Which of the following sets of quantum numbers is correct for an electron in 2p-orbtial ?

Options

A. n = 2
B. l = 1
C. m = -1 to +1
D. all are possible

Answer

To determine the correct set of quantum numbers for an electron in a 2p orbital, we need to analyze each quantum number step by step.

### Step 1: Identify the Principal Quantum Number (n)
The principal quantum number (n) indicates the main energy level or shell of an electron. For a 2p orbital, the principal quantum number is:
- **n = 2**

### Step 2: Identify the Azimuthal Quantum Number (l)
The azimuthal quantum number (l) describes the subshell and is related to the shape of the orbital. The values of l are:
- l = 0 for s orbitals
- l = 1 for p orbitals
- l = 2 for d orbitals
- l = 3 for f orbitals

Since we are dealing with a 2p orbital:
- **l = 1**

### Step 3: Identify the Magnetic Quantum Number (m or ml)
The magnetic quantum number (m) indicates the orientation of the orbital in space. The possible values of m range from -l to +l, including zero. For l = 1 (p orbital), the possible values of m are:
- m = -1, 0, +1

Thus, for the 2p orbital:
- **m can be -1, 0, or +1**

### Step 4: Identify the Spin Quantum Number (s)
The spin quantum number (s) describes the intrinsic spin of the electron and can take on one of two values:
- **s = +1/2 or -1/2**

### Summary of Quantum Numbers for 2p Orbital
Putting it all together, the quantum numbers for an electron in a 2p orbital can be summarized as follows:
- n = 2
- l = 1
- m = -1, 0, or +1
- s = +1/2 or -1/2

### Conclusion
Therefore, any set of quantum numbers that includes n = 2, l = 1, m = -1, 0, or +1, and s = +1/2 or -1/2 is valid for an electron in a 2p orbital.