A neutral atom of an element has two K, eight L, nine M and two N electrons then electronic configuration of the element is `"________"`

Answer

To determine the electronic configuration of the element with the given distribution of electrons, we will follow these steps:

### Step 1: Calculate the Total Number of Electrons
The question states that the neutral atom has:
- 2 electrons in the K shell
- 8 electrons in the L shell
- 9 electrons in the M shell
- 2 electrons in the N shell

To find the total number of electrons, we simply add these values together:

\[ \text{Total electrons} = 2 + 8 + 9 + 2 = 21 \]

### Step 2: Determine the Atomic Number
Since the atom is neutral, the number of electrons is equal to the number of protons. Therefore, the atomic number of the element is 21.

### Step 3: Write the Electronic Configuration
Now, we will write the electronic configuration for an atom with atomic number 21. We fill the orbitals according to the Aufbau principle, which states that electrons occupy the lowest energy orbitals first.

1. **1s** can hold 2 electrons: \(1s^2\)
2. **2s** can hold 2 electrons: \(2s^2\)
3. **2p** can hold 6 electrons: \(2p^6\)
4. **3s** can hold 2 electrons: \(3s^2\)
5. **3p** can hold 6 electrons: \(3p^6\)
6. **4s** can hold 2 electrons: \(4s^2\)
7. **3d** can hold 10 electrons, but we only need to fill 1 for this element: \(3d^1\)

Now, we combine these to write the complete electronic configuration:

\[ \text{Electronic Configuration} = 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^1 \]

### Final Answer
Thus, the electronic configuration of the element is:

\[ \text{"1s}^2 \, \text{2s}^2 \, \text{2p}^6 \, \text{3s}^2 \, \text{3p}^6 \, \text{4s}^2 \, \text{3d}^1\text{"} \]

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