Coordination Compounds

To calculate the magnetic moment of a divalent ion with atomic number 25 (manganese, Mn), we follow these steps:

Step 1: Determine the electronic configuration of manganese. The atomic number is 25, so the electronic configuration is:

Mn: [Ar] 3d⁵ 4s²

Step 2: Account for the divalent state (Mn²⁺). The loss of two electrons occurs from the 4s and 3d orbitals:

Mn²⁺: [Ar] 3d⁵

Step 3: Calculate the number of unpaired electrons. In the 3d⁵ configuration, all five electrons are unpaired.

Step 4: Use the formula for magnetic moment (\mu ):

\mu = √(n(n+2))

where n is the number of unpaired electrons.

Step 5: Substitute the value of n (5 in this case) into the formula:

\mu = √(5(5+2)) = √35

Therefore, the magnetic moment of the Mn²⁺ ion is √35.

The correct answer is √35.

To solve the problem, we need to determine which valence d orbitals of the central metal ion in a tetrahedral complex are raised to higher energy when split in Crystal Field Theory (CFT).

1. Understanding the Tetrahedral Crystal Field Splitting:
In a tetrahedral complex, the central metal ion is surrounded by four ligands arranged tetrahedrally. The d orbitals of the metal ion split into two energy levels due to the interaction with the ligands.

2. Identifying the Higher Energy Orbitals:
In a tetrahedral field, the d orbitals split into two groups:

• Lower energy (e): The and orbitals (collectively referred to as the set) experience less repulsion from the ligands and are stabilized.
• Higher energy (t₂): The , , and orbitals (collectively referred to as the set) experience greater repulsion from the ligands and are raised to higher energy.

3. Correct Option:
From the given choices, the orbitals raised to higher energy are , , and .

Final Answer:
The correct option is .

The d orbital in chemistry is known for its unique shape. Understanding the shapes of atomic orbitals is key to grasping molecular geometry and bond formation. The options provided describe different shapes. Let's examine these:

• Dumb bell: This shape describes p orbitals, which have two lobes separated by a nodal plane passing through the nucleus.
• Double dumb bell: This accurately represents the shape of d orbitals. Each d orbital consists of four lobes (except for the d_z² orbital, which has a different shape) arranged in a cloverleaf pattern, hence the "double dumb bell" description.
• Spherical: This shape pertains to s orbitals, which are perfectly spherical around the nucleus.
• Linear: This shape is not associated with any atomic orbitals but is rather a description of certain molecular geometries like diatomic molecules.

Considering the characteristics and configurations, the shape of the d orbital is Double dumb bell.