Chemistry: The Molecular Nature of Matter and Change
Chemistry: The Molecular Nature of Matter and Change
8th Edition
ISBN: 9781259631757
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 23, Problem 23.88P

(a)

Interpretation Introduction

Interpretation:

For the given complex the orbital splitting diagram has to be drawn using spectrochemial series.

  [Cr(H2O)6]3+

Concept introduction:

The element in the periodic table and count its position in the respective transition series. These elements are in Periods 5 and 6, so the general configuration is

  [noble gas]ns2(n 1)dx.

The spectrochemical series is

  I<Cl<F<OH<H2O<SCN<en<NO2<CN<CO

(a)

Expert Solution
Check Mark

Explanation of Solution

Electron configuration of Cr: [Ar]4s13d5

Charge on Cr: The aqua ligands are neutral, so the charge on Cris+3.

Electron configuration of Cr3+: [Ar]3d3

Six ligands indicate an octahedral arrangement.  Using Hund’s rule, fill the lower energy

t2g orbitals first, filling empty orbitals before pairing electrons within an orbital.

Chemistry: The Molecular Nature of Matter and Change, Chapter 23, Problem 23.88P , additional homework tip  1

(b)

Interpretation Introduction

Interpretation:

For the given complex the orbital splitting diagram has to be drawn using spectrochemial series.

  [Cu(H2O)4]2+

Concept introduction:

The element in the periodic table and count its position in the respective transition series. These elements are in Periods 5 and 6, so the general configuration is

  [noble gas]ns2(n 1)dx.

The spectrochemical series is

  I<Cl<F<OH<H2O<SCN<en<NO2<CN<CO

(b)

Expert Solution
Check Mark

Explanation of Solution

Electron configuration of Cu: [Ar]4s13d10

Charge on Cu: The aqua ligands are neutral, so Cu has a +2 charge.

Electron configuration of Cu2+: [Ar]3d9

Four ligands and a d9 configuration indicate a square planar geometry (only filled d sublevel ions exhibit tetrahedral geometry).  Use Hund’s rule to fill in the nine d electrons.  Thus, the correct orbital-energy splitting diagram shows one unpaired electron.   

Chemistry: The Molecular Nature of Matter and Change, Chapter 23, Problem 23.88P , additional homework tip  2

(c)

Interpretation Introduction

Interpretation:

For the given complex the orbital splitting diagram has to be drawn using spectrochemial series.

  [FeF6]3

Concept introduction:

The element in the periodic table and count its position in the respective transition series. These elements are in Periods 5 and 6, so the general configuration is

  [noble gas]ns2(n 1)dx.

The spectrochemical series is

  I<Cl<F<OH<H2O<SCN<en<NO2<CN<CO

(c)

Expert Solution
Check Mark

Explanation of Solution

Electron configuration of Fe: [Ar]4s23d6

Charge on Fe: Each fluoride ligand has a –1 charge for a total charge of –6, so Fe has a +3 charge to make the overall complex charge equal to –3.

Electron configuration of Fe3+: [Ar]3d5

Six ligands indicate an octahedral arrangement.  Use Hund’s rule to fill the orbitals.

F– is a weak-field ligand, so the splitting energy, Δ, is not large enough to overcome the resistance to electron pairing.  The electrons remain unpaired, and the complex is called high-spin.

Chemistry: The Molecular Nature of Matter and Change, Chapter 23, Problem 23.88P , additional homework tip  3

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Chapter 23 Solutions

Chemistry: The Molecular Nature of Matter and Change

Ch. 23.4 - Prob. 23.6AFPCh. 23.4 - Prob. 23.6BFPCh. 23.4 - Prob. 23.7AFPCh. 23.4 - Prob. 23.7BFPCh. 23.4 - Prob. B23.1PCh. 23.4 - Prob. B23.2PCh. 23 - Prob. 23.1PCh. 23 - Write the general electron configuration of a...Ch. 23 - Prob. 23.3PCh. 23 - Prob. 23.4PCh. 23 - Prob. 23.5PCh. 23 - Prob. 23.6PCh. 23 - (a) What is the range in electronegativity across...Ch. 23 - (a) Explain the major difference between the...Ch. 23 - (a) What behavior distinguishes paramagnetic and...Ch. 23 - Prob. 23.10PCh. 23 - Using the periodic table to locate each element,...Ch. 23 - Using the periodic table to locate each element,...Ch. 23 - Using the periodic table to locate each element,...Ch. 23 - Prob. 23.14PCh. 23 - Prob. 23.15PCh. 23 - What is the highest oxidation state for (a) Ta;...Ch. 23 - What is the highest oxidation state for (a) Nb;...Ch. 23 - Prob. 23.18PCh. 23 - Prob. 23.19PCh. 23 - Prob. 23.20PCh. 23 - Prob. 23.21PCh. 23 - Prob. 23.22PCh. 23 - Prob. 23.23PCh. 23 - Prob. 23.24PCh. 23 - Prob. 23.25PCh. 23 - Prob. 23.26PCh. 23 - What atomic property of the lanthanides leads to...Ch. 23 - Prob. 23.28PCh. 23 - Prob. 23.29PCh. 23 - Give the electron configuration of (a) La; (b)...Ch. 23 - Prob. 23.31PCh. 23 - Only a few lanthanides show an oxidation state...Ch. 23 - Prob. 23.33PCh. 23 - Prob. 23.34PCh. 23 - Describe the makeup of a complex ion, including...Ch. 23 - Prob. 23.36PCh. 23 - Prob. 23.37PCh. 23 - Prob. 23.38PCh. 23 - Prob. 23.39PCh. 23 - Prob. 23.40PCh. 23 - Prob. 23.41PCh. 23 - Prob. 23.42PCh. 23 - Prob. 23.43PCh. 23 - Prob. 23.44PCh. 23 - Prob. 23.45PCh. 23 - Prob. 23.46PCh. 23 - What are the charge and coordination number of the...Ch. 23 - What are the charge and coordination number of the...Ch. 23 - Prob. 23.49PCh. 23 - Give systematic names for the following...Ch. 23 - What are the charge and coordination number of the...Ch. 23 - What are the charge and coordination number of the...Ch. 23 - Prob. 23.53PCh. 23 - Prob. 23.54PCh. 23 - Prob. 23.55PCh. 23 - Prob. 23.56PCh. 23 - Prob. 23.57PCh. 23 - Prob. 23.58PCh. 23 - Prob. 23.59PCh. 23 - Prob. 23.60PCh. 23 - Prob. 23.61PCh. 23 - Prob. 23.62PCh. 23 - For any of the following that can exist as...Ch. 23 - Prob. 23.64PCh. 23 - Prob. 23.65PCh. 23 - Prob. 23.66PCh. 23 - Chromium(III), like cobalt(III), has a...Ch. 23 - When MCl4(NH3)2 is dissolved in water and treated...Ch. 23 - Prob. 23.69PCh. 23 - What is a coordinate covalent bond? Is such a...Ch. 23 - Prob. 23.71PCh. 23 - Prob. 23.72PCh. 23 - Prob. 23.73PCh. 23 - In terms of the theory of color absorption,...Ch. 23 - Prob. 23.75PCh. 23 - Prob. 23.76PCh. 23 - Prob. 23.77PCh. 23 - How do the relative magnitudes of Epairing and Δ...Ch. 23 - Prob. 23.79PCh. 23 - Give the number of d electrons (n of dn) for the...Ch. 23 - Give the number of d electrons (n of dn) for the...Ch. 23 - Prob. 23.82PCh. 23 - How many d electrons (n of dn) are in the central...Ch. 23 - Prob. 23.84PCh. 23 - Prob. 23.85PCh. 23 - Prob. 23.86PCh. 23 - Prob. 23.87PCh. 23 - Prob. 23.88PCh. 23 - Prob. 23.89PCh. 23 - Prob. 23.90PCh. 23 - Prob. 23.91PCh. 23 - Prob. 23.92PCh. 23 - Prob. 23.93PCh. 23 - Prob. 23.94PCh. 23 - Prob. 23.95PCh. 23 - Prob. 23.96PCh. 23 - Prob. 23.97PCh. 23 - Prob. 23.98PCh. 23 - When neptunium (Np) and plutonium (Pu) were...Ch. 23 - Prob. 23.100PCh. 23 - Prob. 23.101PCh. 23 - For the compound [Co(en)2Cl2]Cl, give: The...Ch. 23 - Prob. 23.103PCh. 23 - Prob. 23.104PCh. 23 - Prob. 23.105PCh. 23 - Prob. 23.106PCh. 23 - Prob. 23.107PCh. 23 - Prob. 23.108PCh. 23 - Prob. 23.109PCh. 23 - Prob. 23.110PCh. 23 - Prob. 23.111PCh. 23 - The actinides Pa, U, and Np form a series of...Ch. 23 - Prob. 23.113PCh. 23 - Prob. 23.114PCh. 23 - Prob. 23.115PCh. 23 - Prob. 23.116PCh. 23 - Prob. 23.117PCh. 23 - Prob. 23.118PCh. 23 - Prob. 23.119PCh. 23 - Prob. 23.120PCh. 23 - Prob. 23.121PCh. 23 - Prob. 23.122P
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