What occurs during a redox reaction?

In a redox reaction, a transfer of electrons occurs between two species, leading to the oxidation of one and the reduction of another. When considering the first choice, it reflects the concept of displacement reactions, where a more reactive metal can displace a less reactive metal from its compound. This is due to the differences in their positions in the electrochemical series, where metals higher in the series are more likely to lose electrons and be oxidized compared to those lower in the series.

When a higher metal displaces a lower metal from its compound, it signifies that the higher metal is undergoing oxidation (losing electrons), while the lower metal is being reduced (gaining electrons). This direct relationship between metal reactivity and electron transfer is a crucial part of understanding redox reactions.

The other options do not accurately define the processes at play in redox reactions. While gas may be produced in some reactions, it is not a defining characteristic of redox processes. The mention of electrons being transferred only from the lower metal overlooks the necessary balance in oxidation and reduction that defines redox reactions. Additionally, the formation of only liquids is not a generic outcome of redox reactions, as various phases can result, including solids, liquids, and gases depending on the