In each of the following questions a Statement of Assertion (A ) is given followed by a corresponding statement of Reason (R ) Just below it . Of the statement mark the correct answer as
Assertion .The ionization of s- electron requires more energy than ionization of p- electron of the same shell
Reason. s- electrons are closer to the nucleus than p- electrons and hence are more strongly attracted by the nuclues .

Explanation

To solve the question, we need to analyze both the Assertion (A) and the Reason (R) given:

### Step 1: Understand the Assertion
The assertion states that "The ionization of s-electron requires more energy than ionization of p-electron of the same shell."

- **Ionization energy** is the energy required to remove an electron from an atom.
- In the same shell, s-electrons are generally more stable and closer to the nucleus than p-electrons.

### Step 2: Understand the Reason
The reason states that "s-electrons are closer to the nucleus than p-electrons and hence are more strongly attracted by the nucleus."

- This is true because the s-orbital has a spherical shape and is located closer to the nucleus compared to the p-orbitals, which have a dumbbell shape and are found at a higher energy level in the same shell.

### Step 3: Evaluate the Assertion and Reason
- Since s-electrons are indeed closer to the nucleus, they experience a stronger electrostatic attraction to the positively charged nucleus.
- This means that it requires more energy to remove an s-electron than a p-electron from the same shell.

### Conclusion
- Therefore, the assertion is **incorrect** because it states that ionization of s-electron requires more energy than that of p-electron, which is not true.
- The reason is **correct** as it accurately describes the relative positions of s and p electrons in terms of their proximity to the nucleus.

### Final Answer
- The correct answer is: **Assertion is false, Reason is true.**

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