Hence, Cr and Cu are called exceptional configuration. Half filled or completely filled orbitals are more stable than those with one electron less. The d-orbital can occupy a maximum of 10 electrons. Since chromium had 4 electrons, which is one short of 5 electrons to get just hslf-filled.Click to see full answer. Keeping this in view, why is the electronic configuration of chromium?One explanation for Chromium, then, is that: The maximized exchange energy Πe stabilizes this configuration ( 3d54s1 ). The maximization comes from how there are 5 unpaired electrons, instead of just 4 ( 3d44s2 ).Additionally, why is the electron configuration for copper 1s22s22p63s23p63d104s1 instead of 1s22s22p63s23p63d94s2? A filled sublevel is more stable than a half-filled sublevel. The arrangement of electrons with the same spin is as small as possible. The 4s orbital has higher energy than the 3d orbital. Thereof, how do the electron configurations of chromium and copper contradict? The Aufbau principle states that, hypothetically, electrons orbiting one or more atoms fill the lowest available energy levels before filling higher levels (e.g., 1s before 2s).Why is the electron configuration for copper?It is due to full filled stability which the copper achieves when electron jump to d orbital to achieve full filled stability. 1. Exchange energy -in d orbital there are 5 subshell so ten exchanges of electron is possible which imparts much stability to copper hence this process is exothermic in nature.
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