In chemistry, a sterically induced reduction happens when an oxidized metal behaves as, and exhibits similar reducing properties to, the more reduced form of the metal. This effect is mainly caused by the surrounding ligands that are complexed to the metal and it is the ligands that are involved in the reduction chemistry instead of the metal due to electronic destabilization by being significantly distanced from the metal. Sterically induced reductions commonly involve metals found in the lanthanoid and actinoid series. Background Divalents Lanthanides are extremely reducing (can reduce alkali cations) compounds. Of these divalent lanthanides, Samarium(II) iodide, SmI2, is a common reducing agent that is used in a variety of synthetic applications, mainly because all other divalent lanthanides are unstable. Complexes of Sm(II) have also been investigated and used in similar applications. However, even though Sm(II) complexes and compounds have had tremendous success when used in conjunction with a variety of substrates. There have been instances where chemistry of certain materials cannot be performed due to unclean reactions in which products are not easily isolated from reaction mixtures when Sm(II) compounds are used to perform the desired reduction. In these cases, adjusting the size of the metal (which is commonly and easily done for the trivalent lanthanide compounds) may fine tune the nature of a specific reaction, which should produce desired and clean products. One drawback to this notion is that Sm(II) is uniquely stable compared to other divalent lanthanides, where the other metals in the series tend to exist freely in the trivalent state. The discovery and application of sterically induced reductions allows the unique reducing properties and chemistry to be applicable to all of the lanthanide metals while remaining in their more stable trivalent state. When Sm(III) is complexed with (pentamethylcyclopentadiene) to give the compound , this trivalent species has been shown to have the same reducing reactivity of the Sm(II) derivative. The top reaction is the Sm(III) derivative and the bottom involves the Sm(II) derivative. Notice that the oxidation state of the metal in the top reaction does not change, while the oxidation state changes in the bottom one. If the metal was involved in the reduction the oxidation states should have changed (+3 to +4). For the trivalent compound this is not the case, thus the ligands themselves must be involved in the reduction process via the following redox reaction: → e− + 1/2 But