What are the systematic names for the following ions and compounds? (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+}\) (b) \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\) (c) \(\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{Br}_{2}\right]^{+}\) (d) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\)

Short Answer

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(a) tetraamminedichlorocobalt(III) ion, (b) triamminetrichlorochromium(III), (c) dibromo-bis(ethylenediamine)cobalt(III) ion, (d) hexaamminecobalt(III) chloride

Step by step solution

01

Analyze the structure of the compound

Recognize if the compound is a neutral or charged complex (ion). The ions/atoms written inside the brackets are part of the 'coordination sphere' and the ones outside are counter ions. The cation is named before the anion.
02

Name the ligands

Before naming the central ion, name the ligands first. In alphabetical order, when there's more than one type of ligand. Unidentate ligands such as \(\mathrm{NH}_{3}\) and chloride (\(\mathrm{Cl}^{-}\)) are named as ammine and chloro, respectively. Bidentate ligand such as ethylenediamine (\(\mathrm{en}\)) retains its name.
03

Name the central metal ion

After the ligands, name the central metal. In case of a cation (positive charge), the metal retains its name as is (Cobalt, Chromium, etc.). For an anion, the suffix '-ate' is added to the metal (cobaltate, chromate, etc.). Specification of the oxidation state of the metal ion is done in Roman numerals in parenthesis.
04

Apply the rules to each compound

(a) tetraamminedichlorocobalt(III) ion, (b) triamminetrichlorochromium(III), (c) dibromo-bis(ethylenediamine)cobalt(III) ion, (d) hexaamminecobalt(III) chloride

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Coordination Chemistry
Coordination chemistry is a branch of inorganic chemistry that focuses on the study of compounds featuring central metal atoms or ions surrounded by molecules or ions called ligands. These ligands can donate electrons to the metal, forming what we call coordination complexes or metal complexes.

The central metal typically belongs to the group of transition metals and can exhibit various oxidation states, contributing to the diversity of coordination compounds. Understanding how different ligands attach through coordination bonds to a central atom is crucial not only in chemistry but also in biochemistry, where coordination compounds are involved in many biological processes.
Ligands and Coordination Complexes
Ligands are ions or neutral molecules that bind to the central metal atom or ion in a coordination complex through coordinate covalent bonds. Ligands possess one or more pairs of electrons that can be donated to the metal, which then accepts them in its vacant d-orbitals, forming a coordination bond.

Ligands can be classified based on their denticity –- unidentate ligands, such as ammonia (ammine in coordination chemistry), bond through a single donor atom, while bidentate ligands, like ethylenediamine (en), can attach at two points. The way in which ligands bind and organize themselves around the central metal significantly affects the properties of the resulting coordination compound.
Oxidation State in Coordination Compounds
In coordination compounds, the oxidation state of the metal center is defined as the hypothetical charge it would have if all the ligands were removed along with the electron pairs they shared. To determine the oxidation state, one must consider the charges of all the ligands and the overall charge of the complex.

The oxidation state is essential for the nomenclature of the complex and is indicated by Roman numerals in parentheses following the name of the central metal. For example, in the complex \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\), the cobalt has an oxidation state of III, which is determined after considering the ammine ligands and the chloride counterions.
Nomenclature of Transition Metal Complexes
The nomenclature of transition metal complexes is systematic and follows specific rules. First, the ligands are named in alphabetical order, regardless of their charge. Prefixes like 'di-', 'tri-', and 'tetra-' are used to indicate the number of identical ligands. Unidentate ligands receive a different name than their free form, such as 'ammine' for ammonia.

Bidentate ligands like ethylenediamine keep their common names. The metal is named next, with its oxidation state indicated in parentheses. If the complex ion is negative, the name of the metal ends with the suffix '-ate.' It's important for students to follow these conventions to accurately name any coordination compound they encounter, as demonstrated in the provided exercise.

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Most popular questions from this chapter

Draw structures of all the geometric and optical isomers of each of the following cobalt complexes: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+},(\mathrm{b})\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}\)

A solution made by dissolving \(0.875 \mathrm{~g}\) of \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}\) in \(25.0 \mathrm{~g}\) of water freezes at \(-0.56^{\circ} \mathrm{C}\) Calculate the number of moles of ions produced when 1 mole of \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}\) is dissolved in water and suggest a structure for the complex ion present in this compound.

How many geometric isomers are in the following (b) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right] ?\) species: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]^{-},(\)

Manganese forms three low-spin complex ions with the cyanide ion with the formulas \(\left[\mathrm{Mn}(\mathrm{CN})_{6}\right]^{5-},\) \(\left[\mathrm{Mn (\mathrm{CN})_{6}\right]^{4-},\) and \(\left[\mathrm{Mn}(\mathrm{CN})_{6}\right]^{3-} .\) For each complex ion, determine the oxidation number of Mn and the number of unpaired \(d\) electrons present.

A student has prepared a cobalt complex that has one of the following three structures: \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]\) \(\mathrm{Cl}_{3},\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2},\) or \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl} .\) Explain how the student would distinguish between these possibilities by an electrical conductance experiment. At the student's disposal are three strong electrolytes \(-\mathrm{NaCl}, \mathrm{MgCl}_{2},\) and \(\mathrm{FeCl}_{3}-\) which may be used for comparison purposes.

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