What ions do i need to start learning off by heart? (year 11)

[Raptor]

My textbook has a table which contains various ions and my teacher told me to remember them, however im not sure if it contains all of the ions, can someone please link me to a table or confirm the one i have now has all the ions that i have to know? I'd like to print it out and put it on my wall so a table would be great. I already have this http://www.matrix.edu.au/wp-content/uploads/2012/08/blog_3_solubilityrules.png (is that everything for solubility?) 

Thank you very much.

[clıppy]

That seems like all the ions you'd need to know.
Maybe it was just me but I never actively tried to remember them, I just did enough chemistry questions throughout the years that I learnt them from over-exposure. And if there's something I didn't know, more often than not I could figure it out. Like MgX. if Mg is 2+ then X has to be 2-.

Although with that in mind, it's certainly not a waste to memorise them. It's definitely useful.

[Raptor]

Fair enough, i'm just worried about the poly-atomic ions..
Thanks for the reply though!

[jgoudie]

Yeah this is the Heinemann textbook, these ions are more than enough. 

Focus on the polyatomic ions as the simple ones can mostly be figured out from the name or location on the periodic table:
Copper(I) = Cu⁺,
Copper(II) = Cu²⁺

non-transition elements from their place on the periodic table. 
Mg - group 2 - Mg²⁺,
Cl - group 7 - Cl^-

The free chemisode app I have for iphone and ipad also has common ion flash cards if you are looking for some easy self testing.

My textbook has a table which contains various ions and my teacher told me to remember them, however im not sure if it contains all of the ions, can someone please link me to a table or confirm the one i have now has all the ions that i have to know? I'd like to print it out and put it on my wall so a table would be great. I already have this http://www.matrix.edu.au/wp-content/uploads/2012/08/blog_3_solubilityrules.png (is that everything for solubility?) 

Thank you very much.

[Raptor]

Yeah this is the Heinemann textbook, these ions are more than enough. 

Focus on the polyatomic ions as the simple ones can mostly be figured out from the name or location on the periodic table:
Copper(I) = Cu⁺,
Copper(II) = Cu²⁺

non-transition elements from their place on the periodic table. 
Mg - group 2 - Mg²⁺,
Cl - group 7 - Cl^-

The free chemisode app I have for iphone and ipad also has common ion flash cards if you are looking for some easy self testing.

Is there anything else? Thanks, ill add it to the table.
Oh sweet, ill check out the app now!

[lzxnl]

Simple guide (IMO) to working out ions:

Main group (s, p block), look at the group and you should be able to work out how many electrons to remove or add to form a stable octet. For instance, magnesium is 1s2 2s2 2p6 3s2 (group 2), so it tries to lose two electrons. Similarly, fluorine is 1s2 2s2 2p5 (group 17), so it tries to gain an electron. Use the periodic table!

For polyatomic ions, it may be helpful to find other ways of knowing these ions. Ethanoate ion, for instance, is the conjugate base of ethanoic acid, which is CH₃COOH (you'll need to know this for 1/2 anyway), so the ethanoate ion is CH₃COO^-. Phosphate has an 'ate' ending, indicating that the number of oxygens bonded to the phosphorus is a maximum of 4 (similar to sulfate, although permanganate and perhalates like perchlorate follow a slightly different custom as halogens can bond with from zero to four oxygens), so we have PO₄ with some charge. Phosphorus has 5 valence electrons. If you think of phosphorus as losing all these electrons and bonding to four oxide ions (not quite true but it's a way of remembering it), you'll see that phosphate has a charge of -3. Similarly, sulfate has 4 oxygens as well and sulfur has 6 valence electrons, so thinking of sulfur losing all these electrons to form oxide ions and we have a charge of -2 (this is really an introduction to oxidation numbers hahaha). Thus, sulfate is SO₄^2-.
Nitrogen can only bond to three oxygens, so nitrate consists of a nitrogen bonded to three oxygens. Five valence electrons, three oxides => -1 charge, so nitrate is NO₃^-.
Nitrite is a funny thing because it has the same charge as nitrate but one less oxygen (just remember that). Same with sulfite (SO₃^2-).
If you have something like hydrogen sulfate, think adding a sulfate anion with a positive proton. Add a hydrogen and increase the charge by 1 to get HSO₄^-.

Transition metals (d block) can have differing charges, so the charge is always indicated by a letter. Cu(II) would then be a copper cation after losing two electrons.

I hope this made some sense.