coordination chemistry II: bonding, spectrochemical series

Valence bond theory:

Metal or metal ion: lewis ___

ligand: lewis ___

Hybridization of _, _, and _ orbitals

acid, base, s,p, and d

tetrahedral hybridization

sp³

square planar hybridization

dsp²

trigonal bipyramidal hybridization:

dsp³ or sp³d

octahedral hybridization:

d²sp³ or sp³d²

what hybridization? what does valence electron configuration look like? paramagnetic or diamagnetic?

octahedral (d²sp³), diamagnetic

what hybridization? what does valence electron configuration look like? paramagnetic or diamagnetic?

what hybridization? what does valence electron configuration look like? paramagnetic or diamagnetic?

Crystal field theory: Three types of interactions are considered. what are they?

the more electron-electron repulsion you have the ____ in energy it is

higher

the repulsion between ligand lone pairs and the d orbitals on the metal results in a ____ of the energy of the d orbitals

splitting

electrons in lower d orbitals (?) is canceled out by the destabilizing effect of the electrons in the upper orbitals (?)

t_2g, e_g

(crystal Field Stabilization Energy) CFSE=?

(#e x0.4∆₀) - (#e x 0.6 ∆₀)

In an octahedral complex, ___ _{and ____ have the highest electron-electron repulsion because the orbitals directly overlap with the incoming ligand, sit along axes, higher in energy.}

d_x²-y² and d_z²

in an octahedral complex, d_x²-y² and d_z² have the highest electron-electron repulsion because ?

the orbitals directly overlap with the incoming ligand, sit much higher in energy

in an octahedral complex, __, __, and __ orbitals sit much lower in energy (less electron-electron repulsion) because they do not sit directly along the axes

d_xy, d_yz, d_xz

in an octahedral complex, d_xy, d_yz, d_xz sit in the ___ orbital (lower in energy)

t_2g

in an octahedral complex, d_x²-y² and d_z² sit in the ___ orbital (higher in energy)

e_g

what is crystal field stabilization energy

value of energy required in order for lower energy orbitals to get back to where it wants to be before the ligands came in

the more electrons in the lower orbitals, the ____ the CFSE

greater

2 electrons per chlorine, they each have their own electron pair through covalent bonding (VBT)

everything need to know about VBT

complete this using crystal field theory

What is spin pairing energy

the energy required to place two electrons with opposite spins in the same orbital , overcoming the repulsion between them

if pairing energy is ____ than delta, the complex is high-spin

higher

if pairing energy is lower than delta, the complex is ___

low-spin

low-spin states are associated with?

strong field ligands

high-spin states are associated with?

weak field ligands

in a tetrahedral field, which orbitals have the highest and lowest electron-electron repulsions? what is the highest energy orbital called? the lowest?

highest: d_xy, d_yz, d_xz

lowest: d_x²-y² and d_z², opposite of octahedral complex

t₂, e

Tetrahedral fields can have ___.

distortion

factors affecting magnitude of CFSE:

Geometry of the field:

Tetrahedral are aways ___ or __

weak field or high-spin

factors affecting magnitude of CFSE:

∆₀~ ?

square planar can be either __ or __

high or low-field

factors affecting magnitude of CFSE:

charge on metal ion - greater the charge, ___ the magnitude of ∆

greater the charge, on more ____ are pulled, ___ split

greater (ex: +3 > +2)

metal ligands, greater

factors affecting magnitude of CFSE:

greater the size, ___ the magnitude of ∆

ligand experience less _____ for a large metal ion

greater (ex: Mo³⁺ > Co³⁺), steric hindrance

factors affecting magnitude of CFSE:

relative ability of ligand to split: spectrochemical series

goes from high spin to low spin

greater splitting means ___ bond

stronger

splitting is was reveals colors in ____

spectrochemical series

crystal field theory cannot explain the?

spectrochemical series

these are non-bonding orbitals because

they are not aligned on the axes, no significant overlap

Ligand field theory:

the ___ set of orbitals is non-bonding, and the __ set of orbitals is antibonding

t_2g, e_g

this is just the octahedral complex

Blue complex emits ___ and vice versa

orange

red complex emits ___ and vice versa

green

Violet complex emits ___ and vice versa

yellow

The moment resulting from “electron spin”: spin-only magnetic moment, ___

the moment resulting from orbiting: orbital magnetic moment, __

μ_s, μ_L

μ_s =?

know low spin wont happen because of Cl ligand spectrochemical series

if magnetic moment is 5.8, what is the oxidation state?

5.8 is close to 5.92 (5 unpaired electrons) so could be d⁵, so oxidation state could be +3

The colors exhibited by most
transition metal complexes arises from the _____. As electrons transition from the lower t2g set to the eg set, _____ range is absorbed.

splitting of the d orbitals, light in the visible

∆_o increases with increasing ____ on the metal and going ___ a group of metals.

oxidation number, down

which geometry describes this d-orbital splitting energy diagram

tetrahedral

which geometry describes this d-orbital splitting energy diagram

octahedral

which geometry describes this d-orbital splitting energy diagram

Jahn-Teller elongation

which geometry describes this d-orbital splitting energy diagram

Jahn-Teller compression

Find n,