I need some help with net ionic equations. I can do single replacement, double replacement, etc., but I don't get stuff like gas forming-reactions or the trends when stuff like a strong acid and water are the reactants.
Examples:
1. Moist sodium hydroxide reacts with carbon dioxide gas.
2. Rubidium permanganate is added to solid silver iodide.
Help please? Thank you!
I'm not sure of your general question. For the two questions posted, however,
1. NaOH(moist aq) + CO2 ==> Na2CO3 is a synthesis reaction.
2. RbMnO4 + AgI ==> is a redox reaction. I would expect the MnO4^- to oxidize I^- to I2 and MnO4^- to be reduced. In the dry state, however, I don't think any reaction will take place; i.e., the redox reaction will only occur in aq solution.
Sure, I can help you understand how to write net ionic equations for these types of reactions.
1. Moist sodium hydroxide reacts with carbon dioxide gas:
To write the net ionic equation, you first need to know the balanced complete ionic equation. Let's start with the balanced chemical equation:
NaOH (aq) + CO2 (g) -> Na2CO3 (aq) + H2O (l)
From the balanced equation, we can identify the spectator ions, which are the ions that are present on both sides of the equation and do not participate in the reaction. In this case, sodium ions (Na+) and hydroxide ions (OH-) are the spectator ions.
The net ionic equation only includes the species that undergo a chemical change. Therefore, we remove the spectator ions from the equation:
CO2 (g) + H2O (l) -> Na2CO3 (aq)
This is the net ionic equation for the reaction between moist sodium hydroxide and carbon dioxide gas.
2. Rubidium permanganate is added to solid silver iodide:
Again, we start with the balanced chemical equation:
2 RbMnO4 (aq) + 3 AgI (s) -> 3 AgMnO4 (s) + 2 RbI (aq)
To write the net ionic equation, we identify the spectator ions, which in this case are rubidium ions (Rb+) and iodide ions (I-).
The net ionic equation will then only include the species that undergo a chemical change:
2 RbMnO4 (aq) + 3 AgI (s) -> 3 AgMnO4 (s) + 2 RbI (aq)
Once again, it is the same as the original balanced equation. Therefore, no ions are spectator ions, and the entire balanced equation is the net ionic equation.
In general, when you have gas forming reactions or reactions involving strong acids and water, the net ionic equation may often be the same as the balanced equation. This is because the ions in these reactions typically participate in the reaction itself, without any spectator ions present.
It's important to note that writing net ionic equations requires a good understanding of chemical reactions, balanced equations, and identifying spectator ions. Practice and familiarization with different reaction types will strengthen your understanding of how to write net ionic equations.