[0rion]

Here i am again, marked wrong by Wiley. On all accounts.

Tell me if ive done this wrong or if im just being trodden on again.

Determine the molecular shape and the ideal bond angles of each of the following:
    
Shape of SO3? -> Trigonal Pyramidal
   
Ideal bond angles in SO3?

109.5
    
Shape of I3+? (does this molecule even exist? isnt it meant to be I3-?)

Linear
    
Ideal bond angles in I3+?

180
    
Shape of SbCl52-?

Trigonal Bipyramidal
    
Ideal bond angles in SbCl52-?

This is the part where i got stuck, its a multiple choice thing and it only lets you choose one, so i didnt know whether to pick 90 or 120? In the end i picked 120 and got marked wrong
    
Shape of XeO4?

Square Planar
    
Ideal bond angles in XeO4?

90 degrees

I was marked wrong for ALL of the above, and if they're wrong, why? What am i doing so horribly wrong?

[0rion]

Oh crap, i see what i did wrong for SO3, lol sorry, i mistook it for SO4(2-)

Sorry about that lol :S

But still what the heck is I3+?

And where have i gone wrong with the others

[UG]

XeO4 has a tetrahedral structure with double bonds to each of the oxygens.

[promiseoffaith]

i did it and only got the I₃⁺
one wrong. 

the shape of SbCl₅^2- is square pyramidal
and its bond angles are 90 degrees. 

[Xenophilius]

I₃⁺ has sp³ hybridisation and pyramidal structure.Did I get it right??

[Amanda165]

for I_3⁺ the shape is bent because you have three iodines all joined by single bonds, once you place the rest of the electrons around the central I atom, there are 2 lone pairs, in order to minimise repulsion the shape of it is bent, therefore the angles are 109.5degrees. i just did the same questions on wiley and got that one right.

hope this helps