Chemistry and Chemical Reactivity - AP Edition
Chemistry and Chemical Reactivity - AP Edition
10th Edition
ISBN: 9781337399203
Author: Kotz
Publisher: CENGAGE L
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Chapter 22, Problem 44PS

(a)

Interpretation Introduction

Interpretation: The electronic configuration, magnetic character and the number of unpaired electrons for the given set of high spin complexes has be determined.

Concept introduction: The transition metal atoms have tendency to form complex compounds that are linked to the certain neutral or ionic species which leads to the formation of coordination compounds. There exists a large number of coordination compounds that have a large number of applications in the chemical industry as well as in daily life.

The properties of the coordination compounds depend upon the primary and secondary valancy of the metal ion in the coordination sphere. The electrical conductivity depends upon the number of ions that are produced by complex.

The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.

The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

The five d orbitals get divided into two sets that is dxy, dyz and dxz orbitals forms one set and dx2-y2and dz2 forms another set. The first set are oriented between the x, y and z axes whereas the second set gets oriented along the axis.

Electronic configuration: It is defined as the distribution of electrons present in the atom over orbitals following certain rules like electrons starts filling the lower energy orbital to higher energy, pairing of electrons does not occur until all the orbitals are singly filled and finally no electrons present in orbital can have same set of quantum numbers.

Oxidation State: It is the number which defines number of electrons that are gained or lost by a given chemical substance.

(a)

Expert Solution
Check Mark

Answer to Problem 44PS

The given complex contains 4 unpaired electrons since the given complex is high spin complex where electrons present in higher energy d orbitals. Therefore, the given complex is paramagnetic.

Explanation of Solution

Examining the given complex shows that Fe serves as the central metal atom since it is surrounded by 6 ligands with it. The periodic table clearly shows that the outer electronic configuration of Fe is 4s23d6.

The oxidation state for Fe in given complex is +2 since given complex has 6F and 4K where the charge of F is 1 and for K=1 which is showed as follows,

K4[FeF6]Let x be charge of Fe(4×1)+x+(-1×6)= 04+x6=0x = 2Therefore,oxidation state of Fe is +2.

Now considering the charge of metal atom the outer electrons present in the given complex is six distributed over d orbitals as follows,

GivenHighspincomplex__dx2y2dz2___dxydyzdxz

The above configuration clearly shows that there exist 4 unpaired electrons since the given condition says that it is high spin complex where pairing of electrons does not occur and the electrons tends to present at higher level of d orbitals hence the given complex is paramagnetic.

(b)

Interpretation Introduction

Interpretation: The electronic configuration, magnetic character and the number of unpaired electrons for the given set of high spin complexes should be determined.

Concept introduction: The transition metal atoms have tendency to form complex compounds that are linked to the certain neutral or ionic species which leads to the formation of coordination compounds. There exists a large number of coordination compounds that have a large number of applications in the chemical industry as well as in daily life.

The properties of the coordination compounds depend upon the primary and secondary valancy of the metal ion in the coordination sphere. The electrical conductivity depends upon the number of ions that are produced by complex.

The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.

The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

The five d orbitals get divided into two sets that is dxy, dyz and dxz orbitals forms one set and dx2-y2and dz2 forms another set. The first set are oriented between the x, y and z axes whereas the second set gets oriented along the axis.

Electronic configuration: It is defined as the distribution of electrons present in the atom over orbitals following certain rules like electrons starts filling the lower energy orbital to higher energy, pairing of electrons does not occur until all the orbitals are singly filled and finally no electrons present in orbital can have same set of quantum numbers.

Oxidation State: It is the number which defines number of electrons that are gained or lost by a given chemical substance.

(b)

Expert Solution
Check Mark

Answer to Problem 44PS

The given complex contains 5 unpaired electron and it is paramagnetic.

Explanation of Solution

Examining the given complex shows that Mn serves as the central metal atom since it is surrounded by 6 ligands with it. The periodic table clearly shows that the outer electronic configuration of Mn is 4s23d5.

The oxidation state for Mn in given complex is +2 since given complex has 6F and the charge of F is 1 which is showed as follows,

[MnF6]4Let x be charge of Mnx+(-1×6)= -4x6=4x = 2Therefore,oxidation state of Mn is +2.

Now considering the charge of metal atom the outer electrons present in the given complex is five distributed over d orbitals as follows,

GivenHighspincomplex__dx2y2dz2___dxydyzdxz

The above configuration clearly shows that there exist 5 unpaired electrons since the given condition says that it is high spin complex where pairing of electrons does not occur and the electrons tends to present at higher level of d orbitals hence the given complex is paramagnetic.

(c)

Interpretation Introduction

Interpretation: The electronic configuration, magnetic character and the number of unpaired electrons for the given set of high spin complexes should be determined.

Concept introduction: The transition metal atoms have tendency to form complex compounds that are linked to the certain neutral or ionic species which leads to the formation of coordination compounds. There exists a large number of coordination compounds that have a large number of applications in the chemical industry as well as in daily life.

The properties of the coordination compounds depend upon the primary and secondary valancy of the metal ion in the coordination sphere. The electrical conductivity depends upon the number of ions that are produced by complex.

The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.

The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

The five d orbitals get divided into two sets that is dxy, dyz and dxz orbitals forms one set and dx2-y2and dz2 forms another set. The first set are oriented between the x, y and z axes whereas the second set gets oriented along the axis.

Electronic configuration: It is defined as the distribution of electrons present in the atom over orbitals following certain rules like electrons starts filling the lower energy orbital to higher energy, pairing of electrons does not occur until all the orbitals are singly filled and finally no electrons present in orbital can have same set of quantum numbers.

Oxidation State: It is the number which defines number of electrons that are gained or lost by a given chemical substance.

(c)

Expert Solution
Check Mark

Answer to Problem 44PS

The given complex contains 4 unpaired electrons and it is paramagnetic.

Explanation of Solution

Examining the given complex shows that Cr serves as the central metal atom since it is surrounded by 6 ligands with it. The periodic table clearly shows that the outer electronic configuration of Cr is 4s13d5.

The oxidation state for Cr in given complex is +2 since given complex has 6H2O and the charge of H2O is 0 as it is classified as neutral ligand which is showed as follows,

[Cr(H2O)6]2+Let x be charge of Crx+(0×6)= +2x = 2Therefore,oxidation state of Cr is +2.

Now considering the charge of metal atom the outer electrons present in the given complex is four distributed over d orbitals as follows,

GivenHighspincomplex__dx2y2dz2___dxydyzdxz

The above configuration clearly shows that there exist 4 unpaired electrons since the given condition says that it is high spin complex where pairing of electrons does not occur and the electrons tends to present at higher level of d orbitals hence the given complex is paramagnetic.

(d)

Interpretation Introduction

Interpretation: The electronic configuration, magnetic character and the number of unpaired electrons for the given set of high spin complexes should be determined.

Concept introduction: The transition metal atoms have tendency to form complex compounds that are linked to the certain neutral or ionic species which leads to the formation of coordination compounds. There exists a large number of coordination compounds that have a large number of applications in the chemical industry as well as in daily life.

The properties of the coordination compounds depend upon the primary and secondary valancy of the metal ion in the coordination sphere. The electrical conductivity depends upon the number of ions that are produced by complex.

The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.

The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

The five d orbitals get divided into two sets that is dxy, dyz and dxz orbitals forms one set and dx2-y2and dz2 forms another set. The first set are oriented between the x, y and z axes whereas the second set gets oriented along the axis.

Electronic configuration: It is defined as the distribution of electrons present in the atom over orbitals following certain rules like electrons starts filling the lower energy orbital to higher energy, pairing of electrons does not occur until all the orbitals are singly filled and finally no electrons present in orbital can have same set of quantum numbers.

Oxidation State: It is the number which defines number of electrons that are gained or lost by a given chemical substance.

(d)

Expert Solution
Check Mark

Answer to Problem 44PS

The given complex contains 5 unpaired electron and it is paramagnetic.

Explanation of Solution

Examining the given complex shows that Fe serves as the central metal atom since it is surrounded by 6 ligands with it. The periodic table clearly shows that the outer electronic configuration of Fe is 4s23d6.

The oxidation state for Fe in given complex is +3 since given complex has 6F and 3NH4 where the charge of F is 1 and charge of NH4=1 which is showed as follows,

(NH4)3[FeF6]Let x be charge of Fe(3×1)+x+(-1×6)= 0-3+x-6 =0x-3=0x=3Therefore,oxidation state of Fe is +3.

Now considering the charge of metal atom the outer electrons present in the given complex is four distributed over d orbitals as follows,

GivenHighspincomplex__dx2y2dz2___dxydyzdxz

The above configuration clearly shows that there exist 5 unpaired electrons since the given condition says that it is high spin complex where pairing of electrons does not occur and the electrons tends to present at higher level of d orbitals hence the given complex is paramagnetic.

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Chapter 22 Solutions

Chemistry and Chemical Reactivity - AP Edition

Ch. 22.7 - Prob. 2.2ACPCh. 22.7 - How are the d electrons of Pt distributed in a...Ch. 22.7 - What are the electron configurations for Nd and...Ch. 22.7 - Prob. 3.2ACPCh. 22.7 - Prob. 3.3ACPCh. 22.7 - Prob. 3.4ACPCh. 22 - Identify, based on the position in the periodic...Ch. 22 - Prob. 2PSCh. 22 - Prob. 3PSCh. 22 - Prob. 4PSCh. 22 - Prob. 5PSCh. 22 - Iron is the most abundant transition element in...Ch. 22 - Prob. 7PSCh. 22 - Prob. 8PSCh. 22 - Prob. 9PSCh. 22 - Prob. 10PSCh. 22 - Identify a cation of a first series transition...Ch. 22 - Match up the isoelectronic ions on the following...Ch. 22 - The lanthanide contraction is given as an...Ch. 22 - Prob. 14PSCh. 22 - Prob. 15PSCh. 22 - Prob. 16PSCh. 22 - Prob. 17PSCh. 22 - Prob. 18PSCh. 22 - Which of the following ligands is expected to be...Ch. 22 - One of the following nitrogen compounds or ions is...Ch. 22 - Prob. 21PSCh. 22 - Prob. 22PSCh. 22 - Prob. 23PSCh. 22 - Prob. 24PSCh. 22 - Prob. 25PSCh. 22 - Prob. 26PSCh. 22 - Prob. 27PSCh. 22 - Prob. 28PSCh. 22 - Prob. 29PSCh. 22 - Prob. 30PSCh. 22 - Give the name or formula for each ion or compound,...Ch. 22 - Prob. 32PSCh. 22 - Prob. 33PSCh. 22 - Prob. 34PSCh. 22 - Prob. 35PSCh. 22 - Prob. 36PSCh. 22 - Prob. 37PSCh. 22 - Prob. 38PSCh. 22 - Prob. 39PSCh. 22 - Prob. 40PSCh. 22 - Prob. 41PSCh. 22 - Prob. 42PSCh. 22 - Prob. 43PSCh. 22 - Prob. 44PSCh. 22 - Prob. 45PSCh. 22 - Prob. 46PSCh. 22 - Prob. 47PSCh. 22 - Prob. 48PSCh. 22 - Prob. 49PSCh. 22 - Prob. 50PSCh. 22 - In water, the titanium(III) ion, [Ti(H2O)6]3+, has...Ch. 22 - Prob. 52PSCh. 22 - Prob. 53GQCh. 22 - Prob. 54GQCh. 22 - How many unpaired electrons are expected for...Ch. 22 - Prob. 56GQCh. 22 - Which of the following complex ions is (are)...Ch. 22 - Prob. 58GQCh. 22 - How many geometric isomers are possible for the...Ch. 22 - For a tetrahedral complex of a metal in the first...Ch. 22 - Prob. 61GQCh. 22 - Prob. 62GQCh. 22 - Prob. 63GQCh. 22 - A platinum-containing compound, known as Magnuss...Ch. 22 - Prob. 65GQCh. 22 - Prob. 66GQCh. 22 - Prob. 67GQCh. 22 - How many geometric isomers of the complex ion...Ch. 22 - Prob. 69GQCh. 22 - Prob. 70GQCh. 22 - Prob. 71GQCh. 22 - The square-planar complex Pt(en)Cl2 has chloride...Ch. 22 - The complex [Mn(H2O)6]2+ has five unpaired...Ch. 22 - Experiments show that K4[Cr(CN)6] is paramagnetic...Ch. 22 - Give a systematic name or the formula for the...Ch. 22 - When CrCI3 dissolves in water, three different...Ch. 22 - Prob. 77GQCh. 22 - The glycinate ion, H2NCH2CO2, formed by...Ch. 22 - Prob. 79GQCh. 22 - Nickel and palladium both form complexes of the...Ch. 22 - The transition metals form a class of compounds...Ch. 22 - Cerium, as noted in Applying Chemical Principles:...Ch. 22 - Prob. 84GQCh. 22 - Two different coordination compounds containing...Ch. 22 - Prob. 89SCQCh. 22 - Prob. 90SCQ
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