/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 28 Give the oxidation state of the ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 26: Problem 28

Give the oxidation state of the metal in (a) \(\left[\left.\operatorname{Ir}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right|^{3+}\right.\) (b) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}(\mathrm{CO})_{3}\right]^{3+}\) (c) \(\left[\mathrm{CuCl}_{4}\right]^{2-}\) (d) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

Short Answer

Expert verified
(a) +3, (b) +3, (c) +2, (d) +2.

Step by step solution

01

Understand the Oxidation State Formula

The oxidation state of the central metal ion can be calculated using the formula:\[\text{Oxidation state of the metal} = \text{Charge of the complex} - \sum (\text{Charges of all ligands})\]To determine the charges of the ligands, we use: H\(_2\)O (neutral), NH\(_3\) (neutral), CO (neutral), Cl\(^-\) (charge -1), CN\(^-\) (charge -1).
02

Calculate Oxidation State for Part (a) \[ \left[\text{Ir}(\text{H}_2\text{O})_6\right]^{3+}\]

Since water (H\(_2\)O) is a neutral ligand, it does not contribute to the charge. Therefore, the oxidation state of Ir is simply the charge of the entire complex:\[\text{Oxidation state of Ir} = +3\]
03

Calculate Oxidation State for Part (b) \[\left[\text{Co}(\text{NH}_3)_3(\text{CO})_3\right]^{3+} \]

Both NH\(_3\) and CO are neutral ligands, so they do not contribute to the complex's charge. Thus, the oxidation state of Co is the charge of the complex:\[\text{Oxidation state of Co} = +3\]
04

Calculate Oxidation State for Part (c) \[ \left[\text{CuCl}_4\right]^{2-} \]

Each chloride ion (Cl\(^-\)) has a charge of -1. Therefore, the total charge from the four chloride ions is:\[4 \times (-1) = -4\]To find the oxidation state of Cu:\[\text{Oxidation state of Cu} = -2 - (-4) = +2\]
05

Calculate Oxidation State for Part (d) \[ \left[\text{Ni}(\text{CN})_4\right]^{2-} \]

Each cyanide ion (CN\(^-\)) has a charge of -1, leading to a total charge from the four cyanides:\[4 \times (-1) = -4\]Thus, the oxidation state of Ni is:\[\text{Oxidation state of Ni} = -2 - (-4) = +2\]

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Transition Metals
Transition metals are elements found in the center of the periodic table. They fill the d-block and are known for having unique properties. Unlike other metals, transition metals can have several oxidation states because they can lose different numbers of electrons. This versatility allows them to form a variety of complex ions and coordination compounds.
  • Transition metals often form colorful compounds due to d-electron interactions.
  • They can act as both reducers and oxidizers in reactions.
  • Transition metals are commonly used in industrial catalytic processes.
Understanding these properties helps in determining the behavior and reactivity of metal ions in chemical structures like complex ions.
Coordination Compounds
Coordination compounds consist of a central metal ion surrounded by molecules or ions called ligands. These ligands are connected through coordinate bonds, which are a type of covalent bond where both electrons come from the ligand. Coordination compounds are important because they form the basis for understanding complex ions in chemistry. They have wide applications, such as in medicine, where they are used in drugs and imaging agents, or in materials science.
  • The number of ligands attached to the central metal ion is called the coordination number.
  • The way ligands are arranged around the central ion can affect the compound's properties.
Knowing how to analyze and interpret the make-up of coordination compounds helps to predict the compound's chemical behavior and uses.
Ligand Charge
The charge of a ligand in a coordination compound is crucial to determining the oxidation state of the central metal ion. Ligands can be neutral or negatively charged. The charge of ligands affects the overall charge balance of the complex ion. For example, NH extsubscript{3} and ext{H} extsubscript{2} ext{O} are neutral, but Cl extsuperscript{-} and CN extsuperscript{-} carry a negative charge.
  • The total charge of the ligands needs to be considered when calculating the oxidation state of the metal ion.
  • A ligand's ability to donate electrons makes it an essential part of the bonding in coordination compounds.
This knowledge is fundamental in understanding how to derive the metal oxidation state within complex ions.
Central Metal Ion
In coordination compounds, the central metal ion is the key player around which ligands arrange themselves. It typically comes from a transition metal, accommodating a range of oxidation states. The central metal ion directs the geometry, properties, and reactivity of the entire compound. Recognizing the role and behavior of the central metal ion is necessary for predicting physical and chemical properties.
  • The type of central metal ion influences the strength and type of bonds it can form with ligands.
  • Its oxidation state is crucial for determining the net charge and stability of the compound.
  • Transition metals with unfilled d-orbitals are versatile in forming various coordination compounds.
Understanding the central metal's role aids in predicting how a coordination compound will act in chemical reactions.
Complex Ions
Complex ions are a form of coordination compounds that have an overall ionic charge. They consist of a central metal ion bonded to ligands. In a complex ion, it鈥檚 common to find the central metal ion at a higher oxidation state due to the balancing charges of the ligands. The charge of a complex ion is utilized in calculating the oxidation state of the metal ion within it.
  • The term "complex" refers to the structured nature of these ions, where metal ions and ligands interact intricately.
  • Complex ions play crucial roles in many biological systems and industrial processes.
  • They can lead to the formation of coordination compounds when they precipitate, particularly in water.
Grasping the concept of complex ions helps understand their significant role in both natural and synthetic chemical environments.

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

Give the systematic name for (a) \(\mathrm{K}_{3}\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]\) (b) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{Cl}\right]\left(\mathrm{ClO}_{4}\right)_{2}\) (c) \(\left[\mathrm{Co}(\mathrm{CO})_{4} \mathrm{Cl}_{2}\right] \mathrm{ClO}_{4}\) (d) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Br}_{2}\right] \mathrm{Cl}_{2}\)

Comparing \(\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}\) with \(\left[\mathrm{CoCl}_{6}\right]^{4-}\), indicate whether each of the following statements is true or false: (a) \(\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}\) has more \(d\) electrons than \(\left[\mathrm{CoCl}_{6}\right]^{4-}\). (b) \(\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}\) has the same number of \(d\) electrons as \(\left[\mathrm{CoCl}_{6}\right]^{4-}\). (c) \(\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}\) is paramagnetic, whereas \(\left[\mathrm{CoCl}_{6}\right]^{4-}\) is diamagnetic. (d) \(\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}\) is diamagnetic, whereas \(\left[\mathrm{CoCl}_{6}\right]^{4-}\) is paramagnetic.

Some of the first complexes discovered by Werner in the 1890 s had the empirical formulas given below. Also given are the number of chloride ions per formula unit precipitated by the addition of \(\mathrm{Ag}^{+}(a q) .\) Explain these observations. $$ \begin{array}{lc} \hline \begin{array}{l} \text { Empirical } \\ \text { formula } \end{array} & \begin{array}{l} \text { Number of Cl }^{-} \text {per formula } \\ \text { unit precipitated by } \mathbf{A g}^{+}(a q) \end{array} \\ \hline \mathrm{PtCl}_{2} \cdot 4 \mathrm{NH}_{3} & 2 \\ \mathrm{PtCl}_{2} \cdot 3 \mathrm{NH}_{3} & 1 \\ \mathrm{PtCl}_{2} \cdot 2 \mathrm{NH}_{3} & 0 \end{array} $$

Give the chemical formula for the following complex ions: (a) hexanitrocobaltate(III) (b) trans-dichlorobis(ethylenediamine)platinum(IV) (c) pentacyanocarbonylferrate(II) (d) trans-dichlorodiiodoaurate(III)

Draw all the geometric and any optical isomers for (a) \(\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{Br}_{2}\right]\) (b) \(\left[\mathrm{RuCl}_{2} \mathrm{Br}_{2}\left(\mathrm{NO}_{2}\right)_{2}\right]^{3-}\)
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Kinetics

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.