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Samenvatting les 18 - De coördinatieve binding
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Deze samenvatting omvat: complexen - felle kleuren en vreemde eigenschappen De coördinatieve binding Valence Bond theorie voor complexen
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De coördinatieve binding1. Complexen - felle kleuren en vreemde eigenschappen
● grosso modo (che v overgangsmetalen) = elementen met lege of niet volledige d-orbitalen
● Gedragingen die niet verklaard kunnen w vanuit de conventionele scheikundige modellen
● Meest voorkomende gedragingen:
○ absorberen uv zichtbaar licht (ze zijn dus gekleurd)
○ volgen een niet-conventionele stoichiometrie
○ overgangsmetalen = zeer goede redox-katalysatoren
○ sommige verbindingen v overgangsmetalen zijn stabiel
● Grote gemeenschappelijke factor waarop alle modellen steunen = aanwezigheid v d-e– (of
f-e– vr hogere rijen)
● Alle eig v complexen kunnen verklaard w vanuit de distributie vd e– v
overgangsmetaalionen en hun interactie met liganden
2. De coördinatieve binding (definitie)
● = een binding waarbij een elektronenrijk ligand twee e– doneert in de lege d-orbitalen ve
overgangsmetaal
● = donor-acceptor binding
3. De Valence Bond theorie voor complexen
● complexen ontstaan door gecoördineerde covalente bindingen met lege bindende
metaalorbitalen
● Geometrie w bep door de hybridisatie vd lege metaalorbitalen
● Meest courante hybridisaties
Coördinatie Nr Hybridisatie Basis Oriëntatie
(CN)
2 sp Lineair
3 sp2 Trigonaal planair
4 sp3 Tetraëdrisch
dsp2 Vlak planair
5 d3sp of dsp3 Trigonale bipyramidaal
6 d2sp3 of sp3d2 Octaëdrisch
zie pg 284-286 voorbeelden
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