How to Write the Net Ionic Equation for AgNO3 + NaCl = AgCl + NaNO3

To write the net ionic equation for AgNO3 + NaCl = AgCl + NaNO3 (Silver nitrate + Sodium chloride) we follow main three steps. First, we balance the molecular equation.
Second, we break the soluble ionic compounds into their ions (these are the compounds with an (aq) after them). Finally, we cross out any spectator ions. These are the ions that appear on both sides of the ionic equation.
If you are unsure if a precipitate will be present when writing net ionic equations, you should consult a solubility table for the compound. Another option to determine if a precipitate forms is to have memorized the solubility rules. In this reaction, AgCl will be insoluble and will be a precipitate (solid) and fall to the bottom of the test tube. We therefore write the state symbol (s) after the compound that precipitates out of solution.
If you are unsure if a compound is soluble when writing net ionic equations you should consult a solubility table for the compound.
General Steps:
1. Write the balanced molecular equation.
2. Write the state (s, l, g, aq) for each substance.
3. Split soluble compounds into ions (the complete ionic equation).
4. Cross out the spectator ions on both sides of complete ionic equation.
5. Write the remaining substances as the net ionic equation.
Writing and balancing net ionic equations is an important skill in chemistry and is essential for understanding solubility, electrochemistry, and focusing on the substances and ions involved in the chemical reaction and ignoring those that don’t (the spectator ions).
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[@wbreslyn]

Glad I could help with AgNO3 + NaCl! --- Dr. B

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[@f1yguy4]

Isn't Chlorine diatomic? So why isn't it Cl2 negative 1

[@jackdowling1725]

Do the Na+ and No3- not form any product on the right side of the arrow because it is still (aq) so no solid was formed and they are still separated in their ions in the solvent? If so, would you always cross out any substance that has (aq) on the right side of the arrow?

[@wbreslyn]

Yes, they would be spectator ions. You started out with Na+ and NO3- in solution. And they are still in solution when the reaction is over. AgCl however is a solid and is the precipitate.

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[@veronicaroberts4296]

THANK YOU!!!! Can someone tell me how you know which atoms switch with the others in the compounds?

[@wbreslyn]

Usually the metals (they have positive charges).

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[@nickyjim12]

NaCl is a solid? I have a textbook in front of me that identifies it as one!

[@SoupIsSouppy]

NaCl is table salt

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[@isaacclarke5334]

Hi, can you help me with this one? Sb2S3+ HNO3--- Sb2O5+NO2+S+H2O

[@wbreslyn]

Take a look at this and work backwards ... that should help! www.webqc.org/balance.php?reaction=Sb2S3%2BHNO3%3DSb2O5%2BNO2%2BS%2BH2O - Dr. B

[@Gwyllgi]

I don't mean to be rude, but you don't really show why you do things. Like why you cross out spectator ions, or how you know which is positive and negative. This is just showing the answer, not how to get there.