Chapter 23, Problem 23.45P

(a)

Interpretation Introduction

Interpretation:

For the given complex the systematic name has to be given.

  ${\text{[Ni(H}}_{\text{2}}{\text{O)}}_{\text{6}}{\text{]Cl}}_{\text{2}}$

Concept introduction:

The set of rules for naming a coordination compound is:

1. 1. When naming a complex ion, the ligands are named before the metal ion.
2. 2. Write the names of the ligands in the following order: neutral, negative, positive.  If there are multiple ligands of the same charge type, they are named in alphabetical order.
3. 3. Multiple occurring monodentate ligands receive a prefix according to the number of occurrences: $\text{di-, tri-, tetra-, penta-, or hexa}\text{.}$  Polydentate ligands (e.g., ethylene diamine, oxalate) receive $\text{bis-, tris-, tetrakis-, etc}\text{.}$  Anions end in -ido.  This replaces the final “e” when the anion ends with “-ate” (e.g, sulfate becomes sulfato) and replaces “-ide” (cyanide becomes cyanido).
4. 4. Neutral ligands are given their usual name, with some exceptions: NH₃ becomes ammine; $H_{2}O$ becomes aqua or aquo;$CO$ becomes carbonyl; $\text{NO}$ becomes nitrosyl.
5. 5. Write the name of the central atom/ion. If the complex is an anion, the central atom’s name will end in -ate, and its Latin name will be used if available
6. 6. If the central atom’s oxidation state needs to be specified (when it is one of several possible, or zero), write it as a Roman numeral (or 0) in parentheses.
7. 7. End with “cation” or “anion” as separate words.

(b)

Interpretation Introduction

Interpretation:

For the given complex the systematic name has to be given.

  ${\text{[Cr(en)}}_{\text{3}}{\text{](ClO}}_{\text{4}}{\text{)}}_{\text{3}}$

Concept introduction;

The set of rules for naming a coordination compound is:

1. 1. When naming a complex ion, the ligands are named before the metal ion.
2. 2. Write the names of the ligands in the following order: neutral, negative, positive.  If there are multiple ligands of the same charge type, they are named in alphabetical order.
3. 3. Multiple occurring monodentate ligands receive a prefix according to the number of occurrences: $\text{di-, tri-, tetra-, penta-, or hexa}\text{.}$  Polydentate ligands (e.g., ethylene diamine, oxalate) receive $\text{bis-, tris-, tetrakis-, etc}\text{.}$  Anions end in -ido.  This replaces the final “e” when the anion ends with “-ate” (e.g, sulfate becomes sulfato) and replaces “-ide” (cyanide becomes cyanido).
4. 4. Neutral ligands are given their usual name, with some exceptions: NH₃ becomes ammine; $H_{2}O$ becomes aqua or aquo;$CO$ becomes carbonyl; $\text{NO}$ becomes nitrosyl.
5. 5. Write the name of the central atom/ion. If the complex is an anion, the central atom’s name will end in -ate, and its Latin name will be used if available
6. 6. If the central atom’s oxidation state needs to be specified (when it is one of several possible, or zero), write it as a Roman numeral (or 0) in parentheses.
7. 7. End with “cation” or “anion” as separate words.

(c)

Interpretation Introduction

Interpretation:

For the given complex the systematic name has to be given.

  ${\text{K}}_{\text{4}}{\text{[Mn(CN)}}_{\text{6}}\text{]}$

Concept introduction;

The set of rules for naming a coordination compound is:

1. 1. When naming a complex ion, the ligands are named before the metal ion.
2. 2. Write the names of the ligands in the following order: neutral, negative, positive.  If there are multiple ligands of the same charge type, they are named in alphabetical order.
3. 3. Multiple occurring monodentate ligands receive a prefix according to the number of occurrences: $\text{di-, tri-, tetra-, penta-, or hexa}\text{.}$  Polydentate ligands (e.g., ethylene diamine, oxalate) receive $\text{bis-, tris-, tetrakis-, etc}\text{.}$  Anions end in -ido.  This replaces the final “e” when the anion ends with “-ate” (e.g, sulfate becomes sulfato) and replaces “-ide” (cyanide becomes cyanido).
4. 4. Neutral ligands are given their usual name, with some exceptions: NH₃ becomes ammine; $H_{2}O$ becomes aqua or aquo;$CO$ becomes carbonyl; $\text{NO}$ becomes nitrosyl.
5. 5. Write the name of the central atom/ion. If the complex is an anion, the central atom’s name will end in -ate, and its Latin name will be used if available
6. 6. If the central atom’s oxidation state needs to be specified (when it is one of several possible, or zero), write it as a Roman numeral (or 0) in parentheses.
7. 7. End with “cation” or “anion” as separate words.