Question

identify the species oxidized, the species reduced, the oxidizing agent, and the reducing agent in the following electron transfer reaction. sn^{2+}+co→sn + co^{2+} species oxidized species reduced oxidizing agent reducing agent as the reaction proceeds, electrons are transferred from to .

Explanation:

Step1: Determine oxidation - state changes

Oxidation is the loss of electrons and increase in oxidation state. Reduction is the gain of electrons and decrease in oxidation state. In the reaction $Sn^{2+}+Co\longrightarrow Sn + Co^{2+}$, the oxidation state of $Co$ changes from 0 in $Co$ to + 2 in $Co^{2+}$, and the oxidation state of $Sn$ changes from + 2 in $Sn^{2+}$ to 0 in $Sn$.

Step2: Identify oxidized and reduced species

The species that is oxidized is the one that loses electrons. Here, $Co$ loses electrons and is oxidized. The species that is reduced is the one that gains electrons. Here, $Sn^{2+}$ gains electrons and is reduced.

Step3: Identify oxidizing and reducing agents

The oxidizing agent is the species that causes oxidation (gets reduced in the process). So, $Sn^{2+}$ is the oxidizing agent. The reducing agent is the species that causes reduction (gets oxidized in the process). So, $Co$ is the reducing agent.

Step4: Determine electron - transfer direction

Electrons are transferred from the species that is oxidized to the species that is reduced. So, electrons are transferred from $Co$ to $Sn^{2+}$.

Answer:

Species oxidized: $Co$
Species reduced: $Sn^{2+}$
Oxidizing agent: $Sn^{2+}$
Reducing agent: $Co$
Electrons are transferred from: $Co$ to: $Sn^{2+}$