Question

question 9 of 18
give the full electronic configuration for phosphorus.
electronic configuration:

Explanation:

Step1: Determine the atomic number of phosphorus

The atomic number of phosphorus (\(P\)) is \(15\). This means a neutral phosphorus atom has \(15\) electrons.

Step2: Fill the electron - shells and sub - shells according to the Aufbau principle

• The \(1s\) sub - shell can hold a maximum of \(2\) electrons. So, we start with \(1s^{2}\).
• The \(2s\) sub - shell can also hold \(2\) electrons. Then we have \(2s^{2}\).
• The \(2p\) sub - shell can hold \(6\) electrons. So far, we have \(1s^{2}2s^{2}2p^{6}\) (total of \(2 + 2+6=10\) electrons).
• The \(3s\) sub - shell can hold \(2\) electrons. Now we have \(1s^{2}2s^{2}2p^{6}3s^{2}\) (total of \(10 + 2 = 12\) electrons).
• The remaining \(15-12 = 3\) electrons go into the \(3p\) sub - shell.

Answer:

\(1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}\)