Coordination Compounds

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1 Coordination Compounds
By : A P SINGH BHADOURIYA 19-Sep-18

2 (ii) Complex compounds or coordination compounds :
Introduction Compounds made up of simpler compounds are called molecular/ addition compound. These are of two types : (i) Double salts : K2SO4 and Al2 (SO4)3 give K2SO4.Al2 (SO4)3.24H2O (Potash Alum) is a double salt. (ii) Complex compounds or coordination compounds : e.g. CoCl3 and NH3 Yields CoCl3· (NH3)6 and CoCl3· (NH3)5. is a Complex compounds. 19-Sep-18

3 Difference Between A Double Salt And A Complex:
Double salts such as carnallite, KCl.MgCl2.6H2O, Mohr’s salt, FeSO4.(NH4)2SO4.6H2O, potash alum, K2Al2(SO4)4.24H2O, etc. dissociate into simple ions completely when dissolved in water. K2SO4.Al2 (SO4)3.24H2O (aq) --> 2K+(aq) Al3+ (aq) + 4 SO42-(aq) However, complex compounds such as K4[Fe(CN)6]4 do not dissociate into simple Fe 2+and CN─ ions. K4[Fe(CN)6]4 (aq) > 4K+(aq) [Fe(CN)6]4 4- (aq) CoCl3· (NH3)6 (aq) > 3 Cl─ + [Co(NH3)6]3+ (aq) 19-Sep-18

4 Some important terms related to coordination compounds
(i) Coordination entity: A complex compound that constitutes a central metal (atom or ion) linked with a fixed number of ions or molecules. For example, [Ni(CO)4], [PtCl2(NH3)2], [Fe(CN)6]4–, [Co(NH3)6]3+., etc. (ii) Central atom/ion: The atom or ion to which a fixed number of ions/groups are bound in a certain geometrical arrangement around it. For example, Fe3+ and Ni2+ are the central ions in the coordination compounds [Fe(CN)6]3– and NiCl2.6H2O respectively. Since it accepts a lone pair of electrons for the formation of coordinate bond, it is also referred to as Lewis acids 19-Sep-18

5 It contains only one donor atom.
(iii) Ligands: The atoms, ions or molecules which donate a pair of electrons to the metal atom to form a coordinate bond, are called ligands. For example, NH3, H2O, Cl─, CN─, CO etc. Depending on the number of donor atoms, a ligand can be of following types: Unidentate or Monodentale ligand: It contains only one donor atom. e.g. NH3, H2O, Cl─, CN─, CO in which N,O, Cl, C are the donor atoms which bind with metal atom or ion. 19-Sep-18

6 (b) Didentate or Bidentate ligand: When a ligand has two donor atoms,
e.g. ethane-1,2-diamine (H2NCH2CH2NH2 ), in which the two nitrogen atoms of the amino group act as donor atoms. (c) Polydentate or Multidentate ligand: When several donor atoms are present in a single ligand, e.g. (EDTA4–) (Ethylenediaminetetraacetate), is an important hexadentate ligand which can bind through two nitrogen and four oxygen donor atoms to a central metal ion. 19-Sep-18

7 Ethylene Diamine 19-Sep-18

8 EDTA 19-Sep-18

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10 (d) Chelate ligand: A di- or polydentate ligand is said to be a chelate ligand when it uses its two or more donor atoms to bind a single metal ion. The number of such ligating groups is called the denticity of the ligand. A complex compound in which the donor atoms are attached to the metal so that the metal becomes a part of the heterocyclic ring, is called chelate complex. 19-Sep-18

11 chlorophyl a 19-Sep-18

12 (v) Coordination number (CN):
The number of unidentate ligands directly bonded to the central metal atom/ion is known as the coordination number of that metal ion/atom. e.g. in the complex ions, [ Ag(NH3)2]2+ , [Zn(CN)4]2─ , & [Ni(NH3)6]2+ the coordination number of Ag, Zn and Ni are 2, 4 and 6 respectively. When the bonded ligands are didentate the coordination number is double the number of ligands because the number of bonds linked to the central metal becomes double. e.g. the coordination number of Fe in [Fe(C2O4)3] 3─is 6, because C2O42─is a didentate ligand 19-Sep-18

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14 (vi) Coordination polyhedron:
Spatial arrangement of the ligand atoms which are directly attached to the central atom/ion. For example, the coordination polyhedra of [Ni(CO)4 , [Co(NH3)6]3+ & [PtCl4] are tetrahedral, octrahedral and square planar respectively (vii) Coordination sphere: The coordination complex which constitutes the central atom/ion and the ligands, are represented in a square bracket, collectively termed as coordination sphere. The ionisable groups are written outside the bracket, called counter ions. For example, in the complex K4[Fe(CN)6] the coordination sphere is [Fe(CN)6]4–, and the counter ion is K+. [ 19-Sep-18

15 (viii) Homoleptic and Heteroleptic complexes:
Complexes in which a metal is bound to only one kind of donor groups, are known as homoleptic. e.g., [Co(NH3)6]3+, Complexes in which a metal is bound to more than one kind of donor groups,are known as heteroleptic. e.g., [Co(NH3)4Cl2]+, 19-Sep-18

16 (ix) Charge on a complex ion:
The charge carried by a complex ion is the algebraic sum of charges carried by the central metal ion and the coordinated groups or ions. For example, [Fe(CN)6]3–, Fe3+ = +3 charge, 6 CN─ = 6 × (─1) = ─ 6 Charge Thus charge on [Fe(CN)6] = +3 – 6 = − 3 19-Sep-18

17 Charge on the metal ion:
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18 (i) Cationic complex ; [ Ag(NH3)2]2+ , [Ni(NH3)6]2+
Types of complex ion: (i) Cationic complex ; [ Ag(NH3)2]2+ , [Ni(NH3)6]2+ (ii) Anionic complex ; [Fe(CN)6]3–, [Zn(CN)4]2─ (iii) Neutral complex ; [Co(NH3)3Cl3],[ Ni(CO)4 ] etc 19-Sep-18

19 Werner’s theory of coordination compounds
The main postulates of Werner’s theory (proposed by Werner in 1898), are as follows: a. In coordination compounds metals show two types of linkages (valancies), primary and secondary. b. The primary valancies are normally ionisable and are satisfied by negative ions. c. The secondary valancies are non-ionisable which are satisfied by negative ions or neutral molecules. The secondary valency is equal to the coordination number and is fixed for a metal. d. The ions/groups bound by the secondry linkages to the metal have characteristic spatial arrangements corresponding to different coordination numbers. Werner further postulated that the most common geometrical shapes of coordination compounds are octahedral, tetrahedral and square planar. 19-Sep-18

20 IUPAC Nomenclature of coordination compounds
Writing the formulas of mononuclear (containing single central metal atom) coordination compounds: The central atom is listed first. The ligands are then listed in alphabetical order without considering their charge. Polydentate ligands are also written alphabetically. In case of abbreviated ligand, the first letter of abbreviation is used to determine the position of ligand in alphabetical order. 19-Sep-18

21 (d) The formula of the entire coordination entity, whether
charged or uncharged, is enclosed in square brackets. When ligands are polyatomic, their formulas are enclosed in parantheses. Ligand abbreviations are also enclosed in parantheses. (e) There should be no space between the ligands and the metal within a coordination sphere. When the formula of a charged coordination entity is to be written without that of the counter ion, the charge is indicated outside the square brackets as a right superscript with the number before the sign. e.g.[Ag(NH3)2]2+ , [Ni(NH3)6]2+ [Fe(CN)6]3–, etc. The charge of cation(s) is balanced by the charge of anion(s). 19-Sep-18

22 (ii) Writing the name of coordination compounds:
The name of cation is written first in both positively and negatively charged coordination entities followed by the naming of anion. The legands are named in an alphabetical order before the name of central atom/ion. (This procedure is opposite to that in writing formula). Names of anionic legands and in – O, those of cationic and neutral ligands are the same except aqua for H2O, ammine for NH3, carbonyl for CO and nitrosyl for NO. These are placed within closing marks [ ]. Note: IUPAC recommendations (2004) The anion endings 'ide', 'ate' and 'ite' (cf. Section IR-5.3.3) are changed to 'ido', 'ato' and 'ito', respectively, when generating the prefix for the central atom 19-Sep-18

23 (d) Prefixes mono, di, tri, etc., are used to indicate the
number of the individual ligands in the coordination entity. When the names of the ligands include a numerical prefix, then the terms, bis, tris, tetrakis are used, the ligand to which they refer being placed in parenthesis. e.g., [NiCl2(PPh3)2] is named as dichlorobis(triphenylphosphine) nickel (II). Oxidation state of the metal in cation, anion or neutral coordination entity is indicated by roman numerical in parenthesis. 19-Sep-18

24 If the complex ion is a cation, the metal is named same as
the element. e.g., Co in a complex cation is called cobalt and Pt is called platinum. (g) If the complex ion is an anion, the name of the metal ends with the suffix- ate. e.g., Co in a complex [Co(NH3)5Br]2− anion, is called cobaltate. For some metals, the latin names are used in the complex anions, e.g., ferrate for Fe. The neutral complex molecule is named similar to that of the complex cation. 19-Sep-18

25 triamminetriaquachromium(III) chloride 2. [Co(H2NCH2CH2NH2)3]2(SO4)3
Example 1. Write the IUPAC name of the following coordination compounds: [Cr(NH3)3(H2O)3]Cl3 triamminetriaquachromium(III) chloride 2. [Co(H2NCH2CH2NH2)3]2(SO4)3 tris(ethane-1,2–diammine)cobalt(III) sulphate. 3. [Ag(NH3)2][Ag(CN)2] diamminesilver(I) dicyanoargentate(I) 4. Hg[Co(SCN)4] Mercury tetrathiocyanatocobaltate(III) 5. [CoCl2(en)2]Cl Dichloridobis(ethane-1,2-diamine)cobalt(III) chloride 19-Sep-18

26 Potassium tetrahydroxidoozincate(II) K2[Zn (OH) 4 ]
Example 2. Write the molecular formulas of the following coordination compounds: Potassium tetrahydroxidoozincate(II) K2[Zn (OH) 4 ] (ii) Diamminechloridonitrito-N-platinum(II) [Pt(NH3)2Cl(NO2)] Tetraammineaquachloridocobalt(III) chloride [Co(NH3)4(H2O)Cl] Potassium trioxalatoaluminate(III) K3[Al(C2O4)3] 19-Sep-18

27 Q.1. Write the formulas for the following coordination compounds:
Tetraamineaquachloridocobalt(III) chloride (ii) Potassium tetrahydroxozincate(II) (iii) Potassium trioxalatoaluminate(III) (iv) Dichloridobis(ethane-1,2-diamine)cobalt(III) (v) Tetracarbonylnickel(0) 19-Sep-18

28 Q.2. Write the IUPAC names of the following coordination compounds:
(i) [Co(NH3)6]Cl3 (ii) [Co(NH3)5Cl]Cl2 (iii) K3[Fe(CN)6] (iv) K3[Fe(C2O4)3] (v) K2[PdCl4] (vi) [Pt(NH3)2Cl(NH2CH3)]Cl 19-Sep-18

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