In the chemical reaction, .

Zn(s) + CuSO4(aq) �¨ ZnSO4(aq) + Cu(s),
(A) metallic zinc is the reducing agent.
(B) metallic zinc in reduced.
(C) copper ion is oxidized.
(D) sulfate ion is the oxidizing agent.

To determine which statements are true in the given chemical reaction, we need to understand the concepts of oxidation and reduction.

In a chemical reaction, oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. Oxidation and reduction always occur together and are commonly referred to as redox reactions.

Now let's analyze the given reaction: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)

In this reaction, zinc (Zn) reacts with copper sulfate (CuSO4) to form zinc sulfate (ZnSO4) and solid copper (Cu). Let's break it down step by step:

1. Oxidation state of zinc (Zn) in Zn(s): The oxidation state of an element in its pure, elemental form is always zero. Hence, the oxidation state of Zn is 0.

2. Oxidation state of copper (Cu) in CuSO4(aq): The sulfate ion (SO4) has a charge of -2, and there is one copper (Cu) ion. Taking into account the overall charge of the compound, the oxidation state of Cu in CuSO4 is +2.

During the reaction:

- Zinc loses electrons (oxidation) and is converted to Zn2+ in the aqueous solution ZnSO4. Since the oxidation state of Zn changes from 0 to +2, metallic zinc is being oxidized. So, statement (B) is incorrect.

- Copper ion (Cu2+) in CuSO4 gains electrons (reduction) and is converted to elemental copper (Cu). Since the oxidation state of Cu changes from +2 to 0, copper ion is being reduced. So, statement (C) is correct.

- The sulfate ion (SO4) does not change its oxidation state during the reaction, remaining as -2. It is neither oxidized nor reduced. So, statement (D) is incorrect.

- By process of elimination, the reducing agent is the species that is being oxidized. In this case, metallic zinc (Zn) is being oxidized to Zn2+ in ZnSO4. Therefore, statement (A) is correct.

In summary, the correct statements are:
(A) Metallic zinc is the reducing agent.
(C) Copper ion is oxidized.

Remember the definitions.

Oxidation is the loss of electrons.
Reduction is the gain of electrons.
(The material oxidized is the reducing agent; therefore, the reducing agent loses electrons. The material reduced is the oxidizing agent; therefore, the oxidizing agent gains electrons).
Zn is zero on the left and +2 on the right.
Cu is +2 on the left and zero on the right.
S is +6 on both sides.
O is -2 on both sides.
From those definitions AND I have given you the oxidation states, you should be able to pick out the answer.

is the answer C

The answer is not C.

The reaction shows Cu going from Cu^+2 to Cu or from +2 to zero. That is the gain of electrons. Oxidation is the loss of electrons. It can't be C.

Then A because its going from 0 to +2

Right. Metallic Zn is the reducing agent (it is oxidized in the process).