Copper (Cu) and Chromium (Cr) why the electron arrangement is an exception?
Copper (Cu) and Chromium (Cr) exhibit exceptions in their electron configurations due to the stability associated with having a half-filled or fully filled d-subshell.
For copper (Cu), the electron configuration is [Ar] 3d10 4s1 instead of [Ar] 3d9 4s2. This is because in Cu, one electron from the 4s orbital is promoted to the 3d orbital to achieve a half-filled d-subshell, which is a more stable configuration. The partially filled d-subshell in Cu allows it to have strong metallic bonding, making it a good conductor of electricity and heat.
For chromium (Cr), the electron configuration is [Ar] 3d5 4s1 instead of [Ar] 3d4 4s2. This is because in Cr, one electron from the 4s orbital is promoted to the 3d orbital to achieve a half-filled d-subshell. Furthermore, one of the electrons in the 3d subshell is unpaired, allowing it to form strong covalent bonds with other atoms. This unique electronic configuration also contributes to the unique properties of chromium, including its hardness and corrosion resistance.
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