Br = 1s22s22p63s23p64s23d104p5
or shortened to [Ar] 4s23d104p5 and there are 35 electrons total.
The electronic configuration of Bromine in its ground state is: 1s2 2s2p6 3s2p6d10 4s2p5. Therefore the principal quantum number for the outermost electrons in a Bromine atom is 4.
The ground state electron configuration for sodium is 1s2 2s2 2p6 3s1
The symbol for sulfur is S. Its electron configuration is 1s22s22p63s23p4
5 valence electrons exist in bromine period, at ground state bromine has 3 valence electrons
ground state
The electronic configuration of Bromine in its ground state is: 1s2 2s2p6 3s2p6d10 4s2p5. Therefore the principal quantum number for the outermost electrons in a Bromine atom is 4.
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
5 valence electrons exist in bromine period, at ground state bromine has 3 valence electrons
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