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Samenvatting Chemie Overal vwo 4 - H3
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Samenvatting scheikunde vwo 4 - H3; moleculaire stoffen
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Scheikunde samenvatting - H3Naamgeving moleculaire stoffen:
Voorvoegsel om index weer te geven + naam atoomsoort + eindigt op -ide
Lewisstructuur = alle atoombindingen worden getekend en ook de valentie-
elektronen die geen binding vormen.
Atoombinding (in moleculen):
• Apolaire binding = gemeenschappelijk elektronenpaar bevindt zich even ver van
beide atomen.
• Polaire binding = binding waarbij ene atoom harder trekt aan elektronen waardoor
ene atoom beetje negatief wordt en andere atoom beetje positief.
• Elektronegativiteit = maat voor kracht waarmee atoom elektronen van
atoombinding aantrekt.
• Verschil in elektronegativiteit is ≤ 0,4: binding is apolair.
• Verschil in elektronegativiteit tussen 0,4 - 1,7: binding is polair.
Vanderwaalsbinding (tussen moleculen) = binding tussen moleculen.
• Hoe groter molecuulmassa, hoe sterker vanderwaalsbinding, hoe hoger smelt- en
kookpunt.
• Bij groter contactoppervlak tussen moleculen wordt vanderwaalsbinding sterker.
• Altijd aanwezig in vloeibare en vaste fase.
Dipool-dipoolbinding = binding, naast vanderwaalsbinding, tussen dipoolmoleculen
(= moleculen met ladingsverdeling door polaire atoombinding).
Waterstofbrug = binding tussen NH- en of OH-groepen.
• Waterstofbrugontvangende groepen: C=O
Polaire stoffen lossen goed op in polaire oplosmiddelen;
Apolaire stoffen lossen goed op in polaire oplosmiddelen.
Wet van Avogadro = bij constante temperatuur en druk bevatten gelijke volumes van
verschillende gassen evenveel moleculen en dus evenveel mol.
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