When we write the electronic configuration of Cr (24) as per the ‘Aufbau principle’ the 3d orbital contains 4 electrons and the 4s orbital contains 2 electrons. Half filled subshells feature lower electron-electron repulsions in the orbitals, thereby increasing the stability. Video: Cu, Cu+, and Cu2+ Electron Configuration Notation. In learning chemistry, chromium, and copper, the 3d elements of our environment reveal their general form of electron or electronic structure trends in the periodic table. The d-orbital can occupy a maximum of 10 electrons. Chromium is said to have a configuration of 3d 5 4s 1 as opposed to 3d 4 4s 2. In these cases, a completely full or half full d sub-level is more stable than a partially filled d sub-level, so an electron from the 4s orbital is excited and rises to a 3d orbital. Correct Electron Configuration for Copper (Cu) Copper atoms are said to have a configuration of 3d 10 4s 1 as opposed to 3d 9 4s 2 as might have been expected from the general trend. The probable (expected) electronic configuration of chromium is 1s 2 2s 2 2p 6 3s 2 3p 6 3d 4 4s 2 or [Ar] 3d 4 4s 2. ii The probable (expected) electronic configuration of copper is 1s 2 2s 2 2p 6 3s 2 3p 6 3d 9 4s 2 or [Ar] 3d 9 4s 2. Both of the configurations have the correct numbers of electrons in each orbital, it is just a matter of how the electronic configuration notation is written (here is an explanation why). The completely filled subshells s 2 , p 6 , d 1 0 , f 1 4 and The half filled s 1 , p 3 , d 5 , f 7 subshells have extra stability. i. Reason. There are two main exceptions to electron configuration: chromium and copper. Since chromium had 4 electrons, which is one short of 5 electrons to get just hslf-filled. the reason for abnormality in the electronic configuration of Chromium and Copper is the maximum stability. The electron configurations of chromium and copper seem to disagree with what is expected according to the Aufbau principle. Half filled or completely filled orbitals are more stable than those with one electron less. this happens with Nb and Ag which are underneath Cr and Cu respectively. Half-filled and completely filled subshells seem to be more stable. Hence, Cr and Cu are called exceptional configuration. I have started studying chemistry and I was told to memorise the exceptional electronic configurations of Chromium and Copper. Unfortunately, there is no easy way to explain these deviations in the ideal order for each element. The electron configuration for chromium is NOT #1s^2 2s^2 2p^6 3s^2 3p^6 3d^4 4s^2#, but #color(blue)(1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^1)#.. 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