Why Zn Displaces Cu from a solution? (1 Viewer)

[Accuracy]

i don't quite understand why Zn(s) would want to displace Cu2+ because isn't Zn already stable with neutral charge?
like Zn(s) --> Zn2+ (aq) + 2e- ........why does it want to become electron deficient ie. unstable so it can join another one

 

[nightweaver066]

It is more reactive than copper, meaning it has a greater tendency to donate electrons than copper.

Copper, being less reactive, has a greater tendency to accept electrons.

So if you dip copper in to a Cu2+ solution, zinc will oxidise donating electrons to the copper ions forming Zn2+ and copper solid as the Cu2+ ions accept the electrons.

 

[Accuracy]

It is more reactive than copper, meaning it has a greater tendency to donate electrons than copper.

Copper, being less reactive, has a greater tendency to accept electrons.

So if you dip copper in to a Cu2+ solution, zinc will oxidise donating electrons to the copper ions forming Zn2+ and copper solid as the Cu2+ ions accept the electrons.

if copper has a greater tendency to accept electrons than zinc wouldn't copper WANT to accept electrons from the solution hence it would stay bonded ?

 

[nightweaver066]

if copper has a greater tendency to accept electrons than zinc wouldn't copper WANT to accept electrons from the solution hence it would stay bonded ?

There are no electrons in the solution. When a copper compound dissolutes on water, it forms its copper ion and the anion; no electrons are released.

However, when zinc solid is placed in to the solution, the copper ions will grab electrons from the solid zinc as it has a stronger pull for electrons than zinc does, causing copper solid to form and zinc to ionise in to zinc ions.