. ...
Chemist's user avatar
  • 531
0 votes
1 answer

Why is there a lone pair in thionyl fluoride?

Why is there a lone pair in $\ce{SOF2}$? I drew its structure, which according to me should look like this: Why is there a lone pair on sulfur? Isn't its octet complete? If yes, why should it expand ...
kushal's user avatar
  • 111
3 votes
0 answers

Can the Lewis dot structure of SO2 be experimentally verified?

I have just watched 2 different videos on the Lewis dot structure of sulfur dioxide, $\ce{SO2}$. One says it is $$\ce{O=S=O}$$ and the other says $$\ce{^-O-S^+=O <-> O=S^+-O-}$$ The first ...
G Smith's user avatar
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