Oxidation and Reduction
The process defined as the loss of electrons
Oxidation
The strongest oxidizing agents are found in this part of the redox table
Top left
Electrons flow from ____ to ____
Anode to cathode
Electrolytic cell reactions are ____
Non-spontaneous
The unit of electric charge
Coulomb (C)
The process defined as the gain of electrons
Reduction
If the oxidizing agent is above the reducing agent, the reaction is ___
spontaneous
This part of a voltaic cell balances ion movement between half-cells
Salt bridge
This electrode is positive
anode
The equation relating charge, current, and time
Q=It
In the reaction
Zn(s) + 2H⁺ → Zn²⁺ + H₂(g), this substance is oxidized
Zinc
Ag⁺ + e⁻ → Ag(s) is this type of half-reaction
Reduction half-reaction
These move toward the cathode through the salt bridge
Cations
This causes Cl- to act as the reducing agent instead of water
The chloride anomaly
The value of Faraday's constant
9.65 × 10⁴ C/mol?
The oxidation number of oxygen in peroxides
-1
What is the strongest reducing agent among Zn, Pb, Cu, Ag.
Zinc
The electrode used when the species being oxidized or reduced is not a solid metal
Inert electrode
The process used to obtain high-purity copper from impure copper ore
Electrorefining
The industrial process uses brine to produce chlorine, hydrogen, and sodium hydroxide
Chlor-alkali process
This type of reaction occurs when a single species undergoes both oxidation and reduction simultaneously
disproportionation
The pair Ag⁺(aq) + e⁻ → Ag(s) and Cu(s) → Cu²⁺(aq) + 2 e⁻ will produce a reaction that is ________
Non-spontaneous
When a metal electrode increases in mass, ___ is happening at the cathode
Reduction
This describes the process on which a metal ion in solution gains electrons at the cathode to form a solid metal coating on an object
Electroplating
This cell produces electricity continuously by reacting fuel that is continuously supplied
Fuel cell