Transition metals and orbitals

In summary, the conversation discusses the formation of a π bond in transition metal species with multiple metal-carbon bonds. The π bond is formed when the lobes of a p orbital overlap with two of the lobes of a d orbital, which occurs above and below the plane described by the three sigma bonds of the CH2 group. To form the s portion of the M=C bond, hybrid orbitals such as dx^2-y^2 and dz^2 can be employed.
  • #1
plexus0208
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Homework Statement


Transition metal species are known that contain multiple metal-carbon bonds, for example, M=CH2. Describe how the π portion of the M=C bond would be formed using a pure d orbital on M and in what plane the protons on the CH2 group would lie. (A d orbital is employed because it is lower energy and because it extends out toward the carbon atom, which gives rise to better overlap with the orbital on C.) What hybrid orbitals could be employed to form the s portion of the M=C bond?

Homework Equations



The Attempt at a Solution


For the first part of the problem, I think you can use a dxz orbital on M when the carbon has a pz orbital. But what do they mean by what plane the protons on the CH2 group would lie? Also, advice on the last part of the question would be appreciated...
 
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  • #2
Pi bond is formed when the lobes of a p orbital overlap with 2 of the lobes of the d orbital. This would occur above and below the plane described by the three sigma bonds of the -CH2 group. There are 2 d orbitals on the metal that can interact in that way.
 
  • #3
dx^2-y^2 and dz^2?
 

1. What are transition metals?

Transition metals are a group of elements that are found in the middle of the periodic table. They are characterized by their ability to form multiple oxidation states and their partially filled d-orbitals.

2. What is the significance of d-orbitals in transition metals?

D-orbitals allow transition metals to have different oxidation states and form complex compounds. This is due to the ability of d-orbitals to participate in bonding with other atoms.

3. How many d-orbitals are present in a transition metal atom?

A transition metal atom has five d-orbitals: dxy, dxz, dyz, dz2, and dx2-y2.

4. What is the difference between 3d and 4d transition metals?

The main difference between 3d and 4d transition metals is the energy level of their d-orbitals. 3d transition metals have their d-orbitals filled with electrons in the third energy level, while 4d transition metals have their d-orbitals filled in the fourth energy level.

5. How do transition metals affect the properties of a compound?

Transition metals can greatly influence the properties of a compound due to their ability to form complex structures and multiple oxidation states. This can affect factors such as color, reactivity, and magnetic properties of the compound.

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