IUPAC Nomenclature of Coordination Compounds||Roles for naming of coordination Compounds||Examples

IUPAC Nomenclature of Coordination Compounds||Roles for naming of coordination Compounds||Examples

#iupacnomenclatureofcoordinationcompounds
#namingofcoordinationcompounds #namingofcomplexcompounds #complexcomplounds #complexes #coordination_compound #coordinationnumber #coordinategeometry #nomenclature_of_organic_compounds #nomenclatura #examples #explanation
This Pashto video lecture is about the exploitation and naming or nomenclature of coordination compounds with suitable examples and explanations from second year chemistry chapter no 2.
## Nomenclature of Coordination Compounds

*(According to IUPAC rules)*

The naming of coordination compounds follows **fixed systematic rules** so that each compound has **one correct name**.

---

## Basic Parts of a Coordination Compound

A coordination compound generally consists of:

1. **Central metal atom/ion**
2. **Ligands** (ions or molecules attached to the metal)
3. **Coordination sphere** (written in square brackets `[ ]`)
4. **Counter ions** (outside the bracket)

Example:
[
[K_4[Fe(CN)_6]]
]

---

## Rules for Nomenclature (Step by Step)

---

### **Rule 1: Name the cation first, then the anion**

Whether complex or simple.

Example:
[
[Co(NH_3)_6]Cl_3
]
Name → **Hexaamminecobalt(III) chloride**

---

### **Rule 2: Name ligands before the metal**

Ligands are written **first**, metal comes **after**.

Example:
[
[Cu(NH_3)_4]SO_4
]
Name → **Tetraamminecopper(II) sulfate**

---

### **Rule 3: Naming of ligands**

* **Negative ligands** end with **–o**
* **Neutral ligands** keep their molecular name (with some exceptions)

#### Common Ligands

| Ligand | Name |
| ------ | -------- |
| NH₃ | Ammine |
| H₂O | Aqua |
| CO | Carbonyl |
| NO | Nitrosyl |
| Cl⁻ | Chloro |
| Br⁻ | Bromo |
| CN⁻ | Cyano |
| OH⁻ | Hydroxo |

Example:
[
[Cr(H_2O)_6]Cl_3
]
Name → **Hexaaquachromium(III) chloride**

---

### **Rule 4: Use prefixes for number of ligands**

| Number | Prefix |
| ------ | ------ |
| 2 | Di |
| 3 | Tri |
| 4 | Tetra |
| 5 | Penta |
| 6 | Hexa |

Example:
[
[Ni(CO)_4]
]
Name → **Tetracarbonylnickel(0)**

---

### **Rule 5: Name the metal**

* If the **complex is cationic or neutral**, use **metal name**
* If the **complex is anionic**, add **–ate** to metal name

| Metal | Anionic name |
| ----- | ------------ |
| Fe | Ferrate |
| Cu | Cuprate |
| Ag | Argentate |
| Au | Aurate |
| Co | Cobaltate |

Example:
[
[K_3[Fe(CN)_6]]
]
Name → **Potassium hexacyanoferrate(III)**

---

### **Rule 6: Oxidation state of metal**

* Written in **Roman numerals** in brackets
* Determined after ligand charges

Example:
[
[Fe(CN)_6]^{3-}
]
Oxidation state of Fe = +3
→ **Ferrate(III)**

---

### **Rule 7: Alphabetical order of ligands**

Ligands are named **alphabetically**, ignoring prefixes (di, tri, tetra).

Example:
[
[Co(NH_3)_4Cl_2]^+
]
Name → **Tetraammine dichlorocobalt(III)**

---

## Complete Solved Examples

---

### **Example 1**

[
[Co(NH_3)_5Cl]Cl_2
]

* Ligands: 5 NH₃ (ammine), 1 Cl⁻ (chloro)
* Oxidation state of Co = +3

**Name:**
👉 **Pentaamminechlorocobalt(III) chloride**

---

### **Example 2**

[
[K_4[Fe(CN)_6]]
]

* Complex anion → use **ferrate**
* CN⁻ = cyano
* Fe oxidation state = +2

**Name:**
👉 **Potassium hexacyanoferrate(II)**

---

### **Example 3**

[
[Pt(NH_3)_2Cl_2]
]

* Neutral complex
* Pt oxidation state = +2

**Name:**
👉 **Diamminedichloroplatinum(II)**

---

### **Example 4**

[
[Cr(H_2O)_4Cl_2]Cl
]

* Complex cation
* Cr oxidation state = +3

**Name:**
👉 **Tetraaquadichlorochromium(III) chloride**

---

## Important Exam Tips ⭐

✔ Ammine has **double m**
✔ Aqua, ammine, carbonyl are **neutral ligands**
✔ Oxidation state is **always written in Roman numerals**
✔ For anionic complexes → metal ends in **–ate**

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