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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. Which is not `pi`-acceptor ligand?

A

B

`sigma-C_(5)H_(5)^(-)`

C

`PH_(3)`

D

B_(3)N_(3)H_(6)`

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To determine which ligand is not a π-acceptor ligand, we need to analyze the characteristics of the given ligands based on their ability to accept π-electrons. ### Step-by-Step Solution: 1. **Understanding Ligands**: - Ligands can be classified into classical and non-classical based on their donor and acceptor abilities. - Classical ligands typically donate lone pairs of electrons to the metal center, while non-classical ligands can accept electrons from the metal center. 2. **Definition of π-Acceptor Ligands**: - π-acceptor ligands have empty π* (pi star) orbitals that can accept electron density from the filled d-orbitals of the metal ion, forming π-backbonding. 3. **Analyzing the Ligands**: - **C5H5- (Cyclopentadienyl anion)**: This ligand can accept electrons due to its conjugated system, making it a π-acceptor. - **PH3 (Phosphine)**: Phosphine has a lone pair on phosphorus but does not have empty π* orbitals to accept electrons, making it not a π-acceptor. - **B3N3H6 (Inorganic Benzene)**: This compound has a structure similar to benzene and can participate in π-backbonding due to its conjugated double bonds. - **CH2=CH2 (Ethylene)**: Ethylene can also act as a π-acceptor due to its double bond, which allows for π-backbonding. 4. **Conclusion**: - Among the ligands analyzed, **PH3 (Phosphine)** is the one that does not act as a π-acceptor ligand because it lacks the necessary empty π* orbitals for π-backbonding. ### Final Answer: **PH3 (Phosphine) is not a π-acceptor ligand.**
To determine which ligand is not a π-acceptor ligand, we need to analyze the characteristics of the given ligands based on their ability to accept π-electrons. ### Step-by-Step Solution: 1. **Understanding Ligands**: - Ligands can be classified into classical and non-classical based on their donor and acceptor abilities. - Classical ligands typically donate lone pairs of electrons to the metal center, while non-classical ligands can accept electrons from the metal center. ...
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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:

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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. In compound [M(CO)_(n)]^(z) , the correct match for highest 'M-C' bond length for given M, n and z respectively:

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Assertion Chelates are relatively more stable than non-cheltated complexes Reason Complexes containing ligands which can be easily replaced by other ligands are called labile complexes .

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When degenerate d-orbitals of an isolated atom/ion come under influence of magnetic field of ligands, the degeneray is lost. The two set t_(2g)(d_(xy),d_(yz),d_(xz)) and e_(g) (d_(x^(2))-d_(x^(2)-y^(2)) are either stabilized or destabilized depending upon the nature of magnetic field. it can be expressed diagrammatically as: Value of CFSE depends upon nature of ligand and a spectrochemical series has been made experimentally, for tetrahedral complexes, Delta is about 4/9 times to Delta_(0) (CFSE for octahedral complex). this energy lies in visible region and i.e., why electronic transition are responsible for colour. such transition are not possible with d^(0) and d^(10) configuration. Q. Which of the following is correct arrangement of ligand in terms of the Dq values of their complexes with any particularr 'hard' metal ion:

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?

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