The correct set of quantum numbers (n, l and m) respectively of the unpaired electron of chloine atom is

Options

A. 2,1,0
B. 2,1,1
C. 3,1,1
D. 3,2,1

Explanation

To determine the correct set of quantum numbers (n, l, and m) for the unpaired electron in a chlorine atom, we can follow these steps:

### Step 1: Determine the Electron Configuration of Chlorine
The atomic number of chlorine (Cl) is 17, which means it has 17 electrons. The electron configuration for chlorine is:
- 1s² 2s² 2p⁶ 3s² 3p⁵

### Step 2: Identify the Last Electron
In the electron configuration, the last unpaired electron is in the 3p orbital. The 3p subshell can hold a maximum of 6 electrons, but in chlorine, it has 5 electrons filled, leaving one unpaired electron.

### Step 3: Determine the Principal Quantum Number (n)
The principal quantum number (n) indicates the energy level of the electron. For the unpaired electron in the 3p orbital:
- n = 3

### Step 4: Determine the Azimuthal Quantum Number (l)
The azimuthal quantum number (l) defines the shape of the orbital. For p orbitals:
- l = 1

### Step 5: Determine the Magnetic Quantum Number (m)
The magnetic quantum number (m) specifies the orientation of the orbital. For p orbitals, the possible values of m are -1, 0, and +1. The unpaired electron in the 3p subshell can occupy any of these orientations. In this case, we can choose:
- m = +1 (this is one of the possible values for the unpaired electron)

### Summary of Quantum Numbers
Thus, the correct set of quantum numbers (n, l, m) for the unpaired electron in a chlorine atom is:
- n = 3
- l = 1
- m = +1

### Final Answer
The correct answer is (3, 1, +1).

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