Answer:
[tex]\mathrm{Ca}^{2+} \text { and } \mathrm{Cl} \text { - ions are present in } 1: 2 \text { ratio in a solution of aqueous calcium chloride. }[/tex]
Explanation:
Here in Calcium Chloride ionic bond is present in between calcium and chlorine atoms. As we know according to Octet rule calcium have two excess atoms and for matching nearest noble gas electronic configuration. It donate two electrons to gain more stability and form [tex]\mathrm{Ca}^{2+}[/tex], while chlorine is deficient from one electron to meet nearest noble gas electronic configuration therefore two chlorine atoms accept excess electron from calcium individually and form two[tex]\mathrm{Cl}^{-}[/tex] ions.
[tex]\text { Equation is as follows: } \mathrm{Ca}^{2+}+2 \mathrm{Cl}^{-} \rightarrow \mathrm{CaCl}_{2}[/tex]
Hence aqueous solution of calcium chloride breaks the ionic bond pairing in one [tex]\mathrm{Ca}^{2+}[/tex]and two[tex]\mathrm{Cl}^{-}[/tex]ions: [tex]\mathrm{CaCl}_{2} \longrightarrow \mathrm{H}_{2} \mathrm{O} \quad \mathrm{Ca}^{2+}(\mathrm{ag})+2 \mathrm{Cl}(\mathrm{ag})[/tex]
