Using the s,p,d,f notations, describe the orbitals with the following quantum numbers,
(a) n=1, l=0 (b) n=2, l=1
(c ) n=3, l=0 (d) n=4, l=3
(e ) n=5, l=2

Answer

To solve the problem of describing the orbitals using the s, p, d, f notations based on the given quantum numbers, we will follow these steps:

### Step-by-Step Solution:

1. **Understanding Quantum Numbers**:
- The principal quantum number (n) indicates the energy level or shell.
- The azimuthal quantum number (l) indicates the subshell type:
- l = 0 corresponds to s subshell
- l = 1 corresponds to p subshell
- l = 2 corresponds to d subshell
- l = 3 corresponds to f subshell

2. **(a) For n = 1, l = 0**:
- Here, n = 1 indicates the first energy level.
- l = 0 indicates the s subshell.
- Therefore, the orbital is **1s**.

3. **(b) For n = 2, l = 1**:
- n = 2 indicates the second energy level.
- l = 1 indicates the p subshell.
- Therefore, the orbital is **2p**.

4. **(c) For n = 3, l = 0**:
- n = 3 indicates the third energy level.
- l = 0 indicates the s subshell.
- Therefore, the orbital is **3s**.

5. **(d) For n = 4, l = 3**:
- n = 4 indicates the fourth energy level.
- l = 3 indicates the f subshell.
- Therefore, the orbital is **4f**.

6. **(e) For n = 5, l = 2**:
- n = 5 indicates the fifth energy level.
- l = 2 indicates the d subshell.
- Therefore, the orbital is **5d**.

### Summary of Results:
- (a) n = 1, l = 0 → **1s**
- (b) n = 2, l = 1 → **2p**
- (c) n = 3, l = 0 → **3s**
- (d) n = 4, l = 3 → **4f**
- (e) n = 5, l = 2 → **5d**