The lower the value of `(n+l)` for an orbital, the higher is its energy.
B
If two orbitals have the same value of `(n+l)` the orbital with higher value of n will have lower energy.
C
The energy of an electron in a multi-electron atom depends on quantum number n only
D
The energy of an electron in hudrogen atom depends on quantum number n only
Text Solution
AI Generated Solution
The correct Answer is:
To solve the question of selecting the correct statement regarding atomic structure, we will analyze each statement one by one.
### Step-by-Step Solution:
1. **Statement Analysis**:
- **Statement 1**: "Lower the value of n + l for an orbital, higher is its energy."
- This statement is incorrect. The energy of an orbital increases with an increase in the value of n + l. Therefore, a lower value of n + l corresponds to lower energy.
2. **Statement 2**: "If two orbitals have the same value of n + l, the orbital with higher value of n will have lower energy."
- This statement is also incorrect. If two orbitals have the same n + l value, the orbital with the higher n value will actually have higher energy. For example, comparing 4f and 5d orbitals, both have the same n + l value of 7, but 5d (n=5) has higher energy than 4f (n=4).
3. **Statement 3**: "Energy of electron in a multi-electron atom depends on quantum number n only."
- This statement is incorrect as well. In multi-electron atoms, the energy of an electron depends on both the principal quantum number (n) and the azimuthal quantum number (l). The energy is determined by the sum of n + l.
4. **Statement 4**: "The energy of an electron in a hydrogen atom depends on quantum number n only."
- This statement is correct. In hydrogen and hydrogen-like atoms (like He+, Li2+, etc.), the energy levels depend solely on the principal quantum number (n) because these systems have only one electron, and thus no angular momentum (l) affects the energy.
### Conclusion:
The correct statement is **Statement 4**: "The energy of an electron in a hydrogen atom depends on quantum number n only."
---
