Consider the following complex `[Co(NH_(3))_(5)CO_(3)]ClO_(4)`
The coordination number, oxidation number number of d-electrons and number of unpaired d-electrons on the metal are respectively

Options

A. 6,2,7,3
B. 7,2,7,1
C. 5,3,6,4
D. 6,3,6,0

Answer

To solve the question regarding the complex \([Co(NH_3)_5CO_3]ClO_4\), we need to determine the coordination number, oxidation number, number of d-electrons, and the number of unpaired d-electrons on the metal. Here’s a step-by-step solution:

### Step 1: Identify the Coordination Number
The coordination number is defined as the number of ligand donor atoms that are bonded to the central metal ion. In this complex:
- The complex has 5 ammonia (NH₃) ligands, which are bidentate and donate one pair of electrons each.
- The carbonate ion (CO₃²⁻) acts as a monodentate ligand, donating one pair of electrons.

Thus, the coordination number is:
\[ \text{Coordination Number} = 5 \text{ (from NH}_3\text{)} + 1 \text{ (from CO}_3\text{)} = 6 \]

### Step 2: Determine the Oxidation Number
To find the oxidation number of cobalt (Co) in the complex, we can set up the following equation:
Let the oxidation state of Co be \(x\).

The charges in the complex are:
- Each NH₃ is neutral (0 charge).
- The carbonate ion CO₃ has a charge of -2.
- The overall charge of the complex is +1 (since it is paired with ClO₄⁻, which has a -1 charge).

Setting up the equation:
\[ x + 0 \cdot 5 + (-2) = +1 \]
\[ x - 2 = +1 \implies x = +3 \]

Thus, the oxidation number of cobalt is +3.

### Step 3: Calculate the Number of d-Electrons
Cobalt (Co) has an atomic number of 27. The electron configuration for neutral cobalt is:
\[ \text{Co: } [Ar] 4s^2 3d^7 \]

In the +3 oxidation state, cobalt loses 3 electrons. Typically, the 4s electrons are lost first, followed by the 3d electrons. Therefore, the electron configuration for Co³⁺ is:
\[ \text{Co}^{3+}: [Ar] 3d^6 \]

Thus, the number of d-electrons in Co³⁺ is 6.

### Step 4: Determine the Number of Unpaired d-Electrons
The ligands present in this complex are ammonia (NH₃), which is a strong field ligand. Strong field ligands cause pairing of electrons in the d-orbitals.

For the 3d configuration of Co³⁺:
- The 6 electrons will fill the d-orbitals as follows:
\[ \text{d-orbital filling: } \uparrow\downarrow \, \uparrow\downarrow \, \uparrow\downarrow \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \]

Since all the d-electrons are paired, the number of unpaired d-electrons is:
\[ \text{Number of unpaired d-electrons} = 0 \]

### Summary of Results
- **Coordination Number**: 6
- **Oxidation Number**: +3
- **Number of d-electrons**: 6
- **Number of unpaired d-electrons**: 0

### Final Answer
The coordination number, oxidation number, number of d-electrons, and number of unpaired d-electrons on the metal are respectively: **6, +3, 6, 0**.