Chemistry help! Electron Configuration?

Which of the following electron configurations represent an excited state? (Select all that apply.)
1s22s12p63s1
1s12s22p63p3
1s22s22p23d1
1s22s22p64s1
1s22s22p1
1s22s22p63s2
1s1


And one more please!


Enter the ground state configuration for each of the following excited states. Use the noble gas abbreviation of the configuration. Enter the sublevels in the order in which they are filled. For example, type your answer using the format [Ar]4s2 3d10 4p2 for [Ar]4s23d104p2.

1s22s22p33p1

1s22s12p4

1s12s22p63s23p4

Answer:
The only one in the first set of configurations that is not excited is the 1s22s22p63s2. The rest are all in excited states. They are excited because they do not end the configuration with s2 or p6 orbitals.

I believe that you are looking for these answers in the second question:
1s22s22p4 the element would be oxygen but if it is a noble gas [Ne] would be correct.
1s22s22p3 the element would be Nitrogen and again [Ne] would be correct
1s22s22p63s23p3 element would be Phosphorous noble gas would be Ar

ground state for:
[Ne] 1s2 2s2 2p6
[Ar] 1s2 2s2 2p6 3s2 3p6

I hope that this helps you out thanks
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