Multiple Choice
In a neutral atom, how many electrons can occupy the electron shell closest to the nucleus (the first shell)?
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10. Periodic Properties of the Elements
The Electron Configuration
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What is the total number of partially occupied 2p orbitals in a nitrogen atom (atomic number 7) in its ground state?
A
1
B
3
C
2
D
0
Verified step by step guidance1
Identify the electron configuration of a nitrogen atom (atomic number 7) in its ground state. Nitrogen has 7 electrons, so write the configuration starting from the lowest energy level: 1s, 2s, then 2p orbitals.
Write the electron configuration explicitly: 1s^2 2s^2 2p^3. This means the first two electrons fill the 1s orbital, the next two fill the 2s orbital, and the remaining three electrons occupy the 2p orbitals.
Recall that the 2p subshell has three degenerate orbitals (2p_x, 2p_y, 2p_z), and according to Hund's rule, electrons will occupy these orbitals singly before pairing up.
Since there are three electrons in the 2p subshell, each electron will occupy a separate 2p orbital, making all three 2p orbitals partially occupied (each with one electron).
Conclude that the total number of partially occupied 2p orbitals in nitrogen's ground state is 3.
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