An orbital with `l = 0` is

Options

A. Symmetrical about X axis only
B. Symmetrical about Y axis only
C. Spherically symmetrical
D. Unsymmetrical

Explanation

To solve the question regarding the orbital with azimuthal quantum number \( l = 0 \), we can follow these steps:

### Step 1: Understand the Quantum Numbers
Quantum numbers are used to describe the properties of atomic orbitals. The azimuthal quantum number \( l \) indicates the shape of the orbital.

### Step 2: Identify the Value of \( l \)
For \( l = 0 \), we need to identify which type of orbital corresponds to this value. The values of \( l \) can be:
- \( l = 0 \): s orbital
- \( l = 1 \): p orbital
- \( l = 2 \): d orbital
- \( l = 3 \): f orbital

### Step 3: Determine the Shape of the Orbital
The s orbital (where \( l = 0 \)) has a specific shape. It is spherical in nature. This means that the probability density of finding an electron is uniform in all directions from the nucleus.

### Step 4: Visualize the Orbital
The s orbital can be visualized as a sphere centered around the nucleus of the atom. The nucleus is at the center, and the electron cloud is distributed evenly around it.

### Conclusion
Thus, an orbital with \( l = 0 \) is an **s orbital**, which has a **spherical shape** centered around the nucleus.

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