Anlagen

Periodensystem

bei $T=298,15\;\text{K},$
$p=101,325\;\text{kPa}\:\text{und}\:c=1\;\frac{\text{mol}}{\text{L}}$

reduzierte Form	$\color{#ffffff}{\boldsymbol{\ce{<=>}}}$	oxidierte Form $\color{#ffffff}{(+x\cdot\ce{e-})}$	Standardpotenzial E⁰ in $\color{#ffffff}{\text{V}}$
$\ce{Li}$	$\ce{<=>}$	$\ce{Li+ +e-}$	$-3,04$
$\ce{Na}$	$\ce{<=>}$	$\ce{Na+ +e-}$	$-2,71$
$\ce{Mg}$	$\ce{<=>}$	$\ce{Mg^2+ +2e-}$	$-2,37$
$\ce{Al}$	$\ce{<=>}$	$\ce{Al^3+ +3e-}$	$-1,66$
$\ce{Mn}$	$\ce{<=>}$	$\ce{Mn^2+ +2e-}$	$-1,19$
$\ce{H2 +2OH-}$	$\ce{<=>}$	$\ce{2H2O +2e-}$	$-0,83\:(pH=14)$
$\ce{Zn}$	$\ce{<=>}$	$\ce{Zn^2+ +2e-}$	$-0,76$
$\ce{Cr}$	$\ce{<=>}$	$\ce{Cr^3+ +3e-}$	$-0,74$
$\ce{S^2-}$	$\ce{<=>}$	$\ce{S +2e-}$	$-0,48$
$\ce{Fe}$	$\ce{<=>}$	$\ce{Fe^2+ +2e-}$	$-0,45$
$\ce{Ni}$	$\ce{<=>}$	$\ce{Ni^2+ +2e-}$	$-0,26$
$\ce{Sn}$	$\ce{<=>}$	$\ce{Sn^2+ +2e-}$	$-0,14$
$\ce{Pb}$	$\ce{<=>}$	$\ce{Pb^2+ +2e-}$	$-0,13$
$\ce{H2 +2H2O}$	$\ce{<=>}$	$\ce{2H3O+ +2e-}$	$0,00\:(pH=0)$
$\ce{Cu+}$	$\ce{<=>}$	$\ce{Cu^2+ +e-}$	$+0,15$
$\ce{Cu}$	$\ce{<=>}$	$\ce{Cu^2+ +2e-}$	$+0,34$
$\ce{4OH-}$	$\ce{<=>}$	$\ce{O2 +2H2O +4e-}$	$+0,40\:(pH=14)$
$\ce{Cu}$	$\ce{<=>}$	$\ce{Cu+ +e-}$	$+0,52$
$\ce{2I-}$	$\ce{<=>}$	$\ce{I2 +2e-}$	$+0,54$
$\ce{Fe^2+}$	$\ce{<=>}$	$\ce{Fe^3+ +e-}$	$+0,77$
$\ce{Ag}$	$\ce{<=>}$	$\ce{Ag+ +e-}$	$+0,80$
$\ce{2Br-}$	$\ce{<=>}$	$\ce{Br2 +2e-}$	$+1,07$
$\ce{Pt}$	$\ce{<=>}$	$\ce{Pt^2+ +2e-}$	$+1,18$
$\ce{6H2O}$	$\ce{<=>}$	$\ce{O2 +4H3O+ +4e-}$	$+1,23\:(pH=0)$
$\ce{2Cl-}$	$\ce{<=>}$	$\ce{Cl2 +2e-}$	$+1,36$
$\ce{Au}$	$\ce{<=>}$	$\ce{Au^3+ +3e-}$	$+1,50$
$\ce{2F-}$	$\ce{<=>}$	$\ce{F2 +2e-}$	$+2,87$