Sketch the shape and orientation of the following types of orbitals: (a) s.

Verified step by step guidance

1. Understand that an 's' orbital is a type of atomic orbital that is spherical in shape.
2. Recognize that the 's' orbital is centered around the nucleus of an atom, with no directional preference, meaning it is non-directional.
3. Visualize the 's' orbital as a sphere where the probability of finding an electron is the same at any point equidistant from the nucleus.
4. Note that the size of the 's' orbital increases with the principal quantum number (n), so a 1s orbital is smaller than a 2s orbital, and so on.
5. Remember that the 's' orbital can hold a maximum of 2 electrons, which must have opposite spins according to the Pauli exclusion principle.

Key Concepts

Atomic Orbitals

Atomic orbitals are regions in an atom where there is a high probability of finding electrons. They are defined by quantum mechanics and come in various shapes and sizes, corresponding to different energy levels. The most common types of orbitals are s, p, d, and f, each with unique characteristics that influence the chemical behavior of atoms.

Shape of s Orbitals

s orbitals are spherical in shape and are the simplest type of atomic orbital. They have no angular nodes, meaning the probability of finding an electron is uniform in all directions around the nucleus. The size of the s orbital increases with the principal quantum number, indicating that higher energy s orbitals are larger and can accommodate electrons further from the nucleus.

Orientation of Orbitals

The orientation of orbitals refers to how they are positioned in three-dimensional space relative to each other. For s orbitals, there is no directional orientation since they are spherical. In contrast, p orbitals have specific orientations along the x, y, and z axes, which is important for understanding how atoms bond and interact in molecules.