Mo^3+ = [Kr] 4d^3
Boron has an electronic configuration of 1s22s22p1 (it has 5 electrons). In order to reach the stable electron configuration of a noble gas with a completely filled valence shell, boron atom has to lose 3 electrons to obtain a stable duplet structure (i.e. 2 electrons in its first electron shell). After losing 3 electrons, the boron atom forms a B3+ ion, or a so-called tripositive ion.
The electron configuration for the Co2 ion is Ar 3d7.
The electron configuration of a V3 ion is Ar 3d2.
The electron configuration of the Co2 ion is Ar 3d7.
The electron configuration of an Sc2 ion is Ar 3d1 4s0.
Boron has an electronic configuration of 1s22s22p1 (it has 5 electrons). In order to reach the stable electron configuration of a noble gas with a completely filled valence shell, boron atom has to lose 3 electrons to obtain a stable duplet structure (i.e. 2 electrons in its first electron shell). After losing 3 electrons, the boron atom forms a B3+ ion, or a so-called tripositive ion.
It has 39 electrons and ends in a d orbital. Now finish your homework :)
The electron configuration for the Co2 ion is Ar 3d7.
The electron configuration of a V3 ion is Ar 3d2.
The electron configuration of the Co2 ion is Ar 3d7.
The electron configuration of an Sc2 ion is Ar 3d1 4s0.
The electron configuration of boron is 1s2 2s2 2p1. When boron becomes an ion, it typically loses its outer electron to achieve a stable electron configuration. Therefore, the electron configuration of a boron ion is typically 1s2 2s2.
The electron configuration of an Fe ion is 1s2 2s2 2p6 3s2 3p6 3d6.
The ground-state electron configuration for the V3 ion is Ar 3d2.
Na+ is the formula of the ion formed when sodium achieves a stable electron configuration.
1s2 2s2 2p6 is the electron configuration of the fluoride ion. It has a complete octet and is isoelectronic with neon. Before it becomes an ion, it is 1s2 2s2 2p5 Then it gains an electron and has a negative charge.
The electron configuration of a Copper(II)ion is [Ar]4s0 3d9.