(c) What can you say about the average distance from the nucleus of an electron in a 2s orbital as compared with a 3s orbital?

Key Concepts

Atomic Orbitals

Atomic orbitals are regions around the nucleus of an atom where electrons are likely to be found. Each orbital is defined by a set of quantum numbers, which describe its shape, size, and orientation. The 's' orbitals are spherical in shape, with the 2s and 3s orbitals representing different energy levels, where the principal quantum number (n) indicates the energy level and size of the orbital.

Principal Quantum Number (n)

The principal quantum number (n) is a key quantum number that determines the energy level and size of an electron's orbital. As n increases, the average distance of the electron from the nucleus also increases, leading to larger orbitals. For example, a 3s orbital has a higher principal quantum number than a 2s orbital, indicating that electrons in the 3s orbital are, on average, found further from the nucleus than those in the 2s orbital.

Electron Density and Probability Distribution

Electron density refers to the likelihood of finding an electron in a particular region around the nucleus. The probability distribution of an electron in an orbital can be visualized using electron density maps. In the case of 2s and 3s orbitals, the 3s orbital has a larger volume and a greater average distance from the nucleus, reflecting a higher probability of finding the electron farther away compared to the 2s orbital.