Mnemonic 1: Anode/Cathode Reactions

"AN OX RED CAT"

• ANode = OXidation (loss of electrons)
• REDuction = CAThode (gain of electrons)
• Works for BOTH galvanic and electrolytic cells — no exceptions!

Mnemonic 2: Galvanic vs Electrolytic Polarity

"GANE" — Galvanic Anode Negative; Electrolytic is opposite (anode = positive)

• In Galvanic cells: anode = negative (−), cathode = positive (+)
• In Electrolytic cells: anode = positive (+), cathode = negative (−)
• Just remember: Electrolytic is SWITCHED compared to Galvanic

Mnemonic 3: Electrochemical Series (Reduction Potentials, Most to Least Negative)

"Lovely Kings Never Argue; Zany Fools Hope Copper Saves All Gold Fluorine"

• Li, K, Na, Al; Zn, Fe, H(SHE), Cu, S(Ag), Au, F_{2}
• Left to right: reducing power decreases, oxidizing power increases
• "Z-F-H" is the crucial middle — Zn displaces Fe, Fe displaces H, but Cu cannot displace H

Mnemonic 4: Nernst Equation Number

"Oh-Five-Nine-Two" = 0.0592 (the constant at 25°C)

• Full equation: E = E° − (0.0592/n) log Q
• Think of it as a phone number fragment: 0592

Mnemonic 5: Faraday's Law Formula Check

"w = MIT over nF" (like Massachusetts Institute of Technology / n Faradays)

• w (grams) = M(g/mol) × I(A) × t(s) / [n × F(C/mol)]
• Units check: (g/mol × A × s) / (C/mol) = g/mol × C / (C/mol) = g ✓ [since A·s = C]

Mnemonic 6: O Oxidation Number Exceptions (3 cases)

"POS-SUP" for O exceptions:

• Peroxides: O = −1 ($H_{2}O_{2}$, $Na_{2}O_{2}$, $BaO_{2}$)
• Superoxides: O = −1/2 ($KO_{2}$)
• O$F_{2}$: O = +2 (only fluoride of oxygen)

Mnemonic 7: F = 96500 C/mol

"9-6-5-0-0" → 96500 Coulombs per mole of electrons. Remember: Faraday constant = 96500 (round from 96485). This is charge of 1 mol electrons = Avogadro's number × charge per electron = $6.022 \times 10^{23}$ × $1.6 \times 10^{-19}$ = 96352 C ≈ 96500 C.