oxidation, reduction and redox equations (3.1.7) in papers 1 & 2
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what is oxidation?
• the loss of electrons • shown through the increase in oxidation number.
what is reduction?
• the gain of electrons. • shown through the decrease in oxidation number.
what is an oxidising agent?
• the species that gains electrons, they get reduced in the process.
what is a reducing agent?
• the species that looses electrons, they get oxidised in the process.
whats the oxidation state of group 1, 2 metals, almunium, oxygen, hydrogen, fluorine, chlorine.
• group 1: +1 • group 2: +2 • Al: +3 • O: -2 except in peroxides & F its -1 • H: +1 except in metal hydrides its -1 • F: -1 • Cl: -1 except with O & F
how do you write half equations in acidic solutions?
• balance all the atoms except hydrogen and oxygen. • balance the oxygens by adding h2o to the side with least amount. • balance the hydrogens by adding H+ ions to the side with the least amount. • balalnce charges by adding electrons to the side with the H+ ions.
what are disproportionation reactions?
• when species are both oxidised and reduced.