Complete and balance the following equations. If no reaction...

Complete and balance the following equations. If no reaction occurs, write $\mathrm{NR}$. (a) $\mathrm{Cl}_{2}(\mathrm{~g})+\mathrm{Br}^{-}(\mathrm{aq}) \longrightarrow$ (b) $\mathrm{I}_{2}(\mathrm{~s})+\mathrm{Cl}^{-}(\mathrm{aq}) \longrightarrow$ (c) $\mathrm{I}_{2}(\mathrm{~s})+\mathrm{Br}^{-}(\mathrm{aq}) \longrightarrow$ (d) $\mathrm{Br}_{2}(\ell)+\mathrm{Cl}^{-}(\mathrm{aq}) \longrightarrow$

Complete and balance the following equations. If no reaction occurs, write $\mathrm{NR}$.
(a) $\mathrm{Cl}_{2}(\mathrm{~g})+\mathrm{Br}^{-}(\mathrm{aq}) \longrightarrow$
(b) $\mathrm{I}_{2}(\mathrm{~s})+\mathrm{Cl}^{-}(\mathrm{aq}) \longrightarrow$
(c) $\mathrm{I}_{2}(\mathrm{~s})+\mathrm{Br}^{-}(\mathrm{aq}) \longrightarrow$
(d) $\mathrm{Br}_{2}(\ell)+\mathrm{Cl}^{-}(\mathrm{aq}) \longrightarrow$

Key Concepts

Halogen Displacement Reactions

This concept involves reactions in which a more reactive halogen displaces a less reactive halogen from its compound or ionic form. It is fundamental in understanding why, for example, a halogen in its elemental form might oxidize a halide ion of another halogen to form a new compound, depending on their relative reactivities.

Activity Series of Halogens

The activity series of halogens is an ordered list that ranks halogens by their ability to act as oxidizing agents, generally following the order from fluorine being the most reactive to iodine being the least. This series is used to predict the direction of halogen displacement reactions; a halogen higher in the series will displace one below it from its ionic compounds.

Oxidation-Reduction (Redox) Reactions

Redox reactions involve the transfer of electrons between chemical species, where one species undergoes oxidation (loss of electrons) and another undergoes reduction (gain of electrons). In the context of halogen reactions, the elemental halogen is typically reduced while the halide ion is oxidized if the reaction is favorable.

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the reaction, reflecting the conservation of mass. In redox reactions, balancing also requires equalizing the charge by accounting for the electrons transferred, which can involve separating the reaction into oxidation and reduction half-reactions.

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