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Therefore your structure may include a nitrogen oxygen double bond, a positive formal charge on nitrogen and a negative formal charge at each of the singly bound oxygens. … Better in this case would be molecular orbital theory and or valence bond theory. The molecule itself is a y-aromatic system, the charge is delocalised through the extensive $\pi$ system. …

A quick calculation, DF-BP86/def2-SVP, reveals that the charge of beryllium is $\mathbf{q}(\ce{Be})=0.8$ and of chlorine $\mathbf{q}(\ce{Cl})=-0.4$, based on natural bond orbital analysis. … In quantum chemistry these phenomena are usually very well described by valence bond theory. …

I stated in Is the bond enthalpy of S-O stronger in SO₃ or SO₃²⁻? The bonding picture is usually trivialised as each $\ce{S−O}$ bond being a double bond. … Since each of the $\ce{S-O}$ bond contributes equally to the lowest lying $\pi$ orbital, the bond order is found to be about $1.33$. …

When I did research on the φ bond for What would follow in the series sigma, pi and delta bonds? I came across some predictions about possible φ bond in the ground state. … It should be clarified that a quadruple bond does not necessarily mean that a δ bond is involved. …

That results that the $\ce{C-C}$ bond is composed from $\ce{sp^{2.3} C}$ orbitals. … Since the $\ce{s}$-character in the $\ce{C-C}$ bond in hexachloroethane is much higher than in ethane, the bond length is expected to be shorter. …

I can only repeat myself here: Polarity is an ill-defined concept that has a nice potential for confusion. In most cases, when specifying a molecule as polar, one is colloquially referring to the pres …

A bond can only exist, if it needs energy to break it, i.e. the bond dissociation energy is always positive. … heterolytic bond dissociation energy). …

Hypervalency is an obsolete concept - it was used to explain bonding situations of molecules, that seem to exceed the octet rule. It was accomplished by the help of $\ce{spd}$ hybrid orbitals. It is n …

The crystal structure of metamizole can be found in Acta Cryst. (1979). B35, 612-615. It is also available via the ​Cambridge Crystallographic Data Centre (CCDC) database, entering the DOI: 10.1107/S0 …

The bonding picture is usually trivialised as each $\ce{S-O}$ bond being a double bond. … However, the $\ce{S-O}$ bond in sulfurtrioxide is still stronger and shorter, than in the sulfite anion. …

Due to delocalisation the carbon-carbon bond is significantly shorter than a normal single bond. The right hand side orbitals are taken from a DF-BP85/def2-SVP calculation. …

There is a class of compounds, called carbodiphosphoranes, which formally has a divalent carbon (0) central atom. Employed as a ligand it acts as a sigma and pi donor. This capability is also one of t …

As always, writing a Lewis structure seems to be a trivial task, but sometimes it just isn't. The smaller the molecule becomes, more often than not the bonding situation becomes more complicated and c …

There are quite a few programs out there that let you build ball and stick models of compounds using tabulated bond lengths. … Here is a model of the 3D structures with the hydrogen bond measured. For ortho-fluorophenol it is 2.25 Å and for ortho-nitrophenol it is 1.73 Å. You can see a clear difference already. …

Since Dissenter asked in the comments to my answer: I'm not sure why the $\ce{F_{eq}-S-F'_{eq}}$ bond angles would be compressed, even if the $\ce{S}$ were out of the plane. …