Mg²⁺ ion
[Ne], the same as neon. 0 unpaired electrons, diamagnetic.
Element or ion
Type a symbol, a name or an atomic number, add a charge such as Fe3+ or Cl-, or tap an element in the table. Orbitals fill from m = −l up, spin +½ first.
Mg2+Magnesium ion, 10 electrons
[Ne]
In full: 1s² 2s² 2p⁶. Mg loses 3s². Same electrons as neon (Ne).
Mg loses 3s²like Ne
- Blocks block
- Period3
- Group2
- Outer shell8
- Unpaired0
- MagneticDia
Last electron 2p
- n2shell
- l1p subshell
- m+1orbital
- s−½spin down
Step by step
- Magnesium has 12 electrons: [Ne] 3s².
- The ion has 2 fewer, 10 electrons. Remove them from the highest n first.
- Mg loses 3s².
- Mg²⁺ ion: [Ne], in full 1s² 2s² 2p⁶.
Mg²⁺ ion: the numbers
| Atomic number | 12 |
|---|---|
| Electrons | 10 |
| Period | 3 |
| Group | 2 |
| Block | s block |
| Electrons in the outer shell | 8 |
| Unpaired electrons | 0 |
| Magnetic | diamagnetic |
| Last electron | 2p: n = 2, l = 1, m = +1, s = −1/2 |
Mg²⁺ ion: quick answers
What is the electronic configuration of Mg²⁺?
Mg²⁺ has 10 electrons: 1s² 2s² 2p⁶, or [Ne], the same as neon. Mg loses 3s².
How many unpaired electrons are there in Mg²⁺?
Mg²⁺ has 0 unpaired electrons, so it is diamagnetic.
Why does Mg lose its outer electrons first?
The electrons in the outermost shell are held least strongly, so they are removed first, leaving [Ne].