Which electron configuration represents the electrons of a sulfur atom in an excited state? Choice number 2 (1) 2-6-6 (3) 2-8-4 (2) 2-7-7 (4) 2-8-6 I NEED HELP FAST
The Correct Answer and Explanation is:
The correct electron configuration for an excited state of sulfur would be (2) 2-7-7.
Here’s why:
Sulfur (S) in its ground state has an atomic number of 16, meaning it has 16 electrons. The electron configuration for sulfur in its ground state is:
- 1s² 2s² 2p⁶ 3s² 3p⁴, which corresponds to (2-8-6).
In an excited state, one or more electrons will be promoted to a higher energy level.
Let’s break down the choices:
- 2-6-6: This configuration suggests that the second shell has 6 electrons, and the third shell has 6 electrons. However, this does not fit the total of 16 electrons for sulfur, so this cannot represent a valid excited state.
- 2-7-7: This is the correct answer. This configuration implies that one of the 3p electrons in the third shell has been promoted to the 4s orbital, resulting in 7 electrons in both the second and third shells. This is an excited state where the electron in the 3p orbital has gained enough energy to move to a higher orbital, which increases the energy level of the atom.
- 2-8-4: This configuration represents a sulfur atom with 14 electrons, not 16, which means it’s incorrect for sulfur in any state (ground or excited).
- 2-8-6: This is the ground state configuration of sulfur, where all the electrons are in their lowest possible energy levels. It doesn’t represent an excited state.
Conclusion:
The correct choice is (2) 2-7-7, because in an excited state, one of the 3p electrons has been promoted to a higher energy level (like the 4s orbital).
