/*! 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 20 One of the following nitrogen co... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 22: Problem 20

One of the following nitrogen compounds or ions is not capable of serving as a ligand: \(\mathrm{NH}_{4}^{+}, \mathrm{NH}_{3}\) \(\mathrm{NH}_{2}^{-} .\) Identify this species, and explain your answer.

Short Answer

Expert verified
The species \(\mathrm{NH}_{4}^{+}\) cannot serve as a ligand because it lacks a lone electron pair.

Step by step solution

01

Define a Ligand

A ligand is a molecule or ion that can donate at least one pair of electrons to a central metal atom or ion, forming a coordinate bond. This means a ligand should have at least one pair of non-bonding electrons.
02

Examine Each Species for Lone Pairs

Let's look at each species for the presence of non-bonding electron pairs:- The ammonium ion, \(\mathrm{NH}_{4}^{+}\), has no non-bonding electron pairs because all electrons are involved in bonding, and the nitrogen carries a positive charge.- Ammonia, \(\mathrm{NH}_{3}\), has a lone pair of electrons, making it capable of donating electrons.- The amide ion, \(\mathrm{NH}_{2}^{-}\), also has a lone pair of electrons and can donate to form a bond.
03

Identify the Non-Ligand Species

From the examination, \(\mathrm{NH}_{4}^{+}\) lacks a lone electron pair and, therefore, cannot act as a ligand by donating electrons. In comparison, both \(\mathrm{NH}_{3}\) and \(\mathrm{NH}_{2}^{-}\) have lone pairs and can serve as ligands.

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.

Coordinate Bond
A coordinate bond, also referred to as a dative covalent bond, is a type of chemical bond where both electrons in the bond originate from the same atom. This is different from a typical covalent bond, where each atom provides one electron.
A coordinate bond forms when a ligand donates a pair of electrons to an empty orbital of a central metal atom or ion. This bond is crucial in complex formation.

Key characteristics include:
  • Involvement of electron pair donation from a ligand to a metal center.
  • Common in transition metal complexes.
  • Often denoted with an arrow (鈫�) pointing from the donor atom to the acceptor atom.
Understanding coordinate bonds helps explain why certain species can act as ligands, emphasizing the importance of electron pair availability.
Electron Pair Donation
In chemistry, electron pair donation refers to the process by which a molecule or ion provides a pair of electrons to an electron-deficient species, thereby forming a bond.
This donation is essential for the formation of coordinate bonds, as it allows ligands to attach to metal centers.

Important points include:
  • Electron-rich species, like ligands, typically have lone pairs available.
  • Electron donation leads to complex formation in coordination chemistry.
  • This concept is vital to understanding the reactivity and bonding capabilities of ligands.
By grasping electron pair donation, we can determine which species can act as ligands and understand their role in coordination compounds.
Ammonium Ion
The ammonium ion, \(\mathrm{NH}_{4}^{+}\), is a positively charged ion with no lone electron pairs.
This ion forms by the protonation of ammonia, involving the donation of a hydrogen ion (H鈦�).

Key features include:
  • Has a tetrahedral geometry with four hydrogen atoms bonded to nitrogen.
  • Lacks lone pairs on nitrogen, making it unable to form coordinate bonds.
  • Positively charged, denoted as \(\mathrm{NH}_{4}^{+}\).
This absence of lone electron pairs is what prevents \(\mathrm{NH}_{4}^{+}\) from acting as a ligand, distinguishing it from other nitrogen-based species.
Lone Electron Pairs
Lone electron pairs are pairs of valence electrons not involved in bonding.
These pairs are crucial in determining the ability of molecules or ions to participate in forming coordinate bonds.

Characteristics include:
  • Located on atoms like nitrogen, oxygen, and halogens.
  • Can be donated to electron-deficient species, forming a bond.
  • Essential for the behavior of molecules in chemical reactions.
The presence of lone electron pairs in molecules like \(\mathrm{NH}_3\) and \(\mathrm{NH}_{2}^{-}\) allows them to act as ligands, unlike \(\mathrm{NH}_{4}^{+}\), which lacks such pairs.

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

How many geometric isomers are possible for the square-planar complex ion \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)(\mathrm{CN}) \mathrm{Cl}_{2}\right]^{-} ?\)

Write formulas for the following ions or compounds. (a) dichlorobis(ethylenediamine)nickel(II) (b) potassium tetrachloroplatinate(II) (c) potassium dicyanocuprate(I) (d) tetraamminediaquairon(II)

For a tetrahedral complex of a metal in the first transition series, which of the following statements concerning energies of the \(3 d\) orbitals is correct? (a) The five \(d\) orbitals have the same energy. (b) The \(d_{x^{2}-y^{2}}\) and \(d_{z^{2}}\) orbitals are higher in energy than the \(d_{x y} d_{y y}\) and \(d_{x y}\) orbitals. (c) The \(d_{x z} d_{y z}\) and \(d_{x y}\) orbitals are higher in energy than the \(d_{x^{2}-y^{2}}\) and \(d_{z^{2}}\) orbitals.

What types of isomerism (geometric isomerism, optical isomerism, structural isomerism) are possible in the compound diamminechlorothio-cyanatoplatinum (II)? Identify all possible answers.

Three geometric isomers are possible for \(\left[\mathrm{Co (\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]^{3+} .\) One of the three is chiral; that is, it has a non-superimposable mirror image. Draw the structures of the three isomers. Which one is chiral?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

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.