Al³⁺ 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.
Al3+Aluminium ion, 10 electrons
[Ne]
In full: 1s² 2s² 2p⁶. Al loses 3p¹ then 3s². Same electrons as neon (Ne).
Al loses 3p¹ then 3s²like Ne
- Blockp block
- Period3
- Group13
- Outer shell8
- Unpaired0
- MagneticDia
Last electron 2p
- n2shell
- l1p subshell
- m+1orbital
- s−½spin down
Step by step
- Aluminium has 13 electrons: [Ne] 3s² 3p¹.
- The ion has 3 fewer, 10 electrons. Remove them from the highest n first.
- Al loses 3p¹ then 3s².
- Al³⁺ ion: [Ne], in full 1s² 2s² 2p⁶.
Al³⁺ ion: the numbers
| Atomic number | 13 |
|---|---|
| Electrons | 10 |
| Period | 3 |
| Group | 13 |
| Block | p block |
| Electrons in the outer shell | 8 |
| Unpaired electrons | 0 |
| Magnetic | diamagnetic |
| Last electron | 2p: n = 2, l = 1, m = +1, s = −1/2 |
Al³⁺ ion: quick answers
What is the electronic configuration of Al³⁺?
Al³⁺ has 10 electrons: 1s² 2s² 2p⁶, or [Ne], the same as neon. Al loses 3p¹ then 3s².
How many unpaired electrons are there in Al³⁺?
Al³⁺ has 0 unpaired electrons, so it is diamagnetic.
Why does Al lose its outer electrons first?
The electrons in the outermost shell are held least strongly, so they are removed first, leaving [Ne].