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Arsenic should have 5 electron dots in its Lewis structure, one for each valence electron.
The electron configuration for a neutral arsenic atom is 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^3.
It depends on what elements it combines with and in what arrangement. There are many compounds of arsenic.
Short answer: [Ar] 3d10 4s2 4p3 OR 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3
Arsenic.
[Ar] 4s2 3d10 4p3
The correct electron configuration for arsenic is [Ar] 4s2 3d10 4p3.
Chlorine needs to gain one electron to achieve the same electron arrangement as neon, which has a stable octet (eight valence electrons). By gaining one electron, chlorine will have a full outer shell with eight electrons, resembling the electron arrangement of neon.
The molecular geometry of the arsenate ion (AsO₄³⁻) is tetrahedral. This geometry arises from the arrangement of four oxygen atoms around the central arsenic atom, with bond angles of approximately 109.5 degrees. The ion has a formal charge of -3 due to the presence of one additional electron compared to neutral arsenic.
An electron in an arsenic atom (or an electron in anyatom) will have a charge of -1. That's the characteristic charge of the electron, and all electrons exhibit that characteristic. It is expressed identically in each of the little guys.
The shorthand electron configuration for arsenic (As), which has an atomic number of 33, is [Ar] 4s² 3d¹⁰ 4p³. This notation indicates that arsenic has the same electron configuration as argon (Ar), plus two electrons in the 4s subshell, ten electrons in the 3d subshell, and three electrons in the 4p subshell.
The electron configuration of arsenic is [Ar] 3d10 4s2 4p3. This means that arsenic has 2 electrons in its outermost shell (4s2 4p3) and belongs to the p-block of the periodic table.