The discussion revolves around the concepts of oxidation and reduction, exploring their definitions, differences, and the implications of oxidation states in chemical reactions. Participants examine the electron transfer involved in these processes and question the conventions surrounding their representation.
Participants generally agree on the definitions of oxidation and reduction in terms of electron transfer, but there is a lack of consensus on the implications of oxidation states and how they relate to experimental observations.
The discussion highlights the complexity of oxidation and reduction, including the conventions used in chemistry and the potential for alternative interpretations based on experimental data. There are unresolved questions regarding the representation of reduction and the practical implications of oxidation states.
guyknowslittle said:this is a very good question.
oxidation and reduction describe the loss or gain, respectively, in the number of electrons. For example Li+ ion can be reduced to Li0 (also known as elemental or lithium metal) if one electron is added to it. Similarly, S2- ion can be oxidized to S0 (elemental sulfur) ion by removing two electrons. If multiple covalent bonds exist between atoms (common in organic compounds), reduction manifests in the decrease in the number of bonds. A double bond will be reduced to a single bond (due to a gain in the overall number of electrons by addition of hydrogen).
the reason the oxidation state of an atom is monitored in a compound is simply convention. the reduction state could be monitored as well, in principle.
most chemical reactions involve a gain or loss of electrons.