Nomenclature Of Coordination Compounds

The name of the complex is tris(ethane-1,2-diamine)cobalt(III) sulphate.
Let's break down the name to determine the formula: - "tris" indicates that there are three ligands of the type mentioned in the complex ion.
- "ethane-1,2-diamine" is the IUPAC name for ethylenediamine, which has the formula .
We can abbreviate it as "en".
So, the complex ion contains three "en" ligands.
- "cobalt (III)" indicates that the central cobalt (Co) metal ion has an oxidation state of +3.
- The complex ion is enclosed in square brackets, and the ligands are attached to the central metal ion.
Thus, the complex ion is or .
- "sulphate" indicates that the counter ion is the sulphate ion, which has the formula and a charge of -2.
To form a neutral compound, the total positive charge from the complex ion must balance the total negative charge from the sulphate ions.
The complex ion has a +3 charge.
To balance the charge with ions, we need to find the least common multiple of the charges, which is 6.
To get a total positive charge of +6, we need 2 units of the ion: .
To get a total negative charge of -6, we need 3 units of the ion: .
Therefore, the formula of the compound is .
Looking at the options:
Option (A) : The charges are and , not balanced.

Option (B) : The counter ion is sulphite ( ), not sulphate.

Option (C) : The ligand is incorrect (it's not ethane-1,2-diamine).

Option (D) : The complex ion and the counter ion are correct, and the charges are balanced ( ).

Step 1: Determine the Oxidation State and Electron Configuration For each complex, we calculate the oxidation state of the metal and its electron configuration: - (A) - Mn oxidation state: - Mn atomic number: → Electron configuration: - is not matching. - (B) - Fe oxidation state: - Fe atomic number: → Electron configuration: - In an octahedral field, this configuration corresponds to for high-spin Fe → Correct choice. - (C) - Co oxidation state: - Co atomic number: → Electron configuration: - Ligand is a strong field ligand, leading to a low-spin configuration → Not matching. - (D) - Ni oxidation state: - Ni atomic number: → Electron configuration: - The configuration leads to → Not matching. Conclusion Thus, the correct answer is:

Step 1: Determine the Oxidation State and Electron Configuration For each complex, we calculate the oxidation state of the metal and its electron configuration: - (A) - Mn oxidation state: - Mn atomic number: → Electron configuration: - is not matching. - (B) - Fe oxidation state: - Fe atomic number: → Electron configuration: - In an octahedral field, this configuration corresponds to for high-spin Fe → Correct choice. - (C) - Co oxidation state: - Co atomic number: → Electron configuration: - Ligand is a strong field ligand, leading to a low-spin configuration → Not matching. - (D) - Ni oxidation state: - Ni atomic number: → Electron configuration: - The configuration leads to → Not matching. Conclusion Thus, the correct answer is:

Step 1: Linear polymers include Nylon 6,6, PVC, and Novolac — total of 3. Step 2: Crosslinked polymers include Bakelite and melamine — total of 2. Step 3: Hence, the number of linear and crosslinked polymers respectively are 3 and 2.

Step 1: Identify geometrical isomerism
Geometrical isomerism occurs in complexes where ligands can be arranged differently in space around the central atom. Step 2: Analyze each option
\begin{itemize} \item I. \ce{[Co(en)(NH3)2Cl2]Cl}: Octahedral with two different ligands — exhibits geometrical isomerism (cis/trans). \item II. \ce{[Co(NH3)4Cl2]Cl}: Octahedral, square planar-like — exhibits geometrical isomerism. \item III. \ce{[Co(en)3]Cl3}: Tris-chelate complex with symmetrical bidentate ligands — does not show geometrical isomerism. \item IV. \ce{[Co(en)2Cl2]Br}: Octahedral with two Cl ligands — exhibits geometrical isomerism. \end{itemize}