Question

write the full ground state electron configuration of o+.electron configuration:which neutral atom is isoelectronic with o+?neutral atom:

Explanation:

Step1: Determine the number of electrons in \(O^{+}\)

Oxygen (\(O\)) has an atomic number of \(8\), so a neutral \(O\) atom has \(8\) electrons. \(O^{+}\) has lost one electron, so it has \(8 - 1=7\) electrons.

Step2: Write the electron configuration

Using the Aufbau principle (\(1s<2s < 2p<3s<3p<4s<3d<4p\cdots\)), for \(n = 1\), the \(1s\) sub - shell can hold \(2\) electrons (\(1s^{2}\)). For \(n = 2\), the \(2s\) sub - shell can hold \(2\) electrons (\(2s^{2}\)), and the remaining \(7-(2 + 2)=3\) electrons go into the \(2p\) sub - shell (\(2p^{3}\)). So the electron configuration of \(O^{+}\) is \(1s^{2}2s^{2}2p^{3}\).

Step3: Find the isoelectronic neutral atom

An isoelectronic species has the same number of electrons. A neutral atom with \(7\) electrons has an atomic number of \(7\). The element with atomic number \(7\) is nitrogen (\(N\)).

Answer:

electron configuration: \(1s^{2}2s^{2}2p^{3}\)
neutral atom: \(N\)