Coordination Compounds
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CuSO4.5H2O is blue in colour while CuSO4 is colourless. Why?
CuSO4.5H2O is blue in colour while CuSO4 is colourless. Why?
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Ans: In CuSO4⋅5H2O, water acts as ligand and causes crystal field splitting. This makes d - d transitions possible. On the other hand, in CuSO4, splitting is not possible due to the lack of ligand in the crystal field. As a r
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Why do compounds having similar geometry have different magnetic moments?
Why do compounds having similar geometry have different magnetic moments?
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Ans: Due to the presence of weak and strong field ligands in complexes, compounds with comparable geometry have distinct magnetic moments. The magnetic moment decreases when the CFSE increases, and vice versa.
Example: [Fe (CN
Upvote Arrange following complex ions in increasing order of crystal field splitting energy (Δ0)
[Cr(Cl)6]3- ,[Cr(CN)6]3- ,[Cr(NH3)6]3+
Arrange following complex ions in increasing order of crystal field splitting energy (Δ0)
[Cr(Cl)6]3- ,[Cr(CN)6]3- ,[Cr(NH3)6]3+
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Ans: CFSE is higher when the complex contains strong field ligand. Thus, crystal field splitting energy increases in the order
[Cr (Cl)6]3−< [Cr (NH3)6]3+< [Cr (CN)6]3−.
Because according to spectrochemical series the order of field strength is
C
Upvote Explain why [Fe(H2O)6]3+ has magnetic moment value of 5.92 BM whereas [Fe(CN)6]3- has a value of only 1.74 BM.
Explain why [Fe(H2O)6]3+ has magnetic moment value of 5.92 BM whereas [Fe(CN)6]3- has a value of only 1.74 BM.
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Ans: CN- is a strong ligand and [Fe (CN)6]3- has one paired electron
H2O is a weak ligand and [Fe (H2O)6]3+ has five paired electrons.
Upvote 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+
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+
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Ans: The ligands can be grouped in ascending order of increasing field intensity according to spectrochemical series.
[CoF6]3−, Co3+ → (d6)→ t42g e0g
[FE (CN)6]4−, Fe2+→ (d6)→ t62g e2g
[Cu (NH3)6]2+, Cu2+→ (d9)→ t6
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Ans: In a tetrahedral complex, the d-orbit splits too little compared to an octahedral complex. As a result, orbital energy alone are insufficient to couple. Low spin tetrahedral complexes do not form as a result.
Upvote Based on crystal field theory explain why Co(III) forms a paramagnetic octahedral complex with weak field ligands whereas it forms a diamagnetic octahedral complex with strong field ligands.
Based on crystal field theory explain why Co(III) forms a paramagnetic octahedral complex with weak field ligands whereas it forms a diamagnetic octahedral complex with strong field ligands.
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Ans: Weak field ligands, Electronic configuration of Co (III) is t42g e0g, has 4 paired electrons and it is paramagnetic.
Strong field ligands, Electronic configuration of is Co (III) t62ge0g.
Upvote Magnetic moment of [MnCl4]2- is 5.92 BM. Explain giving reason.
Magnetic moment of [MnCl4]2- is 5.92 BM. Explain giving reason.
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Ans: The existence of five unpaired electrons in the ion's mid-orbits Mn2+ equates to a magnetic moment of 5.92 BM. The number of hybridizations in this case is sp3. As a result, the magnetic moment value of the tetrahe
Upvote A complex of the type [M(AA)2X2]n + is known to be optically active. What does this indicate about the structure of the complex? Give one example of such a complex.
A complex of the type [M(AA)2X2]n + is known to be optically active. What does this indicate about the structure of the complex? Give one example of such a complex.
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Ans: [M (AA)2X2]n + is a bidentate ligand and %X is a monodentate ligand. It is an example of octahedral geometry as well as an ion. There are cis and trans isomers of this ion. Trans isomers are symmetrically active, w
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