The anode and cathode when corrosion happens Let's say $\ce{Fe}$ reacts with $\ce{Cu^{2+}}$ ions. $\ce{Fe}$ would oxidize and therefore give electrons to $\ce{Cu^{2+}}$so that:

$$\ce{Fe-&gt; Fe^{2+}  +2e-}$$
$$\ce{Cu^{2+} +2e^- -&gt;Cu}$$
The overall reaction:

$$\ce{Cu^{2+} +Fe -&gt;Cu +Fe^{2+}}$$

Now this is an example of corrosion, right? And when this type of corrosion happens, the anode is the electrode where oxidation happens and the cathode is the electrode where reduction happens, right?
Therefore iron ($\ce{Fe}$) is the anode where oxidation happens and Copper 2+ ions ($\ce{Cu^{2+}}$) is the cathode where the reduction happens.

My question is, is this all correct? Have I successfully described corrosion (of this type) and given an example of it? Or is there something wrong? I'm 15 and soon I'm having a test in chemistry, and because of my age there's no point in making it "super-advanced", but if there's something I missed or did wrong please point it out, I would be grateful for that!
You are right! What you have written is an example of Galvanic corrosion (Galvanic corrosion occurs when two different metals have physical or electrical contact with each other and are immersed in a common electrolyte).
You have  successfully described Galvanic corrosion and given an example of it