Question
Question 2 (1 point) Which electron configuration represents the electrons of an atom of neon (atomic number 10) in an excited state? a \( \quad 2-7-1 \) b \( \quad 2-8-1 \) c \( \quad 2-7 \) d \( \quad 2-8 \)
Ask by Hanson Howell. in the United States
Feb 25,2025
Upstudy AI Solution
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Answer
The correct electron configuration for neon in an excited state is 2-7-1.
Solution
The ground-state electron configuration for neon (atomic number 10) is 2 electrons in the first energy level and 8 electrons in the second energy level (2-8). In an excited state, one of the electrons is promoted to a higher energy level. Removing one electron from the second shell (leaving 7 there) and placing it into a third shell gives the configuration 2-7-1, which still totals 10 electrons.
Thus, the correct answer is (a) 2-7-1.
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Simplify this solution Bonus Knowledge
In the excited state, electrons can be found in higher energy levels than in their ground state configuration. For neon, the ground state configuration is \( 2-8 \), where all electrons are in the lowest available energy levels. So, if you see a configuration with one or more electrons moved to a higher energy level, that will indicate an excited state. The correct answer for an excited state configuration would be option a \( 2-7-1 \) or b \( 2-8-1 \). Both show the presence of an electron in a higher energy level.
