INORGANIC CHEMISTRY
Coordination Compounds
-
A Lewis base (e donor) donates a pair of electrons to a Lewis acid (e- acceptor) forming a
co-ordinate covalent bond.
1s0 1s 11s11s 1
H+ H H H
H+
+
N:
H
N
H
H
N
H
H
ammonia
sp3 orbitals
H
F
N:
Hydrogen ion has a vacant 1s orbital.
Nitrogen has a full sp 3 orbital.
A co-ordinate covalent bond is formed
when nitrogen donates its lone e - pair
to hydrogen's empty 1s orbital.
ammonium ion
H
H
+
H
H
+
B
H
ammonia
F
F
N
H
B
H
F
sp2 orbitals
F
F
2pz
Boron has a vacant 2p z orbital.
Nitrogen has a full sp 3 orbital.
A co-ordinate covalent bond is formed
when nitrogen donates its lone e - pair
to boron's empty 2p z orbital.
B
N
sp3 orbitals
Ammonia is the Lewis base (electron donor). H+ and BF3 are Lewis acids (electron acceptors).
Similarly, transition metals and their cations are Lewis acids. They have vacant orbitals that can
accept electron pairs from donor atoms (Lewis bases) forming coordination compounds or
complexes. Some examples are shown in the following table.
Lewis Acid
Lewis Base
Complex
Dissociation Constants
Cr+3
+
6H2O
 [Cr(OH2)6]+3
------------Co+3
+
6NH3

[Co(NH3)6]+3
2.2  10-34
Ni+2
+
4CN-

[Ni(CN)4]-2
1.0  10-31
Fe
+
5CO

[Fe(CO)5]
2NH3

Ag
+
+
[Ag(NH3)2]
------------+
6.3  10-8
Lewis bases (anions or molecules) bonded to the central Lewis acid are called ligands (Latin =
tie or bind). Charged coordination complexes also have counter ions associated with them to
satisfy electroneutrality. For example, in [Ag(NH3)2]+NO3-, a nitrate anion is the counter ion.
Counter ions are ionically bonded. When dissolved in water, the NO3- ion separates from the
complex, but the two NH3 ligands remain firmly bound to the Ag+ ion by covalent bonds.
The number of atoms bonded to the central ion/atom of a coordination complex is referred to as
its coordination number. The coordination number of [Ag(NH3)2]+NO3- is two. The coordination
number of [Fe(CO)5] is five. Coordination complexes occur with coordination numbers of 2
through 12, however, coordination numbers of 2, 4 and 6 are most common.
Complexes such as [Fe(CO)5] are usually insoluble in water since they are covalent compounds
in which any dipoles cancel. Complexes such as [Ag(NH3)2]+NO3- are generally very soluble in
water since they are made up of cations, e.g., [Ag(NH3)2]+ and anions, e.g., NO3-.
Importance of Coordination Complexes:
Many biologically important substances are 'd'-transition metal coordination compounds that are
made up of large organic molecules bound to the metal via coordinate covalent bonds, e.g.,
 hemoglobin (blood protein) is a coordination complex involving Fe.
 vitamin B-12 is a cobalt complex (cyanocobalamin)
 phthalocyaine blue is a Cu complex dye used for blue jeans and ink
Coordination Complexes
1
INORGANIC CHEMISTRY



complexing agents are used for water softening (Ca, Mg, Fe removal with EDTA)
an antidote for some metal poisoning (BAL) forms complexes with As, Hg, and Cr.
Fe-carbonyls are anti-knock gasoline additives
Structure of Coordination Compounds:
Structures are determined by the coordination number and VSEPR. Lone pairs of e-'s in
d-orbitals have minimal influence on geometry because they are not in the outer shell.
In the following table, “Co #” refers to coordination number of the central atom or ion.
Geometries of Various Coordination Numbers
Co#
Geometry
2
Hybridization
(nonmetals)
Hybridization
(transition
metals)
Examples
(transition metals)
sp (BeH2)
sp
[Ag(NH3)2]+
[Cu(CN)2]-
linear
sp3 (CH4)
4
sp3
[Zn(CN)4]-2
[Cd(NH3)4]+2
109.5º
[FeCl4][Co(Br)4]-2
tetrahedral
90º
4
sp3d2 (XeF4)
90º
dsp2
[Pd(CO)4]+2
[Pt(NH3)2Cl2]
[Ni(CN)4]-2
square planar
a
5
sp3d (PCl5)
90º
e
d3sp or dsp3
or sp3d
e
120º
e
a
sp3d2 (SF6)
90º
90º
[Fe(CO)5]
[Mn(CO)4NO]
[Ni(CN)5]-3
triangular bipyramidal
e = equitorial position
a = axial position
6
[CuCl5]-3
d2sp3 or
sp3d2
[PtCl6]-2
[Co(NH3)6]+3
[Fe(OH2)6]+2
[Fe(CN)6]-4
[MoF6]-
octahedral
[CoF6]-3
[Ni(H2O)6]+2
[Mn(CN)6]-4
Co #7 [UF7]-3, [ZrF7]-3, Co #8 [Mo(CN)8]-4, [TaF8]-3 and Co #9 [UCl3 hydrate] are known but rare.
Coordination Complexes
2
INORGANIC CHEMISTRY
Types of Ligands:
Ligands of complex ions are molecules and/or ions with one or more donor atoms that each
donates a lone pair of electrons to the metal ion to form a covalent bond. Thus, ligands are Lewis
bases, the metal ion is a Lewis acid, and the complex is a Lewis adduct. Because they have at
least one lone pair of electrons, donor atoms often come from Groups 5A, 6A, or 7A.
Ligands are classified in terms of the number of donor atoms, or 'teeth' that each uses to bond to
the central metal ion.

Unidentate ligands (Latin, 'one-toothed), such as Cl- and NH3 use a single donor atom.

Bidentate ligands have two donor atoms, each of which bond to the central metal ion.
Polydentate ligands have more than two donor atoms.

Some common ligands in coordination compounds are shown below. Note the lone pair of
electrons in each donor atom. Bidentate and polydentate ligands give rise to complexes with ring
structures. For example, ethylenediamine (abbreviated en) has a chain of four atoms
(:N-C-C-N:), so it forms a 5-membered ring. Such ligands seem to grab the metal ion like a
crab's claw, so complex ions that contain them are sometimes called chelates (Greek chela =
crab's claw).
Unidentate
..
H2O
..
.. :F
.. :
: NH3
.. :Cl :
..
Bidentate
.. C N:
thiocyanate ion
:O :
:O :
C
NH
.. 2
H2..N
..
:O
.. N O:
nitrite ion
..
:S
CH2
H2C
..
H
:O
..
hydroxide ion
-
:C N:
cyanide ion
-
ethylenediamine (en)
C
:O:
..
:O: ..
oxalate ion
:O :
:O :
H2C
Polydentate
CH2
CH2
NH
..
H2..N
diethylenetriamine
-
CH2
NH
.. 2
-
..
:O
..
..
:O
..
C
CH2
H2C
:N
C
CH2
CH2
N:
CH2
H2C
.. :
O
..
..
:
.. C O
C
: O:
:O :
ethylenediaminetetracetate (EDTA) ion
Relative Strengths of Ligands:
Lewis bases differ in their ability to donate electrons to the metal ion. The relative strengths of
ligands in coordination complexes has been experimentally determined …
I- < BrWEAK
LIGANDS
< Cl- <
F- < OH- < C2O4-2 < H2O < SCN- < NH3 < en <
NO2- < CN- < CO
Increasing ability to donate an electron pair to a metal ion
Coordination Complexes
STRONG
LIGANDS
3
INORGANIC CHEMISTRY
Nomenclature of Coordination Compounds:
Lewis bases may be anions, molecules, or (rarely) cations and are called 'ligands'. The donor atom is the
atom of the ligand, which actually donates the electrons (underlined in the table). [* = bidentate ligands]
formula
:NH3
name
ammonia
ligand name
formula
name
ligand name
ammine
Cl-
chloride
chloro
H2O
water
aqua
F-
fluoride
fluoro
:CO:
carbon monoxide
carbonyl
:CN:-
cyanide
cyano
phosphine
OH-
hydroxide
hydroxo
nitrite
nitro (NO2-)
:PH3
phosphine
:N=O
nitric oxide
nitrosyl
:NO2-
NO3-
nitrate
nitrato
:NO2-
nitrite
nitrito (ONO-)
NH2-
amide
amido
*SO4-2
sulfate
sulfato
oxalato
SCN-
thiocyanate
thiocyanato
thiosulfate
thiosulfato
pyridine
pyridine
*C2O4-2
oxalate
*CO3-2
carbonate
carbonato
*S2O3-2
*O-2
oxide
oxo
C5H5N:
Coordination number of a metal is the number of donor atoms to which the metal is bonded. If the
ligands are unidentate, then the coordination number is also the number of ligands. For example, in
[Co(en)3]+3 where each ethylenediamine ligand is bidentate, the coordination number is 6, i.e., Co +3 is
bonded to 6 donor atoms (2 donor atoms from each of 3 ethylenediamine ligands).
Coordination sphere is the metal and its ligands but not the uncoordinated counterions, e.g., in
[Co(NH3)6]Cl3, the coordination sphere = [Co(NH3)6]+3.
Nomenclature Rules:
1. If the complex is ionic, name the cation first and the anion second.
2. Within a coordination sphere, name the ligands before the metal
3. Name ligands alphabetically, e.g., ammine before chloro. Prefixes denoting the number of ligands
(e.g., di in dichloro, tri in triammine, etc.) are not alphabetized, however, prefixes which are part of the
ligand name are alphabetized, e.g., in dimethylamine [NH(CH3)2] , di is part of the ligand name and so
is alphabetized.
4. Prefixes bis, tris, tetrakis, pentakis,, etc. are used for ligands that are bidentate, polydentate or already
have a number prefix as part of its name, e.g., bis(diethylamine) has 2 groups of diethylamine and
tris(oxalato) because oxalato is bidentate. Prefixes are not alphabetized. Divalent anions are bidentate.

anionic ligands end in the suffix 'o', e.g., *S2O3-2 = thiosulfato, *S-2 = sulfido, *CO3-2 = carbonato

names of neutral ligands like phosphine (PH3) are usually unchanged except for NH3 (ammine), H2O
(aqua), CO (carbonyl), and NO (nitrosyl)
5. For metals with multiple oxidation states, indicate the oxidation state in Roman numerals in
parentheses following the name of the complex ion or molecule.
6. When the complex is neutral or cationic, the name of the central metal atom is the same as the
element, e.g., chromium, nickel, iron
7. For anionic complexes, the suffix -ate is added to the stem of the metal name, e.g., zincate.
Latin names of metals are used when the English name is clumsy, i.e.,

ferrate not ironate

argentate not silverate

nickelate

plumbate not leadate

cuprate not copperate

zincate

stannate not tinate

chromate

manganate

aurate not goldate

platinate

aluminate
Coordination Complexes
4
INORGANIC CHEMISTRY
WRITING NAMES OF COORDINATION COMPLEXES FROM FORMULAS
NEUTRAL COMPLEXES
CATIONIC COMPLEXES
e.g.,
e.g.,
[Cu(NH3)2]NO3
cationic coordination sphere
ligandsmetal(ox#)
anion
anion
[Cu(ONO)2]
neutral coordination sphere
ligandsmetal(ox#)
ANIONIC COMPLEXES
e.g.,
K2[Cu(CN)4]
cation
anionic coordination sphere
cation
ligandsmetalate(ox#)
potassium tetracyanocuprate(II)
diamminecopper(I) nitrate
dinitritocopper(II)

Oxidation number is given only for metals with more than one possible oxidation state. For Ag+, the ox# is not stated.

Ligands are listed alphabetically. The metal ion is listed after all ligands.

Note that for anionic complexes (only), the suffix ‘ate’ is added to the metal and the Latin name of the metal is used in some cases
(where pronunciation of the English name is awkward).

Prefixes di, tri, tetra, penta, hexa, hepta, etc. are used when more than one of a monodentate ligand is present.

Prefixes bis, tris, tetrakis, pentakis, hexakis, heptakis, etc. are used for bidentate or polydentate ligands, or when the monodentate
ligand already has a prefix in its name, e.g., bis(dimethylamine)

For Names: note the space between cationic coordination sphere and the anion and between cation and anionic coordination
sphere.

For Formulas: note that there are no spaces in formulas.
Coordination Complexes
5
INORGANIC CHEMISTRY
Cationic Complexes:
[Co(NH3)6]Cl3
[Pt(NH3)4Cl2]+2
[Ag(NH3)2]+
[Cr(H2O)4Cl2]Cl
[Co(H2NCH2CH2NH2)3]2(SO4)3
[Fe(H2O)5(SCN)]SO4
[Cu(NH3)2(en)]Br2
hexaamminecobalt(III) chloride
tetraamminedichloroplatinum(IV) ion
diamminesilver ion
tetraaquadichlorochromium(III) chloride
tris(ethylenediamine)cobalt(III) sulfate
pentaaquathiocyanatoiron(III) sulfate
diammineethylenediaminecopper(II) bromide
Neutral Complexes:
[Pt(NH3)2Cl4]
[Co(NH3)3(NO2)3]
[Ni(H2NCH2CH2NH2)2Cl2]
[Ni(CO)4]
[Co2(CO)8]
diamminetetrachloroplatinum(IV)
triamminetrinitrocobalt(III)
dichlorobis(ethylenediamine)nickel(II)
tetracarbonylnickel(0) or nickel tetracarbonyl
octacarbonyldicobalt(0) or dicobalt octacarbonyl
Anionic Complexes:
K3[Co(ONO)6]
[PtCl6]-2
Na2[SnCl6]
K2[Cu(CN)4]
Na2[CrOF4]
Na[Al(OH)4]
Na2[Sn(OH)6]
K4[Ni(CN)2(ox)2]
potassium hexanitritocobaltate(III)
hexachloroplatinate(IV) anion
sodium hexachlorostannate(IV)
potassium tetracyanocuprate(II)
sodium tetrafluorooxochromate(IV)
sodium tetrahydroxoaluminate
sodium hexahydroxostannate(IV)
potassium dicyanobis(oxalato)nickelate(II)
In formulas:
In the coordination sphere, the metal symbol is written first, followed by symbols of its ligands
 Complex ligands are put in parenthesis, even if there is only one ligand is present, e.g., (CN)
and (OH). Monatomic ligands like Cl, Br, etc. are not parenthesized.
 IUPAC rules state

inorganic ligands are listed before organic ligands

anionic ligands are listed before neutral ligands
This last rule can lead to contradictory situations. Indeed literature is rife with examples where
both these rules are ignored. In formulas, it is generally accepted that it is more important to list
the ligands correctly than to place them in order. This leniency is not applied to order of listing
ligands in naming the compounds. Follow the rules carefully for naming compounds.

Name the following coordination compounds:
[Co(en)2Br2]Cl
[Co(PH3)3](NO3)3
[V(NH2)2(NO)2]Cl3
K2[Mn{NH(CH3)2}4(C2O4)2]
[Cr(en)5(SCN)]F2
Na2[MoOCl4]
Coordination Complexes
6
INORGANIC CHEMISTRY
Coordination Number and Geometry of Coordination Compounds:
No single theory is able to successfully predict the coordination number or geometry of all
coordination complexes. No strict rules can be stated, however, the following generalizations are
helpful.
 The most common coordination number of metal complexes is 6, e.g., [Pt(Cl) 6]+2. Most of
these are octahedral. Cr+3 (d3), Co+3 (d6), Fe+2 (d6), and Fe+3 (d5) favor octahedral complexes
regardless of the ligands present. For all di- and tri-positive 1st series transition metals, aqua
ions are octahedral, i.e., [M(H2O6]+2 (or +3).
 4-coordinate complexes are the next most common.
They exist in two geometries,
tetrahedral (sp3 hybridized) and square planar (dsp2 hybridized). Tetrahedral geometries
(bond angles = 109.5) are sterically favored over square planar (bond angles = 90).
 4-coordinate complexes of non transition metals are almost always tetrahedral, e.g., [AlCl4]and SnBr4.
 4-coordinate complexes of the transition metals may exist in either form. Tetrahedral
complexes are especially favored when ligands are weak and relatively large (e.g., Br -) and
metal ions are relatively small, i.e., 1st transition metal series complexes, e.g., VCl4, [FeCl4]-,
[NiBr4]-, [MnCl4]-2, [CdCl4]-2 .
 Ni+2 (3d8) displays square planar geometry with small strong ligands like CN -, tetrahedral
complexes with large weak ligands like F-, Cl-, Br-, I- and forms octahedral complexes with
NH3 and H2O.
 Square planar complexes are more common for larger d8 transition metals, i.e., Pd+2 (4d8),
Pt+2 (5d8), and Au+3 (5d8). Steric constraints are relaxed with these larger metal ions. Less
commonly, square planar complexes are also seen with Co+2 (d7), Co+3 (d6) and Cr+2 (d4).
 2-coordinate transition metal complexes (sp hybridized) are restricted to +1 ions of Group IB,
i.e., Cu+ (3d10), Ag+ (4d10) and Au+ (5d10) and +2 ions of Group 2B, i.e., Zn+2, Cd+2 and Hg+2.
 Odd coordination numbers (1,3,5) are very rare.
Note that a given transition metal ion can form complexes of differing coordination numbers.
Co+2 (3d7) forms both octahedral and tetrahedral complexes
Ni+2 (3d8) forms octahedral, tetrahedral, and square planar complexes (as previously stated).
Valence Bond Theory of Transition Metal Coordination Compounds:
VB theory treats metal to ligand (donor group) bonds as coordinate covalent bonds, formed when
a filled orbital of a donor atom overlaps with an empty hybrid orbital on the central metal atom.
The molecular geometry is predicted using VSEPR.
The theory proposes that the number of metal-ion hybrid orbitals occupied by donor atom lone
pairs determine the geometry of the complexes. Lone pairs of electrons are ignored. Since lone
pairs are in the inner shell, they are believed to have little effect on molecular geometry.
2-Coordinate Compounds:
Linear sp hybridized transition metal complexes:
a. Consider [Ag(NH3)2]+ Ag = 5s1 4d10
4d
5s
5p
Ag+ = 5s 4d10
sp
+
sp
5p
+
[Ag(NH3)2]
Ag
hybridized
:NH3 :NH3
Coordination Complexes
7
INORGANIC CHEMISTRY
b. Consider [Cu(CN)2]- Cu = 4s1 3d10 Cu+1 = 4s 3d10
4p
4s
3d
sp
sp
4p
-
Cu+
[Cu(CN)2]
hybridized
CN- CN
K+ : C
N:
-
Problem: Predict the hybridization state and molecular geometry of [AuCl2]-
Note that when transition metals ionize, electrons from the (n+1)s orbitals are usually removed
before those of the nd orbital (even though the (n+1)s orbital is filled before the nd orbital).
This behavior can be abbreviated as FIFO (First In, First Out, i.e., (n+1) orbitals are first to be
filled when building up the electron configuration of the neutral atom, and first to be emptied
during ionization).
The preferential removal of (n+1)s electrons is not surprising, since the (n+1)s electrons are
farther from the nucleus (held less strongly) than nd electrons.
Four Coordinate Compounds: (Tetrahedral Complexes)
a. Consider [ZnCl4]-2
Zn = 4s2 3d10
4p
4s
3d
Zn+2 = 4s 3d10
sp3
sp3
[ZnCl4]-2
Zn+2
hybridized
tetrahedral
Cl- Cl- Cl Cl
b. Consider [Cd(NH3)4]+2 Cd = 5s2 4d10 Cd+2 = 5s 4d10
4d
5s
5p
sp3
+2
Cd
sp3
[Cd(NH3)4]+2
hybridized
tetrahedral
..
..
.. ..
NH3 NH3 NH3 NH3
Note that all 4-coordinate complexes of a s d10 ion are sp3 hybridized and tetrahedral, e.g.,

4-coordinate complexes of Group 2B M+2 ions: Zn+2, Cd+2, Hg+2

4-coordinate complexes of Group 1B M+1 ions: Cu+1, Ag+1, Au+1
Coordination Complexes
8
INORGANIC CHEMISTRY
In four coordinate complexes of s0d8 ions (Ni+2, Pd+2, Pt+2), two molecular geometries are
encountered, tetrahedral (sp3) and square planar (dsp2).
Consider [NiCl4]-2
Ni = 4s2 3d8
3d
4s
4p
Ni+2 = 4s0 3d8
sp3
hybridized
sp3
3d
-2
+2
Ni
tetrahedral
[NiCl4]
As in previous examples of tetrahedral, sp3 hybridized complexes, the ligand donates electrons to
the vacant sp3 hybrid orbitals. This is true when large, weak ligands are present. However, with
small, strong ligands, such as CN-, two unpaired electrons in half-filled 3d orbitals are forced to
pair up with each other, creating an empty 3d orbital. This gives rise to dsp2 hybridization and the
square planar geometry seen in the following examples.
Four Coordinate Compounds: (Square Planar Complexes):
When very strong ligands are present, four-coordinated d8 metal ions usually form square planar
complexes (rather than tetrahedral).
Consider [Ni(CN)4]-2 Ni = 4s2 3d8
3d
4p
4s
Ni+2
dsp2
3d
dsp2
hybridized [Ni(CN) ]-2
4
4p
4p
4s
3d
Ni+2 = 4s 3d8
square
planar
-
-
-
CN CN- CN CN
In dsp2 hybridization, one d-orbital is empty and receives an electron pair from the ligand. Donor
atoms are situated on the x and y -axes of the square planar structure.
Note that in the term 'dsp2', 'd' precedes 'sp2' indicating that the d-orbital used in hybridization
comes from a lower (inner) shell than the 's' and 'p' orbitals. This is called inner shell
hybridization. In the previous unit on bonding, we saw terms such as 'sp3d'. In this case, where
'd' follows 'sp3', the d-orbital is from the highest energy level, e.g., recall that PCl5 has sp3d
hybridization (triangular bipyramidal geometry). This is called outer shell hybridization.
Six Coordinate Complexes (Octahedral):
Six ligand donor atoms in an octahedral complex are located at the corners of an octahedron.
Valence bond postulates that the orbitals best shaped and best oriented to receive electron pairs
from these directions are the dx2-y2 and dz2 orbitals (directed on the x, y, and z-axes).
Consider [Fe(CN)6]-3
3d
Fe
Fe = 4s2 3d6
4s
Fe+3 = 4s0 3d5
4p
+3
3d
Fe+3
4s
4p
d2sp3
hybridized
3d
d2sp3
-3
[Fe(CN)6]
octahedral
CN- CN- CN- CN- CN- CN-
Coordination Complexes
9
INORGANIC CHEMISTRY
CN- is a strong field donor, forcing inner 3d electrons into a lower spin state and hybridizing
inner 3d orbitals, i.e., d2sp3 (inner shell hybridization). H2O, a weaker field donor, is not able to
bring about inner shell hybridization and the resulting hybridization is thus sp3d2. Both d2sp3 and
sp3d2 complexes are octahedral.
Consider [Fe(H2O)6]+3 Fe = 4s2 3d6
3d
Fe
sp 3d2
4d
4p
4s
Fe+3 = 4s0 3d5
hybridized
+3
sp 3d2
3d
octahedral
[Fe(H2O)6]
4d
+3
H2O H2O H2O H2O H2O H2O
Metal ions in which two d-orbitals are vacant will form inner shell hybridized d2sp3 octahedral
complexes.
Metal ions in which two d-orbitals are not vacant will form either outer shell sp3d2 hybridized
octahedral complexes (with weak ligands) or inner shell d2sp3 hybridized octahedral complexes
with strong ligands (If half-filled d-orbitals are present a low spin state can be forced).
Study the following examples and note where inner and outer shell hybridization occur and why.
d6
x
x
Co+3
3d
x
x
4d
4p
4s
x
x
[Co(NH3)6]+3
= an electron pair donated from a ligand
x
x
x
x
x
x
x
x
strong ligand
d2sp 3
3d
x
x
x
x
[CoF6]-3
4d
4p
4s
x
x
x
x
x
x
x
x
weak ligand
sp 3d2
d5 Mn+2
3d
-4
[Mn(CN)6]
x
x
4d
4p
4s
x
x
x
x
x
x
x
x
x
x
d2sp 3
d8
Ni+2
3d
x
x
[Ni(H2O)6]+2
4d
4p
4s
x
x
x
x
x
x
x
x
x
x
sp 3d2
d3
Cr+3
3d
+3
[Cr(NH3)6]
x
x
x
x
4d
4p
4s
x
x
x
x
x
x
x
x
d2sp 3
Coordination Complexes
10
INORGANIC CHEMISTRY
Sample Problems:
1.
Draw the Lewis structure of the product of the following
PH3
+ AlBr3

Write the formula of the Lewis acid: ……………………………………….
Write the formula of the Lewis base: ………………………………………
2.
Consider [Hg(CN)2]
a) name it …………………………………………………………………………
b) state its molecular geometry …………………………………………………
c) name its hybridization state …………………………………………………..
d) use Valence Bond theory to show how it bonds
3.
Consider [ZnI3]-, a 3-coordinate complex
a) name it …………………………………………………………………………
b) predict its molecular geometry …………………………………………………
c) predict its hybridization state …………………………………………………..
d) use Valence Bond theory to show how it bonds
Coordination Complexes
11
INORGANIC CHEMISTRY
4.
Consider [Ni(CN)5]-3, a 5-coordinate complex
a) name it …………………………………………………………………………
b) predict its molecular geometry …………………………………………………
c) use Valence Bond theory to show how it bonds assuming inner shell hybridization
5.
Name the following complexes:
a) K[Sb(C2O4)2(NH2)2]
b) [Mn(OH)2{NH(CH3)2}4Br](SO4)2
c) K[BF4]
d) [W(CO)2(NO2)3F](NO3)2
6.
Write formulas for the following complexes:
a) potassium hexafluoroantimonate(V)
b) sodium octacyanomolybdate(IV)
c) tetraamminediaquazirconium(IV) bromide
d) nitratodiphosphinethiocyanatopalladium(IV) nitrate
Coordination Complexes
12