Concept explainers
(a)
Interpretation:
The electronic configuration and the number of unpaired electrons in
Concept Introduction:
Spectrochemical series:
A Spectrochemical series is a list of ligands in the order of ligand strength and a list of metal ion based on oxidation number. In crystal field theory ligands modify the difference in energy between the d orbitals
Series of ligands from weak field to strong field is,
(b)
Interpretation:
The electronic configuration and the number of unpaired electrons in
Concept Introduction:
Refer to part (a).
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ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM
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- What types of isomers are possible for the following compounds or complex ions? (a) K[Co(NH3)2Cl4] (b) Pt(en)Cl2 (square-planar) (c) [Co(NH3)5Cl]2+ (d) [Ru(phen)3]Cl3 (e) Na2[MnCl4] (tetrahedral) (f) [Co(NH3)5NO2)2+arrow_forwardWhich of the following octahedral complexes show geometric isomerism? If geometric isomers are possible, draw their structures. (a) [Co(en)Cl4-] (b) [Ni(C2O4)2ClBr4-] (c) [Cd(NH3)2Cl42-]arrow_forwardCopper(II) ion exists in water as the [Cu(H2O)6]2+ ion. Ammonia forms stronger bonds to copper than does water and hence was able to replace the water molecules in this complex ion to form the tetrammine complex, [Cu(NH3)4]2+. What properties of a ligand make it a “strong” ligand? Use your textbook or an encyclopedia of chemistry to find an example of a ligand that would be “stronger” than ammonia and this would be able to replace ammonia from [Cu(NH3)4]2+ .arrow_forward
- Draw the energy diagram for d-orbital electron configuration in the octahedral field for each of the following complex ions. Indicate whether the ion is paramagnetic or diamagnetic: (a) [Cr(H2O)6]3+ (H2O is a weak-field ligand) (b) [Cr(NH3)6]3+ (NH3 is a strong-field ligand) (c) [CoF6]3– (F– is a weak-field ligand) (d) [Co(CN)6]3– (CN– is a strong-field ligand) (e) [Ni(H2O)6]2+ (H2O is a weak-field ligand) (f) [Ni(en)3]2+ (en is a strong-field ligand)arrow_forwardDraw the octahedral crystal field d orbital splitting diagrams for [Fe(OH2)6] 2+ and [Fe(CN)6] 3. Indicate if the diagrams are high spin and low spin. give the names of the d-orbitals (dxz, dxy, dzy, dz2, dx2 - y2) label the appropriate orbital sets eg* and t2g and show how the electrons populate the diagram. (Hint: Pairing energy for 3d orbitals Fe 2+ = 29875 cm-1, Fe 3+ = 19150 cm-1; delta OH for Fe(OH2)6]2+ = 14300 cm-1 and delta OH for [Fe(CN)6]3 - is 35000 cm-1arrow_forwardThe complex ion [Co(CO3)3]3-, an octahedral complex with bidentate carbonate ions as ligands, has one absorption in the visible region of the spectrum at 640 nm. From this information, (a) Predict the color of this complex and explain your reasoning. (b) Is the carbonate ion a weak- or strong-field ligand? (c) Predict whether [Co(CO3)3]3- will be paramagnetic or diamagnetic.arrow_forward
- Some metal complexes have a coordination number of 5. One such complex is Fe(CO)5, which adopts a trigonal bipyramidal geometry. Suppose one of the CO ligands is replaced with a CN- ligand, forming [Fe(CO)4(CN)]-. How many geometric isomers would you predict this complex could have?arrow_forwardThe crystal structure of [Cu(H2O)6]2+ displays axial bond lengths of 238 pm and equatorial bond lengths of 195 pm. Using a crystal field splitting diagram, explain the reason for the difference in bond lengths in this complex.arrow_forwardThe absorption spectrum of the complex ion [Co(NH3)6]3+ has strongly absorbs blue light at a wavelength of about 440 nm. Calculate the crystal field splitting energy (in kJ/mol) for this ion and predict the color a solution containing this complex ion.arrow_forward
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