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What is the electron configuration of a transition element?

The electron configuration of a transition element is characterised by partially filled d orbitals.

Transition elements are those elements in the d-block of the periodic table, which includes groups 3 to 12. The electron configuration of transition elements is characterised by partially filled d orbitals. This is because the d orbitals are energetically close to the outermost s orbital, which means that electrons can easily move between the two orbitals. As a result, transition elements can form a variety of different oxidation states, which is a key characteristic of these elements.

The electron configuration of transition elements can be determined using the Aufbau principle, which states that electrons fill orbitals in order of increasing energy. For example, the electron configuration of chromium (Cr) is [Ar] 3d5 4s1, which means that it has five electrons in its d orbital and one electron in its outermost s orbital. Similarly, the electron configuration of copper (Cu) is [Ar] 3d10 4s1, which means that it has ten electrons in its d orbital and one electron in its outermost s orbital.

The partially filled d orbitals of transition elements are responsible for many of their unique properties, including their ability to form complex ions and compounds, their catalytic activity, and their colourful compounds. These properties make transition elements important in a wide range of applications, from industrial processes to biological systems.

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