How many delectrons can fit in the orbital for which n = 3 and `l` = 1?

Options

A. 10
B. 14
C. 2
D. 6

Explanation

To determine how many electrons can fit in the orbital for which \( n = 3 \) and \( l = 1 \), we can follow these steps:

### Step 1: Identify the Quantum Numbers
The principal quantum number \( n \) is given as 3, and the azimuthal quantum number \( l \) is given as 1.

### Step 2: Determine the Type of Orbital
The azimuthal quantum number \( l \) indicates the type of subshell:
- \( l = 0 \) corresponds to an s-orbital
- \( l = 1 \) corresponds to a p-orbital
- \( l = 2 \) corresponds to a d-orbital
- \( l = 3 \) corresponds to an f-orbital

Since \( l = 1 \), we are dealing with a p-orbital.

### Step 3: Identify the Specific Orbital
For \( n = 3 \) and \( l = 1 \), we are referring to the 3p subshell. The 3p subshell has three degenerate orbitals: \( 3p_x \), \( 3p_y \), and \( 3p_z \).

### Step 4: Determine the Electron Capacity of One Orbital
According to the Pauli Exclusion Principle, each orbital can hold a maximum of 2 electrons, and these electrons must have opposite spins.

### Step 5: Conclusion
Since the question asks for the number of electrons that can fit in a single orbital (not the entire subshell), the answer is that a single p-orbital can hold a maximum of 2 electrons.

Thus, the final answer is:
**2 electrons.**

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