Multiple Choice
Give the set of four quantum numbers that represent the indicated electron in each of the following elements.
Cl– (18th electron)
10. Periodic Properties of the Elements
The Electron Configuration: Quantum Numbers
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Consider the following electron configurations to answer the question.(i) 1s22s22p63s23p64s23d104p65s1
(ii) 1s22s22p63s23p5
(iii) 1s22s22p63s23p64s23d8
(iv) 1s22s22p63s23p64s23d104p6
(v) 1s22s22p43s1
An example of an excited state (higher energy level than the ground state) is ________.
A
(i)
B
(ii)
C
(iii)
D
(iv)
E
(v)
Verified step by step guidance1
Understand the concept of electron configurations: Electron configurations describe the distribution of electrons in an atom's orbitals. The ground state is the lowest energy configuration, while an excited state has electrons in higher energy levels than the ground state.
Examine each electron configuration provided: Look for any configurations where electrons are not in the lowest possible energy levels, indicating an excited state.
Analyze configuration (v): 1s²2s²2p⁴3s¹. Notice that the 3s electron is present, which suggests that an electron from the 2p orbital has been excited to the 3s orbital.
Compare configuration (v) with a typical ground state: The ground state for an atom with 9 electrons (like Fluorine) would be 1s²2s²2p⁵. Configuration (v) shows an electron moved from 2p to 3s, indicating an excited state.
Conclude that configuration (v) is an example of an excited state: The presence of an electron in a higher energy orbital (3s) instead of filling the lower energy 2p orbital confirms it is an excited state.
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