[Ar] 3d3 4s2
Or, expanded:
1s2 2s2 2p6 3s2 3p6 3d3 4s2
The bipositive ion of strontium takes the electron configuration of xenon.
Potassium tends to lend electrons rather than borrow them. As an alkali metal, it has a single electron in its outermost shell, which it readily loses to achieve a stable electron configuration. This electron loss allows potassium to form positively charged ions (K⁺) during chemical reactions, particularly with nonmetals.
Atoms can have as many electron shells as they need. The first electron shell can only contain 2 electrons but the rest can contain 8. Electron arrangement patterns down a group : the # of complete electrons shells increases by 1. The # of group is the same as the # of electrons in the outer shell. (ex. Group 2 there will be 2 electrons in the outer shell) Electron arrangement patterns across a period : the # of complete electron shells stays the same. The # of electrons increases by 1 each time. When a new period starts, that's when a new shell is added. Hope this was helpful :)
The electric field is stronger near the electron and becomes weaker as the distance from the electron increases.
An Ion. More specifically if it gains an electron it becomes an anion and it it loses an electron it becones an cation (pronounced Kat-ion)
The electron configuration for oxygen is [He]2s2.2p4.The electron configuration for sulfur is [Ne]3s2.3p4.
A cation has a depleted electron configuration.
The electron configuration for beryllium, Be, is 1s22s2.
The electronic configuration of einsteinium is: [Rn]5f11.7s2.
The electron configuration of francium is [Rn]7s1.
Hydrogen electron configuration will be 1s1.
Uranium electron configuration: [Rn]5f36d17s2
The electron configuration of beryllium is 1s2 2s2.
The electron configuration for germanium is [Ar]3d10.4s2.4p2.
The electron configuration of boron is [He]2s2.2p1.
The electron configuration for V3 is Ar 3d2.
The electron configuration of V3 is Ar 3d2.