topic 3: redox I
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what is oxidation
electron loss
what is reduction
electron gain
what is the rules for assigning oxidation numbers
• all uncombined elements have an oxidation number of zero • the oxidation numbers of the elements in a compound add up to zero • the oxidation number of a monoatomic ion is equal to the ionic charge • in a polyatomic ion (CO3 2-) the sum of the individual oxidation numbers of the elements adds up to the charge on the ion • several elements have invariable oxidation numbers in their common compounds. Group 1 metals = +1 Group 2 metals = +2 Al = +3 H = +1 (except in metal hydrides where it is –1 eg NaH) F = -1 Cl, Br, I = –1 except in compounds with oxygen and fluorine O = -2 except in peroxides (H2O2 ) where it is –1 and in compounds with fluorine
how can oxidation number of an element with various oxidation numbers be represented
roman numerals
what is the reducing agent
electron donor
what is the oxidising agent
electron acceptor
what is the product when an acid and metal react
salt + hydrogen
what is disproportionation
a reaction where the same species is oxidised and reduced simultaneously
what is used to balance H atoms
H+
what is used to balance out the O
H2O
what is used to balance the oxidation number
electrons