Question

identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfer reaction.

cl₂ + 2cr²⁺→2cl⁻ + 2cr³⁺

as the reaction proceeds, electrons are transferred from to.

Explanation:

Step1: Determine oxidation states

• For \(Cr^{2+}\) to \(Cr^{3+}\): Oxidation state of \(Cr\) changes from \(+2\) to \(+3\) (loss of electrons, oxidation).
• For \(Cl_{2}\) to \(Cl^{-}\): Oxidation state of \(Cl\) changes from \(0\) to \(- 1\) (gain of electrons, reduction).

Step2: Identify species

• Species oxidized: \(Cr^{2+}\) (loses electrons).
• Species reduced: \(Cl_{2}\) (gains electrons).
• Oxidizing agent: \(Cl_{2}\) (causes oxidation of \(Cr^{2+}\), itself gets reduced).
• Reducing agent: \(Cr^{2+}\) (causes reduction of \(Cl_{2}\), itself gets oxidized).
• Electron transfer: Electrons are transferred from \(Cr^{2+}\) (reducing agent) to \(Cl_{2}\) (oxidizing agent).

Answer:

species oxidized: \(Cr^{2+}\)
species reduced: \(Cl_{2}\)
oxidizing agent: \(Cl_{2}\)
reducing agent: \(Cr^{2+}\)
Electrons are transferred from \(Cr^{2+}\) to \(Cl_{2}\)