Question

identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfer reaction.
2fe³+ + cd→2fe²+ + cd²+
species oxidized species reduced
oxidizing agent reducing agent
as the reaction proceeds, electrons are transferred from to.

Explanation:

Step1: Determine oxidation states

Oxidation state of \(Fe\) in \(Fe^{3 +}\) is \(+ 3\), in \(Fe^{2+}\) is \(+2\). Oxidation state of \(Cd\) is \(0\) (elemental form) and in \(Cd^{2+}\) is \(+2\).

Step2: Identify oxidized and reduced species

Species that loses electrons (oxidation state increases) is oxidized. \(Cd\) goes from \(0\) to \(+2\), so \(Cd\) is oxidized. Species that gains electrons (oxidation state decreases) is reduced. \(Fe^{3+}\) goes from \(+3\) to \(+2\), so \(Fe^{3+}\) is reduced.

Step3: Identify oxidizing and reducing agents

Oxidizing agent is the species that gets reduced (\(Fe^{3+}\)). Reducing agent is the species that gets oxidized (\(Cd\)).

Step4: Determine electron transfer

Electrons are transferred from the reducing agent (\(Cd\)) to the oxidizing agent (\(Fe^{3+}\)).

Answer:

species oxidized: \(Cd\)
species reduced: \(Fe^{3+}\)
oxidizing agent: \(Fe^{3+}\)
reducing agent: \(Cd\)
Electrons are transferred from \(Cd\) to \(Fe^{3+}\)