2. Oxidation, Reduction, and Redox Reactions
No description yet. This curated deck is ready for daily study.
Card preview (11)
Oxidation Definition:
• loss of e- • (oxidation state increases)
Reduction Definition:
• Gain of e- • (oxidation state increases)
Reducing Agent Definition:
• e- donor (loses e-) • a reduding agent is itself oxidised
Oxidising Agent Definition:
• e- acceptor (gains e-) • an oxidising agent is itself reduced
What occurs in a redox reaction?
oxidation and reduction take place together
Rules for finding oxidation states:
• uncombined elements/diatomic molecules have an oxidation state of 0 • sum of all the oxidation states in a compund is 0 • oxidation state of a simple ions is equal to its charge • sum of all the oxidation states in a complex ion is equal to its charge
If a substance is oxidised, the oxidation state …
increases
if a substance is reduced, oxidation state ..
decreases
Rules for balancing half equations:
• Balance the main atom (not H or O) • Balance O using H2O • Balance H using H+ • Balance charges using e- (add more to positive side)
Rules for combining half equations:
• multiply 1 or both half equations until they both contain the same number of e- • add the reactants from both half equations together • add the products from both half equations together • cancel out the e-
What occurs in a disproportionation reaction?
1 atom is both reduces and oxidised