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Lewis Acid/Base Interaction Matrix Database


Type 6 Lewis Acid/Base Complexation Chemistry

Ionic Salts
Bonding: Type 6 complexes are, in Pearson-Klopman HSAB terms, classic hard/hard complexes which give rise to charge-controlled ionic salts.
Charge: The charge on a Type 6 complex is always neutral.
Chemistry:

In polar solvents species dissociate to give independently solvated ions. While in solution, the complex anion part of a Type 6 complex is susceptible to ligand transfer or substitution. The s-LUMO ion part of the complex usually acts as a spectator ion, however, choice of ion influences solubility.

Reagents such as lithium aluminium hydride and sodium borohydride act as hydride ion donor complexes. Type 6 hydride complexes are weaker proton abstracters than the very basic Type 5 complexes and they are correspondingly more suitable for use by organic chemists as sources of reducing nucleophilic hydride ion:

Congeneric Series:

Many important ligand replacement congeneric series are known, for example:

Type 6 Lewis acid/base complex (generic)
Beryllium silicate

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Borax

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Calcium tungstate

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Lithium aluminium hydride

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Lithium borohydride

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Lithium tri-tert-butoxy aluminium hydride

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Pentasulfide dianion

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Potassium aluminium hydride

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Potassium borohydride

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Potassium buckide

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Potassium dichromate(VI)

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Potassium hexachloro platinate

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Potassium manganate(V)

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Potassium manganate(VI)

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Potassium nitrate

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Potassium perbromate

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Potassium perchlorate

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Potassium rhenium nonahydride

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Potassium tetrachloroplaninate(II)

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Sodium aluminium hydride

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Sodium argentocyanide

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Sodium aurocyanide

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Sodium borohydride

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Sodium chromate

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Sodium cyanoborohydride

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Sodium dichromate

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Sodium hexafluoroaluminate

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Sodium hexafluorosilicate

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Sodium perchlorate

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Sodium tetrafluoroborate

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Tetrasulfide dianion

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Trisulfide dianion

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Zeise's salt

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