(a)
Interpretation:
The unbalanced oxidation and reduction half-reactions for the reaction
Concept introduction:
Oxidation is the loss of one or more electrons from a substance which is indicated by an increase in oxidation number and reduction is gain of one or more electrons from a substance which is indicated by a decrease in oxidation number.
By comparing the oxidation number of an atom before and after a reaction, it can be predicted whether the reaction is
There are some rules for assigning oxidation numbers to atoms.
- In the elemental state, an atom has zero oxidation number.
- The oxidation number of monoatomic ions is equal to its charge
- In a polyatomic ion, atom usually has the same oxidation number as it has in the monoatomic ion.
- The sum of the oxidation number of polyatomic ions is equal to its net charge while zero for neutral compounds.
(b)
Interpretation:
The unbalanced oxidation and reduction half-reactions for the reaction
Concept introduction:
Oxidation is the loss of one or more electrons from a substance which is indicated by an increase in oxidation number and reduction is gain of one or more electrons from a substance which is indicated by a decrease in oxidation number.
By comparing the oxidation number of an atom before and after a reaction, it can be predicted whether the reaction is oxidation or a reduction reaction.
There are some rules for assigning oxidation numbers to atoms.
- In the elemental state, an atom has zero oxidation number.
- The oxidation number of monoatomic ions is equal to its charge
- In a polyatomic ion, atom usually has the same oxidation number as it has in the monoatomic ion.
- The sum of the oxidation number of polyatomic ions is equal to its net charge while zero for neutral compounds.
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CHEMISTRY-TEXT
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