General electronic configuration of transition metals is

Options

A. `(n-1)d^(1-10)ns^2`
B. `nd^10ns^2`
C. `(n-1)d^10ns^2`
D. `(n-1)d^(1-5)ns^2`

Answer

To determine the general electronic configuration of transition metals, we can follow these steps:

### Step-by-Step Solution:

1. **Understand Transition Metals**: Transition metals are elements found in the d-block of the periodic table. They typically have partially filled d-orbitals.

2. **Identify the General Electronic Configuration**: The electronic configuration for transition metals can be expressed in terms of the principal quantum number (n) and the d-orbital filling.

3. **Write the General Formula**: The general electronic configuration for transition metals is given by:
\[ [\text{Noble gas}] \, (n-1)d^{1-10} \, ns^2 \]
Here, \( n \) represents the principal quantum number of the outermost shell, \( (n-1)d \) represents the d-orbitals that are being filled, and \( ns^2 \) represents the s-orbitals of the outermost shell.

4. **Identify the Range of d-electrons**: The d-orbitals can hold a maximum of 10 electrons, which is why we see \( d^{1-10} \) in the configuration.

5. **Conclusion**: Therefore, the general electronic configuration of transition metals is:
\[ (n-1)d^{1-10} \, ns^2 \]

### Final Answer:
The correct answer is: **(n-1)d^{1-10} \, ns^2**.

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