Question

$\mathrm{Cs}$ react with Chlorine to form?

Answer 1

The reaction of $\mathrm{Cs}$ with Chlorine:

• Alkali metals are known to readily react with halogens to form ionic halides.
• Cesium as the most reactive metal forms cesium halides as it reacts strongly with all halogens.
• Hence, it reacts with chlorine (${\mathrm{Cl}}_2$) to produce cesium (I) chloride ($\mathrm{CsCl}$), which can be shown as:

$\underset{(\mathrm{Cesium})}{2{\mathrm{Cs}}^{+}\left(\mathrm{aq}\right)}+\underset{\left(\mathrm{Chlorine}\right)}{2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)}\to \underset{\mathrm{Cesium}\mathrm{chloride})}{2\mathrm{CsCl}\left(\mathrm{aq}\right)}$

• In this reaction, First, Cesium loses one of its electrons to form a Cesium ${\mathrm{Cs}}^{+}$ ion.
  $\mathrm{Cs}{}_{\left(\mathrm{g}\right)}\to {{\mathrm{Cs}}^{+}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-}$
• Then the Chlorine atom adds one electron to its valence shell to form $\mathrm{C}{\mathrm{l}}^{-}$ ion, given by
  $\mathrm{C}{\mathrm{l}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-}\to \mathrm{C}{{\mathrm{l}}^{-}}_{\left(\mathrm{g}\right)}$
• And finally, the Cesium ion and Chloride ion react with each other,to give Cesium chloride, given by
  ${\mathrm{Cs}}^{+}\left(\mathrm{aq}\right)+{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)\to \underset{(\mathrm{Cesium}\mathrm{Chloride})}{\mathrm{CsCl}\left(\mathrm{aq}\right)}$
• Also, the bond formed between the Cesium and Chlorine to form $\mathrm{CsCl}$ is an example of ionic bonding.

Hence,$\mathrm{Cs}$ react with Chlorine to form $\mathrm{CsCl}$ .