Step-by-step explanation:
The given chemical equation represents a redox (reduction-oxidation) reaction. Redox reactions involve the transfer of electrons between species, resulting in changes in the oxidation states of the elements involved. Let's analyze the oxidation states of the elements in this equation:
On the reactant side:
- Aluminum (Al) has an oxidation state of 0 since it is in its elemental form.
- Copper (Cu) in the Cu(NO3)2 compound has an oxidation state of +2.
- Nitrogen (N) in the Cu(NO3)2 compound has an oxidation state of +5.
- Oxygen (O) in the Cu(NO3)2 compound has an oxidation state of -2.
On the product side:
- Copper (Cu) in the Cu(s) has an oxidation state of 0 since it is in its elemental form.
- Aluminum (Al) in the Al(NO3)3 compound has an oxidation state of +3.
- Nitrogen (N) in the Al(NO3)3 compound has an oxidation state of +5.
- Oxygen (O) in the Al(NO3)3 compound has an oxidation state of -2.
By comparing the oxidation states of the elements before and after the reaction, we can observe the following changes:
- Aluminum (Al) undergoes oxidation, as its oxidation state increases from 0 to +3.
- Copper (Cu) undergoes reduction, as its oxidation state decreases from +2 to 0.
Since there is a transfer of electrons from aluminum to copper, this reaction is classified as a redox reaction. Aluminum loses electrons (oxidation) and copper gains those electrons (reduction).