How many number of unpaired electrons are present in `K^(+)` ?

Explanation

To determine the number of unpaired electrons in the potassium ion \( K^+ \), we can follow these steps:

### Step 1: Identify the atomic number of potassium (K)
Potassium (K) has an atomic number of 19. This means it has 19 electrons in its neutral state.

### Step 2: Write the electronic configuration of neutral potassium (K)
The electronic configuration of neutral potassium can be written as:
\[ \text{K: } 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 \]
This can also be represented in a shorthand notation as:
\[ \text{K: } [Ar] 4s^1 \]
where [Ar] represents the electron configuration of argon, which accounts for the first 18 electrons.

### Step 3: Determine the electronic configuration of \( K^+ \)
When potassium loses one electron to form \( K^+ \), it loses the single electron in the 4s subshell. Therefore, the electronic configuration of \( K^+ \) becomes:
\[ \text{K}^+: [Ar] \]
This means that \( K^+ \) has the same electron configuration as argon.

### Step 4: Analyze the electron configuration for unpaired electrons
The electron configuration of argon ([Ar]) is:
\[ 1s^2 2s^2 2p^6 3s^2 3p^6 \]
In this configuration, all the subshells are fully filled. Therefore, there are no unpaired electrons.

### Step 5: Conclusion
Since \( K^+ \) has a complete electron configuration with no unpaired electrons, we conclude that:
\[ \text{Number of unpaired electrons in } K^+ = 0 \]

### Final Answer
The number of unpaired electrons present in \( K^+ \) is **0**.

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