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Medchem > Coordination Chemistry > Flashcards

Coordination Chemistry Flashcards

1
Q

Transition metals

A
  • found in nature
  • Rocks and Minerals
  • Gem stone colour
  • Biomolecules
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2
Q

Rubies are — due to —

A

red; Cr

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3
Q

Sapphire are — due to presences of — & —

A

blue; Fe; Ti

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4
Q

Many biomolecules contain transition metals that are involved in the functions of these biomolecules

A
  • Vitamin B12 contains Co
  • Hemoglobin, myoglobin, and cytochrome C contain Fe
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5
Q

useful applications for Transition metals and their compounds

A
  • Fe -> used to make steel & stainless steel
  • Ti -> used to make lightweight alloys
  • used as pigments
  • Used in many industrial processes
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6
Q

TiO2 pigment

A

White

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7
Q

PbCrO4 pigment

A

yellow

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8
Q

Fe4[Fe(CN)6]3

A

Prussians blue = blue

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9
Q

e- in partially filled d sublevel

A

absorbs visible light
moves to slightly higher energy d orbital

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10
Q

Properties of transition metals

A
  • Has metallic properties
  • Not as reactive as Grp. 1A, 2A metals
  • Has high MP’s, high BP’s, high density, are hard and strong
  • Has 1 or 2 s electrons in valence shell
  • Differ in # d electrons in n-1 energy level
  • Exhibit multiple oxidation states
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11
Q

[Ar]3d14s2

A

Sc

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12
Q

[Ar]3d24s2

A

Ti

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13
Q

[Ar]3d34s2

A

V

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14
Q

[Ar]3d54s1

A

Cr

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15
Q

[Ar]3d54s2

A

Mn

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16
Q

[Ar] 3d64s2

A

Fe

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17
Q

[Ar] 3d74s2

A

Co

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18
Q

[Ar] 3d84s2

A

Ni

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19
Q

[Ar]3d104s1

A

Cu

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20
Q

[Ar]3d104s2

A

Zn

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21
Q

Characteristics due to d electrons

A
  • Exhibit multiple oxidation states
  • Compounds typically have color
  • Exhibit interesting magnetic properties {paramagnetism
    and ferromagnetism}
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22
Q

Transition metals act as —- acids

A

Lewis

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23
Q

Form complexes/complex ions

A

{lewis acid} Fe3+(aq) + {lewis base} 6CN-(aq) → {complex ion} Fe(CN)63-(aq)

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24
Q

{lewis acid} Ni2+(aq) + {lewis base} 6NH3(aq) →

A

Ni(NH3)62+(aq) {complex ion}

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25
Q

Complex contains

A

central metal ion bonded to one or more molecules or anions

Lewis acid = metal = center of coordination

Lewis base = ligand = molecules/ions covalently bonded to metal in complex

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26
Q

Complex with a net charge =

A

Complex ion

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27
Q

Complexes have —– properties

A

distinct

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28
Q

Coordination compound

A

Compound that contains 1 or more complexes

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29
Q

Coordination compound examples

A

[Co(NH3)6]Cl3

[Cu(NH3)4][PtCl4]

[Pt(NH3)2Cl2]

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30
Q

Coordination sphere

A

Metal and ligands bound to it

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31
Q

Coordination number

A

number of donor atoms bonded to the central metal atom or ion in the complex

Most common = 4, 6
Determined by ligands
Larger ligands and those that transfer substantial negative charge to metal favor lower coordination numbers

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32
Q

Coordination Compound consists of

A

complex ion and necessary counter ions

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33
Q

Complex ion: [Co(NH3)5Cl]2+

A

Counter ions: 2 Cl-

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34
Q

with the knowledge of the charge on a complex ion and the charge on each ligand, one can determine

A

the oxidation number for the metal.

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35
Q

With knowledge of the oxidation number on the metal and the charges on the ligands

A

one can calculate the charge on the complex ion.

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36
Q

Complex ion

A

Species where transition metal ion is surrounded by a certain number of ligands

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37
Q

Transition metal ion are

A

Lewis Acid

38
Q

Ligands are

A

Lewis bases

39
Q

Ligands

A

Molecule or ion having a lone electron pair that can be used to form a bond to a metal ion
(Lewis base)

consists of;
- Coordinate covalent bond
- Monodentate
- Bidentate
- Polydentate

40
Q

coordinate covalent bond

A

metal-ligand bond

41
Q

monodentate

A

one bond to metal ion

42
Q

bidentate

A

two bond to metal ion

43
Q

polydentate

A

more than two bonds to a metal ion possible

44
Q

Complex charge =

A

sum of charges on the metal and the ligands

45
Q

Neutral charge of coordination compound =

A

sum of charges on metal, ligands, and counterbalancing ions

46
Q

[Co(NH3)6]Cl2

A

neutral compound

47
Q

Ligands are classified according to;

A

the number of donor atoms

48
Q

Chelating agents

A

Bidentate - Polydentate
2 or more donor atom

49
Q

Monodentate

A

1 donor atom
Examples:
H2O, CN-, NH3, NO2-, SCN-, OH-, X- (halides), CO, O2-

Example Complexes
[Co(NH3)6]3+
[Fe(SCN)6]3-

50
Q

Bidentate

A

2 donor atom

Examples
oxalate ion = C2O42-
ethylenediamine (en) = NH2CH2CH2NH2
ortho-phenanthroline (o-phen)

Example Complexes
[Co(en)3]3+
[Cr(C2O4)3]3-
[Fe(NH3)4(o-phen)]3+

51
Q

Hexadentate

A

6 donor atoms

ethylenediaminetetraacetate (EDTA) = (O2CCH2)2N(CH2)2N(CH2CO2)24-

Example Complexes
[Fe(EDTA)]-1
[Co(EDTA)]-1

52
Q

Common geometries of complex

A
  • Linear
  • Tetrahedral
  • Square planar
  • Octahedral
53
Q

Coordination # 2
Example: [Ag(NH3)2]+

A

Linear

54
Q

Coordination # 4
Examples: [Zn(NH3)4]2+, [FeCl4]-

A

tetrahedral

55
Q

characteristic of metal ions with 8 d e-’s
Example: [Ni(CN)4]2-

A

Square planar

56
Q

Coordination # 6
Examples: [Co(CN)6]3-, [Fe(en)3]3+

A

Octahedral

57
Q

Myoglobin

A

a protein that stores O2 in cells

58
Q

Nomenclature of Coordination Compounds: IUPAC Rules

A
  • The cation is named before the anion
  1. When naming a complex:
    Ligands are named first
    • alphabetical order
  2. Metal atom/ion is named last
    - oxidation state given in Roman numerals follows in parentheses
  3. Use no spaces in complex name
  4. The names of anionic ligands end with the suffix -o

-ide suffix changed to -o
-ite suffix changed to -ito
-ate suffix changed to -ato

59
Q

bromide, Br-

A

bromo

60
Q

chloride, Cl-

A

chloro

61
Q

cyanide, CN-

A

cyano

62
Q

hydroxide, OH-

A

hydroxo

63
Q
A
63
Q
A
63
Q
A
64
Q
A
65
Q

oxide, O2-

A

oxo

65
Q

fluoride, F-

A

fluoro

65
Q

oxalate, C2O42-

A

oxalato

65
Q

sulfate, SO42-

A

sulfato

65
Q

carbonate, CO32-

A

carbonato

65
Q

Sulfite, SO32-

A

sulfito

65
Q

thiocyanate, SCN-

A

thiocyanato

66
Q

thiosulfate, S2O32-

A

thiosulfato

67
Q

Neutral ligands

A

referred to by the usual name for the molecule

Example
ethylenediamine

Exceptions
- water, H2O = aqua
- ammonia, NH3 = ammine
- carbon monoxide, CO = carbonyl

68
Q

Greek prefixes

A

used to indicate the number of each type of ligand when more than one is present in the complex

di-, 2; tri-, 3; tetra-, 4; penta-, 5; hexa-, 6

69
Q

If the ligand name already contains a Greek prefix, use —

A

alternate prefixes:
bis-, 2; tris-, 3; tetrakis-,4; pentakis-, 5; hexakis-, 6

The name of the ligand is placed in parentheses

70
Q

If a complex is an anion

A

its name ends with the -ate

appended to name of the metal

71
Q

the name of the cation

A

appears first

72
Q

The anion

A

is named last

73
Q

Ligands are listed

A

alphabetically before the metal

74
Q

Prefixes denotes he number of a particular ligand are

A

ignored when alphabetizing.

75
Q

The names of anionic ligands end

A

“o”

76
Q

the endings of the names of neutral ligands are

A

Not charged

77
Q

Prefixes

A

tells the number of a type of ligand in the complex.

78
Q

If the name of the ligand itself has a prefix

A

alternatives like bis-, tris-, etc., are used.

79
Q

If the complex is an anion

A

its ending is changed to -ate

80
Q

The oxidation number of the metal

A

listed as a Roman numeral in parentheses immediately after the name of the metal.

81
Q

Naming of Coordination Compounds

A
  1. Cation then anion
  2. Ligands
    - in alphabetical order before metal ion
    - neutral: molecule name*
    - anionic: -ide → -o
    prefix indicates number of each
  3. Oxidation state of metal ion in () only if more than one possible
  4. If complex ion = anion, metal ending → -ate
82
Q

K2[Co(NH3)2Cl4]

A

potassium diamminetetrachlorocobaltate(II)

83
Q

[Co(NH3)4Cl2]Cl

A

tetraamminedichlorocobalt(III) chloride

84
Q
A

Medchem (1 decks)

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