Question

Discuss the similarities and differences between a \(1 s\) and a \(2 s\) orbital.

Short answer

Both \(1 s\) and \(2 s\) orbitals are spherically shaped and can hold up to two electrons. However, the \(2 s\) orbital is larger and has a higher energy level than the \(1 s\) orbital.

Step-by-step solution

Understanding Orbitals

In atoms, electrons are located in areas called electron clouds or orbitals. The \(s\) orbital is a type of atomic orbital that is spherical in shape and it has different sizes and energy levels. The \(1 s\) and \(2 s\) orbitals are two types of \(s\) orbitals.

Discussing Similarities

In terms of similarities, both the \(1 s\) and \(2 s\) orbitals are spherically shaped. This is a common characteristic for all \(s\) orbitals. Both orbitals can also hold up to two electrons.

Discussing Differences

Despite their similarities, there are noticeable differences between the two orbitals. The major differences are in terms of size and energy level. The \(2 s\) orbital is larger in size and higher in energy level compared to the \(1 s\) orbital. Specifically, electrons in the \(2 s\) orbital are found further away from the nucleus compared to those in the \(1 s\) orbital.