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aaronq

  • 2 years ago

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

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  1. aaronq
    • 2 years ago
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    i figure that it's because of the d orbital availability but I'm unsure

  2. aaronq
    • 2 years ago
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    ps the complex I'm talking about is Chromium (II) acetate hydrate

  3. Preetha
    • 2 years ago
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    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.

  4. aaronq
    • 2 years ago
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  5. aaronq
    • 2 years ago
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    it's actually a dimer, with bridging acetate ligands and 2 waters at the ends of the Z axis

  6. Preetha
    • 2 years ago
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    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.

  7. aaronq
    • 2 years ago
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    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

  8. aaronq
    • 2 years ago
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    Thank you, Preetha. I will try my luck tomorrow at school.

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