Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 21: Problem 35

Name the following coordination compounds. a. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2}\) b. \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{I}_{3}\) c. \(\mathrm{K}_{2}\left[\mathrm{Pt} \mathrm{Cl}_{4}\right]\) d. \(\mathrm{K}_{4}\left[\mathrm{Pt} \mathrm{Cl}_{6}\right]\) e. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2}\) f. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{NO}_{2}\right)_{3}\right]\)

Short Answer

Expert verified
a. hexaamminecobalt(III) chloride b. hexaaquacobalt(III) iodide c. dipotassium tetrachloridoplatinate(II) d. tetrapotassium hexachloridoplatinate(IV) e. pentaamminechloridocobalt(III) chloride f. triamminetrianitritocobalt(III)

Step by step solution

01

Understanding the IUPAC naming system

The IUPAC system for naming coordination compounds uses the following rules: 1. Name the ligands first, in alphabetical order. 2. Name the central metal atom/ion. 3. Use prefixes to indicate the number of ligands. 4. If the complex ion is an anion, the central atom's name ends in '-ate'. 5. If there are multiple complex ions in the compound, enclose each complex ion in square brackets and name them in alphabetical order.
02

Naming the given coordination compounds

a. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2}\) 1. The ligands are six ammonia molecules, named as 'hexaammine'. 2. The central metal atom is Cobalt. 3. The complex ion is a cation. 4. The resulting compound name is: hexaamminecobalt(III) chloride. b. \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]\mathrm{I}_{3}\) 1. The ligands are six water molecules, named as 'hexaaqua'. 2. The central metal atom is Cobalt. 3. The complex ion is a cation. 4. The resulting compound name is: hexaaquacobalt(III) iodide. c. \(\mathrm{K}_{2}\left[\mathrm{Pt} \mathrm{Cl}_{4}\right]\) 1. The ligands are four chloride ions, named as 'tetrachlorido'. 2. The central metal atom is Platinum. 3. The complex ion is an anion. 4. The resulting compound name is: dipotassium tetrachloridoplatinate(II). d. \(\mathrm{K}_{4}\left[\mathrm{Pt} \mathrm{Cl}_{6}\right]\) 1. The ligands are six chloride ions, named as 'hexachlorido'. 2. The central metal atom is Platinum. 3. The complex ion is an anion. 4. The resulting compound name is: tetrapotassium hexachloridoplatinate(IV). e. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2}\) 1. The ligands are five ammonia molecules and one chloride ion, named as 'pentaamminechlorido'. 2. The central metal atom is Cobalt. 3. The complex ion is a cation. 4. The resulting compound name is: pentaamminechloridocobalt(III) chloride. f. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{NO}_{2}\right)_{3}\right]\) 1. The ligands are three ammonia molecules and three nitrite ions, named as 'triamminetrianitrito'. 2. The central metal atom is Cobalt. 3. The complex ion is a cation. 4. The resulting compound name is: triamminetrianitritocobalt(III) (since no counterions are present, we only name the complex ion).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

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

IUPAC Naming System
The International Union of Pure and Applied Chemistry (IUPAC) naming system is a standardized method used globally to ensure clarity and precision in the communication of chemical compound information. When naming coordination compounds, one must follow a specific order and set of rules. Firstly, ligands are named in alphabetical order before the metal ion. Neutral ligands are usually given their molecular name, while anionic ligands end in '-ido'. Numerical prefixes like 'di-', 'tri-' or 'hexa-' indicate the number of each type of ligand.

Next, the central metal is named. If the entire complex is a cation, the metal keeps its elemental name. If it's an anion, the name of the metal ends in '-ate'. Latin names are often used here for metals that have more than one common oxidation state. The oxidation state of the metal is denoted in Roman numerals in parentheses.

Finally, the name of the entire coordination compound is constructed by combining the names of the ligands with that of the central metal, with a space separating the name of the complex ion from any anions or cations outside the brackets.
Ligands Naming
In coordination compounds, ligands are ions or molecules that can donate pairs of electrons to the central metal to form coordinate bonds. The naming of ligands is an integral part of IUPAC nomenclature. Simple ligands, such as halides, have names ending in '-ido' (chloride becomes chlorido, for example). Multidentate ligands, which can bind through multiple atoms, often have names ending in '-en', such as 'ethylenediamine' which becomes 'ethylenediaminetetraacetato' when it loses protons and binds to a metal.

When naming, ligands proceed the metal in both their place in the formula and in the name of the compound, and are listed in alphabetical order based on their names, not the formula symbol (eg. 'ammine' comes before 'chlorido'). Prefixes for numbers of identical ligands include 'mono-', 'di-', 'tri-', 'tetra-', 'penta-', and 'hexa-', modified further for complex names where necessary (eg. 'bis-' for di-, 'tris-' for tri-).
Complex Ions
Complex ions consist of a metal ion at the center with a number of ligands surrounding it, bonded via coordinate covalent bonds. The metal, typically a transition metal with an empty orbital capable of accepting electrons, can thus achieve a stable electronic configuration.

In nomenclature, the complex ion may be either positively charged (a cation) or negatively charged (an anion). Anionic complex ions often have names ending in '-ate', such as 'ferrate' from iron. The charge of the complex ion impacts the overall charge of the coordination compound, determining the need for counter ions, which balance the charge, and their quantity. When multiple ligands coordinate to a single metal ion, this polydentate arrangement can add layers of complexity to naming the ion.
Transition Metals Coordination Chemistry
Transition metals are characterized by their ability to form a wide variety of coordination compounds due to the presence of unfilled d-orbitals. These metals can exhibit multiple oxidation states and often form colorful complexes when they coordinate with different ligands.

The unique properties of transition metals, such as variable oxidation states and the ability to form complexes with many types of ligands, make their coordination chemistry an essential area of study. A particular transition metal can form numerous complexes with distinct geometries (such as octahedral, square planar, and tetrahedral), and each of these can have different stabilities and properties, influencing reactivity and applications in areas ranging from industrial catalysis to medicine. Understanding these aspects is crucial as they directly relate to how a coordination compound functions both in the lab and in industry.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which of the following statement(s) is(are) true? a. The coordination number of a metal ion in an octahedral complex ion is 8 . b. All tetrahedral complex ions are low-spin. c. The formula for triaquatriamminechromium(III) sulfate is \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]_{2}\left(\mathrm{SO}_{4}\right)_{3}\) d. The electron configuration of \(\mathrm{Hf}^{2+}\) is \([\mathrm{Xe}] 4 f^{12} 6 s^{2}\). e. Hemoglobin contains \(\mathrm{Fe}^{3+}\).

Amino acids can act as ligands toward transition metal ions. The simplest amino acid is glycine \(\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}\right) .\) Draw a structure of the glycinate anion \(\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CO}_{2}^{-}\right)\) acting as a bidentate ligand. Draw the structural isomers of the square planar complex \(\mathrm{Cu}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CO}_{2}\right)_{2}\)

Qualitatively draw the crystal field splitting of the \(d\) orbitals in a trigonal planar complex ion. (Let the \(z\) axis be perpendicular to the plane of the complex.)

Molybdenum is obtained as a by-product of copper mining or is mined directly (primary deposits are in the Rocky Mountains in Colorado). In both cases it is obtained as \(\mathrm{MoS}_{2}\), which is then converted to \(\mathrm{MoO}_{3}\). The \(\mathrm{MoO}_{3}\) can be used directly in the production of stainless steel for high-speed tools (which accounts for about \(85 \%\) of the molybdenum used). Molybdenum can be purified by dissolving \(\mathrm{MoO}_{3}\) in aqueous ammonia and crystallizing ammonium molybdate. Depending on conditions, either \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Mo}_{2} \mathrm{O}_{7}\) or \(\left(\mathrm{NH}_{4}\right)_{6} \mathrm{Mo}_{7} \mathrm{O}_{24} \cdot 4 \mathrm{H}_{2} \mathrm{O}\) is obtained. a. Give names for \(\mathrm{MoS}_{2}\) and \(\mathrm{MoO}_{3}\). b. What is the oxidation state of Mo in each of the compounds mentioned above?

Give formulas for the following. a. potassium tetrachlorocobaltate(II) b. aquatricarbonylplatinum(II) bromide c. sodium dicyanobis(oxalato)ferrate(III) d. triamminechloroethylenediaminechromium(III) iodide
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free