Question

Explain how $Zn+2AgN{{O}_{3}}\text{ }\to 2Ag+Zn{{\left( N{{O}_{3}} \right)}_{2}}$ ​is a redox reaction.

Answer 1

Redox is a chemical process that involves changing the oxidation states of atoms. The actual or formal transfer of electrons between chemical species is defined by redox reactions, which usually include one species (the reducing agent) suffering oxidation (losing electrons) while another species (the oxidising agent) experiences reduction (gains electrons).

Complete Step By Step Answer:
To put it another way, oxidation is the loss of electrons or the rise in the oxidation state of an atom, an ion, or a group of atoms in a molecule.
The gain of electrons or a drop in the oxidation state of an atom, an ion, or specific atoms in a molecule is referred to as reduction (a reduction in oxidation state).
Zinc reacts with silver nitrate to create zinc nitrate, which yields silver as a byproduct during or at the conclusion of the reaction. The process occurs because zinc, which produces zinc nitrate, is significantly more reactive than silver, resulting in the formation of silver. This method, in particular, is a substitution reaction in which zinc is used instead of silver.
$\text{Z}{{\text{n}}_{\text{(s)}}}\text{+ 2AgN}{{\text{O}}_{\text{3}}}_{\text{(s)}}\to \text{ Zn}{{\left( \text{N}{{\text{O}}_{\text{3}}} \right)}_{\text{2}}}\text{+ 2Ag}$
$\mathrm{Zn}+2 \mathrm{AgNO}_{3}$
The oxidation state of Zinc is $(0)$
$\mathrm{AgNO}_{3}$
$x+(-1)=0$
$\text{x}=+1\left( \text{A}{{\text{g}}^{+}} \right)$
In the product side
$\to 2\text{Ag}+\text{Zn}{{\left( \text{N}{{\text{O}}_{3}} \right)}_{2}}$
The oxidation state of Silver is $(0)$
$\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}$
$x+2(-1)=0$
$\mathrm{x}=2\left(\mathrm{Zn}^{+2}\right)$
The oxidation number of Zn in $\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}$ goes from 0 to +2. It has been oxidised.
The amount of Ag is decreased. Because it is in the +1 state in $\mathrm{AgNO}_{3}$ and reduced to O in Ag. In a single process, oxidation and reduction took place. As a result, it's a redox reaction.

Note:
Similar to acid–base reactions, oxidation and reduction occur concurrently and cannot occur independently of one another. Because two half-reactions usually occur together to produce a full reaction, oxidation and reduction are each called a half-reaction. In order to balance the half-reaction in terms of electric charge, the acquired or lost electrons are usually explicitly mentioned when writing half-reactions. When the half-reactions are combined to form the net chemical equation, the electrons cancel out.