Could you please check my work about complete ionic and net ionic equations. They really confuse me. My original equation, after I balanced, was:
FeCl2(aq)+Na2S(aq)=FeS(s)+2NaCl(aq). For complete Ionic I think its:
Fe^2+^(aq)+2Cl^-^(aq)+2Na^+^(aq)+S^2-^=FeS(s)+2Na^+^(aq)+2Cl^-^(aq). If that part is correct, I am uncertain if the net ionic would be this:
Fe^2+^(aq)+S^2-^ = FeS(s) I'm still new at this and find it very confusing so any feedback would be appreciated.
Your complete balanced equation is correct. Good work!
Your complete ionic equation is correct except for omitting the (aq) on S^2-(aq) on the left. I'm sure that's just a typo. Still a good job!
Now, how do you turn a complete ionic equation into a net ionic? You've done the hard part; this is the easy part.
Just cancel any ion common to both sides.
Here is your complete ionic equation with the S^2-(aq) correction I made to it.
Fe^2+^(aq)+2Cl^-^(aq)+2Na^+^(aq)+S^2-(aq) = FeS(s)+2Na^+^(aq)+2Cl^-^(aq)
Fe^2+(aq) on the left is not on the right so it stays. 2Cl^-(aq) on the left and the same on the right cancel. Cross those out. 2Na^+(aq) on the left and right cancel. Cross those out. S^2-(aq) on the left is not matched on the right so it stays. That leaves also FeS(s) on the right with none on the left so it stays. What's left is the NET ionic equation.
Fe^2+(aq) + S^2-(aq) ==> FeS(s)
Your complete ionic equation appears to be correct. It correctly breaks down all soluble compounds into their individual ions.
For the net ionic equation, you are on the right track, but you need to consider the charges of the ions involved. The net ionic equation only includes the species that are directly involved in the chemical reaction.
In this case, Fe^2+ and S^2- ions react to form FeS. Since both Fe^2+ and S^2- ions have charges of 2-, there is no need to balance the charges. Therefore, the net ionic equation is:
Fe^2+ (aq) + S^2- (aq) → FeS (s)
This equation represents the essential chemical change occurring in the reaction, without including spectator ions (ions that are present on both the reactant and product side but do not participate in the reaction).
Great job on balancing the original equation and identifying the ionic equations! Keep practicing, and it will become less confusing over time.
To check your work on complete ionic and net ionic equations, let's break it down step by step.
First, you correctly balanced the original equation:
FeCl2(aq) + Na2S(aq) = FeS(s) + 2NaCl(aq)
Now, let's determine the complete ionic equation. In the complete ionic equation, we write all the soluble ionic compounds as separate ions:
Fe^2+(aq) + 2Cl^-(aq) + 2Na^+(aq) + S^2-(aq) = FeS(s) + 2Na^+(aq) + 2Cl^-(aq)
You correctly identified the ions present in solution, including Fe^2+, Cl^-, Na+, and S^2-, and kept FeS as a solid precipitate.
Lastly, we'll find the net ionic equation. In the net ionic equation, we eliminate the spectator ions (ions that appear on both sides of the equation and don't participate in the reaction) to focus on the essential reaction:
Fe^2+(aq) + S^2-(aq) = FeS(s)
You correctly identified the net ionic equation by removing the spectator ions (Na+ and Cl^-) from the equation.
Overall, your work is correct! You successfully balanced the equation, wrote the complete ionic equation, and then determined the net ionic equation. It's great to see that you're working through this topic and asking for feedback. Keep practicing, and it will become less confusing over time.