What is the shape of a P-orbital?

The shape of a P-orbital is best described as an elongated dumbbell. This characteristic shape arises due to the presence of two lobes situated on either side of the nucleus, with a node at the nucleus where the probability of finding an electron is zero.

In the context of atomic orbitals, the P-orbital is one of the types of orbitals that describe the regions in space where electrons are likely to be found. It has a specific orientation in three-dimensional space, with each of the three types of P-orbitals (px, py, pz) oriented along different axes (x, y, and z). This configuration enables P-orbitals to overlap with other orbitals, which is crucial for bonding in molecules.

The other options describe shapes that do not accurately represent the P-orbital structure. A spherical shape corresponds to an S-orbital, which does not have the elongated lobes characteristic of P-orbitals. A planar square does not reflect the three-dimensional nature of P-orbitals, and a cylindrical shape is not applicable because the lobes taper into a node rather than forming a continuous cylinder. Thus, the correct characterization of the P-orbital as an elongated dumbbell shape