Question

Assign oxidation states to all of the species in the following redox reaction. For the reactants, identify electron loss or gain, the species oxidized, the species reduced, the oxidizing agent and the reducing agent. Co(s) + F2(g) Co2+(aq) + 2F-(aq) Oxidation state Electron loss or gain Oxidized or reduced Reducing or oxidizing agent

Answer 1

Answer: Co lose two electrons and thus gets oxidized and acts as reducing agent.

`F_2` gain two electrons and thus gets reduced and acts as oxidizing agent.

Step-by-step explanation:

Oxidation reaction : When there is an increase in oxidation state number by loss of electrons

Reduction reaction : when there is a decrease in oxidation state number by gain of electrons.

`Co(s)+F_2(g)\rightarrow Co^(2+)(aq)+2F^-(aq)`

Cobalt metal has undergone oxidation, as its oxidation state is changing from 0 to 2+.

Florine gas has undergone reduction, as its oxidation state is changing from 0 to -1.

The chemical agent which itself get oxidized and reduce others is called reducing agent. Thus Co is a reducing agent.

The chemical agent which itself get reduced and oxidize others is called oxidizing agent.
`F_2` is an oxidizing agent.