Which electron configuration represents the electrons in an atom of sulfur in an excited state? 2 – 8 – 6 2 – 7 – 7
2 – 8 – 7
2 – 7 – 8

The relations of the quantum numbers allow to find that the correct answer for the configuration of the excited state is:

The electronic configuration of the elements is the distribution of electrons and different levels and sublevels fulfilling the relationships between quantum numbers.  

In the base configuration Sulfur of the periodic table is 2 - 8 - 6

This is at the lowest energy configuration, when the atom acquires energy, an electron from its shell must be promoted to the next level.

That is, an electron from level n = 2 that is full is promoted to level n = 3 since in this shell there is still room for two electrons, the configuration of the excited state is:

                  2- 7 - 7

Let's examine the different alternatives:

1) 2 - 8 -6

False, this is the configuration of the base state

2) 2 - 7 - 7

True. An electron is promoted to the next level due to the excitation of the atom

3) 2 - 8 -7

False, in this configuration the atom becomes an ion

4) 2 - 7 - 8

False, there is an electron transfer between two levels, but there is an extra electron that turns that atom into an ion

In conclusion using the relationships of quantum numbers we can find that the correct answer for the excited state configuration is:

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answer.

i think it's 2-7-7

it is a solid

explanation: