Assertion : For Balmer series of hydrogen spectrum, the value ` n_(1)=2 and n_(2)=3,4,5`.
Reason : The value of n for a line in Balmer series of hydrogen spectrum having the highest wave length is 4 and 6 .

Options

A. If both the assertion and reason are true and reason is correct explanation of the assertion .
B. If both the assertion and reason are true but reason is not a correct explanation of the assertion .
C. If the assertion is true but the reason is false.
D. If both assertion and reason are false.

Explanation

To solve the question, we will analyze the assertion and reason step by step.

### Step 1: Understanding the Assertion
The assertion states that for the Balmer series of the hydrogen spectrum, the values of \( n_1 \) and \( n_2 \) are \( n_1 = 2 \) and \( n_2 = 3, 4, 5 \).

- **Balmer Series**: This series corresponds to transitions where the electron falls to the second energy level (\( n_1 = 2 \)) from higher levels (\( n_2 = 3, 4, 5, \ldots \)).
- Therefore, the assertion is **true**.

### Step 2: Understanding the Reason
The reason states that for a line in the Balmer series of the hydrogen spectrum having the highest wavelength, the values of \( n \) are 4 and 6.

- To find the wavelength, we use the Rydberg formula:
\[ \frac{1}{\lambda} = R \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right) \]
where \( R \) is the Rydberg constant, \( n_1 = 2 \) for the Balmer series, and \( n_2 \) can be 3, 4, 5, etc.
- The wavelength is highest when the difference \( \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right) \) is minimized, which occurs when \( n_2 \) is at its lowest value (3).
- Thus, the highest wavelength corresponds to \( n_1 = 2 \) and \( n_2 = 3 \), not 4 and 6.

Therefore, the reason is **false**.

### Step 3: Conclusion
Since the assertion is true and the reason is false, we conclude that the correct option is:

**Assertion is true, but reason is false.**

### Final Answer
The correct option is **Option 3**: Assertion is true but reason is false.

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