My brain seems to be malfunctioning...why does quadruple bonding occur (in Cr2+) if it’s uncommon in 1st row transition metals?

Question

aaronq · Answer

i figure that it's because of the d orbital availability but I'm unsure

aaronq · Answer

ps the complex I'm talking about is Chromium (II) acetate hydrate

preetha · Answer

What do you mean by quadruple bonding?  Chromium acetate is a simple ionic compound.  The electronic config of Cr is 4s13d5.  The electronic config of Cr+2 is 3d4.  2 electrons are lost.

aaronq · Answer

attachment

aaronq · Answer

it's actually a dimer, with bridging acetate ligands and 2 waters at the ends of the Z axis

preetha · Answer

Ah. Ok, We are talking coordination chemistry.  Ok.You are right.  It has empty d orbitals.
And according to wikipedia you are right.  There is a quadruple bond between the two chromiums.

aaronq · Answer

I found an MO diagram of the bonding, and it apparently consists of a sigma, 2 pi, and one delta bond. i mean i understand why it's bonding and the splitting of the d orbitals. but i'm just not sure why other 1st row transition metals would not be able to form such bonds, i think i came across copper (II) being able to

aaronq · Answer

Thank you, Preetha. I will try my luck tomorrow at school.