The reaction you've written represents a double displacement $orprecipitation$ reaction between magnesium chloride $MgC{l}_2$ and silver nitrate $AgN{O}_3$. In this reaction, silver chloride $AgCl$ is formed as a precipitate along with magnesium nitrate $Mg(N{O}_3{)}_2$ being produced in solution.

Here's the balanced chemical equation:

$${\text{MgCl}}_2(aq)+2{\text{AgNO}}_3(aq)\to 2\text{AgCl}(s)+{\text{Mg(NO}}_3{\text{)}}_2(aq)$$

Explanation:

Reactants:

MgCl₂: Magnesium chloride, typically in aqueous solution.AgNO₃: Silver nitrate, also in aqueous solution.

Products:

AgCl: Silver chloride, which is insoluble in water and precipitates out as a solid $indicatedby(s)$.Mg$N{O}_3$₂: Magnesium nitrate, which remains in solution $indicatedby(aq)$.Reaction Process:When the two aqueous solutions are mixed, the cations and anions exchange partners.Silver ions $A{g}^{+}$ react with chloride ions $C{l}^{-}$ to form solid silver chloride $AgCl$.Magnesium ions $M{g}^{2+}$ react with nitrate ions $N{O}_3^{-}$ to form magnesium nitrate, which dissolves in water.Characteristics of the Reaction:This is a typical example of a precipitation reaction where an insoluble salt $precipitate$ forms when two soluble salts are mixed.The formation of a solid is often visible as a cloudy or milky appearance in the solution due to the formation of the precipitate.

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