Concept explainers
a)
Interpretation: The systematic names for the given compounds to be predicted.
Concept Introduction:
The cation is named before the anion.
Within a complex ion, the Ligands are arranged in an alphabetical order followed by the metal ion name. The anionic Ligand should ends with a letter –o, the neutral Ligand are called by the molecules (some common name for some exception).
When more Ligands are present, Greek prefixes like di, tri, tetra, penta, and hexa to specify their number.
The oxidation number of the metal is represented in roman numerals immediately following the metal ion name.
If the complex ion is an anion, the metal name should end with –ate.
To Identify: The systematic names for the given compounds to be predicted.
b)
Interpretation: The systematic names for the given compounds to be predicted.
Concept Introduction:
The cation is named before the anion.
Within a complex ion, the Ligands are arranged in an alphabetical order followed by the metal ion name. The anionic Ligand should ends with a letter –o, the neutral Ligand are called by the molecules (some common name for some exception).
When more Ligands are present, Greek prefixes like di, tri, tetra, penta, and hexa to specify their number.
The oxidation number of the metal is represented in roman numerals immediately following the metal ion name.
If the complex ion is an anion, the metal name should end with –ate.
To Identify: The systematic names for the given compounds to be predicted.
c)
Interpretation: The systematic names for the given compounds to be predicted.
Concept Introduction:
The cation is named before the anion.
Within a complex ion, the Ligands are arranged in an alphabetical order followed by the metal ion name. The anionic Ligand should ends with a letter –o, the neutral Ligand are called by the molecules (some common name for some exception).
When more Ligands are present, Greek prefixes like di, tri, tetra, penta, and hexa to specify their number.
The oxidation number of the metal is represented in roman numerals immediately following the metal ion name.
If the complex ion is an anion, the metal name should end with –ate.
To Identify: The systematic names for the given compounds to be predicted.
d)
Interpretation: The systematic names for the given compounds to be predicted.
Concept Introduction:
The cation is named before the anion.
Within a complex ion, the Ligands are arranged in an alphabetical order followed by the metal ion name. The anionic Ligand should ends with a letter –o, the neutral Ligand are called by the molecules (some common name for some exception).
When more Ligands are present, Greek prefixes like di, tri, tetra, penta, and hexa to specify their number.
The oxidation number of the metal is represented in roman numerals immediately following the metal ion name.
If the complex ion is an anion, the metal name should end with –ate.
To Identify: The systematic names for the given compounds to be predicted.
Want to see the full answer?
Check out a sample textbook solutionChapter 23 Solutions
Chemistry
- An aqueous solution of [Rh(C2O4)3]3− is yellow. Predict the approximate wavelength and predominant color of light absorbed by the complex.arrow_forwardBriefly speculate on why many cobalt (III) compounds are prepared by oxidizing CO(II) salts rather than by substitituting ligands in cobalt (III) complexes.arrow_forwardWhy are K3[Cr(C2O4)3]*3H2O and K3[Fe(C2O4)3]*3H2O colored, whereas K3[Al(C2O4)3]*3H2O is colorless?arrow_forward
- Mention the types of structural isomerism present in metal complexes and indicate to which of them the following compound pair belongs: [Co(NH3)6][Cr(CN)6] and [Cr(NH3)6][Co(CN)6].arrow_forwardLet us consider the following coordination complexes: [Fe(CN6)]3- Given that the chloride ion and the water molecule are weak field ligands whereas ammonia, CN- and CO are high field ligands, determine the electron structure of the cobalt complex ion using an energy diagram of the d orbitals established according to the crystal field theory.arrow_forwardAqueous solutions of [Mn(H2O)6]2+ are faint pink, so much so that they appear to be colorless, which is in contrast to other coordination complexes that we have seen to this point in the course. a) Please explain why this solution is colorless. b) If the water ligands were changed to bipyridine (bpy) ligands and you had [Mn(bpy)3]2+, would the solution still be colorless? What changes, if any, would you expect to see in the visible spectrum? If the complex would be expected to have absorptions, please note now many.arrow_forward
- How many geometric isomers does the octahedral coordination compound[Co(NH3)3Cl3] have?arrow_forwardIn [Cr(NH₃)₆]Cl₃, the [Cr(NH₃)₆]³⁺ ion absorbs visiblelight in the blue-violet range, and the compound is yellow-orange. In [Cr(H₂O)₆]Br₃, the [Cr(H₂O)₆]³⁺ ion absorbs visiblelight in the red range, and the compound is blue-gray. Explain these differences in light absorbed and color of the compoundarrow_forwardon the basis of crystal field theory explain why Co(III) forms paramagnetic octahedral complex with weak field ligands whereas it forms diamagnetic octahedral complex with strong field ligands.arrow_forward
- When cobalt(II) chloride is treated, under certain condition, with the bidentate ligand, NH2CH2CH2NH2, (which can be represented by the symbol “en”), the compound [CoC12(en)2]Cl is formed. a. What is the coordination number of cobalt in this compound? b. When this compound is treated with aqueous silver nitrate, only one mole of silver chloride is produced per mole of compound. Explain this observation.arrow_forwardWhen cobalt(II) chloride is treated, under certain condition, with the bidentate ligand, NH2CH2CH2NH2, (which can be represented by the symbol “en”), the compound [CoC12(en)2]Cl is formed. a. What is the coordination number of cobalt in this compound?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
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning