Redox reactions are fundamental chemical processes involving electron transfer, altering oxidation states. These reactions occur in combustion, corrosion, and biological functions like cellular respiration. Understanding oxidation, reduction, oxidising and reducing agents, and assigning oxidation states is crucial. Disproportionation reactions and applications in technology and nature highlight redox reactions' significance.
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Redox reactions involve the transfer of electrons between molecules, resulting in changes to their oxidation states
Oxidation
Oxidation is the process of losing electrons
Reduction
Reduction is the process of gaining electrons
Redox reactions involve the transfer of electrons between molecules
Oxidising agents accept electrons and are themselves reduced in the process
Reducing agents donate electrons and are oxidised as a result
The effectiveness of an oxidising or reducing agent is determined by properties such as electronegativity and electron affinity
Oxidation states are hypothetical charges assigned to atoms to reflect the extent of electron loss or gain
Rules for assigning oxidation states include the sum of oxidation states in a neutral molecule must be zero
Certain elements have common oxidation states, such as +1 for alkali metals and -2 for oxygen
Redox equations depict the complete reaction, while half-reaction equations illustrate individual oxidation or reduction processes
Disproportionation reactions involve a single substance being simultaneously oxidised and reduced
Common redox reactions include electrolysis, combustion, and rusting
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In a ______ event, a molecule is stripped of electrons, known as ______, while another molecule undergoes ______, gaining electrons.
redox
oxidation
reduction
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Historical definition of oxidation
Originally, oxidation meant adding oxygen to a substance or removing hydrogen.
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Historical definition of reduction
Initially, reduction referred to the removal of oxygen from a substance or the addition of hydrogen.
