[Al(OH)4] is a complex that Na is bound up to. Na forms a +1 cation when making ionic bonds. This means that the entire [Al(OH)4] has a -1 charge. Then, looking in this complex, you have Al and OH. OH has a -1 charge and there are four of them, so you have a next of -4 from hydroxide. Now the entire [Al(OH)4] complex needs to be net -1, so Al must be 3+ in order to balance out the -4 from hydroxides. Make sense?Hello,
This is a question from AAMC 9 that im having trouble getting:
What is the oxidation state of aluminum in Na[Al(OH)4) that 4 should be a subscript. They say the answer is +3 but i cant wrap my head around it. Thanks!