Multiple Choice
Which of the following represents the correct electron configuration for a neutral atom of titanium (atomic number 22)?
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10. Periodic Properties of the Elements
The Electron Configuration
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Which of the following represents the correct ground-state electron configuration for vanadium (atomic number 23)?
A
1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5
B
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5
C
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3
D
1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^4
Verified step by step guidance1
Identify the atomic number of vanadium, which is 23. This means vanadium has 23 electrons to be placed in orbitals according to the Aufbau principle.
Recall the order of orbital filling based on increasing energy levels: 1s, 2s, 2p, 3s, 3p, 4s, then 3d. Electrons fill lower energy orbitals first before moving to higher ones.
Fill the orbitals step-by-step with electrons: 1s can hold 2, 2s holds 2, 2p holds 6, 3s holds 2, 3p holds 6, 4s holds 2, and then 3d orbitals start filling.
Sum the electrons as you fill: 2 (1s) + 2 (2s) + 6 (2p) + 2 (3s) + 6 (3p) = 18 electrons filled before reaching 4s and 3d orbitals. You have 5 electrons left to place in 4s and 3d orbitals.
According to the Aufbau principle and Hund's rule, the 4s orbital fills before 3d, so place 2 electrons in 4s and the remaining 3 electrons in 3d, resulting in the configuration $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3$.
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