Ground state electronic configuration of nitrogen atom can be represented by

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Explanation

To determine the ground state electronic configuration of a nitrogen atom, we can follow these steps:

### Step 1: Identify the Atomic Number
The atomic number of nitrogen (N) is 7. This means that a nitrogen atom has 7 electrons.

### Step 2: Fill the Electron Shells
Electrons are filled into the atomic orbitals according to the Aufbau principle, which states that electrons occupy the lowest energy orbitals first. The order of filling is as follows:
1. 1s
2. 2s
3. 2p

### Step 3: Fill the 1s Orbital
The 1s orbital can hold a maximum of 2 electrons. Thus, we fill it completely:
- 1s² (2 electrons)

### Step 4: Fill the 2s Orbital
Next, we fill the 2s orbital, which can also hold a maximum of 2 electrons:
- 2s² (2 electrons)

### Step 5: Fill the 2p Orbital
Now, we have 3 electrons left to place in the 2p orbital. The 2p orbital can hold a maximum of 6 electrons, and we will place the 3 electrons in the 2p orbital:
- 2p³ (3 electrons)

### Step 6: Write the Complete Electronic Configuration
Combining all the filled orbitals, the ground state electronic configuration of a nitrogen atom is:
- **1s² 2s² 2p³**

### Step 7: Consider Electron Spin
According to Hund's rule of maximum multiplicity, when electrons occupy degenerate orbitals (like the three 2p orbitals), they will fill each orbital singly with parallel spins before pairing up. Therefore, the 2p electrons will have parallel spins.

### Final Answer
The ground state electronic configuration of a nitrogen atom can be represented as:
- **1s² 2s² 2p³**

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