Magnetism and Crystal Field Theory the formation of complex ions, the dorbitals

Question

Magnetism and Crystal Field Theory the formation of complex ions, the dorbitals of the metal that are oriented head-on" to the ligands will be raised in energy such that they are no longer degenerate with the other dorbitals. The splitting pattem depends on the geometry ofthe complex (Egure 1) Figure 1 of 1 octahedral tetrahedral lanar In an complex with a large A, the electrons will fill the lower onergy dortitals before any eiectrons are placed in the higher energy dorbitals, and so the complex is classified as low spin. In an octahedral complex smal however, the electrons wil fill as the dorbitals are degenerate because the pairing energy exceeds the splitting energy. In situation, the if orbitals beoome populated sooner, and the higher onergy d determines whether an complex is classified as high spin. The field strength of the ligand, which affects 4, A complex is low spin or be high spin because A is relatively small even with a strong-field ligand. tetrahedral high spin, Thus, even though the dortitals are split electrons wil fill as if the d orbitals are degenerate. A square planar complex wil almost always be low spin because A is relatively large even with a weak-field ligand. Part A Consider a metal ion with the outer electron configurason of d In a coordination complex, the number of unpaired oloctrons in that metalion doponds on the orientation and type of ligands that surround it. Classify each description of a complex by the number of unpaired electrons in the d metal ion. Drag the appropriate items to their respective bins. square planar tetrahedral octahedral square planar actahedral strong field strong field weak field tetrahedral 0 unpaired unpaired 2 unpaired 4 unpaired

Explanation / Answer

PART(B)

[MnCl6]4-

oxidation state of Mn is : x + 6(-1) = -4 => x = +2

Mn2+ (Z=25) valence shell electronic configuration is 3d5 4s0

SInce, Cl is weak field ligand it can not pair up the electons against to Hund's rule,

So, the number of unpaired electrons = 5

(each orbital of d-subshell has one electron as there 5 orbitals in d - subshell)

PART(A)

** 0 unpaired : Tetrahedral strong field

1 unpaired:

2 unpaired: square planar strong field, octahedral strong field

3 unpaired:

4 unpaired: square planar weak field, octahedral weak field, tahedral weak field.

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