Answer:
B) [Ne]
Step-by-step explanation:
Note:
Electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals. Electron configurations are typically written in a shorthand notation, using the principal quantum number (n) and the angular momentum quantum number (l) to designate the orbitals.
The four types of electron configurations are:
- s-type orbitals: These orbitals have an angular momentum quantum number of l = 0. The s-orbital can hold up to two electrons.
- p-type orbitals: These orbitals have an angular momentum quantum number of l = 1. The p-orbital can hold up to six electrons.
- d-type orbitals: These orbitals have an angular momentum quantum number of l = 2. The d-orbital can hold up to ten electrons.
- f-type orbitals: These orbitals have an angular momentum quantum number of l = 3. The f-orbital can hold up to fourteen electrons.
The electron configuration of an atom is determined by the Aufbau principle, which states that electrons fill the lowest energy orbitals first.
For the Question:
A neutral nitrogen atom has 7 electrons. When it becomes an N-3 ion, it gains 3 electrons. This gives it a total of 10 electrons, the same as the neon atom. The electron configuration of N-3 is therefore [Ne], which is shorthand for 1s2 2s2 2p6.
The other options are incorrect.
- Ar has 18 electrons,
- Ne has 10 electrons,
- He has 2 electrons, and
- H has 1 electron.