The general outer electronic configuration of transition metals is

Options

A. `ns^(2) nd^(1-10)`
B. `ns^(2) np^(1) (n-1) d^(1-10)`
C. `ns^(2) np^(6) (n-1) d^(1-1)`
D. `ns^(0-2) (n-1) d^(1-10)`

Explanation

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

### Step 1: Understand the Definition of Transition Metals
Transition metals are elements found in the d-block of the periodic table. They are characterized by the presence of d electrons in their outermost shells.

### Step 2: Identify the General Electronic Configuration
The general outer electronic configuration of transition metals can be expressed as:
\[ \text{(n-1)d}^{1-10} \text{ns}^{0-2} \]
Where:
- \( n \) is the principal quantum number of the outermost shell.
- \( (n-1)d \) indicates that the d subshell is being filled.
- \( ns \) indicates that the s subshell of the outermost shell can hold up to 2 electrons.

### Step 3: Analyze the Electron Filling Order
Transition metals typically have:
- 1 to 10 electrons in the d subshell (from \( d^1 \) to \( d^{10} \)).
- 0 to 2 electrons in the s subshell (from \( s^0 \) to \( s^2 \)).

### Step 4: Provide Examples
For example:
- Scandium (Sc) has the electronic configuration: \[ \text{[Ar]} 4s^2 3d^1 \]
- Titanium (Ti) has the electronic configuration: \[ \text{[Ar]} 4s^2 3d^2 \]

These examples illustrate how the general configuration applies to specific transition metals.

### Conclusion
Thus, the general outer electronic configuration of transition metals is:
\[ \text{(n-1)d}^{1-10} \text{ns}^{0-2} \]

---