3.2 Electron transfer reactions

• Electron transfer, oxidation state change

• Oxygen gain/loss, hydrogen loss/gain

• Oxidizing/reducing agents

• Deduce oxidation states and identify oxidized/reduced species

• Separate oxidation and reduction

• Show electron loss/gain

• Deduce redox half-equations and equations in acidic or neutral solutions

• Metals: ease of oxidation

• Halogens: ease of reduction

• Metal displacement reactions

• Predict metal oxidation and halogen reduction using supplied data

• Release H₂ gas

• Deduce equations for reactive metals with dilute acids

• Oxidation at anode

• Reduction at cathode

• Signs/polarities in voltaic vs. electrolytic cells

• Identify anode/cathode from electrode reactions

• Spontaneous redox → electrical energy

• Electron flow: anode → cathode (external circuit)

• Ion movement across salt bridge

• Include metal/metal ion half-cells, circuit, and salt bridge

• Redox reactions reversible with electrical energy

• Deduce charging reactions from discharge reactions and compare cell types

• Electrical energy → chemical energy

• Non-spontaneous reactions

• Electrolysis of molten salts

• Explain current conduction and deduce molten salt electrolysis products

• Primary alcohols → aldehydes → carboxylic acids

• Secondary alcohols → ketones

• Include distillation/reflux setup and that tertiary alcohols are not oxidized similarly

• Carboxylic acids → aldehydes → primary alcohols

• Ketones → secondary alcohols

• Include hydride ion role; specific reducing agents and mechanisms are not assessed

• Addition of H₂ lowers unsaturation

• Alkenes + H₂, alkynes + H₂

• Deduce hydrogenation products of alkenes and alkynes

• Hydrogen half-cell = 0 V by convention

• Ease of oxidation/reduction

• Use standard conditions and electrode potential data to compare oxidizing/reducing ability

• Calculate from E⦵ values

• Positive E⦵cell = spontaneous

• Predict feasible redox reactions from E⦵cell

• ΔG⦵ = −nFE⦵cell

• Link electron number, Faraday constant, and spontaneity

• Competing reactions at electrodes

• Water oxidation/reduction

• Deduce products from standard electrode potentials; include water and aqueous solutions

• Electrolytic coating with metal layer

• Explain the metal object as cathode and the coating metal as ion source