September 19, 2024, 01:31:28 PM
Forum Rules: Read This Before Posting

### Topic: How does copper form a Cu 2+ ion? (Electron Configuration)  (Read 136771 times)

0 Members and 1 Guest are viewing this topic.

#### khaoz

• Guest
##### How does copper form a Cu 2+ ion? (Electron Configuration)
« on: February 13, 2006, 08:42:14 PM »
Normally, the electron configuration for copper would be [Ar] 4s1 3d10. What would be the configuartion for a Cu2+ stable ion be?

• Full Member
• Posts: 225
• Mole Snacks: +14/-7
• University of New England Australia
##### Re:How does copper form a Cu 2+ ion? (Electron Configuration)
« Reply #1 on: February 18, 2006, 04:08:50 PM »
Cu = [Ar]3d104s1 this configuration does not follow the n+l rule. in other words if you use box notation to map out the electron configuration of Cu2+ you dont fill the 4s orbital first.

so,if:Cu=[Ar]3d104s1=29=atomic number=nu-mber of electrons

Then, Cu2+ indicates that 2 electrons have been given up by the copper atom and the electron configuration is therefore:

Cu2+= [Ar]3d9 =27= atomic number = number of electrons
« Last Edit: February 18, 2006, 04:11:28 PM by madscientist »
The only stupid question is a question not asked.

#### DeP

• New Member
• Posts: 5
• Mole Snacks: +0/-0
##### Re: How does copper form a Cu 2+ ion? (Electron Configuration)
« Reply #2 on: January 08, 2011, 06:17:46 AM »
For Cu2+ you have indeed 27 electrons,
but first you have to fill in the 4s orbital and than the 3d orbital
so then you have  for Cu2+ a [Ar]3d74s2 electron configuration

The reason that they for Cu0 fill in first the 3d orbital instead of the 4s orbital, is because a full 3d orbital is more stable than an incompletely filled 3d orbital

#### vmelkon

• Chemist
• Full Member
• Posts: 474
• Mole Snacks: +28/-10
• Gender:
##### Re: How does copper form a Cu 2+ ion? (Electron Configuration)
« Reply #3 on: January 08, 2011, 01:50:18 PM »
For Cu2+ you have indeed 27 electrons,
but first you have to fill in the 4s orbital and than the 3d orbital
so then you have  for Cu2+ a [Ar]3d74s2 electron configuration

The reason that they for Cu0 fill in first the 3d orbital instead of the 4s orbital, is because a full 3d orbital is more stable than an incompletely filled 3d orbital

An electron jumps from the 3d to the 4s?