Question

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

Explanation:

Step1: Determine the atomic number of P

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

Step2: Fill the electron orbitals according to the Aufbau principle

• Fill the \(1s\) orbital first. The \(1s\) orbital can hold \(2\) electrons: \(1s^{2}\).
• Then fill the \(2s\) orbital (holds \(2\) electrons): \(2s^{2}\).
• Next, fill the \(2p\) orbitals. The \(2p\) sublevel has \(3\) orbitals and can hold \(6\) electrons: \(2p^{6}\).
• Then fill the \(3s\) orbital (holds \(2\) electrons): \(3s^{2}\).
• Finally, fill the \(3p\) orbitals. After filling the previous orbitals (\(1s^{2}2s^{2}2p^{6}3s^{2}\), which accounts for \(2 + 2+6 + 2=12\) electrons), there are \(15 - 12 = 3\) electrons left for the \(3p\) sublevel: \(3p^{3}\).

Answer:

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