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Molecular orbital studies at the ab initio level implicate (nN →σ*C-N) type interactions between a lone pair on N and an antiperiplanar σ* orbital of the adjacent C-N bond as being responsible for the anomeric effect [9].
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In all cases, the % desorption is high at pH 1.2 and this could be attributed to the reaction between H+ and a lone pair of electrons in both the secondary amine groups of the adsorbent and the tertiary nitrogen of RhB.
The PGB then donates a lone pair of electrons to the carbon.
NH3 is a polar molecule, and there exists a lone pair of electrons in its electronic structure.
A-H + B: A − + B-H+ In this representation both the base, B, and the conjugate base, A−, are shown carrying a lone pair of electrons and the proton, which is a Lewis acid, is transferred between them.
Quinclorac is another example of an active auxin exhibiting a depletion of ring electron density due to a Cl and a lone pair on the N atom.
It is based on the similarity in volume between an electronic lone pair and oxide or fluoride anions, and on the vacancy created by the replacement of a lone-pair by a non-lone-pair cation.
Thus, the socket property is obtained by boron atoms introduced in the graphene matrix, while the plug property is offered by a lone-pair of the molecular adsorbate.
spectra of mixture model compounds suggests that this polar interaction belongs to an n π* interaction between the lone pair electrons of the N-atoms in the s-triazine ring and the π*-orbital of the phenylene rings neighbouring to the sulfone linkage.
The existence of intermolecular NH⋯Cl hydrogen bonds due to the interaction between the lone pair of oxygen with the antibonding orbital was established by NBO analysis.
These results show that the hyperconjugation between the lone pair orbitals of oxygen as donors and some σ * or π * orbitals as acceptors can occur.
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