Unit 3: Electrochemistry

A comprehensive set of vocabulary flashcards covering the fundamental concepts, components, and industrial applications of electrochemistry and electrolysis as outlined in the Unit 3 lecture notes.

Electrolysis

The process in which electrical energy is used to cause an otherwise non-spontaneous chemical reaction to take place, typically occurring in an environment with free charged ions.

Electrolyte

A solution or liquid that conducts electricity, containing free ions that carry electrical charge between two electrodes.

Cathode

The negative electrode (connected to the negative terminal) that attracts positively charged ions (cations) and is the site where reduction occurs.

Anode

The positive electrode (connected to the positive terminal) that attracts negatively charged ions (anions) and is the site where oxidation occurs.

Oxidation-Reduction (Redox)

The reaction process by which electrons are gained or lost by the chemical species (ions) involved in the reaction.

Oxidation

The process by which electrons are lost, causing the oxidation state number of the chemical species to increase.

Reduction

The process by which electrons are gained, causing the oxidation state number of the chemical species to decrease.

Reducing Agent (Reductant)

A chemical species in a reaction from which electrons are easily removed; it is the species that undergoes oxidation.

Oxidising Agent (Oxidant)

A chemical species in a reaction which has a tendency to gain electrons; it is the species that undergoes reduction.

Standard Reduction Potential

A value used to predict which cation will be reduced at the cathode and which anion will be oxidized at the anode when multiple ions are present in an electrolytic cell.

Brine

Concentrated sodium chloride ($NaCl$) in water, often pumped from salt mines and used industrially to produce sodium hydroxide, chlorine gas, and hydrogen.

Blistered Copper

Impure copper containing approximately $98\%$ copper, used as the anode during the electrolytic refining process to produce pure copper.

Slime

The residue of impurities that drops to the bottom of the electrolytic tank during copper purification, typically containing silver, gold, arsenic, and iron.

Electroplating

An electrolysis process used to coat one metal with another, such as coating zinc onto corrugated iron to prevent rusting or steel with tin.

Hofmann Voltmeter

An experimental apparatus used for the electrolysis of dilute acids, such as dilute sulfuric acid ($H_2SO_4$), to produce hydrogen and oxygen gases.

Electrolytic Refining

The process of purifying impure metals, such as copper, using an electrolytic cell where the impure metal is the anode and pure metal is the cathode.