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Chem 105 > Unit 3: Coordination Chemistry > Flashcards

Unit 3: Coordination Chemistry Flashcards

1
Q

What are the similar properties of transition metals?

A
  • Relatively high electrical conductivity
  • Relatively high thermal conductivity
  • More than 1 oxidation state
  • Often form complex ions
  • Most can absorb visible light
  • Many compounds are paramagnetic
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2
Q

What are the different properties of transition metals?

A
  • Melting points
  • Hardness
  • Oxides
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3
Q

What groups follow the stability rule in regard to electron configuration?

A

Group 6 and group 11

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4
Q

What makes up a coordination compound?

A

It is made of a complex ion and counter ions.

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5
Q

What is coordination numbers?

A

The number of bonds from the ligands to the central metal atom.

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6
Q

What are counter ions?

A

Ions which are needed to maintain charge neutrality of the compound.

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7
Q

What shape forms from a coordination # = 2?

A

Linear, is the least common shape.

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8
Q

What shape forms from a coordination # = 4?

A

Square planar or tetrahedral

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9
Q

What shape forms from a coordination # = 6?

A

Octahedral, most common

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10
Q

How can you determine whether a CN of 4 will be square planar or tetrahedral?

A

If the electron configuration of the metal is nd8 the shape will most likely be square planar.
For all other metals, it will be tetrahedral.

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11
Q

What is a ligand?

A

It is a neutral molecule or an ion with a lone pair of e-‘s

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12
Q

What is a monodenate/unidentate ligand?

A

It is attached to the metal by one bond.

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13
Q

fluoro

A

F-

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14
Q

chloro

A

Cl-

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15
Q

bromo

A

Br-

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16
Q

iodo

A

I-

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17
Q

cyano

A

CN-

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18
Q

hydroxo

A

OH-

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19
Q

aqua

A

H20

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20
Q

ammine

A

NH3

21
Q

carbonyl

A

CO

22
Q

nitrosyl

A

NO

23
Q

Polydentate lignads?

A

Attached to metal by more than 1 bond or pair of electrons.

24
Q

Bidentate?

A

2 pairs e-

25
Q

ethylenediamine

A

en

26
Q

oxalate

A

ox2-

27
Q

How do you name a complex ion?

A
  1. Cation named before anion
  2. Name ligands before metal
  3. Use prefixes for ligands
  4. Designate the oxidation # of metal using Roman numerals
28
Q

What is different about period 4 transition metals?

A

They are active enough to reduce H+ from acid solution.

29
Q

What are the two main types of isomers?

A

Structural isomers and stereoisomers.

30
Q

What are the two types of structural isomers?

A

Coordination isomers
- Ligand and counter-ion exchange

Linkage isomers
- Different donor atom

31
Q

What are the two types of stereoisomers?

A

Geometric isomers
- Different arrangements around the metal ion

Optical isomers
- non-superimposable mirror images

32
Q

What are the bond names for SCN-?

A

via sulfur: thiocyanato
via nitrogen: isothiocyanato

33
Q

What are the bond names for OCN-?

A

via oxygen: cyanato
via nitrogen: isocyanato

34
Q

What are the bond names for NO2-?

A

via nitogen: nitro
via oxygen: nitrito

35
Q

What is a cis geometric isomer?

A

Identical ligands are 90* apart.

36
Q

What is a trans geometric isomer?

A

Identical ligands are 180* apart

37
Q

What is a facial geometric isomer?

A

All 3 identical ligands are 90* apart

38
Q

What is a meridional geometric isomer?

A

2 identical ligands are 180* apart and 1 identical ligand is 90* apart from the other 2.

39
Q

What is the crystal field theory?

A

It is a bonding model which explains the properties of transition metals.

40
Q

What is the eg set?

A

dz2, dx2-y2

The orbital energy goes up (destabilized)

The ligand lone pair is aligned with the orbital

41
Q

What is the t2g set?

A

dxy, dxz, dyz

The orbital energy goes down (stabilized)

The ligand lone pair is between orbitals

42
Q

What is a free ion?

A

d-orbitals have same energy (degenerate)

43
Q

Crystal field splitting?

A

Energy splitting, explains the magnetic properties of transition metals.

44
Q

What happens if the crystal field splitting is small?

A
  • Pairing is not favorable
  • e- will fill t2g and eg sets before pairing
  • Forms high-spin complexes
  • High # of unpaired e-
45
Q

What happens if the crystal field splitting is large?

A
  • Pairing is favorable
  • e- will fill t2g set first then eg set
  • Forms low-spin complexes
  • Low # of unpaired e-
46
Q

Does the magnitude of the crystal-splitting energy increase with the more valance e-?

A

Yes

47
Q

What is a diamagnetic species?

A

Not attracted to a magnetic field and all electrons are paired.

48
Q

What is a paramagnetic species?

A

Attracted to a magnetic field and has unpaired electrons.

49
Q

Why do we observe colours in transition metals?

A

The splitting of energy splits the d-orbital into 2 levels, which causes energy to be absorbed.
We see the colour is the opposite of the wavelength absorbed.

Chem 105 (5 decks)

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