Generally in a chemical reaction, you should put phase states all the time. I think personally it's even more important for net ionic equations.
I vaguely remember that putting the phase states for the products and the reactants was worth like 1 point on the AP Chemistry test.
I might be wrong, though.
Take for example HCL.
As a gas, HCL(g) is called hydrogen chloride gas.
But, when hydrogen chloride gas is dissolved in water to form an aqueous solution(aq) - you get the all too familiar hydrochloric acid.
HCL(g) = hydrogen chloride
HCL(aq) = hydrochloric acid
For a net ionic equation that yields HCL ... one could see how different interpretations could arise to due a lack of phase symbols.
Generally in a chemical reaction, you should put phase states all the time. I think personally it's even more important for net ionic equations.
I vaguely remember that putting the phase states for the products and the reactants was worth like 1 point on the AP Chemistry test.
I might be wrong, though.
Take for example HCL.
As a gas, HCL(g) is called hydrogen chloride gas.
But, when hydrogen chloride gas is dissolved in water to form an aqueous solution(aq) - you get the all too familiar hydrochloric acid.
HCL(g) = hydrogen chloride
HCL(aq) = hydrochloric acid
For a net ionic equation that yields HCL ... one could see how different interpretations could arise to due a lack of phase symbols.
Using Episkey's example:
For HCl, you don't need to indicate charge, but when you actually do net ionic equations or such, you NEED to indicate charge for aqueous ions, like H+(aq) and Cl-(aq).
[FONT="Times New Roman"]I guess it probably wouldn't hurt to do it anyways (and it wouldn't take long either). By the way, are you still playing mabi? I haven't seen you on Ruairi in forever.[/FONT]
Using Episkey's example:
For HCl, you don't need to indicate charge, but when you actually do net ionic equations or such, you NEED to indicate charge for aqueous ions, like H+(aq) and Cl-(aq).
Usually, salts like NaCl become free ions in solution so unless the salt is dissolved you can consider it a solid. If it's in water, (aq). The only gas phase ions that I can think of off the top of my head are... Radical species that you won't have to worry about, Ammonium, NO2, and Ozone. Elemental gases all have a formal charge of 0.
You learn something new every day! :skip:
I was like .. aha! "But there's H+" ... Then I said to myself, but that's found in aqueous solutions ... yeah.
Couldn't noble gaseous ions also be an example? Or are they not gas particles anymore, once they become ions?
Of course ions of noble gases aren't common.
In my years of taking Chemistry, I only saw He+ once on a test.
[SPOILER="Spoiler"]Happy second bar![/SPOILER]
You learn something new every day! :skip:
I was like .. aha! "But there's H+" ... Then I said to myself, but that's found in aqueous solutions ... yeah.
Couldn't noble gaseous ions also be an example? Or are they not gas particles anymore, once they become ions?
Of course ions of noble gases aren't common.
In my years of taking Chemistry, I only saw He+ once on a test.
[SPOILER="Spoiler"]Happy second bar![/SPOILER]
Noooo, must talk about mooooorreeeee chemistry!
[FONT="Times New Roman"]Exactly! I still have a whole semester (and the summer) before I start college (and go into Biochemistry) But I wouldn't expect to find any noble gas containing molecules in something that's still alive <.< (Helium = high voice lulz?)
Anyhow, this thread's purpose should be over, I'll be closing it I guess
Edit: nvm, i dunno how to do that[/FONT]
Noooo, must talk about mooooorreeeee chemistry!
[FONT="Times New Roman"]Kk, what makes a salt bridge balance a galvanic cell thingy? I don't think I understand how (not that I need to know for class)[/FONT]