Question

What is the electron configuration of a bromide ion?

Answer 1

Hint: The electron configuration is the distribution of electrons in atomic or molecular orbitals of an atom, molecule, or other physical structure. Atomic electron configurations follow a standard notation in which all electron-containing atomic subshells are arranged in a series.

Complete answer:
Divide the periodic table into parts that display the atomic orbitals, or the regions where electrons are found, to calculate an electron configuration. The s-block is made up of groups one and two, the d-block is made up of groups three to twelve, the p-block is made up of groups thirteen to eighteen, and the f-block is made up of the two rows at the bottom. The energy levels that form the orbitals and electrons are represented by rows one through seven.
Bromine, with the symbol \[Br\] and the atomic number \[35\] , is a chemical element. \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^{10}}4{p^5}\] is the electronic configuration of the bromine atom. We can also write it in the noble gas form as \[\left[ {Ar} \right]4{s^2}3{d^{10}}4{p^5}\] since \[Ar\] is a noble gas. Argon, with the symbol \[Ar\] and the atomic number \[18\], is a chemical element.
The electronic configuration of the bromide ion is \[\left[ {Ar} \right]4{s^2}3{d^{10}}4{p^6}\] since it has acquired one charge by gaining one more electron. We can also write it as \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^{10}}4{p^6}\] .
So, the answer is \[\left[ {Ar} \right]4{s^2}3{d^{10}}4{p^6}\] .

Note:
Remember that the atomic number of Bromine is 35. By helping in the determination of an atom's valence electrons, electron configurations provide insight into the chemical behavior of elements. It also aids in the classification of elements into various blocks.