Multiple Choice
Which element has the ground state electron configuration [Ar] 4s^2 3d^{10} 4p^5?
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10. Periodic Properties of the Elements
The Electron Configuration
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Which of the following electron configurations represents an excited-state nitrogen atom?
A
1s^2 2s^1 2p^4
B
1s^2 2s^2 2p^1 3s^2
C
1s^2 2s^2 2p^2 3s^1
D
1s^2 2s^2 2p^3
Verified step by step guidance1
Recall that the ground-state electron configuration of a nitrogen atom (atomic number 7) is $1s^2 2s^2 2p^3$, meaning the electrons fill the lowest energy orbitals first according to the Aufbau principle.
Understand that an excited state occurs when one or more electrons absorb energy and move to a higher energy orbital, resulting in a configuration different from the ground state but still following the Pauli exclusion principle and Hund's rule.
Examine each given configuration to see if it deviates from the ground state by having electrons promoted to higher energy orbitals or rearranged within the same shell in a way that is not the lowest energy arrangement.
For example, check if any electron from the $2s$ or $2p$ orbitals is moved to a higher orbital like $3s$, or if the distribution of electrons in $2s$ and $2p$ orbitals is altered from the ground state pattern.
Identify the configuration(s) where electrons occupy higher energy orbitals or have an unusual distribution compared to the ground state, which indicates an excited state.
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