Question

Using the sample question above, show the complete ionic and net ionic forms of the following equations. If all species are spectator ions, please indicate that there is No Net Ionic Equation. 

Note: you need to make sure the original equation is balanced before proceeding!

1.     Molecular Equation: 

MnCl₂ (aq) + (NH₄)₂CO₃ (aq)  MnCO₃ (s) + NH₄Cl (aq)

Complete Ionic Equation: 

Net Ionic Equation:

Identify spectator ions: 

Answer 1

1.     Molecular Equation: After balancing the equation we have

MnCl_2(aq) + (NH₄)₂CO_3(aq)  $\to$  MnCO_3 (s) + 2 NH₄Cl_(aq)

Complete Ionic Equation: By separating the ionic substances we have

 $Mn^{+2}_{(aq)} + 2 Cl^-_{(aq)} + 2 \,{NH_4}^+_{(aq)} +CO^{-2}_{3\, (aq)} \to MnCO_{3\,(s)}+2 \,{NH_4}^+_{(aq)}+2 Cl^-_{(aq)}$

Net Ionic Equation: The non-spectator ions (and the product they form) are represented by

$Mn^{+2}_{(aq)} +CO^{-2}_{3\, (aq)} \to MnCO_{3\,(s)}$

Identify spectator ions: The only ions that are present as reactants and products are the $Cl^- \text{ and } NH^+_4$ aqueous ions.

Reference

• Chang, R., & Goldsby, K. A. (2010). Chemistry. Chemistry, 10th ed.; McGraw-Hill Education: New York, NY, USA.