Question

According to valence bond theory the metal atom or ion can make use of which of the following orbitals to yield hybrid orbitals, that can form bonds with ligands.

• A. \((n-1)d,\ (n-1)s,\ np\)
• B. \((n-1)d,\ ns,\ np\)
• C. \((n-1)d,\ ns,\ (n-1)p\)
• D. \(nd,\ (n-1)s,\ (n-1)p\)

Hint:

In Valence Bond Theory, hybridization in coordination compounds generally involves: \[ (n-1)d,\ ns,\ np \] orbitals of the central metal ion. These combine to form hybrid orbitals that accommodate ligand lone pairs.

Answer 1

The Correct Option is B

Step 1: Recall the basis of Valence Bond Theory (VBT).
According to Valence Bond Theory, a central metal atom or ion forms coordinate bonds with ligands by using vacant hybrid orbitals.
These hybrid orbitals are formed by mixing suitable atomic orbitals of comparable energies.

Step 2: Identify the orbitals involved in hybridization.
For transition metal complexes, the orbitals generally involved are: \[ (n-1)d,\ ns,\ np \] These orbitals hybridize to form various types of hybrid orbitals such as \[ dsp^2,\ sp^3,\ d^2sp^3,\ sp^3d^2 \] depending upon the coordination number and geometry of the complex.

Step 3: Examine the incorrect options.
The \((n-1)s\) and \((n-1)p\) orbitals are inner-shell orbitals and are not generally involved in the hybridization schemes proposed by VBT for coordination compounds.
Hence options containing \[ (n-1)s \] or \[ (n-1)p \] are incorrect.

Step 4: State the correct orbital set.
Thus, the metal ion utilizes \[ (n-1)d,\ ns,\ np \] orbitals to generate hybrid orbitals that accept lone pairs from ligands.

Step 5: Final conclusion.
Therefore, \[ \boxed{(n-1)d,\ ns,\ np} \] is the correct answer.
Hence, option (2) is correct.