Anomalous electron configurations Some atoms, such as some transition metals and some elements in the lanthanide and actinide series, do not adhere strictly to Hund's rule and Pauli's principle

Anomalous electron configurations Some atoms, such as some transition metals and some elements in the lanthanide and actinide series, do not adhere strictly to Hund's rule and Pauli's principle. The reason the anomalies are observed is the unusual stability of both half-filled pnd completely filled subshells. This behavior can be explained with an example of the chromium atom. Using Hund's rule and Pauli's principle, you can write the expected electron configuration of the Cr atom that strictly follows these rules as 1s2 2s2 2p6 3a2 3pe As2 3d4 . However, by moving an electron from the 4s orbital to the 3d orbital you obtain a half-filled 3d orbital. This half-filled orbital is more stable than the combination of the filled 4s orbital and the partially filled 3d orbital. Thus, the observed electron configuration of the Cr atom is 1s22s22p63s23p64s13d5. Mo has an anomalous electron configuration. Write the observed electron configuration of Mo Express your answer in complete form in order of increasing orbital energy. For example, 1s22s2 should be entered as 1s^22s^2.