How would you write the net ionic equation for [Co (en) 2Cl2]Cl with AgNO3.
Is it AgNO3 ----> Cl^- + 3Ag^+?
Cl^- + Ag^+ ==> AgCl
Cl^- comes from the last Cl (the Cl outside the sphere of coordination) and the Ag^+ comes from the AgNO3.
To write the net ionic equation for a reaction, we need to start by first writing the balanced chemical equation.
The given reactants are [Co(en)2Cl2]Cl and AgNO3. When these two compounds react, a double replacement reaction occurs, where the chlorine ions from [Co(en)2Cl2]Cl switch places with the nitrate ions from AgNO3.
The balanced chemical equation is:
[Co(en)2Cl2]Cl + 2AgNO3 → 2AgCl + [Co(en)2(NO3)2]Cl
Now, to write the net ionic equation, we need to remove the spectator ions, which are the ions that appear on both sides of the equation without undergoing any change. In this case, the chloride ions (Cl-) and the nitrate ions (NO3-) are spectator ions.
The net ionic equation is:
[Co(en)2Cl2]Cl + 2AgNO3 → 2AgCl + [Co(en)2(NO3)2]Cl
Therefore, the net ionic equation for the reaction between [Co(en)2Cl2]Cl and AgNO3 is not AgNO3 ----> Cl^- + 3Ag^+.