[briteyellowness]

rank the following in order of increasing standard reduction potential:

Br2, F2, I2, Cl2

the answer is: F2, Cl2, Br2, I2.

so how do you find increasing standard reduction potentials?  since it's gain of electrons, i thought electronegativity would come into account?  or is it electron affinity?  

but why is it the bigger the radius, the easier it is to add an electron?
wait... is it because there's a smaller pull from the protons cuz it's more shielded?

[madscientist]

im not sure if this will help or not but here goes,

E^o_cell= delta G^o / (-n)(F) = ? V

n = number of moles of electrons
F= Faradays constant

cheers,

madscientist :albert:

[sdekivit]

use the fact that F2 pulls stronger to it's electrons thand Cl2, Cl2 stronger then Br2 en Br2 stronger than I2 (why?). What element needs will thus ionize easier ?

[briteyellowness]

urm... i thought F2 would ionize easier cuz it was the most electronegative... but i guess that wasn't the right way to go since it had the smallest reduction potential?

[sdekivit]

since F pulls strongly to it's electrons it's easier to accept an electron than it is to let a Cl-atom accept an electron ( thus: the elektronegativity of F2 is higher than that of Cl2)

F2 is therefore a stronger oxidator and thus ahs a higher reduction potential then Cl2. The elektronegativity thus decreases when we go down in group 17.

[briteyellowness]

kay thanks, i think i inverted it and got it confused and then tried to make up a random rule to make the wrong inversion seem right.