The name of the given complex ions is to be stated. Concept introduction: Rules followed in the naming of coordination compound: In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element. An ‘o’ is added to the root name of anion. Greek prefix is used to express the number of ligands. Roman numeral is used to denote the oxidation state of metal ion. In case of more than one type of ligand present in a compound, they are named alphabetically. The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals. To determine: The name of the complex ion [ Ru(NH 3 ) 5 Cl ] 2+

Question

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Answer 1

Question

Chapter 21, Problem 34E

(a)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ru(NH3)5Cl]2+$

(a)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Explanation of Solution

Explanation

The complex ion is $[Ru(NH3)5Cl]2+$ . This ion contains positive charge.

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Ruthenium $(Ru)$ is $x$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of ruthenium is $+3$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Hence, the name of anion is pentaamminechloro.

Therefore, the name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

(b)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(CN)6]4−$

(b)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Explanation of Solution

Explanation

The complex ion is $[Fe(CN)6]4−$ . This ion contains negative charge.

Oxidation state of Cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of iron $(Fe)$ is $x$ .

The given complex compound contains six Cyanide ions and one Iron ion. Since, the overall charge on complex ion is $−4$ . Therefore,

$6(−1)+x=−4x=+2$

Therefore, the oxidation state of Iron is $+2$ .

The given complex compound contains six Cyanide ions. Hence, the name of anion is hexacyano. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

(c)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Mn(NH2CH2CH2NH2)3]2+$

(c)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Explanation of Solution

Explanation

The complex ion is $[Mn(NH2CH2CH2NH2)3]2+$ . This ion contains positive charge.

Oxidation state of neutral Ethylenediamine $(NH2CH2CH2NH2)$ ligand is $0$ .

It is assumed that the oxidation state of Manganese $(Mn)$ is $x$ .

The given complex compound contains three ethylenediamine ions and one Manganese ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$3(0)+x=+2x=+2$

Therefore, the oxidation state of Manganese is $+2$ .

The given complex compound contains three Ethylenediamine ions. Hence, the name of anion is triethylenediamine. The Latin name of Manganese is Manganate.

Therefore, the name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

(d)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(NH3)5NO2]2+$

(d)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(NH3)5NO2]2+$ . This ion contains positive charge.

Oxidation state of Nitrite $(NO2−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Cobalt $(Co)$ is $x$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of Cobalt is $+3$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Hence, the name of anion is pentaamminenitro.

Therefore, the name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

(e)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ni(CN)4]2−$

(e)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Explanation of Solution

Explanation

The complex ion is $[Ni(CN)4]2−$ . This ion contains negative charge.

Oxidation state of cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of metal ion Nickel $(Ni)$ is $x$ .

The given complex compound contains four Cyanide ions and one Nickel ion. Since, the overall charge on complex ion is $−2$ . Therefore,

$4(−1)+x=−2x=+2$

Therefore, the oxidation state of Nickel is $+2$ .

The given complex compound contains four Cyanide ions. Hence, the name of anion is tetracyano. The Latin name of Nickel is Nickelate.

Therefore, the name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

(f)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Cr(NH3)4(Cl)2]+$ .

(f)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Explanation of Solution

Explanation

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Chromium $(Cr)$ is $x$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of Chromium is $+3$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Hence, the name of anion is tetraamminedichloro.

Therefore, the name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

(g)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(C2O4)3]3−$

(g)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Explanation of Solution

Explanation

The complex ion is $[Fe(C2O4)3]3−$ . This ion contains negative charge.

Oxidation state of Oxalate $(C2O42−)$ ligand is $−2$ .

It is assumed that the oxidation state of Iron $(Fe)$ is $x$ .

The given complex compound contains three Oxalate ions and one Iron ion. Since, the overall charge on complex ion is $−3$ . Therefore,

$3(−2)+x=−3x=+3$

Therefore, the oxidation state of iron is $+3$ .

The given complex compound contains three Oxalate ions. Hence, the name of anion is trioxalate. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

(h)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(SCN)2(H2O)4]+$

(h)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(SCN)2(H2O)4]+$ . This ion contains positive charge.

Oxidation state of Thiocyanate $(SCN−)$ is $−1$ .

Oxidation state of neutral Water $(H2O)$ is $0$ .

It is assumed that the oxidation state of metal ion cobalt $(Co)$ is $x$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of cobalt is $+3$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Hence, the name of anion is tetraaquadithiocyanato.

Therefore, the name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Conclusion

Conclusion

In the naming complex ion, anion is named first, whereas metal ion is named second.

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Answer 2

Question

Chapter 21, Problem 34E

(a)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ru(NH3)5Cl]2+$

(a)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Explanation of Solution

Explanation

The complex ion is $[Ru(NH3)5Cl]2+$ . This ion contains positive charge.

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Ruthenium $(Ru)$ is $x$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of ruthenium is $+3$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Hence, the name of anion is pentaamminechloro.

Therefore, the name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

(b)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(CN)6]4−$

(b)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Explanation of Solution

Explanation

The complex ion is $[Fe(CN)6]4−$ . This ion contains negative charge.

Oxidation state of Cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of iron $(Fe)$ is $x$ .

The given complex compound contains six Cyanide ions and one Iron ion. Since, the overall charge on complex ion is $−4$ . Therefore,

$6(−1)+x=−4x=+2$

Therefore, the oxidation state of Iron is $+2$ .

The given complex compound contains six Cyanide ions. Hence, the name of anion is hexacyano. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

(c)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Mn(NH2CH2CH2NH2)3]2+$

(c)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Explanation of Solution

Explanation

The complex ion is $[Mn(NH2CH2CH2NH2)3]2+$ . This ion contains positive charge.

Oxidation state of neutral Ethylenediamine $(NH2CH2CH2NH2)$ ligand is $0$ .

It is assumed that the oxidation state of Manganese $(Mn)$ is $x$ .

The given complex compound contains three ethylenediamine ions and one Manganese ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$3(0)+x=+2x=+2$

Therefore, the oxidation state of Manganese is $+2$ .

The given complex compound contains three Ethylenediamine ions. Hence, the name of anion is triethylenediamine. The Latin name of Manganese is Manganate.

Therefore, the name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

(d)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(NH3)5NO2]2+$

(d)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(NH3)5NO2]2+$ . This ion contains positive charge.

Oxidation state of Nitrite $(NO2−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Cobalt $(Co)$ is $x$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of Cobalt is $+3$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Hence, the name of anion is pentaamminenitro.

Therefore, the name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

(e)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ni(CN)4]2−$

(e)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Explanation of Solution

Explanation

The complex ion is $[Ni(CN)4]2−$ . This ion contains negative charge.

Oxidation state of cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of metal ion Nickel $(Ni)$ is $x$ .

The given complex compound contains four Cyanide ions and one Nickel ion. Since, the overall charge on complex ion is $−2$ . Therefore,

$4(−1)+x=−2x=+2$

Therefore, the oxidation state of Nickel is $+2$ .

The given complex compound contains four Cyanide ions. Hence, the name of anion is tetracyano. The Latin name of Nickel is Nickelate.

Therefore, the name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

(f)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Cr(NH3)4(Cl)2]+$ .

(f)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Explanation of Solution

Explanation

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Chromium $(Cr)$ is $x$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of Chromium is $+3$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Hence, the name of anion is tetraamminedichloro.

Therefore, the name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

(g)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(C2O4)3]3−$

(g)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Explanation of Solution

Explanation

The complex ion is $[Fe(C2O4)3]3−$ . This ion contains negative charge.

Oxidation state of Oxalate $(C2O42−)$ ligand is $−2$ .

It is assumed that the oxidation state of Iron $(Fe)$ is $x$ .

The given complex compound contains three Oxalate ions and one Iron ion. Since, the overall charge on complex ion is $−3$ . Therefore,

$3(−2)+x=−3x=+3$

Therefore, the oxidation state of iron is $+3$ .

The given complex compound contains three Oxalate ions. Hence, the name of anion is trioxalate. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

(h)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(SCN)2(H2O)4]+$

(h)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(SCN)2(H2O)4]+$ . This ion contains positive charge.

Oxidation state of Thiocyanate $(SCN−)$ is $−1$ .

Oxidation state of neutral Water $(H2O)$ is $0$ .

It is assumed that the oxidation state of metal ion cobalt $(Co)$ is $x$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of cobalt is $+3$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Hence, the name of anion is tetraaquadithiocyanato.

Therefore, the name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Conclusion

Conclusion

In the naming complex ion, anion is named first, whereas metal ion is named second.

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Answer 3

Question

Chapter 21, Problem 34E

(a)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ru(NH3)5Cl]2+$

(a)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Explanation of Solution

Explanation

The complex ion is $[Ru(NH3)5Cl]2+$ . This ion contains positive charge.

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Ruthenium $(Ru)$ is $x$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of ruthenium is $+3$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Hence, the name of anion is pentaamminechloro.

Therefore, the name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

(b)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(CN)6]4−$

(b)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Explanation of Solution

Explanation

The complex ion is $[Fe(CN)6]4−$ . This ion contains negative charge.

Oxidation state of Cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of iron $(Fe)$ is $x$ .

The given complex compound contains six Cyanide ions and one Iron ion. Since, the overall charge on complex ion is $−4$ . Therefore,

$6(−1)+x=−4x=+2$

Therefore, the oxidation state of Iron is $+2$ .

The given complex compound contains six Cyanide ions. Hence, the name of anion is hexacyano. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

(c)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Mn(NH2CH2CH2NH2)3]2+$

(c)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Explanation of Solution

Explanation

The complex ion is $[Mn(NH2CH2CH2NH2)3]2+$ . This ion contains positive charge.

Oxidation state of neutral Ethylenediamine $(NH2CH2CH2NH2)$ ligand is $0$ .

It is assumed that the oxidation state of Manganese $(Mn)$ is $x$ .

The given complex compound contains three ethylenediamine ions and one Manganese ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$3(0)+x=+2x=+2$

Therefore, the oxidation state of Manganese is $+2$ .

The given complex compound contains three Ethylenediamine ions. Hence, the name of anion is triethylenediamine. The Latin name of Manganese is Manganate.

Therefore, the name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

(d)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(NH3)5NO2]2+$

(d)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(NH3)5NO2]2+$ . This ion contains positive charge.

Oxidation state of Nitrite $(NO2−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Cobalt $(Co)$ is $x$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of Cobalt is $+3$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Hence, the name of anion is pentaamminenitro.

Therefore, the name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

(e)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ni(CN)4]2−$

(e)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Explanation of Solution

Explanation

The complex ion is $[Ni(CN)4]2−$ . This ion contains negative charge.

Oxidation state of cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of metal ion Nickel $(Ni)$ is $x$ .

The given complex compound contains four Cyanide ions and one Nickel ion. Since, the overall charge on complex ion is $−2$ . Therefore,

$4(−1)+x=−2x=+2$

Therefore, the oxidation state of Nickel is $+2$ .

The given complex compound contains four Cyanide ions. Hence, the name of anion is tetracyano. The Latin name of Nickel is Nickelate.

Therefore, the name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

(f)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Cr(NH3)4(Cl)2]+$ .

(f)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Explanation of Solution

Explanation

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Chromium $(Cr)$ is $x$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of Chromium is $+3$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Hence, the name of anion is tetraamminedichloro.

Therefore, the name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

(g)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(C2O4)3]3−$

(g)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Explanation of Solution

Explanation

The complex ion is $[Fe(C2O4)3]3−$ . This ion contains negative charge.

Oxidation state of Oxalate $(C2O42−)$ ligand is $−2$ .

It is assumed that the oxidation state of Iron $(Fe)$ is $x$ .

The given complex compound contains three Oxalate ions and one Iron ion. Since, the overall charge on complex ion is $−3$ . Therefore,

$3(−2)+x=−3x=+3$

Therefore, the oxidation state of iron is $+3$ .

The given complex compound contains three Oxalate ions. Hence, the name of anion is trioxalate. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

(h)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(SCN)2(H2O)4]+$

(h)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(SCN)2(H2O)4]+$ . This ion contains positive charge.

Oxidation state of Thiocyanate $(SCN−)$ is $−1$ .

Oxidation state of neutral Water $(H2O)$ is $0$ .

It is assumed that the oxidation state of metal ion cobalt $(Co)$ is $x$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of cobalt is $+3$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Hence, the name of anion is tetraaquadithiocyanato.

Therefore, the name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Conclusion

Conclusion

In the naming complex ion, anion is named first, whereas metal ion is named second.

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Answer 4

Question

Chapter 21, Problem 34E

(a)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ru(NH3)5Cl]2+$

(a)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Explanation of Solution

Explanation

The complex ion is $[Ru(NH3)5Cl]2+$ . This ion contains positive charge.

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Ruthenium $(Ru)$ is $x$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of ruthenium is $+3$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Hence, the name of anion is pentaamminechloro.

Therefore, the name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

(b)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(CN)6]4−$

(b)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Explanation of Solution

Explanation

The complex ion is $[Fe(CN)6]4−$ . This ion contains negative charge.

Oxidation state of Cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of iron $(Fe)$ is $x$ .

The given complex compound contains six Cyanide ions and one Iron ion. Since, the overall charge on complex ion is $−4$ . Therefore,

$6(−1)+x=−4x=+2$

Therefore, the oxidation state of Iron is $+2$ .

The given complex compound contains six Cyanide ions. Hence, the name of anion is hexacyano. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

(c)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Mn(NH2CH2CH2NH2)3]2+$

(c)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Explanation of Solution

Explanation

The complex ion is $[Mn(NH2CH2CH2NH2)3]2+$ . This ion contains positive charge.

Oxidation state of neutral Ethylenediamine $(NH2CH2CH2NH2)$ ligand is $0$ .

It is assumed that the oxidation state of Manganese $(Mn)$ is $x$ .

The given complex compound contains three ethylenediamine ions and one Manganese ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$3(0)+x=+2x=+2$

Therefore, the oxidation state of Manganese is $+2$ .

The given complex compound contains three Ethylenediamine ions. Hence, the name of anion is triethylenediamine. The Latin name of Manganese is Manganate.

Therefore, the name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

(d)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(NH3)5NO2]2+$

(d)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(NH3)5NO2]2+$ . This ion contains positive charge.

Oxidation state of Nitrite $(NO2−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Cobalt $(Co)$ is $x$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of Cobalt is $+3$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Hence, the name of anion is pentaamminenitro.

Therefore, the name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

(e)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ni(CN)4]2−$

(e)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Explanation of Solution

Explanation

The complex ion is $[Ni(CN)4]2−$ . This ion contains negative charge.

Oxidation state of cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of metal ion Nickel $(Ni)$ is $x$ .

The given complex compound contains four Cyanide ions and one Nickel ion. Since, the overall charge on complex ion is $−2$ . Therefore,

$4(−1)+x=−2x=+2$

Therefore, the oxidation state of Nickel is $+2$ .

The given complex compound contains four Cyanide ions. Hence, the name of anion is tetracyano. The Latin name of Nickel is Nickelate.

Therefore, the name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

(f)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Cr(NH3)4(Cl)2]+$ .

(f)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Explanation of Solution

Explanation

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Chromium $(Cr)$ is $x$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of Chromium is $+3$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Hence, the name of anion is tetraamminedichloro.

Therefore, the name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

(g)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(C2O4)3]3−$

(g)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Explanation of Solution

Explanation

The complex ion is $[Fe(C2O4)3]3−$ . This ion contains negative charge.

Oxidation state of Oxalate $(C2O42−)$ ligand is $−2$ .

It is assumed that the oxidation state of Iron $(Fe)$ is $x$ .

The given complex compound contains three Oxalate ions and one Iron ion. Since, the overall charge on complex ion is $−3$ . Therefore,

$3(−2)+x=−3x=+3$

Therefore, the oxidation state of iron is $+3$ .

The given complex compound contains three Oxalate ions. Hence, the name of anion is trioxalate. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

(h)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(SCN)2(H2O)4]+$

(h)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(SCN)2(H2O)4]+$ . This ion contains positive charge.

Oxidation state of Thiocyanate $(SCN−)$ is $−1$ .

Oxidation state of neutral Water $(H2O)$ is $0$ .

It is assumed that the oxidation state of metal ion cobalt $(Co)$ is $x$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of cobalt is $+3$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Hence, the name of anion is tetraaquadithiocyanato.

Therefore, the name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Conclusion

Conclusion

In the naming complex ion, anion is named first, whereas metal ion is named second.

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Answer 5

Chapter 21, Problem 34E

(a)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ru(NH3)5Cl]2+$

(a)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Explanation of Solution

Explanation

The complex ion is $[Ru(NH3)5Cl]2+$ . This ion contains positive charge.

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Ruthenium $(Ru)$ is $x$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of ruthenium is $+3$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Hence, the name of anion is pentaamminechloro.

Therefore, the name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

(b)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(CN)6]4−$

(b)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Explanation of Solution

Explanation

The complex ion is $[Fe(CN)6]4−$ . This ion contains negative charge.

Oxidation state of Cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of iron $(Fe)$ is $x$ .

The given complex compound contains six Cyanide ions and one Iron ion. Since, the overall charge on complex ion is $−4$ . Therefore,

$6(−1)+x=−4x=+2$

Therefore, the oxidation state of Iron is $+2$ .

The given complex compound contains six Cyanide ions. Hence, the name of anion is hexacyano. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

(c)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Mn(NH2CH2CH2NH2)3]2+$

(c)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Explanation of Solution

Explanation

The complex ion is $[Mn(NH2CH2CH2NH2)3]2+$ . This ion contains positive charge.

Oxidation state of neutral Ethylenediamine $(NH2CH2CH2NH2)$ ligand is $0$ .

It is assumed that the oxidation state of Manganese $(Mn)$ is $x$ .

The given complex compound contains three ethylenediamine ions and one Manganese ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$3(0)+x=+2x=+2$

Therefore, the oxidation state of Manganese is $+2$ .

The given complex compound contains three Ethylenediamine ions. Hence, the name of anion is triethylenediamine. The Latin name of Manganese is Manganate.

Therefore, the name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

(d)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(NH3)5NO2]2+$

(d)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(NH3)5NO2]2+$ . This ion contains positive charge.

Oxidation state of Nitrite $(NO2−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Cobalt $(Co)$ is $x$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of Cobalt is $+3$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Hence, the name of anion is pentaamminenitro.

Therefore, the name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

(e)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ni(CN)4]2−$

(e)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Explanation of Solution

Explanation

The complex ion is $[Ni(CN)4]2−$ . This ion contains negative charge.

Oxidation state of cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of metal ion Nickel $(Ni)$ is $x$ .

The given complex compound contains four Cyanide ions and one Nickel ion. Since, the overall charge on complex ion is $−2$ . Therefore,

$4(−1)+x=−2x=+2$

Therefore, the oxidation state of Nickel is $+2$ .

The given complex compound contains four Cyanide ions. Hence, the name of anion is tetracyano. The Latin name of Nickel is Nickelate.

Therefore, the name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

(f)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Cr(NH3)4(Cl)2]+$ .

(f)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Explanation of Solution

Explanation

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Chromium $(Cr)$ is $x$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of Chromium is $+3$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Hence, the name of anion is tetraamminedichloro.

Therefore, the name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

(g)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(C2O4)3]3−$

(g)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Explanation of Solution

Explanation

The complex ion is $[Fe(C2O4)3]3−$ . This ion contains negative charge.

Oxidation state of Oxalate $(C2O42−)$ ligand is $−2$ .

It is assumed that the oxidation state of Iron $(Fe)$ is $x$ .

The given complex compound contains three Oxalate ions and one Iron ion. Since, the overall charge on complex ion is $−3$ . Therefore,

$3(−2)+x=−3x=+3$

Therefore, the oxidation state of iron is $+3$ .

The given complex compound contains three Oxalate ions. Hence, the name of anion is trioxalate. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

(h)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(SCN)2(H2O)4]+$

(h)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(SCN)2(H2O)4]+$ . This ion contains positive charge.

Oxidation state of Thiocyanate $(SCN−)$ is $−1$ .

Oxidation state of neutral Water $(H2O)$ is $0$ .

It is assumed that the oxidation state of metal ion cobalt $(Co)$ is $x$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of cobalt is $+3$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Hence, the name of anion is tetraaquadithiocyanato.

Therefore, the name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Conclusion

Conclusion

In the naming complex ion, anion is named first, whereas metal ion is named second.

Answer 6

Chapter 21, Problem 34E

(a)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ru(NH3)5Cl]2+$

(a)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Explanation of Solution

Explanation

The complex ion is $[Ru(NH3)5Cl]2+$ . This ion contains positive charge.

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Ruthenium $(Ru)$ is $x$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of ruthenium is $+3$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Hence, the name of anion is pentaamminechloro.

Therefore, the name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Answer 7

Chapter 21, Problem 34E

(a)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ru(NH3)5Cl]2+$

Answer 8

(a)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Explanation

The complex ion is $[Ru(NH3)5Cl]2+$ . This ion contains positive charge.

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Ruthenium $(Ru)$ is $x$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of ruthenium is $+3$ .

The given complex compound contains five Ammonia ions and a Chlorine ion. Hence, the name of anion is pentaamminechloro.

Therefore, the name of complex ion $[Ru(NH3)5Cl]2+$ is pentaamminechlororuthenium(III).

Answer 13

(b)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(CN)6]4−$

(b)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Explanation of Solution

Explanation

The complex ion is $[Fe(CN)6]4−$ . This ion contains negative charge.

Oxidation state of Cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of iron $(Fe)$ is $x$ .

The given complex compound contains six Cyanide ions and one Iron ion. Since, the overall charge on complex ion is $−4$ . Therefore,

$6(−1)+x=−4x=+2$

Therefore, the oxidation state of Iron is $+2$ .

The given complex compound contains six Cyanide ions. Hence, the name of anion is hexacyano. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Answer 14

(b)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(CN)6]4−$

Answer 15

(b)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Explanation

The complex ion is $[Fe(CN)6]4−$ . This ion contains negative charge.

Oxidation state of Cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of iron $(Fe)$ is $x$ .

The given complex compound contains six Cyanide ions and one Iron ion. Since, the overall charge on complex ion is $−4$ . Therefore,

$6(−1)+x=−4x=+2$

Therefore, the oxidation state of Iron is $+2$ .

The given complex compound contains six Cyanide ions. Hence, the name of anion is hexacyano. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(CN)6]4−$ is hexacyanoferrate(II).

Answer 20

(c)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Mn(NH2CH2CH2NH2)3]2+$

(c)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Explanation of Solution

Explanation

The complex ion is $[Mn(NH2CH2CH2NH2)3]2+$ . This ion contains positive charge.

Oxidation state of neutral Ethylenediamine $(NH2CH2CH2NH2)$ ligand is $0$ .

It is assumed that the oxidation state of Manganese $(Mn)$ is $x$ .

The given complex compound contains three ethylenediamine ions and one Manganese ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$3(0)+x=+2x=+2$

Therefore, the oxidation state of Manganese is $+2$ .

The given complex compound contains three Ethylenediamine ions. Hence, the name of anion is triethylenediamine. The Latin name of Manganese is Manganate.

Therefore, the name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Answer 21

(c)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Mn(NH2CH2CH2NH2)3]2+$

Answer 22

(c)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

Explanation

The complex ion is $[Mn(NH2CH2CH2NH2)3]2+$ . This ion contains positive charge.

Oxidation state of neutral Ethylenediamine $(NH2CH2CH2NH2)$ ligand is $0$ .

It is assumed that the oxidation state of Manganese $(Mn)$ is $x$ .

The given complex compound contains three ethylenediamine ions and one Manganese ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$3(0)+x=+2x=+2$

Therefore, the oxidation state of Manganese is $+2$ .

The given complex compound contains three Ethylenediamine ions. Hence, the name of anion is triethylenediamine. The Latin name of Manganese is Manganate.

Therefore, the name of complex ion $[Mn(NH2CH2CH2NH2)3]2+$ is triethylenediaminemanganate(II).

Answer 27

(d)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(NH3)5NO2]2+$

(d)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(NH3)5NO2]2+$ . This ion contains positive charge.

Oxidation state of Nitrite $(NO2−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Cobalt $(Co)$ is $x$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of Cobalt is $+3$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Hence, the name of anion is pentaamminenitro.

Therefore, the name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Answer 28

(d)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(NH3)5NO2]2+$

Answer 29

(d)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

Explanation

The complex ion is $[Co(NH3)5NO2]2+$ . This ion contains positive charge.

Oxidation state of Nitrite $(NO2−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Cobalt $(Co)$ is $x$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Since, the overall charge on complex ion is $+2$ . Therefore,

$5(0)+1(−1)+x=+2x=+3$

Therefore, the oxidation state of Cobalt is $+3$ .

The given complex compound contains five Ammonia ions and one Nitrite ion. Hence, the name of anion is pentaamminenitro.

Therefore, the name of complex ion $[Co(NH3)5NO2]2+$ is pentaamminenitrocobalt(III).

Answer 34

(e)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ni(CN)4]2−$

(e)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Explanation of Solution

Explanation

The complex ion is $[Ni(CN)4]2−$ . This ion contains negative charge.

Oxidation state of cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of metal ion Nickel $(Ni)$ is $x$ .

The given complex compound contains four Cyanide ions and one Nickel ion. Since, the overall charge on complex ion is $−2$ . Therefore,

$4(−1)+x=−2x=+2$

Therefore, the oxidation state of Nickel is $+2$ .

The given complex compound contains four Cyanide ions. Hence, the name of anion is tetracyano. The Latin name of Nickel is Nickelate.

Therefore, the name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Answer 35

(e)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Ni(CN)4]2−$

Answer 36

(e)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Answer 37

(e)

Expert Solution

Answer 38

(e)

Expert Solution

Answer 39

Expert Solution

Answer 40

Explanation of Solution

Explanation

The complex ion is $[Ni(CN)4]2−$ . This ion contains negative charge.

Oxidation state of cyanide $(CN−)$ ligand is $−1$ .

It is assumed that the oxidation state of metal ion Nickel $(Ni)$ is $x$ .

The given complex compound contains four Cyanide ions and one Nickel ion. Since, the overall charge on complex ion is $−2$ . Therefore,

$4(−1)+x=−2x=+2$

Therefore, the oxidation state of Nickel is $+2$ .

The given complex compound contains four Cyanide ions. Hence, the name of anion is tetracyano. The Latin name of Nickel is Nickelate.

Therefore, the name of complex ion $[Ni(CN)4]2−$ is tetracyanonickelate(II).

Answer 41

(f)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Cr(NH3)4(Cl)2]+$ .

(f)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Explanation of Solution

Explanation

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Chromium $(Cr)$ is $x$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of Chromium is $+3$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Hence, the name of anion is tetraamminedichloro.

Therefore, the name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Answer 42

(f)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Cr(NH3)4(Cl)2]+$ .

Answer 43

(f)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Answer 44

(f)

Expert Solution

Answer 45

(f)

Expert Solution

Answer 46

Expert Solution

Answer 47

Explanation of Solution

Explanation

The name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Oxidation state of Chlorine $(Cl−)$ is $−1$ .

Oxidation state of neutral Ammonia $(NH3)$ is $0$ .

It is assumed that the oxidation state of metal ion Chromium $(Cr)$ is $x$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of Chromium is $+3$ .

The given complex compound contains four Ammonia ions and two Chlorine ions. Hence, the name of anion is tetraamminedichloro.

Therefore, the name of complex ion $[Cr(NH3)4(Cl)2]+$ is tetraamminedichlorochromium(III).

Answer 48

(g)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(C2O4)3]3−$

(g)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Explanation of Solution

Explanation

The complex ion is $[Fe(C2O4)3]3−$ . This ion contains negative charge.

Oxidation state of Oxalate $(C2O42−)$ ligand is $−2$ .

It is assumed that the oxidation state of Iron $(Fe)$ is $x$ .

The given complex compound contains three Oxalate ions and one Iron ion. Since, the overall charge on complex ion is $−3$ . Therefore,

$3(−2)+x=−3x=+3$

Therefore, the oxidation state of iron is $+3$ .

The given complex compound contains three Oxalate ions. Hence, the name of anion is trioxalate. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Answer 49

(g)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Fe(C2O4)3]3−$

Answer 50

(g)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Answer 51

(g)

Expert Solution

Answer 52

(g)

Expert Solution

Answer 53

Expert Solution

Answer 54

Explanation of Solution

Explanation

The complex ion is $[Fe(C2O4)3]3−$ . This ion contains negative charge.

Oxidation state of Oxalate $(C2O42−)$ ligand is $−2$ .

It is assumed that the oxidation state of Iron $(Fe)$ is $x$ .

The given complex compound contains three Oxalate ions and one Iron ion. Since, the overall charge on complex ion is $−3$ . Therefore,

$3(−2)+x=−3x=+3$

Therefore, the oxidation state of iron is $+3$ .

The given complex compound contains three Oxalate ions. Hence, the name of anion is trioxalate. The Latin name of Iron is Ferrate.

Therefore, the name of complex ion $[Fe(C2O4)3]3−$ is trioxalateferrate(III).

Answer 55

(h)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(SCN)2(H2O)4]+$

(h)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Explanation of Solution

Explanation

The complex ion is $[Co(SCN)2(H2O)4]+$ . This ion contains positive charge.

Oxidation state of Thiocyanate $(SCN−)$ is $−1$ .

Oxidation state of neutral Water $(H2O)$ is $0$ .

It is assumed that the oxidation state of metal ion cobalt $(Co)$ is $x$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of cobalt is $+3$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Hence, the name of anion is tetraaquadithiocyanato.

Therefore, the name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Conclusion

Conclusion

In the naming complex ion, anion is named first, whereas metal ion is named second.

Answer 56

(h)

Interpretation Introduction

Interpretation: The name of the given complex ions is to be stated.

Concept introduction: Rules followed in the naming of coordination compound:

In the naming of coordination compound, the name of anion (ligand) comes first. Metal ion is named second, which is the name of element.

An ‘o’ is added to the root name of anion.

Greek prefix is used to express the number of ligands.

Roman numeral is used to denote the oxidation state of metal ion.

In case of more than one type of ligand present in a compound, they are named alphabetically.

The suffix ‘-ate’ is added to metal ion if complex ion contains negative charge. Latin names are also used to identify the name of metals.

To determine: The name of the complex ion $[Co(SCN)2(H2O)4]+$

Answer 57

(h)

Expert Solution

Answer to Problem 34E

Answer

The name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Answer 58

(h)

Expert Solution

Answer 59

(h)

Expert Solution

Answer 60

Expert Solution

Answer 61

Explanation of Solution

Explanation

The complex ion is $[Co(SCN)2(H2O)4]+$ . This ion contains positive charge.

Oxidation state of Thiocyanate $(SCN−)$ is $−1$ .

Oxidation state of neutral Water $(H2O)$ is $0$ .

It is assumed that the oxidation state of metal ion cobalt $(Co)$ is $x$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Since, the overall charge on complex ion is $+1$ . Therefore,

$4(0)+2(−1)+x=+1x=+3$

Therefore, the oxidation state of cobalt is $+3$ .

The given complex compound contains two Thiocyanate ions and four Water ions. Hence, the name of anion is tetraaquadithiocyanato.

Therefore, the name of complex ion $[Co(SCN)2(H2O)4]+$ is tetraaquadithiocyanatocobalt(III).

Answer 62

Conclusion

Conclusion

In the naming complex ion, anion is named first, whereas metal ion is named second.

Answer 63

Ch. 21 - What two first-row transition metals have...Ch. 21 - Prob. 2RQ Ch. 21 - Prob. 3RQ Ch. 21 - Prob. 4RQ Ch. 21 - Prob. 5RQ Ch. 21 - Prob. 6RQ Ch. 21 - Prob. 7RQ Ch. 21 - Prob. 8RQ Ch. 21 - Prob. 9RQ Ch. 21 - Prob. 10RQ

Concept explainers

Answer to Problem 34E

Explanation of Solution

Answer to Problem 34E

Explanation of Solution

Answer to Problem 34E

Explanation of Solution

Answer to Problem 34E

Explanation of Solution

Answer to Problem 34E

Explanation of Solution

Answer to Problem 34E

Explanation of Solution

Answer to Problem 34E

Explanation of Solution

Answer to Problem 34E

Explanation of Solution

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