Which of the following would most likely be oxidizing agents, and which would most likely be reducing agents? (Hint: Think in terms of tendencies to lose or gain electrons.) a. Cl2 b. K c. Ag+ d. Zn2+
An oxidizing agent is one that accepts electrons, being reduced, and oxidizing other atoms.
A reducing atent is one that releases electrons, getting oxidized and reducing other atoms.
See each choice:
a. Cl₂
Cl₂ is the diatomic molecule formed by the covalent bonding of two Cl atoms.
The oxidation state of the molecule is zero (this is a rule, the oxidation state of any atom alone or bonded to other atom of the same kind is zero).
Since, Cl is highly electronegative, it will mostly behave as oxidizing agent, i.e. it will accept electrons reducing itself while oxidizing other atoms.
b. K
K (potassium) is an alkaline metal, which means that it has a valence electron. It is relatively easy for K to donate its electron. In this process K will oxidize itself (incrrease its oxidation state) while reduce other atoms, so this is would most likely be a reducing agent.
c. Ag⁺
Since, Ag⁺ has a positive charge, it will gain stability by accepting an electron, meaning that it will get reduced, most likely being an oxidizing agent.
d. Zn²⁺
Similarly to the case above, the cation Zn²⁺ would gain stability by gaining electrons, which means that it would most likely get reduced, and be an oxidizing agent.
