Is this electron configuration 1s22s22p63p4 correct?
From the Periodic Table the first part of the configuration gives 1s22s22p6 neon (Ne) but after that an outer-shell appears to be missing, could it be possibily 3s23p4 if that's the case the element is sulphur (S)
S: [Ne] 3s23p4
Zinc. The 4s2 is supposed to be written before the 3d10.
Rn
radon
Germanium
lead
Noble Gas Notation: [Ar] 3d10 4s2 Electron Configuration: 1s2, 2s22p6, 3s23p6, 4s23d10 Electron Arrangement in Shell: 2, 8, 18, 2
3d11 is not possible, The element with the electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 is Selenium (Se).
The condensed electron configuration of rubidium is [Kr] 5s1 in the 1st group of period V
The electron configuration of zinc is 1s22s22p63s23p64s23d10
Lithium (Li) has the electron configuration 1s2 2s1.
That is Arsenic.
Bromine
Noble Gas Notation: [Ar] 3d10 4s2 Electron Configuration: 1s2, 2s22p6, 3s23p6, 4s23d10 Electron Arrangement in Shell: 2, 8, 18, 2
3d11 is not possible, The element with the electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 is Selenium (Se).
That's the electron configuration of an atom of molybdenum. Atomic number, 42.
The condensed electron configuration of rubidium is [Kr] 5s1 in the 1st group of period V
The electron configuration of zinc is 1s22s22p63s23p64s23d10
As3- = [Kr] [Kr] =1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
Lithium (Li) has the electron configuration 1s2 2s1.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p1 is the electron configuration for Indium.
The element, indium, is in group 13, period 5 of the periodic table. Thus its electron configuration is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s2 4d10 5p1. This can also be written as [Kr] 4d10 5s2 5p1 since krypton's electron configuration is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s2.
The element that has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 is Bromine