Redox (reduction/oxidation) reactions are those where a transfer of electrons has occurred. One species is oxidised (lost electrons) and other species must be reduced (gain electrons). Consider the following reaction and identify which species is oxidised (loses electrons) and which is reduced (gains electrons). Na(s) + ½Cl2(g) → NaCl(s) Hint: considering the oxidation numbers of each species before and after might be helpful. If oxidation number increases oxidation has occured, if oxidation has decreased, reduction has occurred.

Question

Redox (reduction/oxidation) reactions are those where a transfer of electrons has occurred. One species is oxidised (lost electrons) and other species must be reduced (gain electrons). Consider the following reaction and identify which species is oxidised (loses electrons) and which is reduced (gains electrons). Na(s) +  ½Cl2(g) →  NaCl(s) Hint: considering the oxidation numbers of each species before and after might be helpful. If oxidation number increases oxidation has occured, if oxidation has decreased, reduction has occurred.

BlackTom AI · Accepted Answer

We start by restating the reaction and recalling the key concept: in a redox reaction, electrons are transferred from the species that is oxidized to the species that is reduced.

Option a: Na oxidised, Cl reduced. To assess this, assign oxidation states: sodium in Na(s) has oxidation state 0. In NaCl(s), sodium is typically +1 and chlorine is -1. Since sodium loses electrons to go from 0 to +1, it is oxidized. Chlorine gains electrons to go from 0 (in Cl2) to -1 (in Cl- in NaCl), so it is reduced. This option matches the expected electron transfer pattern for the reaction given.

Option b: Na reduced, Cl oxidised. If we suppose sodium were reduced, its oxidation state would have to decrease from its initial value. In the reaction, sodium goes from 0 to +1, not a decrease, so this option contradicts the actual electron flow observed. Moreover, chloride is not converted to a species with a higher oxidation state (it becomes more negative), so labeling both roles oppositely conflicts with the stoichiometry and the known product NaCl.

Option c: Not a redox reaction (no electron transfer has occurred). The formation of NaCl from Na(s) and Cl2(g) clearly involves electron transfer: Na loses electrons and Cl gains electrons to form ionic bonds in the solid salt. Therefore, this statement denies the fundamental redox change occurring in the reaction, which is inconsistent with the chemical process described.

Overall, the reasoning hinges on oxidation state changes: a rise in oxidation state indicates oxidation, while a drop indicates reduction. The species that increases its oxidation state is the one that loses electrons, and the species that decreases its oxidation state is the one that gains electrons. The reaction Na(s) + 1/2 Cl2(g) → NaCl(s) demonstrates this electron movement through the formation of Na+ and Cl− ions in the solid salt, confirming the redox character of the process.

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