Concept explainers
(a)
Interpretation:
The type of ligands which are pi-acids in general has to be given.
Concept Introduction:
Pi-acid or Pi- acceptor:
Ligands having empty orbitals, which can interact with metal d-orbitals for the formation of
(b)
Interpretation:
The type of ligands which are pi-base in general has to be given.
Concept Introduction:
Pi-base or Pi-donor:
In coordination chemistry, a pi-donor ligand is a kind of ligand that is capable with filled non-bonding orbital that overlap with metal-base orbitals. If the ligand molecule has pi electrons in d-orbitals they are referred as pi-donor.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
Chemical Principles: The Quest for Insight
- Platinum(II) forms many complexes, among them those with the following ligands. Give the formula and charge of each complex. (a) two ammonia molecules and one oxalate ion (C2O42-) (b) two ammonia molecules, one thiocyanate ion (SCN-), and one bromide ion (c) one ethylenediamine molecule and two nitrite ionsarrow_forwardFour different octahedral chromium coordination compounds exist that all have the same oxidation state for chromium and have H2O and Cl as the ligands and counterions. When 1 mole of each of the four compounds is dissolved in water, how many moles of silver chloride will precipitate upon addition of excess AgNO3?arrow_forwardGive the number of unpaired electrons in octahedral complexes with strong-field ligands for (a) Rh3+ (b) Mn3+ (c) Ag+ (d) Pt4+ (e) Au3+arrow_forward
- Would you expect salts of the gold(I) ion, Au+, to be colored? Explain.arrow_forwardThe molecule dimethylphosphinoethane [(CH3)2PCH2CH2P(CH3)2, which is abbreviated dmpe] is used as a ligandfor some complexes that serve as catalysts. A complex thatcontains this ligand is Mo(CO)4(dmpe). (a) Draw the Lewisstructure for dmpe, and compare it with ethylenediamine asa coordinating ligand. (b) What is the oxidation state of Moin Na2[Mo(CN)2(CO)2(dmpe)]? (c) Sketch the structure ofthe [Mo(CN)2(CO)2(dmpe)]2- ion, including all the possibleisomers.arrow_forward(a) A complex containing three pyridine and three ammonia ligands bound to a Ni(II) ion was found to have C3v symmetry. Draw and name the complex. (b) Describe the advantages of molecular orbital theory over Lewis models to describe diatomic species. (c) [Ni(II)Br4]2- is a tetrahedral complex while [Ni(II)(CN)4]2− is square-planar. Explain the reasons for the different coordination geometries in these two species.arrow_forward
- Draw the geometrical isomers of complex [Pt(en)2Cl2]2+. (ii) On the basis of crystal field theory, write the electronic configuration for d4 ion, if Δ0> P. (iii) Write the hybridization type and magnetic behaviour of the complexarrow_forward(a) Calculate the number of unpaired electrons in the following gaseous state ions: Mn2+, Cr3+, V3+ and Fe2+ which one of these in the most stable in aqueous solutions? (At. nos. V = 23, Cr = 24, Mn = 25, Fe = 26) (b) Explain the following observations: (i) The transition metal ions are usually coloured in aqueous solutions. (ii) Cu(I) is not stable in an aqueous solution. (iii) The highest oxidation state of a transition metal is exhibited in its oxide or fluoride.arrow_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
- For the complex [Fe(en)2Cl2]Cl, identify the following: (i) Oxidation number of iron. (ii) Hybrid orbitals and shape of the complex. (iii) Magnetic behaviour of the complex. (iv) Number of its geometrical isomers. (v) Whether there may be optical isomer also. (vi) Name of the complex.arrow_forwardgive an example of tetradentate ligand.arrow_forwardConsider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 . (a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all work. (b) How many valence d electrons does the metal center have? Justify your answer. (c) How many unpaired electrons per molecule would a magnetic susceptibility experiment predict? What would the S number be for this transition metal center? Justify your answers. (d) What electronic transition results from absorption of 864-nm light? (e) Calculate the ligand stabilization energy (in units of ∆o) and units of coulombic (Πc) energy. (f) How would the ligand field strengths (∆o) of [Fe(NH3)6] 2+ and [Fe(bipy)3] 2+ differ from that of [FeBr6] 4−? Why?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning