Multiple Choice
Which of the following is true when drawing a box (orbital) diagram for the electron configuration of an atom?
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10. Periodic Properties of the Elements
The Electron Configuration
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Which of the following represents the correct electron configuration for a neutral atom of vanadium (atomic number 23)?
A
1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^4
B
1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^1
C
1s^2 2s^2 2p^6 3s^2 3p^6 3d^4 4s^2
D
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3
Verified step by step guidance1
Identify the atomic number of vanadium, which is 23. This means a neutral vanadium atom has 23 electrons to be placed in orbitals according to the Aufbau principle.
Recall the order of orbital filling based on increasing energy: 1s, 2s, 2p, 3s, 3p, 4s, then 3d. Electrons fill lower energy orbitals first before moving to higher energy orbitals.
Write the electron configuration by filling orbitals in order until all 23 electrons are assigned: start with 1s^2, then 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, and finally place the remaining electrons in the 3d orbitals.
Count the electrons after filling 1s through 3p orbitals: 2 + 2 + 6 + 2 + 6 = 18 electrons. Subtract this from 23 to find how many electrons remain to fill 4s and 3d orbitals.
Assign 2 electrons to the 4s orbital (since it fills before 3d), then place the remaining electrons in the 3d orbitals. This will give the correct electron configuration for vanadium.
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