Left-side elements in periodic table are stable in oxide state. In order to produce their metals from the oxides, the molten CaCl₂ is useful as the media where CaO is dissolved. By applying 3.0 V above melting temperature of CaCl₂ (1045 K), CaO in CaCl₂ melt electrochemically decomposes into metallic Ca and oxygen. The deposited Ca at cathode can work as reductant for the stable oxides. Because of strong reducing ability of Ca, Ti can be produced directly from TiO₂. This calciothermic reduction forms a lot of CaO at the cathode, but it dissolves in CaCl₂ and decomposes again by electrolysis. This OS process could be applied to TiO₂ or other oxides. Even if electric insulators such as Al₂O₃ were used, metallic Al could be obtained. V₂O₅ and Bi₂O₃ are molten oxides, but they could be reduced to metallic state. It is noted that Al and Bi are liquid metals at the operating temperature.

The trials to decrease the residual oxygen in Ti are introduced from TiO₂ and CaTiO₃. By optimizing the cathodic structure, CaO content in the bath, H₂O removal and cooling procedures, 1500 mass ppm oxygen could be achieved.

Oxygen anions at carbon anode form CO and CO₂ gas bubbles. If gas bubbles do not leave from the anodic surface, CO₂ gas forms CO₃^2-. Carbonate ions are reduced by Ca to carbon, or electrochemically deposite carbon on cathode. These parasite reactions decrease the current efficiency. Quick removal of CO₂ gas bubbles from anode is a key.

By applying TiS₂ or V₃S₄ as the starting materials, good quality of metallic Ti or V, respectively, could be realized because they do not form solid solution with sulfur. The sulfur gas deposited at the cold parts of reaction vessel, and can be used for sulfide formation.