Chapter 22: Problem 15
What are the systematic names for the following ions and compounds? (a) \(\left[\mathrm{cis}-\mathrm{Co}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]^{+}\) (b) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{3}\) (c) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2}\)
Short Answer
Step by step solution
Analyze the Complex Ion (a)
Name the Ligands in (a)
Determine Oxidation State for (a)
Assign the Systematic Name for (a)
Analyze the Complex Compound (b)
Name the Ligands in (b)
Determine Oxidation State for (b)
Assign the Systematic Name for (b)
Analyze the Complex Compound (c)
Name the Ligands in (c)
Determine Oxidation State for (c)
Assign the Systematic Name for (c)
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Coordination Chemistry
- Coordination Sphere: This is where the metal ion and the directly attached ligands reside. The coordination sphere is usually enclosed in square brackets.
- Central Metal: In coordination compounds, the central metal atom or ion serves as the "anchor." It is most often a transition metal like cobalt (Co) or platinum (Pt).
- Complex Ion: When the coordination sphere carries a charge, it becomes a complex ion, which could be either positively or negatively charged depending on the balance of charges between the metal center and the ligands.
Ligands and Complex Ions
Types of Ligands
- Monodentate Ligands: These attach to the metal atom at a single point. Common examples include chloride (Cl) and ammonia (NH3).
- Bidentate Ligands: These form two bonds with the central metal ion. An example is ethylenediamine (en), often mentioned in contexts like cis-bis(ethylenediamine)dichlorocobalt(III) ion.
Complex Ions
When ligands bind with a central metal ion, they form a complex ion. The charge on the complex ion depends on the sum of the charges of the metal and the ligands. For example, both the complex ions \( [\text{Co} (\text{NH}_3)_5\text{Cl}]^{2+} \) and \( [\text{Pt} (\text{NH}_3)_5 \text{Cl}]^{3+} \) are formed by different combinations of neutral and charged ligands.Oxidation States
Determining Oxidation States
- Identify all ligands and their charges, if any.
- Identify the overall charge of the complex ion, if given.
- Set up an equation that sums the charges of the metal and ligands to equal the charge of the complex. Solve for the oxidation state of the metal.