Answer
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Step 1:
In the case of a nitrogen (N) atom, which has 7 electrons, we need to add 3 electrons to form an anion with a -1 charge, denoted as N${}^{-}$.
To form an anion, electrons are added to the neutral atom.
Step 2:
The atomic number of nitrogen is 7, which means it has 7 protons in its nucleus. The principal quantum number (n) for nitrogen is 2, as it has a full 1s subshell and 2s and 2p subshells that can accommodate more electrons.
Step 3:
When adding electrons to form an anion, we first fill up the existing subshells before moving on to the next principal quantum number. In this case, we need to add 3 electrons to the 2p subshell.
Step 4:
The 2p subshell can hold a maximum of 6 electrons, with 2 electrons having opposite spins in each of the three 2p orbitals (2p${}_{x}$, 2p${}_{y}$, and 2p${}_{z}$).
After adding the 3 electrons, the 2p subshell will have 5 electrons, and each orbital will have 2 electrons.
Step 5:
Therefore, the 2p subshell is the subshell added to form an N${}^{-}$ anion.
Final Answer
The 2p subshell is added to form an N${}^{-}$ anion.
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