Understanding Orbital Shapes
When discussing atomic orbitals, the quantum number "l" (azimuthal quantum number) plays a crucial role in determining the shape of the orbital. In this context, when "l" equals 1, it indicates a specific type of orbital.

Orbital Types Based on "l" Value
- The value of "l" can take on integer values from 0 to n-1, where "n" is the principal quantum number.
- Each value of "l" corresponds to a different type of atomic orbital:
- **l = 0**: s orbital (spherical shape)
- **l = 1**: p orbital (dumbbell shape)
- **l = 2**: d orbital (double dumbbell shape)
- **l = 3**: f orbital (complex shape)

For l = 1: The Dumbbell Shape
- The p orbitals, which correspond to l = 1, are characterized by their dumbbell shape.
- This shape features two lobes on either side of the nucleus, resembling a figure-eight or a dumbbell.
- The orientation of the p orbitals can be along the x, y, or z axes, denoted as px, py, and pz, respectively.

Key Characteristics of p Orbitals
- **Shape**: Dumbbell-shaped with two lobes.
- **Nodal Plane**: There is a nodal plane where the probability of finding an electron is zero, located between the two lobes.
- **Electron Density**: The electron density is concentrated in the lobes, which affects chemical bonding and molecular geometry.
In summary, the orbital with l = 1 is indeed a p orbital, which is characterized by a dumbbell shape, making option 'B' the correct answer.