Which of the following represents the electronic configuration of d-block elements

Options

A. `(n-1) s^(2)nd^(1-10)`
B. `(n-1)d^(1-10) ns^(1-2)`
C. `(n-1)s^(2) p^(6), ns^(1)`
D. `ns^(2) p^(2) d^(1)`

Answer

To determine the electronic configuration of d-block elements, we need to understand the general characteristics of these elements and their electron configurations. Here’s a step-by-step solution:

### Step 1: Identify the d-block elements
- The d-block elements are found in groups 3 to 12 of the periodic table. These elements are also known as transition metals.

### Step 2: Understand the electronic configuration
- The general electronic configuration of d-block elements can be represented as:
\[ [noble \, gas] \, ns^2 \, (n-1)d^{1-10} \]
Here, \( n \) represents the principal quantum number of the outermost shell.

### Step 3: Analyze the configuration
- The \( ns^2 \) part indicates that there are 2 electrons in the outermost s subshell.
- The \( (n-1)d^{1-10} \) part indicates that the d subshell can hold up to 10 electrons, starting from 1 to 10.

### Step 4: Example configurations
- For example, the electronic configuration of Scandium (Sc, atomic number 21) is:
\[ [Ar] \, 4s^2 \, 3d^1 \]
- For Titanium (Ti, atomic number 22), it is:
\[ [Ar] \, 4s^2 \, 3d^2 \]
- This pattern continues for all d-block elements.

### Conclusion
- The general electronic configuration of d-block elements is \( [noble \, gas] \, ns^2 \, (n-1)d^{1-10} \).