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This is handy because the knowledge that you should have from 1st semester redox chemistry should allow you to review the table and not have to much trouble at all thinking about why the values are on which side and correspond with other values below and above and why the values change for electyrolytic cells. And in senior chem where I made the table it helped me to first understand.
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Annode Oxidation Gain of oxygen
Loss of hydrogen
Loss of 𝒆
+𝑒 in products
Oxidation StrongestReductant
Anode Corrodes Faster
REDuction CAThode
Loss of oxygen Gain of hydrogen
Gain of 𝒆 +𝑒 in reactants
Reduction StrongestOxident
Cathode 𝒆 →→
Voltaic Cell Spontaneous
Negative Electrode HASLower E0
E0 x-1 Solid forms (plating)
Positive Electrode HASHigest E0
←← 𝑃𝑜𝑠𝑖𝑡𝑖𝑣𝑒 𝐼𝑜𝑛𝑠 (𝐶𝑎𝑡𝑖𝑜𝑛𝑠) 𝐴+ 𝐴−𝑁𝑒𝑔𝑎𝑡𝑖𝑣𝑒 𝐼𝑜𝑛𝑠 (𝐴𝑛𝑖𝑜𝑛𝑠) →→
Zn s |Zn(NO3)2 aq ||Cu(NO3)2 aq |Cu(s)
Electrolytic Cells Non Spontaneous
Positive Electrode Highest E0
E0 x-1 Becomes basic 𝑝𝐻 ↑
Negative Electrode Lowest E0
GOES AS PREDICTED
Becomes acidic 𝑝𝐻 ↓ Solid forms on electrode
𝐴+𝑃𝑜𝑠𝑖𝑡𝑖𝑣𝑒 𝐼𝑜𝑛𝑠 (𝐶𝑎𝑡𝑖𝑜𝑛𝑠) →→ ←← 𝑁𝑒𝑔𝑎𝑡𝑖𝑣𝑒 𝐼𝑜𝑛𝑠 (𝐴𝑛𝑖𝑜𝑛𝑠) 𝐴−
H2O2 ∶ O = −1 CuH2: H = −1 Cl=-1 Br=-1 H=+1 O=-2 Ag=+1
K Na Li Ba Ca Mg Al Zn Fe Ni Sn Pb H2 Cu Ag Hg
←strongest REDUCTANT weakest→ 𝑤𝑜𝑛𝑡 𝑟𝑒𝑎𝑐𝑡 𝑤𝑖𝑡ℎ 𝑎𝑐𝑖𝑑 ← 𝐻2 → will react
