Chromium 2+ ion uses only unfilled d-orbitals to form 6 dative bonds?

Thread starter adf89812
Start date Aug 3, 2024
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Acid base Inorganic chemistry

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SUMMARY

The discussion centers on the electronic configuration of Chromium (Cr) and its 2+ ion state. It establishes that the correct configuration for a neutral chromium atom is [Ar] 4s¹ 3d⁵, while for the Cr 2+ ion, the configuration is [Ar] 3d⁴. The focus is on identifying the unfilled d-orbitals that allow for the formation of six dative bonds in the Cr 2+ ion. The conclusion emphasizes the importance of understanding orbital occupancy in transition metals for predicting bonding behavior.

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Understanding of electronic configurations in transition metals
Knowledge of dative bonding and coordination chemistry
Familiarity with the periodic table and orbital filling rules
Basic concepts of oxidation states and ion formation

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Study the electronic configuration of other transition metals, focusing on their oxidation states
Learn about ligand field theory and its application to dative bonding
Research the properties and applications of Cr 2+ in coordination complexes
Explore the implications of orbital hybridization in transition metal chemistry

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Chemistry students, educators, and professionals in materials science or coordination chemistry who seek to deepen their understanding of transition metal bonding and electronic configurations.

Aug 3, 2024

adf89812

TL;DR: Is any part of the picture text wrong?

I find the one (4s) + 3(4p) + 2(d) incorrect according to my knowledge.

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Aug 3, 2024

DrJohn

Start by finding the electronic configuration of a chromium atom - which orbitals are occupied.
Then move on to the configuration of a Cr 2+ ion.
Then which orbitals are empty.