argon is because it's the last noble gas used to get to Br.. it's like a short cut, instead of writing 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5 you can skip a lot of it by taking th last noble gas used which is the 3p^6(Ar) and continue from there like so: [Ar] 4s^2 3d^10 4p^5
The electronic configuration of Br atom is [Ar] 4s2 3d10 4p5. Since, bromide ion has gained 1- charge by acquiring one more electron, its electronic configuration is [Ar] 4s2 3d10 4p6.
The electron configuration for Br is [Ar]3d104s24p5.
1s2
2s2 2p6
3s2 3p6
4s2 3d10 4p5
Or
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
Or
[Ar] 4s2 3d10 4p5
The electronic configuration of Br- ion is 1s22s22p63s23p64s23d104p6
Bromine's atomic number is 35. Therefore, it has 35 protons and 35 electrons. Filling in the first 35 electron orbitals gives us 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5.
[Ar] 4s2 3d10 4p5
or
2, 8, 18, 7
7
The pseudo noble-gas electron configuration has the outer three orbitals filled, the s, p and d- s2p6d10 (18 electrons total) and so is fairly stable. Elements that attain this electron configuration are at the right side of the transition metals (d-block). Br-, I-, Se2-
No. No two elements have the same electron configuration.
Every elements have the electrons of an atom distribution or a molecule in molecular orbitals and it is called electron configuration. The element that can be grouped in the family with above electron configuration is called antimony.
These elements are B, Al Br.
Both Li and K lose electrons to get noble gas configuration. Br gains an electron to get noble gas configuration. So K is more likely to form a compound with Br.Potassium is a metal in group 1. It usually forms ionic compounds with other non metallic elements. From these elements, it is more likely to bond with bromine. Recall that lithium is as in the same family as potassium.
The bromide ion, which has a charge of 1-, has one more electron than a neutral bromine atom. Its electron configuration is isoelectric with the noble gas krypton, so it has 36 electrons. Its electron configuration is [Ar]3d10 4s2 4p6. I apologize that the superscripts are not working. I put a space between the different sublevels to make it easier to understand.
The pseudo noble-gas electron configuration has the outer three orbitals filled, the s, p and d- s2p6d10 (18 electrons total) and so is fairly stable. Elements that attain this electron configuration are at the right side of the transition metals (d-block). Br-, I-, Se2-
Electron configuration is a term applied to chemical elements not to compounds.
No. No two elements have the same electron configuration.
Br typically gains one electron to achieve a stable electron configuration, rather than losing electrons.
Every elements have the electrons of an atom distribution or a molecule in molecular orbitals and it is called electron configuration. The element that can be grouped in the family with above electron configuration is called antimony.
These elements are B, Al Br.
The group of elements that have a stable electron configuration are the noble gases.
Both Li and K lose electrons to get noble gas configuration. Br gains an electron to get noble gas configuration. So K is more likely to form a compound with Br.Potassium is a metal in group 1. It usually forms ionic compounds with other non metallic elements. From these elements, it is more likely to bond with bromine. Recall that lithium is as in the same family as potassium.
35Br = [Ar core],4s2,3d10,4p5
Yes it is possible to write the noble gas configuration of all elements, though it is not possible to list all of them here.
Br-, like the other halogens F-, Cl-, Br-, I-. They would obtain one electron to have noble gas electron configuration. Therefore, one negative charge.