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Elza [17]
2 years ago
8

In the reaction shown,

Chemistry
1 answer:
exis [7]2 years ago
8 0

Answer:

Ni (s) is oxidized because it loses electrons. This makes it the reducing agent.

CuCl₂ (aq) is reduced because it gains electrons. This makes it the oxidizing agent.

Explanation:

In the reaction:

Ni(s) + CuCl₂(aq) → Cu(s) + NiCl₂(aq)

Ni (s) is oxidized because it loses electrons. This makes it the reducing agent.

------------> Ni (s) has an oxidation number of 0. All lone atoms (that are not ions) have a 0 oxidation number.

-------------> In NiCl₂ (aq), chlorine must have an oxidation number of -1, and because there are two chorine atoms, they contribute a total -2 charge. To make the overall charge neutral, nickel must have an oxidation number of +2 to balance the charges.

--------------> Because nickel goes from an oxidation number of 0 to +2, this indicates that it lost electrons and was reduced.

CuCl₂ (aq) is reduced because it gains electrons. This makes it the oxidizing agent.

-------------> In CuCl₂ (aq), chlorine must have an oxidation number of -1, and because there are two chorine atoms, they contribute a total -2 charge. To make the overall charge neutral, copper must have an oxidation number of +2 to balance the charges.

------------> Cu (s) has an oxidation number of 0. All lone atoms (that are not ions) have a 0 oxidation number.

--------------> Because copper goes from an oxidation number of +2 to 0, this indicates that it gained electrons and was oxidized.

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