Chapter 20, 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  ${\left[{\text{Ru(NH}}_3{\text{)}}_{\text{5}}\text{Cl}\right]}^{\text{2+}}$

Answer to Problem 34E

Answer

The name of complex ion ${\left[{\text{Ru(NH}}_3{\text{)}}_{\text{5}}\text{Cl}\right]}^{\text{2+}}$ is pentaamminechlororuthenium(III).

Explanation of Solution

Explanation

The complex ion is ${\left[{\text{Ru(NH}}_3{\text{)}}_{\text{5}}\text{Cl}\right]}^{\text{2+}}$. This ion contains positive charge.

Oxidation state of Chlorine $\left({\text{Cl}}^{-}\right)$ is $-1$.

Oxidation state of Ammonia $\left({\text{NH}}_3\right)$ is $0$.

It is assumed that the oxidation state of metal ion Ruthenium $\left(\text{Ru}\right)$ is $x$.

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

$\begin{array}{c}5\left(0\right)+1\left(-1\right)+x=+2\\ x=+3\end{array}$

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 ${\left[{\text{Ru(NH}}_3{\text{)}}_{\text{5}}\text{Cl}\right]}^{\text{2+}}$ 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 ${\left[{\text{Fe(CN)}}_{\text{6}}\right]}^{\text{4}-}$

Answer to Problem 34E

Answer

The name of complex ion ${\left[{\text{Fe(CN)}}_{\text{6}}\right]}^{\text{4}-}$ is hexacyanoferrate(II).

Explanation of Solution

Explanation

The complex ion is ${\left[{\text{Fe(CN)}}_{\text{6}}\right]}^{\text{4}-}$. This ion contains negative charge.

Oxidation state of Cyanide $\left({\text{CN}}^{-}\right)$ ligand is $-1$.

It is assumed that the oxidation state of iron $\left(\text{Fe}\right)$ is $x$.

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

$\begin{array}{c}6\left(-1\right)+x=-4\\ x=+2\end{array}$

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 ${\left[{\text{Fe(CN)}}_{\text{6}}\right]}^{\text{4}-}$ 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 ${\left[{\text{Mn(NH}}_2{\text{CH}}_2{\text{CH}}_2{\text{NH}}_2{\text{)}}_{\text{3}}\right]}^{\text{2+}}$

Answer to Problem 34E

Answer

The name of complex ion ${\left[{\text{Mn(NH}}_2{\text{CH}}_2{\text{CH}}_2{\text{NH}}_2{\text{)}}_{\text{3}}\right]}^{\text{2+}}$ is triethylenediaminemanganate(II).

Explanation of Solution

Explanation

The complex ion is ${\left[{\text{Mn(NH}}_2{\text{CH}}_2{\text{CH}}_2{\text{NH}}_2{\text{)}}_{\text{3}}\right]}^{\text{2+}}$. This ion contains positive charge.

Oxidation state of neutral Ethylenediamine $\left({\text{NH}}_2{\text{CH}}_2{\text{CH}}_2{\text{NH}}_2\right)$ ligand is $0$.

It is assumed that the oxidation state of Manganese $\left(\text{Mn}\right)$ is $x$.

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

$\begin{array}{c}3\left(0\right)+x=+2\\ x=+2\end{array}$

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 ${\left[{\text{Mn(NH}}_2{\text{CH}}_2{\text{CH}}_2{\text{NH}}_2{\text{)}}_{\text{3}}\right]}^{\text{2+}}$ 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 ${\left[{\text{Co(NH}}_3{\text{)}}_{\text{5}}{\text{NO}}_{\text{2}}\right]}^{2+}$

Answer to Problem 34E

Answer

The name of complex ion ${\left[{\text{Co(NH}}_3{\text{)}}_{\text{5}}{\text{NO}}_{\text{2}}\right]}^{2+}$ is pentaamminenitrocobalt(III).

Explanation of Solution

Explanation

The complex ion is ${\left[{\text{Co(NH}}_3{\text{)}}_{\text{5}}{\text{NO}}_{\text{2}}\right]}^{2+}$. This ion contains positive charge.

Oxidation state of Nitrite $\left({\text{NO}}_2{}^{-}\right)$ is $-1$.

Oxidation state of neutral Ammonia $\left({\text{NH}}_3\right)$ is $0$.

It is assumed that the oxidation state of metal ion Cobalt $\left(\text{Co}\right)$ is $x$.

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

$\begin{array}{c}5\left(0\right)+1\left(-1\right)+x=+2\\ x=+3\end{array}$

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 ${\left[{\text{Co(NH}}_3{\text{)}}_{\text{5}}{\text{NO}}_{\text{2}}\right]}^{2+}$ 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  ${\left[{\text{Ni(CN)}}_{\text{4}}\right]}^{\text{2}-}$

Answer to Problem 34E

Answer

The name of complex ion ${\left[{\text{Ni(CN)}}_{\text{4}}\right]}^{\text{2}-}$ is tetracyanonickelate(II).

Explanation of Solution

Explanation

The complex ion is ${\left[{\text{Ni(CN)}}_{\text{4}}\right]}^{\text{2}-}$. This ion contains negative charge.

Oxidation state of cyanide $\left({\text{CN}}^{-}\right)$ ligand is $-1$.

It is assumed that the oxidation state of metal ion Nickel $\left(\text{Ni}\right)$ is $x$.

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

$\begin{array}{c}4\left(-1\right)+x=-2\\ x=+2\end{array}$

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 ${\left[{\text{Ni(CN)}}_{\text{4}}\right]}^{\text{2}-}$ 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 ${\left[{\text{Cr(NH}}_3{\text{)}}_{\text{4}}{\left(\text{Cl}\right)}_2\right]}^{\text{+}}$.

Answer to Problem 34E

Answer

The name of complex ion   ${\left[{\text{Cr(NH}}_3{\text{)}}_{\text{4}}{\left(\text{Cl}\right)}_2\right]}^{\text{+}}$ is tetraamminedichlorochromium(III).

Explanation of Solution

Explanation

The name of complex ion ${\left[{\text{Cr(NH}}_3{\text{)}}_{\text{4}}{\left(\text{Cl}\right)}_2\right]}^{\text{+}}$ is tetraamminedichlorochromium(III).

Oxidation state of Chlorine $\left({\text{Cl}}^{-}\right)$ is $-1$.

Oxidation state of neutral Ammonia $\left({\text{NH}}_3\right)$ is $0$.

It is assumed that the oxidation state of metal ion Chromium $\left(\text{Cr}\right)$ is $x$.

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

$\begin{array}{c}4\left(0\right)+2\left(-1\right)+x=+1\\ x=+3\end{array}$

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 ${\left[{\text{Cr(NH}}_3{\text{)}}_{\text{4}}{\left(\text{Cl}\right)}_2\right]}^{\text{+}}$ 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 ${\left[{\text{Fe(C}}_2{\text{O}}_4{\text{)}}_{\text{3}}\right]}^{\text{3}-}$

Answer to Problem 34E

Answer

The name of complex ion ${\left[{\text{Fe(C}}_2{\text{O}}_4{\text{)}}_{\text{3}}\right]}^{\text{3}-}$ is trioxalateferrate(III).

Explanation of Solution

Explanation

The complex ion is ${\left[{\text{Fe(C}}_2{\text{O}}_4{\text{)}}_{\text{3}}\right]}^{\text{3}-}$. This ion contains negative charge.

Oxidation state of Oxalate $\left({\text{C}}_2{\text{O}}_4{}^{2-}\right)$ ligand is $-2$.

It is assumed that the oxidation state of Iron $\left(\text{Fe}\right)$ is $x$.

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

$\begin{array}{c}3\left(-2\right)+x=-3\\ x=+3\end{array}$

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 ${\left[{\text{Fe(C}}_2{\text{O}}_4{\text{)}}_{\text{3}}\right]}^{\text{3}-}$ 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 ${\left[{\text{Co(SCN)}}_{\text{2}}{\left({\text{H}}_{\text{2}}\text{O}\right)}_4\right]}^{+}$

Answer to Problem 34E

Answer

The name of complex ion ${\left[{\text{Co(SCN)}}_{\text{2}}{\left({\text{H}}_{\text{2}}\text{O}\right)}_4\right]}^{+}$ is tetraaquadithiocyanatocobalt(III).

Explanation of Solution

Explanation

The complex ion is ${\left[{\text{Co(SCN)}}_{\text{2}}{\left({\text{H}}_{\text{2}}\text{O}\right)}_4\right]}^{+}$. This ion contains positive charge.

Oxidation state of Thiocyanate $\left({\text{SCN}}^{-}\right)$ is $-1$.

Oxidation state of neutral Water $\left({\text{H}}_2\text{O}\right)$ is $0$.

It is assumed that the oxidation state of metal ion cobalt $\left(\text{Co}\right)$ is $x$.

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

$\begin{array}{c}4\left(0\right)+2\left(-1\right)+x=+1\\ x=+3\end{array}$

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 ${\left[{\text{Co(SCN)}}_{\text{2}}{\left({\text{H}}_{\text{2}}\text{O}\right)}_4\right]}^{+}$ is tetraaquadithiocyanatocobalt(III).

Conclusion

Conclusion

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