The element (noble gas) Krypton
Krypton and Selenide ion have 36 electrons and are isoelectronic
None. The Se2- ion is isoelectronic with Krypton.
Oxygen, O ,and selenium Se. O (oxygen) would have to gain two electrons in order to achieve the same number of electrons as Ne (neon, a noble gas). Selenium would gain two to achieve the same number of electrons as Kr, krypton (noble gas). They would form the oxide, O2- and selenide Se2- ions
Se2- 1s22s22p63s23p64s23d104p6
Options are not given in the question. But the following species will have the same electronic configuration as Br- ion: Neutral atom: Kr Cations: Rb+, Sr2+ Anion: Se2-
Krypton and Selenide ion have 36 electrons and are isoelectronic
None. The Se2- ion is isoelectronic with Krypton.
Se2- is incorrect the answer is As 3-
Oxygen, O ,and selenium Se. O (oxygen) would have to gain two electrons in order to achieve the same number of electrons as Ne (neon, a noble gas). Selenium would gain two to achieve the same number of electrons as Kr, krypton (noble gas). They would form the oxide, O2- and selenide Se2- ions
Se2-
SELENIDE
A selenide contain the anion Se(2-).
The oxidation states of selenium are: -2, +2, +4, +6.
O, O2-, S2-, and Se2-O is smaller than O2- because O2- has 2 extra electrons but the same amount of protons as O, so they are held less tightly and the atom is bigger. Atom size increases as you move down the periodic table, so O2- < S2- < Se2-.
Formula: Se2-
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-
Se2- 1s22s22p63s23p64s23d104p6