The electronic configuration of `Sc^(3+)`is:

Explanation

To determine the electronic configuration of the scandium ion \( \text{Sc}^{3+} \), we will follow these steps:

### Step 1: Identify the Atomic Number of Scandium
The atomic number (Z) of scandium (Sc) is 21. This means that a neutral scandium atom has 21 electrons.

### Step 2: Write the Electronic Configuration of Neutral Scandium
The electronic configuration of a neutral scandium atom can be written as:
- First, fill the 1s orbital: \( 1s^2 \)
- Next, fill the 2s orbital: \( 2s^2 \)
- Then, fill the 2p orbitals: \( 2p^6 \)
- After that, fill the 3s orbital: \( 3s^2 \)
- Next, fill the 3p orbitals: \( 3p^6 \)
- Now, fill the 4s orbital: \( 4s^2 \)
- Finally, fill the 3d orbitals: \( 3d^1 \)

So, the complete electronic configuration of neutral Scandium is:
\[ \text{Sc: } 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^1 \]
This can also be represented in shorthand notation as:
\[ \text{Sc: } [\text{Ar}] 3d^1 4s^2 \]
where \([Ar]\) represents the electron configuration of Argon (which has 18 electrons).

### Step 3: Determine the Configuration for \( \text{Sc}^{3+} \)
To find the electronic configuration of \( \text{Sc}^{3+} \), we need to remove 3 electrons from the neutral Scandium configuration.

- The first two electrons to be removed will come from the \( 4s \) orbital (since \( 4s \) is filled before \( 3d \) in the order of filling).
- The third electron will be removed from the \( 3d \) orbital.

So, we remove:
- 2 electrons from \( 4s^2 \) → \( 4s^0 \)
- 1 electron from \( 3d^1 \) → \( 3d^0 \)

After removing these electrons, we are left with:
\[ \text{Sc}^{3+}: [\text{Ar}] \]
This indicates that \( \text{Sc}^{3+} \) has the same electronic configuration as Argon.

### Final Answer
The electronic configuration of \( \text{Sc}^{3+} \) is:
\[ \text{Sc}^{3+}: [\text{Ar}] \]

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