What is the colour of:
1. Cu+
2. Cu2+
3. Cu3+?
Copper(I) is diamagnetic; therefore, the ion is expected to be colorless unless due to other factors than unpaired electrons(e.g. to the anion). Copper(II) compounds are blue to green, to turquoise. Binary compounds of copper(III) are not common.
Daniel cell is a primary cell which cannot supply steady current for a long time. Daniel cell produces an emf of 1.08 volt.
1. Cu+ is the color of "copper in a happy mood." It's a silvery-white color.
2. Cu2+ is the color of "copper feeling content." It has a pale blue color.
3. Cu3+ is the color of "copper getting really agitated!" It's a dark blue color. Watch out, you don't want to make copper too mad!
To determine the colors of Cu+, Cu2+, and Cu3+ ions, we need to refer to the concept of electronic configurations and the absorption of light.
1. Cu+:
Cu+ has lost one electron from the neutral copper atom (Cu) and has a 1+ charge. The electronic configuration of Cu+ is [Ar] 3d10, where [Ar] represents the electron configuration of argon. The empty 4s orbital causes a shift in energy levels, resulting in a different absorption of light compared to the neutral copper atom. However, the Cu+ ion does not absorb visible light. As a result, it appears colorless to the naked eye.
2. Cu2+:
Cu2+ has lost two electrons from the neutral copper atom (Cu) and carries a 2+ charge. The electronic configuration of Cu2+ is [Ar] 3d9. Due to the presence of only one electron in the 3d orbital, the Cu2+ ion readily absorbs light in the visible range. It absorbs light in the blue-green portion of the spectrum around 600-800 nm and appears to have a pale blue color.
3. Cu3+:
Cu3+ is an oxidized form of the copper atom, in which three electrons have been lost. However, Cu3+ is not commonly observed in stable compounds as it is highly oxidizing and unstable. As a result, there is limited information about its color or electronic configuration.
In summary, Cu+ is colorless, Cu2+ appears pale blue, and Cu3+ is generally unstable and uncommon.