Multiple Choice
Given the electron configuration 1s^2 2s^2 2p^3, how many unpaired electrons are present in this atom?
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10. Periodic Properties of the Elements
The Electron Configuration
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
How many electrons are required to completely fill all five d orbitals in a given energy level?
A
12
B
8
C
6
D
10
Verified step by step guidance1
Recall that each d subshell consists of 5 orbitals.
Understand that each orbital can hold a maximum of 2 electrons with opposite spins, according to the Pauli exclusion principle.
Calculate the total number of electrons that can fill all 5 d orbitals by multiplying the number of orbitals by the number of electrons per orbital: $5 \times 2$.
This multiplication gives the total electrons needed to completely fill the d subshell.
Conclude that the d subshell can hold 10 electrons when fully occupied.
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