What will happen if CuSO4 is taken as electrolyte.Zn & Cu are two electrodes.?

[conFusing]

What will happen if CuSO4 is taken as electrolyte.Zn & Cu are two electrodes.??

If we take copper sulfate as an electrolyte and zinc and copper as two electrodes...and allow the current to flow...Wat will happen...

Here is till where i have understood...
When we will start current flow...then,CuSO₄ will dissociate into ions of Cu²⁺ and SO₄^2-...and in zinc electrode it will also dissciate to form Zn2+ and 2e-...the 2 electrons formed will jump down and reduce Cu+ to Cu metal...and so there loss of electrons in zinc and so it should become positively charged...(unlike book where it is given tht its is negatively charged,...)
So the thing which i haven't understood is ----Why zinc plate gets negatively charged even when it has lost electrons to reduce copper

 

[I_am_no1]

CuSO₄ = Cu²⁺ + SO₄^2-

Zn have 2 electrons in its last orbital so they can easily leave it. And Cu have 6 electron in its last orbital (they need 2 more electrons to get a stable form) that's why it can easily take 2 electrons !

When you give ANODE and CATHODE connection using wire then thsose two electrons will m0ve through that wire and the flow of electron is called electricity!

ANODE: Zn = Zn²⁺ + 2e

CATHODE: Cu²⁺ + 2e = Cu

 

[quicknote]

ions to copper metal...

I can explain that the reason zinc becomes negatively charged is due to the flow of electrons from the zinc electrode to the copper electrode. This flow of electrons creates a build-up of negative charge on the zinc electrode, while the copper electrode becomes positively charged due to the loss of electrons.

This process is known as galvanic corrosion, where the more reactive metal (zinc) loses electrons to the less reactive metal (copper). This results in the zinc electrode becoming negatively charged and the copper electrode becoming positively charged.

In terms of the electrolyte, the dissociation of CuSO4 into Cu2+ and SO42- ions is necessary for the flow of electrons to occur. The Cu2+ ions will be attracted to the negatively charged zinc electrode and will accept electrons from it, while the SO42- ions will be attracted to the positively charged copper electrode and will release electrons to it.

Overall, in this setup, the zinc electrode acts as the anode (where oxidation occurs) and becomes negatively charged, while the copper electrode acts as the cathode (where reduction occurs) and becomes positively charged. This process will continue until the concentration of either the Cu2+ or Zn2+ ions becomes too low to sustain the flow of electrons.

In summary, taking CuSO4 as an electrolyte and using zinc and copper as electrodes will result in a flow of electrons from the zinc electrode to the copper electrode, resulting in a negatively charged zinc electrode and a positively charged copper electrode.