All Questions
Tagged with orbitals transition-metals
19
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Do the paired electrons of subshells' degenerate orbitals contribute to the total exchange energy?
For instance, in d7, there are 5 electrons with the same spin, and 2 electron with the opposite spin, meaning that there are only 3 unpaired electrons. So, which of these would be correct?
(i) Total ...
11
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2
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Exchange energy of d6 configuration
In NCERT Chemistry book, it is given as:
Exchange energy is responsible for the stabilization of energy state. Exchange energy is approximately proportional to the total number of possible pairs of ...
2
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0
answers
70
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Ionic radius for tetrahedral metal–ligand complexes
The ionic radii for metal–ligand complexes that are in an octahedral coordination are easy to find. I understand that when the $\mathrm{e_g}$ orbital is filled, the ionic radius increases because the ...
1
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2
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Octahedral Crystal Field Splitting Orbital Degeneracy
How are the $\mathrm{e_g}$ orbitals degenerate with each other?
Note: This isn't a homework question. After the semester ended (I don't go to MIT), I ended up on MIT open course-ware to watch some ...
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Octahedral Crystal Field Splitting Orbital Energy Levels [closed]
(image source)
In the above diagram, where do the 3/5 and 2/5 come from? Also, how are the $\ce{e_g}$ orbitals degenerate with each other?
24
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What is d-orbital collapse?
When I was perusing the works of Schwarz on atomic structure, I came across the unfamiliar term of d-orbital collapse.
He describes it as a variation in energetic sequence from group 1 to 3 elements ...
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1
answer
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Why does 2+ oxidation state become more stable relative to 3+ oxidation state for first row of transition metals? [duplicate]
I viewed an image showing all the possible oxidation states of each element in the first row of transition metals, and the main oxidation states highlighted in a different colour.
I noticed all ...
2
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Trend in the infrared stretching of molecular hydrogen to group 8 transitions metals?
While going through old notes, in relation to the Dewar-Chatt-Duncanson model, it states that the stretching frequency for $\ce{N2}$ to the group 8 transition metals ($\nu(\ce{NN})$) proceeds as:
\...
4
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1
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What's the configuration of chromium(III) in aqueous medium according to crystal field theory?
It has $\mathrm{3d^3}$ configuration, but how will we decide if they enter $\mathrm{t_{2g}}$ or $\mathrm{e_g}$ orbitals since we don't know which complex will form?
5
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Relative orbital energies of Mn and Ni
In this MO diagram, why are the atomic Mn $3d$ orbitals higher in energy than the Ni $3d$ orbitals?
9
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In an octahedral complex, what happens to the electrons donated by the ligand?
I am trying to understand how complexes are coloured. After some reading, I found out this was due to the d-d splitting induced by the coordinate bonds of ligands to the central metal ion. The ...
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How many d-electrons are in the outer shell of metals like Cadmium (this is counting the 4d electrons)?
First I know similar questions have been asked about counting d-electrons.
However, my question is about the electrons in the 4d orbital. For example if I have CdS. The cadmium has a charge of +2. ...
11
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1
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What type of bonding is there among d-block metals?
Metallic bond strength in $\mathrm{d}$-block elements increases up to the middle and then decreases. Why does pairing decrease the strength of metallic bond? What does pairing have to do with metallic ...
2
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1
answer
303
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General notation for one of the d-orbitals
What is the general notation to represent the d-orbital with $l=2$, $m_l=0$, i.e. the orbital normally referred to as $\mathrm{d}_{z^2}$. To elaborate more, this orbital can be ordered in various ways ...
7
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How many electrons are in the d orbitals of NiCl2·6H2O?
On Wikipedia, it says that
$\ce{NiCl2·6H2O}$ consists of separated trans-$\ce{[NiCl2(H2O)4]}$ molecules
linked more weakly to adjacent water molecules. Only four of the six
water molecules in ...
9
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2
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Why do copper (II) complexes contain so many valence electrons?
Consider tetraaminecopper (II) ion. $\ce{[Cu(NH3)4]^2+}$ or $\ce{[Cu(NH3)4(H2O)2]^2+}$.
The copper(II) ion has the electron configuration $\mathrm{[Ar]\ 3d^9}$. How do the 4 electron pairs from the ...
3
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1
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Spectrochemical Series - Sigma Donor Capability
I fully understand and recognise the manner and which the series works.
I cannot find any references for the change in sigma donor capability moving up the series.
For example, comparing $\ce{Cl-}$ ...
16
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1
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Splitting of $d$ orbitals when ligands approach central metal ion
In my high school chemistry book, it is written that when ligands approach the central metal ion (transition metal ion) to form dative bonds, the $3d$ orbitals split into two: two which are in higher ...
72
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4
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Why do elements in columns 6 and 11 assume 'abnormal' electron configurations?
When I look around for why copper and chromium only have one electron in their outermost s orbital and 5/10 in their outermost d orbital, I'm bombarded with the fact that they are more stable with a ...