Question

use the periodic table to answer the question.
how would the electron configuration of nitrogen change to make a stable configuration?
(1 point)
it would lose five electrons.
it would gain two electrons.
it would lose four electrons.
it would gain three electrons.

Explanation:

Step1: Determine the electron configuration of nitrogen

Nitrogen has an atomic number of 7. Its electron configuration is \(1s^{2}2s^{2}2p^{3}\). The valence shell (second shell) has 5 electrons (\(2s^{2}2p^{3}\)). A stable configuration (like noble - gas configuration) for the second shell would have 8 electrons.

Step2: Calculate the number of electrons to gain or lose

To reach 8 electrons in the valence shell, if it gains electrons: \(8 - 5=3\). Losing electrons is less favorable as it would require losing 5 electrons (a higher energy - consuming process).

Answer:

It would gain three electrons.