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Chapter 23: Q23.86P (page 1060)

What is the distinction between a weak-field ligand and a strong-field ligand? Give an example of each.

Short Answer

Expert verified

Strong-field ligands give larger splitting energy ∆and weak-field ligands give smaller splitting energy ∆. Example for strong-field ligand: CO Example for weak-field ligand:Cl-

Step by step solution

01

Definition of ligand

A ligand is an ion or molecule (functional group) that binds to a central metal atom to form a coordination complex.

02

Explanation

The main distinction between weak-field ligands and strong-field ligands is that the strong-field ligands give larger splitting energy∆ because they cause large splitting of d orbitals and the weak-field ligands give smaller splitting energy∆ because they don't cause large splitting of d orbitals.

Example for strong-field ligand: CO Example for weak-field ligand: Cl-

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Most popular questions from this chapter

Chromium(III), like cobalt(III), has a coordination number of 6 in many of its complex ions. Compounds are known that have the traditional formula CrCl3_nNH3, where n= 3 to 6. Which of the compounds has an electrical conductivity in an aqueous solution similar to that of an equimolar NaCl solution?

Question: Correct each name that has an error:

(a) Na[FeBr4]sodium tetrabromoferrate(II)

(b) [NiNH36]2-nickel hexaammine ion

(c) [CoNH33I3]triamminetriiodocobalt(III)

(d) [VCN6]3-hexacyanovanadium(III) ion

(e) K[FeCl4]potassium tetrachloroiron(III)

The metal ion in platinum(IV) complexes, like that in cobalt(III) complexes, has a coordination number of 6 and often has Cl-ions and NH3molecules as ligands. For the traditional (before the work of Werner) formulasPtCl4·6NH3and localid="1663359663004" PtCl4·4NH3,(a) give the modern formula and charge of the complex ion, and(b) predict the moles of ions per mole of compound dissolved and moles of AgCl formed with excess AgNO3.

Solutions of KMnO4are used in redox titrations because dark purple MnO4-oxidizing agent changes to the faint pink Mn2+as it is reduced. The end point occurs when a slight purple remains as more KMnO4is added. If a sample that has reached this end point stands for a long time, the purple fades and a suspension of a small amount of brown, muddy MnO2appears. Use standard electrode potentials to explain this result.

Which of these ligands can participate in linkage isomerism?

(a) SCN-

(b)S2O32-(thiosulfate)

(c) HS-

Explain with Lewis structures.
See all solutions

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