Crystal Field Theory
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- Опубликовано: 14 окт 2024
- We are used to using a theory like VSEPR theory to predict molecular geometry, but unfortunately with coordination compounds, things are not so simple, because of those pesky d orbitals on the central metal atom. Crystal field theory is a model that is quite successful in predicting the geometries of these compounds, as well as other characteristics, like magnetic behavior, and color, so let's learn about this theory now!
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This topic is taught to what grade student -schooling or college or other ???
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I like your explanations. They are brief and concise. I have a background in Chemistry. When it comes to ligands, do we not have pi acceptor and pi donor ligands? If you do not have a video on that could you do one? Also do you have something on the spectrochemical series?
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So why exactly do the ligands repel these orbitals making them energetically unfavorable while in classic bond theory we explain the formation of a chemical bond by OVERLAPPING orbitals?
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Thanks
Very short time....you are give the nice explanation about crystal field theory
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Hi, I absolutely love your videos, they have already helped me a lot throughout my undergrad degree, so thanks a lot!! Just one question, at 5:16 in your diagram for square planar complexes, shouldn’t the dz2 orbital be lower in energy than the dxy orbital?
Yes it should be. In order of highest to lowest:
(dx2-y2) > (dxy) > (dz2) > (dxz, dyz)
This is so good. Thanks a lot!
Can you explain when two more more different ligands are coordinated and how these affects the high spin and low spin complexity
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Thanks sir I got your all points but cofused in axis of d orbitals
I remember it by the exponent meaning on the axis (e.g. x^2 - y^2 means the orbitals are on the x and y axis, and z^2 meaning the orbitals are on the z axis) and for the orbitals that are in between the axis, the notation tells you which axis they are between (e.g. xz means the orbital lies between the x and z axis, yz means the orbital lies between the y and z axis, and xy means the orbital lies between the x and y axis). Hope that helps!
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Can we have one explaining the interactions of the lobes and electrostatic repulsion to
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So weak field ligands show less colour and strong filled ligands show more colour as the difference in energies is sfl is greater than wfl, right?
This is a great one.
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Awesome!!!! i can now understand coordination compound crystal clear! XD
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Sir please explain innert pair effect
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Sir Please explain stereoisomerism in coordination compounds 🙏🙏🙏
Sir does crystal field theory has any limitations?
so many limitations
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Can you also make a video on Ligand Field theory???
That's coming in the inorganic series!
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What is the CFSE value of co(NH3)6+3
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Hello , I have seen on internet that shape of dz² is square planar . Is it correct ? And what do it mean even ?
no there are no two-dimensional orbitals, check out my tutorial on quantum numbers for the orbital shapes
@@ProfessorDaveExplains ok , thank you
At 4:54, it ligands approach dxy dxz dyz, so it means in tetrahedral higher energy shells get filled first? But in octahedral the lower shell got filled?
So it's always the lower-energy orbitals that get filled first, it's just that the identity of the lower-energy orbitals changes depending on the geometry.