Aluminum, Al, has 13 electrons. It is in period 3 and group 3A, so it is a P block element with 3 valence electrons. The ground state configuration would be 1s2 2s2 2p6 3s3
1s2, 2s2 2p6 ,3s2 3p1
It is the electron configuration of a neutral, not excited atom.
The ground state electron configuration for nitrogen is [He]2s2.2p3.
The ground state electron configuration of the hydrogen atom is 1s1, and for helium it is 1s2.
Electron configuration of rubidium is 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2,4p6, 5s1 Electrons per shell 2,8,18,8,1 Electron configuration is also represented by [Kr], 5s1. Atomic No. 37, It is Group 1 Alkali metals Period 5 It is an s-block element.
The electron configuration of lead is [Xe]4f14.5d10.6s2.6p2.
The ground state electron configuration for sodium is 1s2 2s2 2p6 3s1
The symbol for sulfur is S. Its electron configuration is 1s22s22p63s23p4
It is the electron configuration of a neutral, not excited atom.
None in the ground state atom, which has an electronic configuration of 1s2
The electron configuration of 1s22s22p3s1 is not the ground state electron configuration of any element. This configuration contains 8 electrons, which in the ground state would be oxygen. The ground state configuration of oxygen is 1s22s22p4.
Antimony, symbol Sb has an atomic number of 51. This is the number of protons in the nucleus of an atom of Sb, and in a neutral atom it is also the number of electrons. The ground state electron configuration for antimony is: 1s22s22p63s23p63d104s24p64d105s25p3
Br = 1s22s22p63s23p64s23d104p5 or shortened to [Ar] 4s23d104p5 and there are 35 electrons total.
Minor quibbling about the format of the question aside, sulfur is the element with that ground state electronic configuration.
Ground state configuration is nothing but the Electronic configuration of the metal in the ground state ie, the thing under normal condition. So, obviously the Ground state configuration of magnesium in [Ne] 3s2 (Atomic number 12).
Ground state electron configuration of zinc (Zn): [Ar]3d104s2.
ground state
[Xe] Normally the electronic configuration for Barium would be [Xe] 6s2, but since you want it for Ba2+, you're missing two electrons. You get rid of the 6s2 and get [Xe].