Multiple Choice
You will not need to memorize the quantum numbers for each element because you can see them in:
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10. Periodic Properties of the Elements
The Electron Configuration
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Which of the following is the correct electron configuration for a neutral nitrogen (N) atom?
A
1s^2 2s^2 2p^4
B
1s^2 2s^2 2p^6
C
1s^2 2s^2 2p^3
D
1s^2 2s^2 2p^5
Verified step by step guidance1
Step 1: Determine the atomic number of nitrogen (N). The atomic number tells us the number of electrons in a neutral atom. For nitrogen, the atomic number is 7, so it has 7 electrons.
Step 2: Recall the order in which electron orbitals are filled according to the Aufbau principle: 1s, 2s, then 2p. Each orbital can hold a specific maximum number of electrons: 1s and 2s can hold 2 electrons each, and the 2p subshell can hold up to 6 electrons.
Step 3: Begin filling the orbitals with the 7 electrons of nitrogen. First, fill the 1s orbital with 2 electrons: $1s^{2}$. Then fill the 2s orbital with 2 electrons: $2s^{2}$. This accounts for 4 electrons so far.
Step 4: Place the remaining 3 electrons in the 2p subshell. Since 2p can hold up to 6 electrons, and nitrogen has 3 electrons left, the configuration for 2p will be $2p^{3}$.
Step 5: Combine all parts to write the full electron configuration for nitrogen: $1s^{2} 2s^{2} 2p^{3}$. This matches the correct electron configuration for a neutral nitrogen atom.
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