Each of the two neutral hydrogen atoms can be regarded as giving up an electron to, and thereby reducing, one of the carbon atoms. A chemical reaction in which an atom or ion loses electrons, thus undergoing an increase in valence. And if you've ever breathed, which is a good bet, you've experienced oxidation.
The oxidation-state concept clarifies the relationship between oxygen-atom, hydrogen-atom, and electron transfer.When bonds are present between two elements that differ little in electronegativity, however, oxidation-state assignments become doubtful, and the distinction between redox and nonredox processes is not evident.There is a general reluctance, particularly regarding organic systems, to assume oxidation-state changes when the reaction results can be accounted for by the transfer or addition of water (H), hydrogen chloride (HCl)."How life alters Climate" (photosynthesis, animal respiration, phytoplankton, ocean exchange, soil exchange, the organic carbon sub-cycle (Box 4-2), deforestation, fossil fuel combustion [396-398], CO pulls CO2 from atmosphere. The statements below were taken from this summary by Elaine Matthews.Electron-pair bonding is often diagrammed so as to show all the bonding and nonbonding valence electrons—e.g., the structures of atomic hydrogen, atomic hydrogen chloride shown below (each dot represents one valence electron): The hydrogen chloride diagram reflects the presence, in the internuclear region, of two electrons that are under the mutual attractive influence of both the hydrogen and chlorine nuclei.
Oxidation states for the hydrogen and chlorine in HCl are assigned according to the net charges that remain on H and Cl when the shared electrons are assigned to the atom that has the greater attraction for them.The largest single source of atmospheric carbon dioxide (CO into the atmosphere.Statistics indicate that fossil fuel use accounts for emissions to the atmosphere of ~5.5 Gt C (Gt C = billions of metric tons of carbon) annually.The oxidation states of the atoms involved are added up algebraically in the table, and their sum must always equal the net charge on the molecule.There is no physical reality to oxidation states; they simply represent the results of calculations based on a formal rule.Removing an electron from an iron atom having a valence of 2 changes the valence to 3. In all these cases, oxygen is added to another substance.