Respuesta :
Answer:
The answer is: R, O, N
Explanation:
Oxidizing agent is a chemical species that carries out the oxidation of another chemical species and gets reduced itself .
Whereas, reducing agent is a chemical species that carries out the reduction of another chemical species and gets oxidized itself .
a) NO₃⁻ → NH₃
In the nitrate ion ( NO₃⁻), the oxidation state of the nitrogen (N) atom is +5.
Whereas, the oxidation state of the nitrogen (N) atom in ammonia (NH₃) is -3.
Thus in this reaction, nitrogen atom is getting reduced from +5 to -3 oxidation state.
Therefore, it requires a reducing agent (R).
b) PO₃³⁻ → PO₄³⁻
In the phosphite ion ( PO₃³⁻), the oxidation state of the phosphorus (P) atom is +3.
Whereas, the oxidation state of the phosphorus (P) atom in phosphate ion (PO₄³⁻) is +5.
Thus in this reaction, phosphorus atom is getting oxidized from +3 to +5 oxidation state.
Therefore, it requires an oxidizing agent (O).
c) AgCl → Ag⁺ + Cl⁻
The oxidation state of silver (Ag) atom and chlorine (Cl) atom is +1 and -1, respectively.
In this reaction, the oxidation states of silver (Ag) atom and chlorine (Cl) atom remains unchanged.
Therefore, it does not require a oxidizing agent or a reducing agent (N).
Oxidation involves electron loss while reduction requires electron gain.
Oxidation has to do with the loss of electrons and reduction has to do with the gain of electrons. An oxidizing agent gains electrons in a redox reaction while a reducing agent looses electrons in a redox reaction.
Let us consider the conversions individually;
- The conversion from NO3^- to NH3 requires a reducing agent because eight electrons are gained by NO3^- in the process.
- The conversion from PO3^3- to PO4^3- requires an oxidizing agent since two electrons are lost by PO3^3-.
- The conversion; AgCl --------> Ag^+ + Cl^- is neither an oxidation nor reduction so it requires neither an oxidizing nor a reducing agent.
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