Differences between oxidizing and reducing agent

S.N Oxidizing agent Reducing agent
1. 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.
2. All the oxides like SO2, SO3, CO3, CaO, FeO, etc. All the hydrides like NaH, H2S, and polymeric hydrides like LiAlH4, NaBH4, etc.
3. All –ic componds like Fe3+, Sn++, Cu++, etc. All –ous compounds as Fe++, Hg++, etc.
4. All oxyacids like H2SO4, HNO3, HClO4, etc. All hydracids like HCl, HBr, etc.
5. 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.
6. Fluorine is the strongest oxidizing agent. Lithium is strongest reducing agent in solution and cesium is the strongest reducing agent in dry state.
7. If the elements get reduced, it is called oxidizing agent. If the elements get oxidized, it is called reducing agent.
8. It is also called electron acceptor. It is also called electron donor.
9. Oxidation number of this agent decreases. Oxidation number of this agents increases.
10. It is also called oxidant. It is also called reductant.

Oxidation-Reduction - an overview | ScienceDirect Topics

 Image source: sciencedirect


i) https://chemed.chem.purdue.edu/genchem/topicreview/bp/ch19/oxred_3.php

ii) https://www.bbc.co.uk/bitesize/guides/z2r44wx/revision/1

Differences between oxidizing and reducing agent