Question

(b) 1s and 2s orbitals are different in the following ways: symmetry around the nucleus holds a maximum of two electrons orbital shape distance of electrons from the nucleus size of the orbital

Explanation:

• Symmetry around the nucleus: Both \(1s\) and \(2s\) orbitals are spherically symmetric around the nucleus. So this is not a difference.
• Holds a maximum of two electrons: Any \(s\) - orbital (including \(1s\) and \(2s\)) can hold a maximum of 2 electrons. So this is not a difference.
• Orbital shape: Both \(1s\) and \(2s\) orbitals are spherical in shape. So this is not a difference.
• Distance of electrons from the nucleus: The principal quantum number \(n\) represents the energy level and the average distance of the electron from the nucleus. For \(n = 1\) (\(1s\) orbital) and \(n=2\) (\(2s\) orbital), electrons in the \(2s\) orbital are, on average, farther from the nucleus than electrons in the \(1s\) orbital.
• Size of the orbital: As \(n\) increases, the size of the orbital increases. Since \(n = 2\) for the \(2s\) orbital and \(n = 1\) for the \(1s\) orbital, the \(2s\) orbital is larger than the \(1s\) orbital.

Answer:

distance of electrons from the nucleus, size of the orbital