Final answer:
The electron configuration for a neutral phosphorus atom is 1s²2s²2p⁶3s²3p³.
Step-by-step explanation:
Electronic Configuration of Phosphorus Atoms
To write the electron configuration for a neutral atom of phosphorus, we need to distribute its 15 electrons across the available atomic orbitals following the aufbau principle. These electrons are placed in the orbitals in order of increasing energy levels.
The first two electrons will fill the 1s subshell, giving us 1s². Next, two electrons will fill the 2s subshell, resulting in 2s². Six electrons will then go into the 2p subshell: 2p⁶. After the second energy level is filled, we move to the third energy level where two electrons will fill the 3s subshell, giving us 3s². Finally, the remaining three electrons will occupy the 3p subshell, resulting in 3p³.
Combining all of these together, the electron configuration for a neutral phosphorus atom is 1s²2s²2p⁶3s²3p³.