The electronic configuration of an atom of Nitrogen is 1s\(^2\) 2s\(^2\) 2p\(^1_x\) 2p\(^1_y\) 2p\(^1_z\) because the atom is
in an excited state
undergoing energy changes
unstable and ready to combine with another
simply obeying rules governing electron configuration
Explanation
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The electronic configuration of an atom of Nitrogen is 1s² 2s² 2p³, which means that there are two electrons in the 1s orbital, two electrons in the 2s orbital, and three electrons in the 2p orbitals. The given configuration, 1s² 2s² 2p¹x 2p¹y 2p¹z, is not the ground state configuration of Nitrogen.
The reason for this configuration is that the atom is in an excited state. In an excited state, an electron has absorbed energy and moved to a higher energy level or orbital. In this case, one of the electrons in the 2p orbital has absorbed energy and moved to a higher energy level, resulting in the given configuration.
Therefore, the correct answer is A. in an excited state.
This configuration is characteristic of an atom in an excited state, where an electron has been promoted to a higher energy level.
The best answer for me is A.
MySchool is wrong
The subscripts only appear in the electronic configuration of an atom when the atom is excited
