These equations below show two standard reduction potentials. fe3+(aq) + e– fe2+(aq)

= +0.43 V

The two standard reduction potentials are;

Fe³⁺(aq) + e⁻ → Fe²⁺(aq) E₀ = +0.77 V

Cu²⁺(aq) + 2e⁻ → Cu(s)    E₀ = +0.34 V

The overall reaction is;

Fe³⁺(aq) + Cu(s) → Fe²⁺(aq) + Cu²⁺(aq)

To calculate the standard cell potential of the overall reaction, we use the equation;

Ecell = E redu, cathode - E red, anode

From the reaction; Copper lost electrons to form copper ions (Cu²⁺) (Oxidation) while Fe³⁺ gained electrons to form Fe²⁺ (reduction)

Therefore;

E cell = + 0.77 v - (+0.34 v)

        = + 0.43 V

Hence, the standard cell potential of the overall reaction is +0.43 V

4) transferred from the valence shell of one atom to the valence shell of another atom

Explanation:

Electrons are located outside of the nucleus which contains the protons and the neutrons.

For bonds to form, valence electrons located in the outermost shell electrons are involved. These are the valence electrons. These outer shell electrons can be shared or transferred between two combining atoms to form stable atoms.

In ionic bonds, the electrons are transferred from one specie to another. The atom that loses the electrons becomes positively charged and the receiving atom becomes negatively charged. This is the crux of ionic bonds.