According to me, $\ce{Fe^{2+}}$ should be a better reducing agent because $\ce{Fe^2+}$ after getting oxidized will attain a stable $\ce{d^5}$ configuration, whereas $\ce{Cr^2+}$ will get a $\ce{d^3}$ configuration. I think the half filled $\ce{d^5}$ configuration is more stable than the $\ce{d^3}$ configuration. Why is this not so?

According to me, $\ce{Fe^{2+}}$ should be a better reducing agent because $\ce{Fe^2+}$ - after being oxidized - will attain a stable $\ce{d^5}$ configuration, whereas $\ce{Cr^2+}$ will attain a $\ce{d^3}$ configuration. I think the half filled $\ce{d^5}$ configuration is more stable than the $\ce{d^3}$ configuration. Why is this not so?

According to me $\ce{Fe^{2+}}$ should be a better reducing agent because $\ce{Fe^{2+}}$ after getting oxidized will get a stable $d^5$ configuration and $\ce{Cr^{2+}}$ will get a $d^3$ configuration. I think the half filled $d^5$ configuration is more stable than the $d^3$ configuration. Why is this not so?

According to me, $\ce{Fe^{2+}}$ should be a better reducing agent because $\ce{Fe^2+}$ after getting oxidized will attain a stable $\ce{d^5}$ configuration, whereas $\ce{Cr^2+}$ will get a $\ce{d^3}$ configuration. I think the half filled $\ce{d^5}$ configuration is more stable than the $\ce{d^3}$ configuration. Why is this not so?

According to me Fe(+2) should be a better reducing agent because Fe(+2) after getting oxidized will get a stable d5 configuration and Cr(+2) will get d3 configuration. I think half filled d5 configuration is more stable than d3 configuration. Why is is it so?

According to me $\ce{Fe^{2+}}$ should be a better reducing agent because $\ce{Fe^{2+}}$ after getting oxidized will get a stable $d^5$ configuration and $\ce{Cr^{2+}}$ will get a $d^3$ configuration. I think the half filled $d^5$ configuration is more stable than the $d^3$ configuration. Why is this not so?