‘The electron configuration of nitrogen is 1s2 2s2 2p3 How many more electrons does nitrogen need to have full and stable outer energy level
The Correct Answer and Explanation is:
The electron configuration of nitrogen is 1s² 2s² 2p³. To determine how many more electrons nitrogen needs to have a full and stable outer energy level, we first need to consider the number of electrons nitrogen currently has in its second energy level (the outermost shell).
In nitrogen’s configuration, the 2s and 2p orbitals make up the second energy level:
- 2s² means there are 2 electrons in the 2s orbital.
- 2p³ means there are 3 electrons in the 2p orbital.
This gives a total of 5 electrons in the second energy level.
The second energy level can hold a maximum of 8 electrons (since the s orbital can hold 2 electrons and the p orbital can hold 6 electrons). To fill the second energy level and make it stable, nitrogen needs to reach 8 electrons in this level. Therefore, nitrogen needs 3 more electrons (8 – 5 = 3) to complete its outermost energy level.
These 3 electrons would complete the 2p orbital, which can hold a total of 6 electrons, making the outer shell full and stable. This is similar to how noble gases, such as neon, have a stable outer energy level with 8 electrons.
In summary, nitrogen needs 3 more electrons to have a full and stable outer energy level, completing its 2p orbital and achieving a stable electron configuration.
