Concept explainers
- a)
Interpretation: The oxidation number of the metal ion for the given coordination compound to be predicted.
Concept Introduction:
Lewis acid: The species which accepts the lone pair of electrons.
Lewis base: The species which donates lone pair of electrons.
Donor atom: The neutral molecule or the negatively charged species which donates pair of electrons is known as Donor atom.
Coordinate covalent bonds: A covalent bond in which the Ligand donates both electrons to the metal ion to construct a bonding interaction known as coordinate covalent bond.
To Identify: The oxidation number of the metal ion for the given coordination compound to be predicted.
- b)
Interpretation: The oxidation number of the metal ion for the given coordination compound to be predicted.
Concept Introduction:
Lewis acid: The species which accepts the lone pair of electrons.
Lewis base: The species which donates lone pair of electrons.
Donor atom: The neutral molecule or the negatively charged species which donates pair of electrons is known as Donor atom.
Coordinate covalent bonds: A covalent bond in which the Ligand donates both electrons to the metal ion to construct a bonding interaction known as coordinate covalent bond.
To Identify: The oxidation number of the metal ion for the given coordination compound to be predicted.
- c)
Interpretation: The oxidation number of the metal ion for the given coordination compound to be predicted.
Concept Introduction:
Lewis acid: The species which accepts the lone pair of electrons.
Lewis base: The species which donates lone pair of electrons.
Donor atom: The neutral molecule or the negatively charged species which donates pair of electrons is known as Donor atom.
Coordinate covalent bonds: A covalent bond in which the Ligand donates both electrons to the metal ion to construct a bonding interaction known as coordinate covalent bond.
To Identify: The oxidation number of the metal ion for the given coordination compound to be predicted.
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Chapter 23 Solutions
Chemistry
- 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_forwardIron(II) forms a complex in hemoglobin. Two of the possibilities are [Fe(H2O)6]2+ and [Fe(CN)6]4– (a) [Fe(H2O)6]2+ and [Fe(CN)6]4– should have the same geometry. What is this coordination environment? Draw it please. (b) For both [Fe(H2O)6]2+ and [Fe(CN)6]4–, draw an energy diagram showing orbital splitting (c) Predict the number of unpaired electrons(d) Identify the ion as low spin or high spin.(e) Is either ion paramagnetic?(f) What would the color of each form of these forms ofhemoglobin?arrow_forward
- Name the compounds (a) [Cr(H2O)4Cl2]Cl, (b) K4[Ni(CN)4].arrow_forwardFor any of the following that can exist as isomers, state thetype of isomerism and draw the structures: (a) [Co(NH3)5Cl]Br2 (b) [Pt(CH3NH2)3Cl]Br (c) [Fe(H2O)4(NH3)2]2+arrow_forwardExplain why at equal concentrations [Fe(CN)6]³ is deep red while [Fe(CN)6] is pale yellow.arrow_forward
- Does Fe(OH2)4 (CN)2 have any optically active isomers?arrow_forwardA chemist prepared aqueous solutions of the following complex ions: [Cr(OH)6]³, [Cr(NH3)6]³+, and [Cr(NH3)5Cl]²+. He obtained 3 different colors of solution: green, red-violet, and yellow. Match the colored solutions with the correct complex ion. O [Cr(NH3)6]³+ is red-violet; [Cr(NH3)5Cl]²+ is yellow; [Cr(OH)]³- is green O [Cr(NH3)6]³+ is yellow; [Cr(NH3)5Cl]²+ is red-violet; [Cr(OH)6]³¯ is green O [Cr(NH3)]³+ is yellow; [Cr(NH3) 5Cl]²+ is green; [Cr(OH)6]³ is red-violet [Cr(NH3)6]³+ is green; [Cr(NH3)5Cl]²+ is red-violet; [Cr(OH)]³ is yellowarrow_forwardGive systematic names for the following formulas:(a) K[Ag(CN)2] (b) Na2[CdCl4] (c) [Co(NH3)4(H2O)Br]Br2arrow_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: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning