The correct set of four quantum numbers for the valence electron of rubidium (Z = 37) is

Options

A. 5, 1, 1, `+1//2`
B. 6, 0, 0, `+1//2`
C. 5, 0, 0, `+1//2`
D. 5, 1, 0, `+1//2`

Explanation

To determine the correct set of four quantum numbers for the valence electron of rubidium (Z = 37), we will follow these steps:

### Step 1: Determine the Electronic Configuration
The first step is to write the electronic configuration of rubidium. The atomic number (Z) of rubidium is 37, which means it has 37 electrons. The electronic configuration can be written as follows:

1. Fill the orbitals in the order of increasing energy:
- 1s²
- 2s²
- 2p⁶
- 3s²
- 3p⁶
- 4s²
- 3d¹⁰
- 4p⁶
- 5s¹

Thus, the complete electronic configuration of rubidium is:
**1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s¹**

### Step 2: Identify the Valence Electron
The valence electron is the outermost electron, which in this case is found in the 5s orbital. Therefore, the valence electron of rubidium is in the 5s subshell.

### Step 3: Assign the Principal Quantum Number (n)
The principal quantum number (n) indicates the energy level of the electron. For the 5s electron:
- **n = 5**

### Step 4: Assign the Azimuthal Quantum Number (l)
The azimuthal quantum number (l) defines the shape of the orbital. For an s orbital:
- **l = 0** (since s corresponds to l = 0)

### Step 5: Assign the Magnetic Quantum Number (ml)
The magnetic quantum number (ml) specifies the orientation of the orbital. For an s orbital (where l = 0):
- **ml = 0**

### Step 6: Assign the Spin Quantum Number (ms)
The spin quantum number (ms) indicates the spin of the electron. Electrons can have a spin of +1/2 or -1/2. Since we are considering the first electron in the 5s orbital:
- **ms = +1/2**

### Final Set of Quantum Numbers
Putting it all together, the set of four quantum numbers for the valence electron of rubidium is:
- **n = 5**
- **l = 0**
- **ml = 0**
- **ms = +1/2**

Thus, the correct set of quantum numbers is: **(5, 0, 0, +1/2)**.