Given below are two statements :
Statement I : In hydrogen atom , the frequency of radiation emitted when an electrin jumps from lower energy orbit `(E_(1))` to higher energy orbit `(E_(2))` to lower energy orbit `(E_(1))` is associated with frequency of radiation given as `f=(E_(2)-E_(1))//h`
This condition is Bohr's frequency condition
In the light of the above statements ,choose the correct answer from the options given below :

Options

A. Both statement I and statement II are true
B. Both statement I and statement II are false
C. Statement I is correct but statement II is false
D. Statement I is incorrect but statement II is true

Answer

To solve the given question, we need to analyze both statements regarding the behavior of electrons in a hydrogen atom according to Bohr's model.

### Step-by-Step Solution:

1. **Understanding Statement I**:
- Statement I claims that when an electron jumps from a lower energy orbit (E1) to a higher energy orbit (E2), the frequency of radiation emitted is given by the formula:
\[ f = \frac{E_2 - E_1}{h} \]
- However, this is incorrect. When an electron moves from a lower energy state to a higher energy state, it **absorbs** energy, not emits it. Therefore, the correct relationship should be:
\[ hf = E_2 - E_1 \]
- This means that the energy absorbed is equal to the difference in energy levels, which contradicts the statement.

2. **Understanding Statement II**:
- Statement II states that when an electron jumps from a higher energy orbit (E2) to a lower energy orbit (E1), the frequency of radiation emitted is given by:
\[ f = \frac{E_2 - E_1}{h} \]
- This statement is correct. When an electron transitions from a higher energy state to a lower energy state, it emits a photon, and the energy of that photon is indeed equal to the difference in energy levels:
\[ hf = E_2 - E_1 \]

3. **Conclusion**:
- Since Statement I is false and Statement II is true, the correct answer is that Statement 1 is incorrect and Statement 2 is correct.

### Final Answer:
- The correct option is: **Statement 1 is incorrect but Statement 2 is true.**

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