Vinculum chemicum

Vincula chemica formando novae substantiae creantur. Exempli causa duae quantitates hydrogenii plus una oxigenii dant duas aquae (sive oxidi dihydrogenii). In quaque molecula aquae duo vincula habemus, una inter quoque hydrogenium et illud oxygenium.

Vinculum chemicum(-i, n.) est quaedam electronum communicatio quae atomos in moleculas unit. Haec notio (de per electronum communicationem atomos uniendo), e mechanica quantica deducta, hodie in axiomatica scientiae chemicae notione constat.

Species vinculi inter atomos

Exemplum vinculi covalentis inter carbonia. Inter carbonia sunt duo vincula speciei σ et π.

Inter duas atomos sunt tres vinculi chemici species, quae discrepant secundum eorum virium magnitudinem: covalens apolare, convalens polare, et ionicum. Forma vinculi dependet a differentia inter atomorum electronegavitates. Si differentia est maior, deinde onus electricum distincte ab alia atomo propius ad alteram commovetur. Si differentia est maxima, onus electricum absolute ab alia ad alteram commovetur et deinde atomi onus affixae dicuntur ionta.

Vinculum covalens apolare

Vincula covalentia creantur si differentia electronegavitatium inter atomos est minus quam 2.1 (secundum formulam electronegativitatis Pauling). Et si differentia est minus quam 0.5, vincula covalentia dicuntur apolaria. Exempla vinculi covalentis apolaris sunt vincula inter carbonium et hydrogenium in methano.

Vincula metallica et semimetallica, sicut in metalles et semimetalles, sunt species vinculi covalentis apolaris specialis ubi electrones inter milles atomorum aequaliter partitur. Vincula aromatica eadem sunt sed, ut in benzene, sunt inter manum atomi.

Vinculum covalens polare

Vincula covalentia dicuntur polaria si differentia electronegavitatium inter atomos vinculum formandas est aequalis aut maior quam 0.5 et minus quam 2.1. Exempla vinculi covalentis polaris sunt vincula inter oxygenium et hydrogenium in aqua et vincula inter ferrum et duos anulos aromaticos in ferroceni (C₅H₅-Fe-C₅H₅).

Vinculum ionicum

Vincula ionica inter atomos creantur si differentia electronegativitatium est aequalis aut maior quam 2.1. Quamquam in vacuo vincula ionica fortior quam covalens esse potest, in aquato inbecillior generaliter sunt, quis omne ion moleculas aquae ad se attrahit, tantum ut onus suum et vim electrostaticam inter ionta attenuat. Exempla vinculi ionici sunt vincula in chlorido natrii et hydroxido kalii.

Species vinculi inter moleculas

Sunt duae species vinculi inter moleculas principales: hydrogenica et van der Waals. Vincula harum specierum saepe non chemica sed physica esse dicuntur.

Vinculum hydrogenicum

Exemplum vinculi hydrogenici inter duas moleculas aquae.

Hydrogenica appellantur vincula inter moleculas quae hydrogenium habent atomis eius altae electronegativitatis affixum, ita ut e molecula proton exponatur(i.e., forma ionica hydrogenii) . Exemplum maximi momenti est aqua, in quo hydrogenium ad oxygenium affixum est. Oxygenium negativum uni moleculae adfixum attrahit hydrogenium positivum alterae moleculae affixum, et vice versa. Hic attractus inter moleculas multas proprietates aquae explicat praesertim congregrationem moleculae aquae ut status eius fluidus solidusque formetur.

Vinculum van der Waals

Vincula van der Waals, imbellissimae formae vinculi inter moleculas pro Iohanne Diderik van der Waals appellatae, sunt ob interactiones electrostaticas quae in polare molecularum constitutione dependent.

Moleculae nuncupantur polares si onus electricum negativum a positivo in eis separatum est super totam moleculam in promedio. Quantitas polaritatis est mensura eiusdem orta ex illius quantitate oneris separati et distantia separationis coniunctim.

Secundum Iacobum Israelachvili sunt quattuor formae virium van der Waals: vis Keesom operat solum quando ambae moleculae sunt polares, vis Debye operat quando quam minime una ex duabus moleculis est polaris et vis London semper operat vel quando neutra molecula est polaris, ob fluctuationum dipolarum quanticarum causam. Vis London quoque sicut vis Casimir scitur quando ea inter laminas metallicas operat.

Fontes

Pagina Latinata est ex en:Chemical bond, en:Covalent bond,en:Hydrogen bond,en:van der Waals' forces, 11 Martii 2007.
Israelachvili, Jacob N. 1992. Intermolecular and Surface Forces. 2nd ed. Academic Press, Elsevier, Ltd. ISBN 0-12-375181-0.

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