Crystal Field Theory Flashcards

1
Q

isomers

A

same formula, different properties

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2
Q

isomers divide into?

A

structural isomers (different bonds) and stereoisomers (same bonds, different arrangements)

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3
Q

structural isomers divide into?

A

coordination-sphere isomers and linkage isomers

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4
Q

stereoisomers divide into?

A

geometric isomers and optical isomers

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5
Q

structural isomers

A

linkage, hydration, ionisation, coordination

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6
Q

linkage isomers

A

a single ligand has two or more donor atoms and can attach in more than one way eg. SCN

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7
Q

hydration isomers

A

water swaps with a ligand

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8
Q

ionisation isomers

A

change of anionic ligands with counter anions

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9
Q

coordination isomers

A

both a complex anion and cation are present - multiple combinations of ligands with two metal centres

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10
Q

geometric isomers

A

cis: identical ligands are adjacent
trans: identical ligands are on opposite sides of a metal centre
fac: three identical ligands on one side of an octahedral
mer: identical isomers lie around the meridian (two on one side, one adjacent)

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11
Q

optical isomers

A

occur commonly when there is more than one bidentate ligand

non-superimposable mirror images

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12
Q

colour - how does it happen and exceptions?

A

electrons in partially filled d-orbitals absorb visible light and move to d-orbitals with slightly higher energy
Sc3+, Ti4+, Zn2+ are exceptions (filled or empty d-subshells)

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13
Q

paramagnetic

A

attracted to a magnetic field (unpaired electrons)

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14
Q

ferromagnetic

A

if electrons are aligned in the same direction

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15
Q

diamagnetic

A

not magnetic (paired electron spins)

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16
Q

crystal field theory

A

explains stability, colour and magnetism but not metal-ligand bonding
describes how energies of d orbitals on the metal are affected as ligands approach

note: complexes result in electrostatic attractions between metal cation and negative charges on lone pairs on ligands (not covalent)

17
Q

what happens to the energy of the metal d-orbitals when 6 ligands approach?

A

ligands can approach directly (alone x,y,z axes) or between axes
directly results in greater ligand, d-orbital repulsion and therefore take more energy to form

18
Q

eg orbitals

A

direct head-to-head repulsion (more unstable). dz^2 and dx^2-y^2

19
Q

t2g orbitals

A

tangible repulsion leads to lower energy for dxy, dxz and dyz orbitals

20
Q

what is the energy difference between eg and t2g orbitals?

A

delta oct or delta o