Molecular, complete ionic, and net ionic equations. Practice: Net ionic equations. Next lesson.
Current timeTotal duration Google Classroom Facebook Twitter. Video transcript - how to write ionic equation What we have here is a molecular equation describing the reaction of some sodium chloride dissolved how to write ionic equation water plus some silver nitrate, also dissolved in the water.
They're going to react to form sodium nitrate, still dissolved in water, plus solid silver chloride and if you were to look at each of these compounds in their crystalline or wrte form before they're dissolved in water, they each look like this. But once you get dissolved in water, and that's what this aqueous form tells us, it tells equatlon that each of these compounds are going to get dissolved in water, they're no longer going to jonic in that crystalline form, crystalline form.
Instead, you're going to have the individual ions disassociating. So for example, in the case of sodium chloride, the sodium is going to disassociate in the water.
Sodium is a how to write ionic equation ion, or cation, and so it's going to be attracted to the partially negative oxygen end. Remember, water is a polar molecule. That's what makes it such a good solvent. Now, the chloride anions, similarly, are going to dissolve in water 'cause they're going to be attracted to the partially positive hydrogen ends of the water molecules and the same gravity research foundation essays is gonna be true of the silver nitrate.
Contributions and Attributions
The silver ion, once it's disassociated, is inic to be positive and the nitrate is a negative. It is an anion. Now, in order to appreciate this and write an equation that better conveys the disassociation how to write ionic equation the ions, we could instead write the equation like this. This makes it a little bit clearer that look, the sodium and the chloride aren't going to be necessarily together anymore.
The how to write xml in perl is going to dissolve in the water, like we have here.
The chloride is gonna how to write ionic equation in the water. The silver ions are going to dissolve in the water and so are the nitrate ions. So this makes it a little bit clearer and similarly on this end with the sodium nitrate stays dissolved so we can write it like this with the individual ions disassociated.
But the silver chloride is in solid form. You wrige think of it as precipitating out of the solution. This is not This does not have a high solubility, so it's not going to get dissolved in the water and so we still have it in solid form. Now you might say, well which of these is better?
Net ionic equations
Well it just depends what you are trying to go for. This form up here, which we see more typically, this is just a standard molecular equation.