Not shure wheter this counts as homework help or science education. The lecturer asked us to find out about the electron structures of 3 ions:Co+ , Zn(2+) and Br+ that is suppose to differ from the basic rule/principle for determening the basic electron configuration of ions. I can't find anything on what makes these three ions different from the rest in the textbook i have and would realy appreciate it if some of you guys can please help me with it.

If you can tell us what answers you're working our them, it would help us see if you're doing anything wrong. The best hint I can give you is to make sure you pay attention to which orbitals have the highest energy when you are removing them to generate your ions. This should be easy for the bromonium ion (which is a weird example to have given you, by the way; are you sure that one is written down correctly?), but the cobalt and zinc being transition metals are slightly different, although the logic is the same; electrons are removed from the highest energy orbitals first.

It seems we misunderstood the lecturer. She only wanted to make shure we remember that the 4s orbital has an higher energy value than the 3d orbital in ions unlike in regular atoms. And i'm well aware that a Br+ ion would not form under any natural curcumstances. Please excuse my terminology, i'm not English.

 

 

Well, it does, it's just a weird thing to ask you. And yes, I was hinting towards what you've managed to work out.