Cu⁺ ion
[Ar] 3d¹⁰. 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.
Cu+Copper ion, 28 electrons
[Ar] 3d10
In full: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰. Cu loses 4s¹
Cu loses 4s¹
- Blockd block
- Period4
- Group11
- Outer shell18
- Unpaired0
- MagneticDia
Last electron 3d
- n3shell
- l2d subshell
- m+2orbital
- s−½spin down
Step by step
- Copper has 29 electrons: [Ar] 3d¹⁰ 4s¹.
- The ion has 1 fewer, 28 electrons. Remove them from the highest n first.
- Cu loses 4s¹.
- Cu⁺ ion: [Ar] 3d¹⁰, in full 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰.
Cu⁺ ion: the numbers
| Atomic number | 29 |
|---|---|
| Electrons | 28 |
| Period | 4 |
| Group | 11 |
| Block | d block |
| Electrons in the outer shell | 18 |
| Unpaired electrons | 0 |
| Magnetic | diamagnetic |
| Last electron | 3d: n = 3, l = 2, m = +2, s = −1/2 |
Cu⁺ ion: quick answers
What is the electronic configuration of Cu⁺?
Cu⁺ has 28 electrons: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰, or [Ar] 3d¹⁰. Cu loses 4s¹.
How many unpaired electrons are there in Cu⁺?
Cu⁺ has 0 unpaired electrons, so it is diamagnetic.
Why does Cu lose its outer electrons first?
Electrons leave from the highest n first. The 4s level fills before 3d, but once 3d holds electrons the 4s electrons are the outermost, so they are lost first.