1s2 2s2 2p6 3s2 3p6 4s2 3d3 For abbreviation: [Ca] 3d3
Vanadium, V, atomnumber 23 has the following electron configuration:
1s2, 2s2 2p6, 3s2 3p6, 4s2, 3d3
It is not [Ar] 4s2
In V 3+ the element Vanadium is giving away 3 of its electrons. 50.9 - 3 is 47.9, about the same as Titanium (Ti). So the answer would be [Ar] 4s^0 3d^2
In3+ ion:
[Kr] 4d10
or
2, 8, 18, 18
[Ar] or 1s2 2s2 2p6 3s2 3p6
The electron configuration for the aluminum ion is identical to that of neon: 1s22s22p6
No, the former answer (striked through below this) is very wrong!Hydrogen (elemental H atom) contains only 1 (one!) electron (1s1) and since a H ion (H+) has lost that one to become stable, this H+ ion has no (zero!) electrons at all.Only the very rare and exceptional, negatively charged hydride ion H- ion contains two electrons (1s2 configuration, not favoured, not enough electronegativity)Yes. A Hydrogen atom "wants" to be stable, so it gains an electron to be iso-electronic with helium. After that, its electron configuration is 1s2. H+
an atom that gains an electron becomes a negative ion, called an anion.
As a neutral atom lose an electron then it becomes a positive ion As it gains an electron then it becomes a negative ion
The charge is 2+.
The electron configuration for a magnesium cation Mg2 plus is 1s2.2s2.2p6.
hafnium
The electron configuration of copper(II) is [Ar] 3d9 . Copper is [Ar] 3d10 4s1
The electron configuration of selenium for a 2- ion is [Kr]4s2.3d10.4p6.
Al+3 aluminum
There are four electrons in a Beryllium atom. Hence the mono positive ion has only three electrons. Therefore the electron configuration is 1s2 2s1.
.. [Li]+ [:I:]- (put the last 2 pairs above and below the "I" this wont let me) ..
Rhodium (Rh) forms a 3 plus ion that has the electron configuration Kr4d6. Rhodium has oxidation states of 2,3 and 4, so it can loan out 2, 3 or 4 electrons depending on the circumstances of a chemical reaction.
The electron configuration of thaliium III ion is [XE] 4f14 5d10.
Al3+
Al3+
Na+ is the formula of the ion formed when sodium achieves a stable electron configuration.