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CHEM 121 Studioby Learn4Less · UBC CHEM 121

CHEM 121 glossary

Diamagnetic

Having every electron paired, so the species is weakly pushed out of a magnetic field. Only species whose occupied subshells (or MOs) are all completely filled are diamagnetic.

ZnX2+\ce{Zn^2+}, 3d103d^{10}: every orbital holds a pair.

Example

Zinc, [Ar] 4s2 3d10[\mathrm{Ar}]\,4s^2\,3d^{10}, and NX2\ce{N2} are diamagnetic. An even electron count is not enough: FeX2+\ce{Fe^2+} has 24 electrons but 4 are unpaired.

See alsoParamagneticUnpaired electronElectron configuration