Which of the following describes an s orbital?

The s orbital is characterized by its spherical shape, which means that the probability distribution of finding an electron is uniform in all directions around the nucleus. This spherical symmetry is a fundamental property of s orbitals and indicates that there are no angular nodes present within the orbital. As a result, electrons in an s orbital are equally likely to be found at various distances from the nucleus in any direction.

In contrast, the other shapes mentioned—dumbbell, complex, and zigzag—are associated with different types of atomic orbitals. For example, the dumbbell shape corresponds to p orbitals, which have two lobes on either side of the nucleus. The complex shapes usually refer to d and f orbitals that exhibit more intricate arrangements with multiple lobes and angular nodes. The zigzag shape does not correspond to any standard atomic orbital shape in quantum chemistry.

The distinction of the s orbital’s spherical symmetry is crucial in understanding electron configurations and the structure of atoms, which is essential for predicting chemical behavior and bonding.