The orbital angular momentum of electron in the `n_(1)th` shell of element of atomic number `Z_(1) is L_(1)` an the same in the `n_(2)th` shell of element of atomic number `Z_(2) is L_(2)` If `L_(2)gtL_(1)` then

Options

A. `n_(2) gt n_(1)`
B. `Z_(2) gtZ_(1)`
C. `n_(2)Z_(2) gt n_(1)Z_(1)`
D. Both (a) and (b)

Explanation

To solve the problem, we need to analyze the relationship between the orbital angular momentum of electrons in different shells of atoms with different atomic numbers.

### Step-by-Step Solution:

1. **Understanding Orbital Angular Momentum**:
The orbital angular momentum \( L \) of an electron in a shell is given by the formula:
\[ L = n \frac{h}{2\pi} \]
where \( n \) is the principal quantum number (shell number) and \( h \) is Planck's constant.

2. **Expressing Angular Momentum for Different Shells**:
For the \( n_1 \) shell of an element with atomic number \( Z_1 \):
\[ L_1 = n_1 \frac{h}{2\pi} \]
For the \( n_2 \) shell of an element with atomic number \( Z_2 \):
\[ L_2 = n_2 \frac{h}{2\pi} \]

3. **Given Condition**:
We are given that \( L_2 > L_1 \). This implies:
\[ n_2 \frac{h}{2\pi} > n_1 \frac{h}{2\pi} \]
Since \( \frac{h}{2\pi} \) is a constant, we can simplify this to:
\[ n_2 > n_1 \]

4. **Analyzing Atomic Numbers**:
The problem does not provide a direct relationship between the atomic numbers \( Z_1 \) and \( Z_2 \) and the angular momentum. Therefore, we cannot conclude that \( Z_2 > Z_1 \) based solely on the angular momentum comparison.

5. **Conclusion**:
From the above analysis, we can conclude that if \( L_2 > L_1 \), then it must be true that:
\[ n_2 > n_1 \]
However, we cannot make any conclusions about the relationship between \( Z_1 \) and \( Z_2 \).

### Answer:
The correct option is that \( n_2 > n_1 \).