Question

draw: draw the orbital diagram for the following elements. be sure to label the orbitals below the boxes (ie. 1s, 2s, etc...) 14.) lithium

Explanation:

Step1: Determine the atomic number of lithium

The atomic number of lithium (\(Li\)) is \(3\). This means a neutral lithium atom has \(3\) electrons.

Step2: Apply the Aufbau principle

The Aufbau principle states that electrons fill orbitals in order of increasing energy. The order is \(1s<2s < 2p<3s<3p<4s<3d\cdots\).
For \(n = 1\), the \(1s\) sub - shell (1 orbital, \(l = 0\)) is filled first. It can hold a maximum of \(2\) electrons.
For \(n=2\), the \(2s\) sub - shell (1 orbital, \(l = 0\)) is filled next.

Step3: Fill the orbitals with electrons

• The \(1s\) orbital: We put \(2\) electrons in the \(1s\) orbital. According to the Pauli exclusion principle, each electron has an opposite spin. So, we represent the \(1s\) orbital as \(\uparrow\downarrow\) (labeled \(1s\) below the box).
• The \(2s\) orbital: After filling the \(1s\) orbital, we have \(3- 2=1\) electron left. We put this electron in the \(2s\) orbital. Since there is only one electron in the \(2s\) orbital, it is represented as \(\uparrow\) (labeled \(2s\) below the box).

Answer:

The orbital diagram for lithium has a \(1s\) orbital (labeled \(1s\) below its box) with two electrons (\(\uparrow\downarrow\)) and a \(2s\) orbital (labeled \(2s\) below its box) with one electron (\(\uparrow\)).