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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: 0rion on March 23, 2009, 03:34:04 AM

Title: Oxidation states of Transition metals?
Post by: 0rion on March 23, 2009, 03:34:04 AM
Hey guys

How do you work out the oxidation state of a transition metal?

Take AlPO3 for example...

so O is 2-, making it 6-

then im guessing Al is + something and P just makes it equal zero from there (thats how ive been taught)

But how do you work out what Al is? I know it can have multiple valencies, so i dont know how to specify its oxidation state :S

thanks guys

Title: Re: Oxidation states of Transition metals?
Post by: macman104 on March 23, 2009, 03:47:46 AM
Split them first, if you can into ions, cation and anion.  Find each individual oxidation state, then combine.

Can you split AlPO3 into a cation/anion pair?
Title: Re: Oxidation states of Transition metals?
Post by: 0rion on March 23, 2009, 04:43:39 AM
*slaps head* i have now split the molecule...

what is the oxidation state of Al?
Title: Re: Oxidation states of Transition metals?
Post by: macman104 on March 23, 2009, 04:48:43 AM
What did you split them into, and can you include the charges on the ions?

This is an neutral ionic compound, so the charges of the anion and cation must be equal.