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Ch.21 - Transition Elements and Coordination Chemistry
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook
All textbooksMcMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.79b
Chapter 21, Problem 21.79b

Assign a systematic name to each of the following ions.
(c) [Fe(H2O)5NCS]2+
(d) [Cr(NH3)2(C2O4)2]-

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1
Identify the central metal ion in each complex and determine its oxidation state.
For complex (c), [Fe(H_2O)_5NCS]^2+, identify the ligands: water (H_2O) and thiocyanate (NCS). Water is a neutral ligand, and thiocyanate is a monodentate ligand with a charge of -1.
Determine the oxidation state of iron (Fe) in complex (c) by considering the overall charge of the complex (+2) and the charges of the ligands.
For complex (d), [Cr(NH_3)_2(C_2O_4)_2]^-, identify the ligands: ammonia (NH_3) and oxalate (C_2O_4). Ammonia is a neutral ligand, and oxalate is a bidentate ligand with a charge of -2.
Determine the oxidation state of chromium (Cr) in complex (d) by considering the overall charge of the complex (-1) and the charges of the ligands.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Coordination Compounds

Coordination compounds consist of a central metal atom or ion bonded to surrounding molecules or ions, known as ligands. The nature of these ligands, whether they are neutral or charged, and their arrangement around the metal center significantly influence the compound's properties and nomenclature.

Ligand Naming and Classification

Ligands are classified based on the number of donor atoms they possess. Monodentate ligands bind through a single atom, while bidentate and polydentate ligands can attach through multiple atoms. The systematic naming of ligands follows specific rules, such as using prefixes like 'di-', 'tri-', and 'tetra-' to indicate the number of identical ligands present.
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Ligand Classification

Oxidation States and Charge

The oxidation state of a metal in a coordination compound is crucial for determining its systematic name. It reflects the charge of the metal ion after accounting for the charges contributed by the ligands. Understanding how to calculate the overall charge of the complex is essential for correctly naming the compound and ensuring that the name reflects its chemical identity.
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Related Practice
Textbook Question

What is the systematic name for each of the following coordination compounds? 

(a) Cs[FeCl4]

(b) [V(H2O)6](NO3)3

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Textbook Question

What is the systematic name for each of the following ions? 

(c) [Co(CO3)3]3-

(d) [Pt(en)2(SCN)2]2+

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Textbook Question

Predict the number of unpaired electrons for each of the following.

(c) Mn3+

(d) Cr2+

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Textbook Question

Cobalt(III) trifluoroacetylacetonate, Co(tfac)3, is a sixcoordinate, octahedral metal chelate in which three planar, bidentate tfac ligands are attached to a central Co atom:

(b) Diastereoisomers A and B have dipole moments of 6.5 D and 3.8 D, respectively. Which of your diastereoisomers is A and which is B?

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Textbook Question

Tell how many diastereoisomers are possible for each of the following complexes, and draw their structures. 

(c) [Cu(H2O)4Cl2]+

(d) Ru(NH3)3I3

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Textbook Question

Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons. 

(b) [NiBr4]2- (tetrahedral) 

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