Question

write the complete ground - state electron configuration of bromine. for multi - digit superscripts or coefficients, use each number in succession.

Explanation:

Step1: Determine the atomic number of bromine

The atomic number of bromine (\(Br\)) is \(35\). This means a neutral bromine atom has \(35\) electrons.

Step2: Fill the electron orbitals following the Aufbau principle

• The \(1s\) orbital can hold \(2\) electrons: \(1s^{2}\)
• The \(2s\) orbital can hold \(2\) electrons: \(2s^{2}\)
• The \(2p\) orbital can hold \(6\) electrons: \(2p^{6}\)
• The \(3s\) orbital can hold \(2\) electrons: \(3s^{2}\)
• The \(3p\) orbital can hold \(6\) electrons: \(3p^{6}\)
• The \(4s\) orbital can hold \(2\) electrons: \(4s^{2}\)
• The \(3d\) orbital can hold \(10\) electrons: \(3d^{10}\)
• After filling \(4s\) and \(3d\), we move to \(4p\). Since we have \(35-(2 + 2+6 + 2+6 + 2+10)=3\) electrons left for the \(4p\) orbital: \(4p^{5}\)

Answer:

\(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{5}\)