ZnOH4^2- --> ZnO2^2- + 2H2O

What is the oxidation agent, reducing agent, substance oxidized, and substance reduced?

Well, Zn isn't changed either way, so the OH is the only factor left here...
I simplified ZnOH4^-2 --> ZnO2^2- and 2HOH, but still I'm not quite understanding which is which. I know that there is LEO and GER or OIL RIG, but could you clarify this for me?
Thanks.

I have news for you; there is no redox here. Prove it?

Let me rewrite it because you've omitted parentheses.
Zn(OH)4^2- ==> ZnO2^2- + 2H2O

Zn(OH)4^2.
Zn = +2
O = 4*-2 = -8
H = 4*+1 = +4
+2-8+4 = -2 which = charge on the complex ion.

ZnO2^2-
Zn = +2
O = 2*-2 = -4
+2-4= -2 and that's the charge on the ion.

You know water is neutral at 2*1 = 2 for H and -2 for O.

There is no LEO or GER

In order to determine the oxidation agent, reducing agent, substance oxidized, and substance reduced, we need to identify the elements and their oxidation states before and after the reaction.

Starting with the equation: ZnOH4^2- --> ZnO2^2- + 2H2O

Oxidation is the loss of electrons, and reduction is the gain of electrons. We can use this information to determine which compounds/elements are being oxidized and reduced.

Looking at the equation, we can see that the Zn atom's oxidation state doesn't change, so it is neither oxidized nor reduced. This means that it doesn't play a role as an oxidizing agent or reducing agent.

Now let's consider the OH^- and O2^- ions:

In the reactant ZnOH4^2-, each oxygen atom has an oxidation state of -2, while the hydrogen atom has an oxidation state of +1. The overall charge on the ion is -2. In the product ZnO2^2-, each oxygen atom also has an oxidation state of -2, but there is no hydrogen present. The overall charge on the ion is -2.

From this comparison, we can see that the oxygen atoms in the ZnOH4^2- ion have undergone a reduction (reduction is the gain of electrons), resulting in the formation of the ZnO2^2- ion. Therefore, the OH^- ions are the reducing agents, and they have been oxidized.

In the process of reduction, electrons are gained, and in this case, they are gained by the oxygen atoms. Therefore, the OH^- ions are reduced.

In summary:
- The reducing agent is OH^-.
- The oxidizing agent is not present as there is no compound or element that gains electrons.
- The substance oxidized is OH^-.
- The substance reduced is OH^-.

Remember, it's important to keep track of oxidation states to determine which species are being oxidized or reduced.

To determine the oxidation agent, reducing agent, substance oxidized, and substance reduced in the given reaction, we can apply the concept of redox reactions.

In the reaction: ZnOH4^2- → ZnO2^2- + 2H2O

First, let's determine the oxidation states of the elements involved:
- In ZnOH4^2-, the oxidation state of Zn is +2 since it is a Group 2 element and OH is -1. Thus, the oxidation state of oxygen (O) is -2.
- In ZnO2^2-, the oxidation state of Zn is also +2, and oxygen (O) must have an oxidation state of -1 to balance the charge on the ion.

Now, let's analyze the changes in oxidation states:

1. Substance oxidized: The substance that undergoes an increase in oxidation state is being oxidized. In this case, the oxygen in the OH groups has an oxidation state of -2 in ZnOH4^2-. But in ZnO2^2-, the oxygen has an oxidation state of -1. Therefore, oxygen is being oxidized from -2 to -1.

2. Substance reduced: The substance that undergoes a decrease in oxidation state is being reduced. In this case, the zinc (Zn) ions have an oxidation state of +2 in both ZnOH4^2- and ZnO2^2-. So, there is no change in the oxidation state of zinc, and thus, it is not being reduced.

3. Oxidizing agent: The oxidizing agent is the species that causes another species to be oxidized. In this reaction, the OH groups are causing the oxidation of oxygen. Therefore, the OH groups are acting as the oxidizing agent.

4. Reducing agent: The reducing agent is the species that causes another species to be reduced. Since there is no change in the oxidation state of zinc, there is no reducing agent.

To summarize:
Substance oxidized: Oxygen (from -2 to -1)
Substance reduced: None (there is no change in the oxidation state of zinc)
Oxidizing agent: OH groups
Reducing agent: None

Remember that LEO (Loss of Electrons is Oxidation) and GER (Gain of Electrons is Reduction) or OIL (Oxidation Is Loss) RIG (Reduction Is Gain) can be helpful mnemonics for understanding redox reactions.