Write the net ionic equation for the precipitation reaction between ammonium sulfide and cadmium nitrate.

Sure thing! Let's see what happens when our buddy ammonium sulfide meets cadmium nitrate:

Ammonium sulfide (NH4)2S + Cadmium nitrate Cd(NO3)2

First, let's break them down into their ions:

(NH4)2S -> 2 NH4+ + S2-
Cd(NO3)2 -> Cd2+ + 2 NO3-

Now, let's swap the ions so we get the potential products:

2 NH4+ + Cd2+ + 2 NO3- + S2-

And it's time to party! But what's that? It seems like some of our ions will form an insoluble compound, resulting in a precipitate. In this case, the insoluble compound is CdS, which is more commonly known as cadmium sulfide.

So, when our friend ammonium sulfide drops by, the net ionic equation is:

Cd2+ + S2- -> CdS (precipitate)

Voila! The cadmium ions (Cd2+) and sulfide ions (S2-) team up to create the lovely cadmium sulfide precipitate. Ah, chemistry... always finding new ways to bring people together!

To write the net ionic equation for the precipitation reaction between ammonium sulfide (NH4)2S and cadmium nitrate Cd(NO3)2, we need to identify the soluble compounds and the insoluble precipitate formed.

The soluble compounds are ammonium nitrate (NH4NO3) and cadmium nitrate (Cd(NO3)2), while the insoluble precipitate is cadmium sulfide (CdS).

First, let's write the balanced equation for this reaction:

(NH4)2S + Cd(NO3)2 -> CdS + 2NH4NO3

Next, we will separate the soluble compounds into their constituent ions:

(NH4)2S (aq) + Cd(NO3)2 (aq) -> CdS (s) + 2NH4NO3 (aq)

Now, we need to eliminate any spectator ions that do not participate in the formation of the insoluble precipitate. In this case, the nitrate ions (NO3-) and the ammonium ions (NH4+) are spectator ions. Thus, we can write the net ionic equation:

S2- (aq) + Cd2+ (aq) -> CdS (s)

Therefore, the net ionic equation for the precipitation reaction between ammonium sulfide and cadmium nitrate is:

S2- (aq) + Cd2+ (aq) -> CdS (s)

To write the net ionic equation for a precipitation reaction, we first need to identify the species that form insoluble compounds. In this case, ammonium sulfide (NH42S) and cadmium nitrate (Cd(NO3)2) are the reactants.

1. Write the balanced molecular equation:
NH42S + Cd(NO3)2 -> CdS + 2NH4NO3

2. Determine the states of each compound:
NH42S (aq) + Cd(NO3)2 (aq) -> CdS (s) + 2NH4NO3 (aq)

3. Split the soluble compounds into ions:
NH42S (aq) -> 2 NH4+ (aq) + S2- (aq)
Cd(NO3)2 (aq) -> Cd2+ (aq) + 2 NO3- (aq)
2 NH4NO3 (aq) -> 2 NH4+ (aq) + 2 NO3- (aq)

4. Write the net ionic equation by eliminating spectator ions:
S2- (aq) + Cd2+ (aq) -> CdS (s)

Therefore, the net ionic equation for the precipitation reaction between ammonium sulfide and cadmium nitrate is:
S2- (aq) + Cd2+ (aq) -> CdS (s)

(NH4)2S(aq) + Cd(NO3)2(aq) ==> CdS(s) + 2NH4NO3(aq) is the molecular equation.

S^-2(aq) + Cd^+2(aq) ==> CdS(s) is the net ionic equation.