Chemical Forums

Chemistry Forums for Students => High School Chemistry Forum => Topic started by: khaoz on February 13, 2006, 08:42:14 PM

Title: How does copper form a Cu 2+ ion? (Electron Configuration)
Post by: khaoz 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?

Title: Re:How does copper form a Cu 2+ ion? (Electron Configuration)
Post by: madscientist 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

Title: Re: How does copper form a Cu 2+ ion? (Electron Configuration)
Post by: DeP 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

Title: Re: How does copper form a Cu 2+ ion? (Electron Configuration)
Post by: vmelkon on January 08, 2011, 01:50:18 PM

Quote from: DeP 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

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