Question

Explain how a ground-state electron configuration differs from an excited state electron configuration.

a) In a ground state, electrons are in lower energy levels, while in an excited state, electrons move to higher energy levels.
b) In a ground state, electrons are in higher energy levels, while in an excited state, electrons move to lower energy levels.
c) In a ground state, electrons have more energy than in an excited state.
d) In a ground state, electrons have less energy than in an excited state.

Answer 1

A ground-state electron configuration has electrons in the lowest available energy levels, while in an excited state, electrons have absorbed energy and are at higher energy levels. A photon's absorption raises electrons to an excited state, which have more potential and kinetic energy than ground state electrons.

Step-by-step explanation:

The difference between a ground-state electron configuration and an excited state electron configuration relates to the energy levels at which electrons reside within an atom. In the ground state, electrons occupy the lowest available energy levels, whereas in an excited state, the electrons have absorbed energy and moved to higher energy levels. Energy-level diagrams demonstrate this concept by plotting energy vertically, with the ground state at the bottom and excited states above. The absorption of a photon raises an electron from the ground state to an excited state, resulting in more potential and kinetic energy. When the electron falls back to a lower energy level, it emits energy, typically as a photon.

Therefore, the correct answer to the student's question is: a) In a ground state, electrons are in lower energy levels, while in an excited state, electrons move to higher energy levels.