Summary
Summary IEB Chemie B: Chemiese Bindings
Hierdie dokument is deur 'n Fisiese Wetenskappe onderwyser opgestel vir klasgee doeleindes. Dit volg die IEB se SAGs en brei op dit uit.
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IEBChemie
B: Chemiese Bindings
1. Intramolekulêre Bindings
Wanneer sekere atome aan mekaar bind, vorm hulle nuwe bindings met nuwe eienskappe
(Bv. Na is ’n baie vlugtige element wat ’n baie erge reaksie met water toon, terwyl Cℓ ’n baie
giftige nie-metaal is, wat gebruik word om mikro-organismes in swembadwater te vernietig,
maar saam maak dit tafelsout).
Die manier hoe elemente saambind, hang van baie eienskappe van die elemente af.
Intramolekulêre bindings is hoe elemente met mekaar bind om molekules/verbindings te
vorm.
Makliker manier om die bindings te onderskei:
Nie-metaal x nie-metaal → kovalente bindings
Nie-metaal x metaal → ioniese bindings
Metaal x metaal → metaalbindings
Die tipe binding wat vorm, hang ook af van die verskil tussen die elektronegatiwiteit van die
elemente wat bind.
Elektronegatiwiteit = mate van die neiging van ’n atoom om ’n bindingspaar elektrone aan
te trek.
Kovalente binding
- Dit is die deling van ten minste een paar elektrone tussen twee atome van nie-
metale
2 Tipes:
- Nie-polêre kovalente (suiwer kovalente) binding.
o Kan bepaal word deur die verskil tussen elektronegatiwiteit < 0,9
o Hier is ’n gelykopdeling van elektrone
- Polêr kovalente binding
o Verskil tussen elektronegatiwiteit ≥ 0,9 of ≤ 2
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