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The value of 'spin only' magnetic moment...

The value of 'spin only' magnetic moment for one of the following configuration is `2.84B.M.` The correct one is:

A

`d^(4)` (in strong ligand field )

B

`d^(4)` (in weak ligand field )

C

`d^(3)` (in weak as well as in strong fields)

D

`d^(5)` (in strong ligand field )

Text Solution

AI Generated Solution

The correct Answer is:
To solve the problem regarding the spin-only magnetic moment of coordination compounds, we will analyze the given configurations step by step. ### Step-by-Step Solution: 1. **Understanding the Magnetic Moment Formula**: The spin-only magnetic moment (μ) is calculated using the formula: \[ μ = \sqrt{n(n + 2)} \text{ Bohr Magneton (B.M.)} \] where \( n \) is the number of unpaired electrons. 2. **Analyzing the Configurations**: We have four configurations to analyze: - **Option 1**: \( d^4 \) strong field - **Option 2**: \( d^4 \) weak field - **Option 3**: \( d^3 \) (both strong and weak field) - **Option 4**: \( d^5 \) strong field 3. **Calculating for Each Configuration**: - **Option 1: \( d^4 \) Strong Field**: - In a strong field, electrons pair up. The configuration is \( t_{2g}^4 e_g^0 \). - Number of unpaired electrons \( n = 2 \). - Magnetic moment: \[ μ = \sqrt{2(2 + 2)} = \sqrt{8} = 2.84 \text{ B.M.} \] - **Option 2: \( d^4 \) Weak Field**: - In a weak field, electrons do not pair. The configuration is \( t_{2g}^3 e_g^1 \). - Number of unpaired electrons \( n = 4 \). - Magnetic moment: \[ μ = \sqrt{4(4 + 2)} = \sqrt{24} \approx 4.89 \text{ B.M.} \] - **Option 3: \( d^3 \) (Strong Field)**: - In a strong field, the configuration is \( t_{2g}^3 e_g^0 \). - Number of unpaired electrons \( n = 3 \). - Magnetic moment: \[ μ = \sqrt{3(3 + 2)} = \sqrt{15} \approx 3.87 \text{ B.M.} \] - **Option 4: \( d^5 \) Strong Field**: - In a strong field, the configuration is \( t_{2g}^5 e_g^0 \). - Number of unpaired electrons \( n = 5 \). - Magnetic moment: \[ μ = \sqrt{5(5 + 2)} = \sqrt{35} \approx 5.92 \text{ B.M.} \] 4. **Conclusion**: The only configuration that gives a magnetic moment of \( 2.84 \text{ B.M.} \) is **Option 1: \( d^4 \) Strong Field**. ### Final Answer: The correct configuration is **Option 1: \( d^4 \) Strong Field**.

To solve the problem regarding the spin-only magnetic moment of coordination compounds, we will analyze the given configurations step by step. ### Step-by-Step Solution: 1. **Understanding the Magnetic Moment Formula**: The spin-only magnetic moment (μ) is calculated using the formula: \[ μ = \sqrt{n(n + 2)} \text{ Bohr Magneton (B.M.)} ...
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Velence bond theroy describes the bonding in complexs in terms of coordinate -covalent bond resulting from overlap filled ligand orbitals with vacant metal hybrid orbitals This theory explains magnetic behaviour and geometrical shape of coordination compounds Magnetic moment of a complex compound can be determined experimentally and theoretically by using spin only formula Magnetic moment sqrtn (n+2)BM (where n = No. unpaired electrons) . The value of of spin only magnetic moment for octahedral complex of the following configuration is 2.84BM The correct statement is (a) d^(4) (in weak field ligand) (b) d^(2) (in weak field and in strong field ligand) (c) d^(3) (in weak field and in strong field ligand) (d) d^(5) (in strong field ligand) .

The calculated spin only magnetic moment of Cr^2+ ion is:

Knowledge Check

  • The spin only magnetic moment value of Cr(CO)_(6) is

    A
    2.84 B.M
    B
    4.90 B.M.
    C
    5.92 B.M
    D
    0 B.M.
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