(a) Assertion and Reason both are true, Reason is the correct explanation of Assertion. (b) Assertion and Reason both are true but Reason is not the correct explanation of Assertion. (c) Assertion...
Assertion (A): Complexes of MX6 and MX5L type (X and L are unidentate) do not show geometrical isomerism. Reason (R): Geometrical isomerism is not shown by complexes of coordination number 6.
(a) Assertion and Reason both are true, Reason is the correct explanation of Assertion. (b) Assertion and Reason both are true but Reason is not the correct explanation of Assertion. (c) Assertion...
Assertion (A): Linkage isomerism arises in coordination compounds containing ambidentate ligand. Reason (R): Ambidentate ligand has two different donor atoms.
(a) Assertion and Reason both are true, Reason is the correct explanation of Assertion. (b) Assertion and Reason both are true but Reason is not the correct explanation of Assertion. (c) Assertion...
Assertion (A): [Cr(H2O)6]Cl2 and [Fe(H2O)6]Cl2 are reducing in nature. Reason (R): Unpaired electrons are present in their J-orbitals.
(a) Assertion and Reason both are true, Reason is the correct explanation of Assertion. (b) Assertion and Reason both are true but Reason is not the correct explanation of Assertion. (c) Assertion...
Assertion (A): Toxic metal ions are removed by the chelating ligands. Reason (R): Chelate complexes tend to be more stable.
(a) Assertion and Reason both are true, Reason is the correct explanation of Assertion. (b) Assertion and Reason both are true but Reason is not the correct explanation of Assertion. (c) Assertion...
Match the compounds given in Column I with the oxidation state of cobalt present in it (given in Column II) and assign the correct code. with the oxidation state of cobalt present in it (given in Column II) and assign the correct code.
Solution: \[\left( c \right)\text{ }\left( A\text{ }\to \text{ }5 \right),\text{ }\left( B\text{ }\to \text{ }1 \right),\text{ }\left( C\text{ }\to \text{ }4 \right),\text{ }\left( D\text{...
Match the complex species given in Column I with the possible isomerism given in Column II and assign the correct code:
Solution: \[\left( d \right)\text{ }\left( A\text{ }\to 4 \right),\text{ }\left( B\to \text{ }1 \right),\text{ }\left( C\text{ }\to 2 \right),\text{ }\left( D\text{ }\to 3 \right)\] Isomerism...
Match the complex ions given in Column I with the hybridisation and number of unpaired electrons given in Column II and assign the correct code :
Solution: \[\left( a \right)\text{ }\left( A\text{ }\to \text{ }3 \right),\text{ }\left( B\text{ }\to 1 \right),\text{ }\left( C\text{ }\to \text{ }5 \right),\text{ }\left( D\to \text{ }2...
Match the coordination compounds given in Column I with the central metal atoms given in Column II and assign the correct code : Code : (i) A (5) B (4) C (1) D (2) (ii) A (3) B (4) C (5) D (1) (iii) A (4) B (3) C (2) D (1) (iv) A (3) B (4) C (1) D (2)
Solution: \[\left( b \right)\text{ }\left( A\text{ }\to 5 \right),\text{ }\left( B\text{ }\to \text{ }4 \right),\text{ }\left( C\text{ }\to \text{ }1 \right),\text{ }\left( D~\to 2 \right)\] ...
Match the complex ions given in Column I with the colours given in Column II and assign the correct code :
Solution: \[\left( b \right)\text{ }\left( A\text{ }\to 4 \right),\text{ }\left( B\text{ }\to \text{ }3 \right),\text{ }\left( C\text{ }\to \text{ }2 \right),\text{ }\left( D\text{ }\to \text{ }1...
Name the type of isomerism when ambidentate ligands are attached to a central metal ion. Give two examples of ambidentate ligands.
Solution: Ambidendate ligands are those having diverse two restricting destinations. Example: Isothiocyanato Thiocyanato and Nitrite-N Nitrito-O The kind of isomerism when ambidentate ligands are...
CuSO4.5H2O is blue while CuSO4 is colourless. Why?
Solution: In CuSO4.5H2O, there are water particles that go about as ligands. The electrons will invigorate to higher d orbital and show tone. While, in CuSO4, there are no water particles to go...
Give the electronic configuration of the following complexes based on Crystal Field Splitting theory. [CoF6]3–, [Fe(CN)6]4– and [Cu(NH3)6]2+.
Solution: \[{{[CO{{F}_{\mathbf{6}}}]}^{\mathbf{3}-}}:\text{ }C{{o}^{\mathbf{3}+}}~({{d}^{\mathbf{6}}})\]
Which of the following complexes show linkage isomerism? (a) [CO(NH3)5(NO2)]2+ (b) [CO(H2O)5CO]3+ (c) [Cr(NH3)5SCN]2+ (d) [Fe(en)2Cl2]+
Solution: (a, c) NO2 and SCN are ambidentate ligands subsequently, show linkage isomerism.
Identify the correct statements for the behaviour of ethane-1, 2-diamine as a ligand. (a) It is a neutral ligand (b) It is a didentate ligand (c) It is a chelating ligand (d) It is a unidentate ligand
Solution: hence, option a, b and c are correct
Identify the optically active compounds from the following: (a) [Co(en)3]3+ (b) trans-[Co(en)2Cl2]+ (c) cis-[Co(en)2Cl2]+ (d) [Cr(NH3)5Cl]
Solution:
Which of the following complexes are heteroleptic? (a) [Cr(NH3)6]3+ (b) [Fe(NH3)4 Cl2]+ (c) [Mn(CN)6]4– (d) [Co(NH3)4Cl2]
Solution: (b, d) In complexes, [Fe(NH3)4Cl2]+ and [CO(NH3)4Cl2], metal is bonded to more than one sort of ligands subsequently, they are heteroleptic.
Which of the following complexes is homoleptic? (a) [Co(NH3)6]3+ (b) [Co(NH3)4 Cl2]+ (c) [Ni(CN)4]2– (d) [Ni(NH3)4Cl2]
Solution: (a, c) In complexes [Co(NH3)6]3+ and [Ni(CN)4]2-, both Co and Ni are connected to one sort of ligands just subsequently, they are homoleptic. hence, option a and c are correct
An aqueous pink solution of cobalt(II) chloride changes to deep blue on the addition of an excess of HCl. This is because____________. (a) [Co(H2O)6]2+ is transformed into [CoCl6]4– (b) [Co(H2O)6]2+ is transformed into [CoCl4]2– (c) tetrahedral complexes have smaller crystal field splitting than octahedral complexes. (d) tetrahedral complexes have larger crystal field splitting than octahedral complex.
Solution: (b, c) Aqueous pink arrangement of cobalt (II) chloride is because of electronic progress of electron from t2g to eg energy level of [Co(H2O)6]2+ complex. At the point when overabundance...
Which of the following options are correct for [Fe(CN)6]3- complex? (a) d2sp3 hybridisation (b) sp3d2 hybridisation (c) Paramagnetic (d) Diamagnetic
Solution: hence, option a and c are correct for [Fe(CN)6]3- complex
Atomic number of Mn, Fe, Co and Ni are 25, 26 27 and 28 respectively. Which of the following outer orbital octahedral complexes have same number of unpaired electrons? (a) [MnCl6]3- (b) [FeF6]3- (c) [CoF6]3- (d) [Ni(NH3)6]2+
Solution: so, option a and c are the correct answer
The atomic number of Mn, Fe and Co are 25, 26 and 27 respectively. Which of the following inner orbital octahedral complexions are diamagnetic? (a) [Co(NH3)6]3+ (b) [Mn(CN)6]3– (c) [Fe(CN)6]4– (d) [Fe(CN)6]3–
Solution: hence , a and c are the correct answer
IUPAC name of [Pt(NH3)2Cl(NO2)] is (a) platinum diaminechloronitrite (b) chloronitrito-N-ammineplatinum (II) (c) diamminechloridonitrito-N-platinum (II) (d) diamminechloronitrito-N-platinate (II).
Solution: (c) [Pt(NH3)2Cl(NO2)] is diamminechloridonitrito-N-platinum (II)
What kind of isomerism exists between [Cr(H2O)6]Cl3 (violet) and [Cr(H2O)5Cl)Cl2.H2O (greyish- green)? (a) Linkage isomerism (b) Solvate isomerism (c) Ionisation isomerism (d) Coordination isomerism
Solution: (b) The given mixtures have diverse number of water atoms inside and outside the organize circle.
Which of the following species is not expected to be a ligand? (a) NO (b) NH4– (c) NH2CH2CH2NH2 (d) CO
Solution: (b) Ligand should give a pair of electrons or inexactly held electron pair to metal and shape a M – L bond,
A chelating agent has two or more than two donor atoms to bind to a single metal ion. Which of the following is not a chelating agent? (a) Thiosulphate (b) Oxalato (c) Glycinato (d) Ethane-1, 2-diamine
Solution: (a) Thiosulphate or S2O3–isn't a chelating specialist since it is a monodentate ligand.
The compounds [Co(SO4)(NH3)5]Br and [CO(SO4)(NH3)5]Cl represent (a) linkage isomerism (b) ionization isomerism (c) coordination isomerism (d) no isomerism.
Solution: (d) [Co(SO4)(NH3)5]Br and [CO(SO4)(NH3)5]Cl address no isomerism since they are different compounds.
Due to the presence of ambidentate ligands coordination compounds show isomerism. Palladium complexes of the type [Pd(C6H5)2(SCN)2] and [Pd(C6H5)2(NCS)2] are (a) linkage isomers (b) coordination isomers (c) ionisation isomers (d) geometrical isomers
Solution: (a) The ligands having two distinctive holding locales are known as ambident ligands e.g., NCS, NO2, and so forth Here, NCS has two restricting locales at N and S. Subsequently, NCS...
The CFSE for octahedral [CoCl6]4– is 18,000 cm–1. The CFSE for tetrahedral [CoCl4]2– will be (a) 18,000 cm–1 (b) 16,000 cm–1 (c) 8,000 cm–1 (d) 20,000 cm–1
Solution:
Indicate the complex ion which shows geometrical isomerism. (a) [Cr(H2O)4Cl2]+ (b) [Pt(NH3)3 Cl] (c) [Co(NH3)6]3+ (d) [Co(CN)5(NC)]3–
Solution:
The correct IUPAC name of [Pt(NH3)2Cl2] is (a) diamminedichloridoplatinum (II) (b) diamminedichloridoplatinum (IV) (c) diamminedichloridoplatinum (I) (d) dichloridodiammineplatinum (IV)
Solution: (a) [Pt(NH3)2Cl2] is diamminedichloridoplatinum (II) .
When 1 mol CrCl3.6H2O is treated with an excess of AgNO3, 3 mol of AgCl are obtained. The formula of the complex is : (a) [CrCl3 (H2O)3].3H2O (b) [CrCl2(H2O)4]Cl.2H2O (c) [CrCl(H2O)5]Cl2.H2O (d) [Cr(H2O)6]Cl3
Solution: (d) 3 mol of AgCl implies 3Cl are given in the arrangement henceforth, the equation of the complex will be [Cr(H2O)6]Cl3.
When 0.1 mol COCl3(NH3)5 is treated with excess of AgNO3, 0.2 mol of AgCl are obtained. The conductivity of solution will correspond to (a) 1:3 electrolyte (b) 1:2 electrolyte (c) 1:1 electrolyte (d) 3:1 electrolyte
Solution: (b) One mole of AgNO3 accelerates one mole of chloride particle. In the above response, when 0.1 mole COCl3(NH3)5 is treated with abundance of AgNO3, 0.2 mole of AgCl are obtained hence,...
The colour of the coordination compounds depends on the crystal field splitting. What will be the correct order of absorption of wavelength of light in the visible region, for the complexes, [Co(NH3)6]3+, [Co(CN)6]3–, [Co(H2O)6]3+ (a) [Co(CN)6]3–> [Co(NH3)6]3+>[Co(H2O)6]3+ (b) [Co(NH3)6]3+> [Co(H2O)6]3+> [Co(CN)6]3– (c) [Co(H2O)6]3+> [Co(NH3)6]3+> [Co(CN)6]3– (d) [Co(CN)6]3–> [Co(NH3)6]3+> [Co(H2O)6]3+
Solution:
Which of the following complexes formed by Cu2+ ions is most stable?
Solution: (b) The greater the value of log K, the more prominent will be strength of complicated compound shaped. For response, For this response, log K has most elevated worth among the...
For what reason do compounds having comparable calculation have an alternate attractive second?
Solution: They vary in the quantity of combined and unpaired electrons. A solid field ligand will cause blending of electrons while a feeble field ligand won't cause matching. Blending or not...
Mastermind following complex particles in expanding request of precious stone field parting energy (DO) : [Cr(Cl)6]3–, [Cr(CN)6]3–, [Cr(NH3)6]3+.
Solution: The expanding request of gem field energy is [Cr(Cl)6]3–<[Cr(NH3)6]3+ <[Cr(CN)6]3– This is additionally the request for field strength of the ligands as indicated by the...
Clarify why [Fe(H2O)6]3+ has an attractive second worth of 5.92 BM while [Fe(CN)6]3–has a worth of just 1.74 BM.
Solution: For [Fe(H2O)6]3+, H2O is a powerless field ligand will not cause matching of electrons. Along these lines, the quantity of unpaired electrons will be 5. [Fe(CN)6]3–, Fe3+ has six unpaired...
Why are low twist tetrahedral edifices not framed?
Solution: For tetrahedral edifices, the gem field parting energy is excessively low. It is lower than blending energy in this way, the matching of electrons isn't supported and consequently the...
In view of gem field hypothesis clarify why Co(III) structures a paramagnetic octahedral complex with feeble field ligands though it frames a diamagnetic octahedral complex with solid field ligands.
Solution: The electronic design will be t42g e2g. It has 4 unpaired electron and paramagnetic. With weal ligand Δ0 < p. The design with solid field ligand will be t62g e0g. the Δ0 > p and...
The attractive snapshot of [MnCl4]2–is 5.92 BM. Clarify giving an explanation.
Solution: An attractive snapshot of 5.92 BM implies there are 5 unpaired electrons in light of the fact that \[Attractive\text{ }Moment\text{ }=\text{ }\surd \text{ }n\left( n+2 \right)\] The...
A complex of the kind [M(AA)2X2]n+is known to be optically dynamic. What does this demonstrate about the design of the complex? Give one illustration of such complicated.
Solution: The design must be cis-octahedral. Model for a particularly mind boggling is [Co(en)2Cl2]+ which is optically dynamic.
A coordination compound CrCl3.4H2O hastens silver chloride when treated with silver nitrate. The molar conductance of its answer relates to a sum of two particles. Compose the primary recipe of the compound and name it.
Solution: Assuming it structures silver chloride, there is without one chlorine iota outside the coordination circle. The primary recipe must be [Cr(H2O)4Cl2]Cl. The name of this complex is...
Organize the accompanying buildings in the expanding request of conductivity of their answer: [Co(NH3)3Cl3], [Co(NH3)4Cl2] Cl, [Co(NH3)6]Cl3 , [Cr(NH3)5Cl]Cl2
Solution: The expanding request of conductivity is as per the following: [Co(NH3)3Cl3]<[Co(NH3)4Cl2]Cl< [Cr(NH3)5Cl]Cl2<[Co(NH3)6]Cl3
What will be the correct order for the wavelengths of absorption in the visible region for the following:
\[{{[\mathbf{Ni}{{(\mathbf{N}{{\mathbf{O}}_{\mathbf{2}}})}_{\mathbf{6}}}]}^{\mathbf{4}}},\text{ }{{[\mathbf{Ni}{{(\mathbf{N}{{\mathbf{H}}_{\mathbf{3}}})}_{\mathbf{6}}}]}^{\mathbf{2}+}},\text{ }{{[\mathbf{Ni}{{({{\mathbf{H}}_{\mathbf{2}}}\mathbf{O})}_{\mathbf{6}}}]}^{\mathbf{2}+}}?\]
Because all of the complexes have the same metal ion, the energy absorption is determined by the ligands' CFSE values. The ligands' CFSE values are in the order of H2O < NH3 < NO2- according...
Amongst the following, the most stable complex is \[\left( i \right)\text{ }{{[Fe{{({{H}_{2}}O)}_{6}}]}^{3+}}\left( ii \right)\text{ }{{[Fe{{(N{{H}_{3}})}_{6}}]}^{3+}}~\left( iii \right)\text{ }{{[Fe{{({{C}_{2}}{{O}_{4}})}_{3}}]}^{3}}~~~\left( iv \right)\text{ }{{[FeC{{l}_{6}}]}^{3}}\]
Fe has an oxidation state of +3 in all circumstances. The chelating ligand (C2O4)3 is a bidentate chelating ligand that produces chelating rings. As a result, the most stable complex is ( iii ).
What is the oxidation number of cobalt in K[Co(CO)4]?
Amongst the following ions which one has the highest magnetic moment value? \[\left( i \right)\text{ }{{[Cr{{({{H}_{2}}O)}_{6}}]}^{3+}}\left( ii \right)\text{ }{{[Fe{{({{H}_{2}}O)}_{6}}]}^{2+}}\left( iii \right)\text{ }{{[Zn{{({{H}_{2}}O)}_{6}}]}^{2+}}\]
How many ions are produced from the complex Co(NH3)6Cl2 in solution?
(i) 6 (ii) 4 (iii) 3 (iv) 2
(iii) The answer is 3. The given complex [ Co( NH3)6 ]Cl2 ionizes to give three ions, viz one [ Co( NH3)6] + and two Cl – ions.
Discuss briefly giving an example in each case the role of coordination compounds in:
(i) analytical chemistry and (ii) extraction/metallurgy of metals.
(i) Role in analytical chemistry:Determination of hardness of the water. (ii) Complexes are generated during the extraction of metals from ores, and they play a role in metallurgy and...
Discuss briefly giving an example in each case the role of coordination compounds in:
(i) biological systems (ii) medicinal chemistry
(i) Role in biological systems: There are various essential coordination compounds in the bodies of animals, such as hemoglobin, which is an iron coordination compound. In plants, chlorophyll...
What is meant by the chelate effect? Give an example.
The metal-ligand bond becomes more stable when a polydentate or bidentate ligand attaches to a metal ion in such a way that it takes on the structure of a ring. Chelate rings are the name for these...
Explain the violet color of the complex \[{{[\mathbf{Ti}{{({{\mathbf{H}}_{\mathbf{2}}}\mathbf{O})}_{\mathbf{6}}}]}^{\mathbf{3}+}}~\] on the basis of crystal field theory.
The degree/level of association among the species involved in a state of equilibrium determines the stability of a coordination molecule in a solution. The formation constant or stability constant...
Write down the IUPAC name for each of the following complexes and indicate the oxidation state, electronic configuration, and coordination number. Also, give stereochemistry and magnetic moment of the complex: \[\left( i \right)\text{ }[CrC{{l}_{3}}{{\left( py \right)}_{3}}]\left( ii \right)\text{ }Cs[FeC{{l}_{4}}]\left( iii \right)\text{ }{{K}_{4}}[Mn{{\left( CN \right)}_{6}}]\]
Write down the IUPAC name for each of the following complexes and indicate the oxidation state, electronic configuration and coordination number. Also, give stereochemistry and magnetic moment of the complex:
(i) K[Cr(H2O)2(C2O4)2].3H2O (ii) [Co(NH3)5Cl]Cl2
n = 0.Thus, Magnetic moment = 0
Give the oxidation state, d orbital occupation and coordination number of
the central metal ion in the following complexes:
(i) (NH4)2[CoF4] (ii) [Mn(H2O)6]SO4
Give the oxidation state, d orbital occupation and coordination number of
the central metal ion in the following complexes:
(i) K3[Co(C2O4)3] (iii) (NH4)2[CoF4]
Discuss the nature of bonding in metal carbonyls.
The metal-carbon bond in metal carbonyls has both the and bond characteristics. The carbonyl carbon donates a lone pair of electrons to the metal's vacant orbital, forming a connection. The filled d...
\[{{[\mathbf{Fe}{{\left( \mathbf{CN} \right)}_{\mathbf{6}}}]}^{\mathbf{4}}}~\mathbf{and}\text{ }{{[\mathbf{Fe}{{({{\mathbf{H}}_{\mathbf{2}}}\mathbf{O})}_{\mathbf{6}}}]}^{\mathbf{2}+}}~\] are of different colours in dilute solutions. Why?
[Fe( H2O)6 ]2+ and [ Fe( CN)6 ]2+ have H2O and CN- ligands respectively. CN- has a higher CFSE (crystal field splitting energy) than water because it is a strong field ligand. As a result,...
A solution of [Ni(H2O)6]2+ is green but a solution of [Ni(CN)4]2– is colorless. Explain
[ Ni (H2O)6 ] is made up of the Ni+2 ion, which has a 3d8 electrical structure. Because H2O is a weak ligand, there are two unpaired electrons in this arrangement that cannot pair up. The d – d...
\[{{[\mathbf{Cr}{{(\mathbf{N}{{\mathbf{H}}_{\mathbf{3}}})}_{\mathbf{6}}}]}^{\mathbf{3}+}}\] is paramagnetic while [Ni(CN)4]2– is diamagnetic. Explain why.
In [ Ni ( CN)4 ] 2−, Ni has an oxidation state of +2. Thus, it has d 8configuration.Ni 2+ : Because CN- is a strong field ligand, electrons in 3d orbitals couple. Ni 2+ undergoes dsp2 hybridization...
What is crystal field splitting energy? How does the magnitude of ∆o decide the actual configuration of d orbitals in a coordination entity?
The difference in energy between the two levels ( t2g and eg ) that have split from a degenerated d orbital due to the presence of a ligand is known as crystal-field splitting energy. It is...
What is the spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.
The Spectrochemical series is a set of common ligands arranged in ascending order of their crystal-field splitting energy (CFSE). CFSE readings are higher in strong field ligands. Weak field...
Draw a figure to show the splitting of d orbitals in an octahedral crystal field.
Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory: \[\left( i \right)\text{ }{{[Co{{({{C}_{2}}{{O}_{4}})}_{3}}]}^{3}}\] \[\left( ii \right)\text{ }{{[Co{{F}_{6}}]}^{3-}}\]
(i) Here, the oxidation state of cobalt is +3.Orbitals of Co 3+ ion : Oxalate is a field ligand with a low affinity. As a result, the electrons in the 3d orbital will not pair.Because there are six...
Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory: \[\left( i \right)\text{ }{{[Fe{{\left( CN \right)}_{6}}]}^{4}}\] \[\left( ii \right)\text{ }{{[Fe{{F}_{6}}]}^{3}}\]
(i) Here, the oxidation state of Fe is +3.Fe 2+ : Electronic configuration is 3d6Orbitals of Fe2+ ion : CN− is a strong field ligand, so it causes the unpaired 3d electrons to pair up: There are six...
What is the coordination entity formed when an excess of aqueous KCN is added to an aqueous solution of copper sulfate? Why is it that no precipitate of copper sulphide is obtained when \[{{H}_{2}}S\left( g \right)\] is passed through this solution?
As a result of the foregoing procedure, the coordination entity obtained is K2[Cu(CN)4 ].The above coordination entity does not ionize to produce Cu2+ ions since it is extremely stable. When...
Aqueous copper sulfate solution (blue in color) gives: (i) a green precipitate with aqueous potassium fluoride and (ii) a bright green solution with aqueous potassium chloride. Explain these experimental results.
The presence of [Cu( H2O)4]2+ ions in an aqueous CuSO4 solution gives it a blue colour. (i) As a result, when KF is introduced, H2O ligands are replaced by F- ligands, resulting in green [ CuF4 ]2+...
Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of these will exhibit optical isomers?
None of the isomers exhibit optical isomerism.
Draw all the isomers (geometrical and optical) of \[{{[Co{{(N{{H}_{3}})}_{2}}C{{l}_{2}}\left( en \right)]}^{+}}\]
Draw all the isomers (geometrical and optical) of: (i) \[{{[CoC{{l}_{2}}{{\left( en \right)}_{2}}]}^{+}}\] (ii) \[{{[Co(N{{H}_{3}})Cl{{\left( en \right)}_{2}}]}^{2+}}\]
(i) (ii)
Draw the structures of optical isomers of \[{{[Cr{{(N{{H}_{3}})}_{2}}C{{l}_{2}}\left( en \right)]}^{+}}\]
Draw the structures of optical isomers of:
(i) [Cr(C2O4)3]3– (ii) [PtCl2(en)2]2+ Solution: (i) (ii)
How many geometrical isomers are possible in the following coordination entities? (i) [Cr(C2O4)3]3– (ii) [Co(NH3)3Cl3]
( i ) In [ Cr(C2O4)3] 3− no geometric isomers are present because it is a bidentate ligand. ( ii ) In [ Co( NH3)3 Cl3 ]two isomers are possible.
List various types of isomerism possible for coordination compounds, giving an example of each.
The various types of isomerism that can be observed in coordination compounds are 🙁 i ) Geometrical isomerism : ( ii ) Optical isomerism : (iii) Coordination isomerism :This kind of isomerism...
Using IUPAC norms write the systematic names of the following: (i) [Ni(NH3)6]Cl2 (ii) [Co(en)3]3+ (iii) [Ni(CO)4]
( i ) Hexaamminenickel(II) chloride ( ii ) Tris(ethane-1, 2-diammine) cobalt(III) ion ( iii ) Tetracarbonylnickel(0)
Using IUPAC norms write the systematic names of the following: (i) [Mn(H2O)6]2+ (ii) [NiCl4]2–
(i ) Hexaquamanganese(II) ion ( ii) Tetrachloridonickelate(II) ion
. Using IUPAC norms write the systematic names of the following: (i) [Ti(H2O)6]3+ (ii) [Co(NH3)4Cl(NO2)]Cl
(i ) Hexaquatitanium(III) ion ( ii ) Tetraamminichloridonitrito-N-Cobalt(III) chloride
Using IUPAC norms write the systematic names of the following: (i) [Co(NH3)6]Cl3 (ii) [Pt(NH3)2Cl(NH2CH3)]Cl
( i ) Hexaamminecobalt(III) chloride ( ii ) Diamminechlorido(methylamine) platinum(II) chloride
Using IUPAC norms write the formulas for the following: (i) Tetrabromidocuprate(II) (ii) Pentaamminenitrito-N-cobalt(III)
( i ) [ Cu (Br)4] 2− ( ii ) [Co ( ONO )( NH3)5] 2+
Using IUPAC norms write the formulas for the following: (i) Potassium tri(oxalato)chromate(III) (ii) Hexaammineplatinum(IV)
(i ) K3 [ Cr ( C2O4)3] ( ii ) [ Pt (NH3)6] 4+
Using IUPAC norms write the formulas for the following: (i) Pentaamminenitrito-O-cobalt(III) (ii) Hexaamminecobalt(III) sulphate
(i ) [ Co (NO2) ( NH3)5] 2+ ( ii) [ Co( NH3)6]2 (SO4)3
Using IUPAC norms write the formulas for the following: (i) Diamminedichloridoplatinum(II) (ii) Potassium tetracyanidonickelate(II)
( i ) [ Pt ( NH3)2Cl2] ( ii) K2[ Ni(CN )4]
Using IUPAC norms write the formulas for the following: (i) Tetrahydroxidozincate(II) (ii) Potassium tetrachloridopalladate(II)
( i ) [Zn(OH)4]2 – ( ii ) K2[ Pd Cl4]
Specify the oxidation numbers of the metals in the following coordination entities:
Solution: (i) (ii) (iii)
Specify the oxidation numbers of the metals in the following coordination entities:
(i) $\left[\mathrm{Co}\left(\mathrm{H}{2} \mathrm{O}\right)(\mathrm{CN})(\mathrm{en}){2}{ }^{R+}\right.$
(ii) $\left[\mathrm{CoBr}{2}(\mathrm{en}){2}{ }^{+}\right.$
What is meant by unidentate, bidentate, and ambidentate ligands? Give two examples for each.
(a) Unidentate ligands: these are ligands with one donor site. Example Cl–, NH3 (b) Bidentate – these are ligands with two donor sites.Example – Ethane-1,2-diamine, Oxalate ion ( C2O42- ) (c)...
Explain with two examples each of the following: coordination entity, ligand, coordination number, coordination polyhedron, homoleptic and heteroleptic.
(a) Ligands are neutral chemicals or negative ions that are bonded to a metal atom in a coordination entity. Cl-, –OH as an exampleThey are electrically charged radicals or species. ( b )...
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.
When FeSO4is combined with (NH4)2SO4 in a 1: 1 molar ratio, a double salt is formed. FeSO4 (NH4)2SO4 .6H2O. This salt is in charge of supplying Fe 2+ . CuSO 4 in a 1:4 ratio with aqueous ammonia...
Explain the bonding in coordination compounds in terms of Werner’s postulates.
( a ) There are two types of valencies in metals: primary and secondary valencies. Primary valencies are satisfied by negative ions, and secondary valencies are filled by both neutral and negative...