Question
How would the electron configuration of nitrogen change to make a stable configuration
A. It would gain two electrons
B. It would lose four electrons
C. It would lose five electrons
D. It would gain three electrons
A. It would gain two electrons
B. It would lose four electrons
C. It would lose five electrons
D. It would gain three electrons
Answers
GPT-4o mini
The electron configuration of nitrogen (atomic number 7) is \(1s^2 2s^2 2p^3\). To achieve a stable electron configuration, nitrogen typically seeks to attain the stable electronic configuration of a noble gas, such as neon, which has 8 electrons in its outer shell.
To achieve this stable configuration, nitrogen would need to gain 3 electrons to fill its 2p subshell, giving it a total of 8 electrons in its outer shell (2 in the 1s and 2 in the 2s and 4 in the 2p, making it \(1s^2 2s^2 2p^6\)).
Therefore, the correct answer is:
**D. It would gain three electrons.**
To achieve this stable configuration, nitrogen would need to gain 3 electrons to fill its 2p subshell, giving it a total of 8 electrons in its outer shell (2 in the 1s and 2 in the 2s and 4 in the 2p, making it \(1s^2 2s^2 2p^6\)).
Therefore, the correct answer is:
**D. It would gain three electrons.**