Which of the following electron configurations correspond to an excited state? Identify the atoms and write the full, ground

I think it’s 1s22s23p1 not sure doe

1. Is2 2s2 2p3

2. Nitrogen

Explanation: The number of electron present In C = 6

But an extra electron is added since the charge on C is -1, this therefore makes the total electron 7.

1. By arrangement, the Electronic configuration is therefore;

Ans: 1s2 2s2 2p3

2. It is explained how C has 7 electrons, we can proceed then.

Neutral atom have atomic number of 7.

The element with atomic number of 7 is;

Ans: NITROGEN

- [tex]1s^22s^22p^4[/tex] .

Explanation:- Atomic number for fluorine(F) is 9 and it's electron configuration is [tex]1s^22s^22p^5[/tex] . [tex]F^+[/tex] is formed when F loses one electron from it's valence shell.

[tex]F\rightarrow F^++1e^-[/tex]

Second shell is the valence shell for fluorine and so it loses one electron from 2p to form  [tex]F^+[/tex]  and the electron configuration of the ion becomes [tex]1s^22s^22p^4[/tex] .

Electron configuration is the dissemination of electrons of an atom or molecule in molecular orbitals. Oxygen is composed of eight electrons in its atom, wherein there are two in 1s subshell; then two in 2s subshell; then four in 2p subshell. Its full ground electron configuration is: 1s^2 2s^2 2p^4

Co3+ is Cobalt with three electrons removed (It's positive by 3). So, the abbreviated notation for Cobalt, minus three electrons (Coming from 4s and 3d) is: [Ar]4s1, 3d5