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Ligands are broadly classified into two ...

Ligands are broadly classified into two classes classical and non-classical ligands, depending on their donor annd acceptor ability. Classical ligands form classical complexes while non-classical ligands form non-classical complex. Bonding mechanism in non-classical is called synergic bonding.
Q. In compound `[M(CO)_(n)]^(z)`, the correct match for highest 'M-C' bond length for given M, n and z respectively:

A

Shortening of M – CO bond

B

Lengthening of M – CO bond

C

No effect

D

None of these

Text Solution

Verified by Experts

The correct Answer is:
A
Due to synergic bonding between carbon and metal, M–CO bond length shortens.
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Ligands are broadly classified into two classes classical and non-classical ligands, depending on their donor annd acceptor ability. Classical ligands form classical complexes while non-classical ligands form non-classical complex. Bonding mechanism in non-classical is called synergic bonding. Q. Synergic bonding is absent in:

Ligands are broadly classified into two classes classical and non-classical ligands, depending on their donor annd acceptor ability. Classical ligands form classical complexes while non-classical ligands form non-classical complex. Bonding mechanism in non-classical is called synergic bonding. Q. Which is not pi -acceptor ligand?

Ligands are broadly classified into two classes classical and non-classical ligands, depending on their donor annd acceptor ability. Classical ligands form classical complexes while non-classical ligands form non-classical complex. Bonding mechanism in non-classical is called synergic bonding. Q. Which is not pi -acceptor ligand?

Give the number of ligand(s) which is/are non-classical ligand an pi donor as well as pi acceptor ligand CO,PH_(3), PF_(3),C_(3)H_(5)^(Θ) ,C_(5)H_(5) Θ .

Consider the two complexation equilibria in aqueous solution, between the cobalt (II) ion Co^(2+) (aq) and ethylenediamine (en) on the one hand and ammonia NH_(3) on the other. [Co(H_(2)O)_(6)]^(2+)+6NH_(3)hArr[Co(NH_(3))_(6)]^(2+)+6H_(2)O ...(1) [Co(H_(2)O_(6))]^(2+)+3enhArr[Co(en)_(3)]^(2+)+6H_(2)O ..(2) Electronicaly, the ammonia and en ligands are very similar, since both bond through N and since the liwis base strengths of their nitrogen atoms are similar. This means that DeltaH^(@) must be very similar for the two reactions, since six Co-N bonds are formed in each case. Interestingly however, the equilibrium constant is 100,000 times larger for the second reaction than it is for the first. This is the so called chelate effect: "the enhanced affinity of chelating ligands for a metal ion compared to similar non-chelating (monodentate) ligands for the same metal". The chelate effect is entropy-driven. Q. What may be main reason for reaction (2) having relatively such a large equilibrium constant?

Give the number of ligand(s) which is//are non-classical ligand CO, NO, C_(2)H-(4),C_(3)H_(5) Θ , H^(Θ) .

Give number of non-classical ligands which are negative ligands CN^(Θ), S_(2)O_(3)^(2-),C_(3)H_(5)^(Θ),C_(5)H_(5)^(Θ) .

Velence bond theroy describes the bonding in complexs in terms of coordinate -covalent bond resulting from overlap filled ligand orbitals with vacant metal hybrid orbitals This theory explains magnetic behaviour and geometrical shape of coordination compounds Magnetic moment of a complex compound can be determined experimentally and theoretically by using spin only formula Magnetic moment sqrtn (n+2)BM (where n = No. unpaired electrons) . Ni^(2+) cation combines with a uninegative monodentate ligand X^(Θ) to form paramagnetic complex [NiCI_(4)]^(2-) The number of unpaired electrons(s) in central metal cation and geometry of this complex respectively are (a) One,tetrahedral (b) Two,tetrahedral (c ) One,square planar (d) Two, square planar .

Consider the two complexation equilibria in aqueous solution, between the cobalt (II) ion Co^(2+) (aq) and ethylenediamine (en) on the one hand and ammonia NH_(3) on the other. [Co(H_(2)O)_(6)]^(2+)+6NH_(3)hArr[Co(NH_(3))_(6)]^(2+)+6H_(2)O ...(1) [Co(H_(2)O_(6))]^(2+)+3enhArr[Co(en)_(3)]^(2+)+6H_(2)O ..(2) Electronicaly, the ammonia and en ligands are very similar, since both bond through N and since the liwis base strengths of their nitrogen atoms are similar. This means that DeltaH^(@) must be very similar for the two reactions, since six Co-N bonds are formed in each case. Interestingly however, the equilibrium constant is 100,000 times larger for the second reaction than it is for the first. This is the so called chelate effect: "the enhanced affinity of chelating ligands for a metal ion compared to similar non-chelating (monodentate) ligands for the same metal". The chelate effect is entropy-driven. Q. Which of the following can be classified as a chelating ligand?

Two important physical evidences supporting the synergic bonding in non-classical complexes are bond lengths and vibrational spectra. Vibrational spectra is based on the fact that the compression and extension of a bond may be analogous to the behaviour of a spring and obeys Hook's law. overline(v)=(1)/(2pic)sqrt((k)/(mu))cm^(-1) where, k=force force constant of the bond which is directly proportional to bonnd strength of CO mu= reduced mass of ligand overline(v) =stretching frequency of the CO bond c=velocity of light Q. In which of the following ligand, sigma -bond order does not change during synergic bonding in their respective complexes:

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