Coordination Compounds
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9.21 Draw all the isomers (geometrical and optical) of:
(i) [CoCl2(en)2] +
(ii) [Co(NH3)Cl(en)2] 2+
(iii) [Co(NH3)2Cl2(en)]+
9.21 Draw all the isomers (geometrical and optical) of:
(i) [CoCl2(en)2] +
(ii) [Co(NH3)Cl(en)2] 2+
(iii) [Co(NH3)2Cl2(en)]+
Two types of ligand : chloride ion is unidentate ligand and -en (ethylenediamine) is bidentate ligand with two sites of attachment. The complexes in which two symmetrical bidentate chelating ligands AA and two monodentate ligands a, are coordinated to central metal atom M, exhibit the phenomenon of
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9.20 Draw the structures of optical isomers of: (i) [Cr(C2O4)3] 3– (ii) [PtCl2(en)2] 2+ (iii) [Cr(NH3)2Cl2(en)]+
9.20 Draw the structures of optical isomers of: (i) [Cr(C2O4)3] 3– (ii) [PtCl2(en)2] 2+ (iii) [Cr(NH3)2Cl2(en)]+
Optical isomers are the one which rotate the plane polarized light by a certain angle when passed through them and are mirror images of each other, also called as stereoisomer.
(i) C2O4 2- is a bidentate ligand so it can attach to central atom at two sites, forming a chelate ring. In the complexes o
Upvote 9.19 How many geometrical isomers are possible in the following coordination entities? (i) [Cr(C2O4)3] 3– (ii) [Co(NH3)3Cl3]
9.19 How many geometrical isomers are possible in the following coordination entities? (i) [Cr(C2O4)3] 3– (ii) [Co(NH3)3Cl3]
(i) No geometrical isomer is possible for [Cr (C2O4)3]3– because the ligand C2O 2- is bidentate ligand (which have two sites of attachment to the central atom) and also in the coordination sphere it is the only ligand bond to it.
(ii) In the coordination sphere of [Co (NH3)3Cl3] there are two
Upvote 9.18 List various types of isomerism possible for coordination compounds, giving an example of each.
9.18 List various types of isomerism possible for coordination compounds, giving an example of each.
Isomers are the compounds which have same chemical formula but different arrangement of atoms in space. There are principle two types of isomerism:
(i) Stereo isomerism
(ii) Geometrical isomerism
(iii) Optical isomerism
(iv) Structural isomerism
(v) Ionisation isomerism
(vi) Linkage isomerism
(vii)
Upvote 9.17 Using IUPAC norms write the systematic names of the following:
(i) [Co(NH3)6]Cl3
(ii) [Pt(NH3)2Cl(NH2CH3)]Cl
(iii) [Ti(H2O)6] 3+
(iv) [Co(NH3)4Cl(NO2)]Cl
(v) [Mn(H2O)6] 2+
(vi) [NiCl4] 2–
(vii) [Ni(NH3)6]Cl2
(viii) [Co(en)3] 3+
(ix) [Ni(CO)4]
9.17 Using IUPAC norms write the systematic names of the following:
(i) [Co(NH3)6]Cl3
(ii) [Pt(NH3)2Cl(NH2CH3)]Cl
(iii) [Ti(H2O)6] 3+
(iv) [Co(NH3)4Cl(NO2)]Cl
(v) [Mn(H2O)6] 2+
(vi) [NiCl4] 2–
(vii) [Ni(NH3)6]Cl2
(viii) [Co(en)3] 3+
(ix) [Ni(CO)4]
(i) Starting with cation, the complex ion contains six ammonia molecules with cobalt in + 3 oxidation The name of compound: [Co (NH3)6]Cl3 is hexaamminecobalt (III) chloride.
(ii) The complex ion is cation, so there are 2 ammonia molecules, one chloride ion and methyammine molecule qith plati
Upvote 9.16 Using IUPAC norms write the formulas for the following:
(i) Tetrahydroxidozincate(II)
(ii) Potassium tetrachloridopalladate(II)
(iii) Diamminedichloridoplatinum(II)
(iv) Potassium tetracyanidonickelate(II)
(v) Pentaamminenitrito-O-cobalt(III)
(vi) Hexaamminecobalt(III) sulphate
(vii) Potassium tri(oxalato)chromate(III)
(viii) Hexaammineplatinum(IV)
(ix) Tetrabromidocuprate(II)
(x) Pentaamminenitrito-N-cobalt(III)
9.16 Using IUPAC norms write the formulas for the following:
(i) Tetrahydroxidozincate(II)
(ii) Potassium tetrachloridopalladate(II)
(iii) Diamminedichloridoplatinum(II)
(iv) Potassium tetracyanidonickelate(II)
(v) Pentaamminenitrito-O-cobalt(III)
(vi) Hexaamminecobalt(III) sulphate
(vii) Potassium tri(oxalato)chromate(III)
(viii) Hexaammineplatinum(IV)
(ix) Tetrabromidocuprate(II)
(x) Pentaamminenitrito-N-cobalt(III)
(i) Tetrahydroxidozincate (II) = [Zn (OH)4]-2
Tetrahydroxi means 4 hydroxide ions with zinc in + 2 oxidation state. Hydroxide ions have a negative charge of -1, so balancing the overall charge of the coordination compound to be zero we get the formula as : [Zn (OH)4]-2
(ii) Potassium tetrachlo
Upvote 9.15 Specify the oxidation numbers of the metals in the following coordination entities:
(i) [Co(H2O)(CN)(en)2] 2+
(ii) [CoBr2(en)2] +
(iii) [PtCl4] 2–
(iv) K3[Fe(CN)6]
(v) [Cr(NH3)3Cl3]
9.15 Specify the oxidation numbers of the metals in the following coordination entities:
(i) [Co(H2O)(CN)(en)2] 2+
(ii) [CoBr2(en)2] +
(iii) [PtCl4] 2–
(iv) K3[Fe(CN)6]
(v) [Cr(NH3)3Cl3]
(i) Let Oxidation of Co be x and charge on the complex is given as + 2
H2O has Oxidation Number: 0
CN has Oxidation Number: -1
en has Oxidation Number :0
(ii) Let Oxidation number of Co be x and charge on the complex is given as + 1
Br has Oxidation number: 1
en has oxidation number : 0
(iii
Upvote 9.14 What is meant by unidentate, didentate and ambidentate ligands? Give two examples for each.
9.14 What is meant by unidentate, didentate and ambidentate ligands? Give two examples for each.
Ligands are the neutral or negatively charged entities surrounding the central metal atom of the coordination complex which possesses at least one unshared pair of electrons.
Based on the number of donor sites of these ligands, Ligands are classified as:
Unidentate ligands: These Ligands which have on
Upvote 9.13 Explain with two examples each of the following: coordination entity, ligand, coordination number, coordination polyhedron, homoleptic and heteroleptic.
9.13 Explain with two examples each of the following: coordination entity, ligand, coordination number, coordination polyhedron, homoleptic and heteroleptic.
(1) Coordination Entity: Coordination entity is a charged entity having positive or negative charge in which the central atom is surrounded by molecules which may be neutral/negatively charged called Ligands
Examples:
i. Cationic Complexes: [Cu (H2O)6]2+, [Al (H2O)6]3+
ii. Anionic Complexes: [CuCl4]2-
Upvote 9.12 FeSO4 solution mixed with (NH4)2SO4 solution in 1:1 molar ratio gives the test of Fe2+ ion but CuSO4 solution mixed with aqueous ammonia in 1:4 molar ratio does not give the test of Cu2+ ion. Explain why?
9.12 FeSO4 solution mixed with (NH4)2SO4 solution in 1:1 molar ratio gives the test of Fe2+ ion but CuSO4 solution mixed with aqueous ammonia in 1:4 molar ratio does not give the test of Cu2+ ion. Explain why?
The reaction is given below:
FeSO4 + (NH4)2SO4 + 6H2O → FeSO4 (NH4)2SO4.6H2O (Mohr Salt)
FeSO4, when reacted with (NH4)SO4, does not form any complex whereas they form a double salt, FeSO4. (NH4)2SO4.6H2O - (Mohr salt) which dissociates into ions in the solution. So, it gives the test of Fe2+ ions.
CuS
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