||Almost all non-metals like O2, F2, and Cl2 are oxidizing agents.
||All the metals like Na, K, Ca, Mg and some non-metals like C, H, P and S are reducing agents.
||All the oxides like SO2, SO3, CO3, CaO, FeO, etc.
||All the hydrides like NaH, H2S, and polymeric hydrides like LiAlH4, NaBH4, etc.
||All –ic componds like Fe3+, Sn++, Cu++, etc.
||All –ous compounds as Fe++, Hg++, etc.
||All oxyacids like H2SO4, HNO3, HClO4, etc.
||All hydracids like HCl, HBr, etc.
||Compounds containing elements in highest oxidation state e.g. KMnO4, HClO4, CrO3, FeCl3, HgCl2, etc.
||Compounds containing elements in lower oxidation state e.g. FeCl2, Cu2O, FeSO4, Hg2Cl2, Na2S2O3, etc.
||Fluorine is the strongest oxidizing agent.
||Lithium is strongest reducing agent in solution and cesium is the strongest reducing agent in dry state.
||If the elements get reduced, it is called oxidizing agent.
||If the elements get oxidized, it is called reducing agent.
||It is also called electron acceptor.
||It is also called electron donor.
||Oxidation number of this agent decreases.
||Oxidation number of this agents increases.
||It is also called oxidant.
||It is also called reductant.
Image source: sciencedirect
Differences between oxidizing and reducing agent