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Samenvatting Chemie Overal vwo 5 - H11
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Samenvatting scheikunde vwo 5 - H11; redoxreacties
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Scheikunde samenvatting - H11Redoxreactie = reactie waarbij elektronenoverdracht plaatsvindt.
• Oxidator: neemt elektronen op
• Reductor: staat elektronen af
Onedel metaal > sterke reductor
Edelmetaal > zwakke reductor
Redoxkoppel = bij elkaar horend oxidator-reductorpaar (bv: Ag en Ag⁺).
• Geconjugeerde reductor = Ag-atoom
• Geconjugeerde oxidator = Ag⁺-ion
Standaardelektrodepotentiaal = V₀ = maat voor sterkte van oxidator in redoxkoppel.
• Hoe hoger V₀, hoe sterker oxidator en hoe zwakker reductor.
• Aflopend: ΔV₀ = V₀(ox) - V₀(red) ≥ 0,3 V
• Evenwicht: -0,3 V < ΔV₀ < 0,3 V
• Geen reactie: ΔV₀ ≤ -0,3 V
Stappenplan redoxreactie opstellen:
1. Schrijf alle deeltjes op.- Bij oplossingen is H₂O zowel oxidator als reductor.
2. Bepaal de sterkste oxidator en reductor m.b.v. tabel 48.
3. Bepaal of reactie wel of niet, en hoe die verloopt (ΔV₀).
4. Stel halfreacties op.
5. Maak elektronen kloppend.
6. Tel beide halfreacties op.- e⁻ weglaten in totaalreacties.
Uitzonderingen op Binas tabel 48`;
• HSO₄⁻ en SO₄²⁻ zijn alleen oxidator in geconcentreerd zwavelzuur.
• Bij verdund salpeterzuur ontstaat NO(g), bij geconcentreerd salpeterzuur ontstaat
NO₂(g).
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