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. Reason. 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. The sequence of filling of electrons in 3 d subshell gets disturbed in chromium and copper and these elements possess exceptional configuration. The electron configurations of chromium and copper seem to disagree with what is expected according to the Aufbau principle. Half filled subshells feature lower electron-electron repulsions in the orbitals, thereby increasing the stability. Half-filled and completely filled subshells seem to be more stable. the reason for abnormality in the electronic configuration of Chromium and Copper is the maximum stability. 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. 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 d-orbital can occupy a maximum of 10 electrons. I have started studying chemistry and I was told to memorise the exceptional electronic configurations of Chromium and Copper. Half filled or completely filled orbitals are more stable than those with one electron less. There are two main exceptions to electron configuration: chromium and copper. 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. 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. Therefore we have (still incorrect) 1s 2 2s 2 2p 6 3s 2 3p 6 3d 9 4s 2. Three d nine. Similarly, completely filled subshells also increase the stability of the atom. 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. Since chromium had 4 electrons, which is one short of 5 electrons to get just hslf-filled. 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)#.. Interestingly enough, Tungsten is more stable with an electron arrangement of #[Xe]4f^14 5d^4 6s^2#.. this happens with Nb and Ag which are underneath Cr and Cu respectively. 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