Question #1e14c

1 Answer

An isolated #Ca# atom is diamagnetic, since its electron configuration shows no unpaired electrons.

#Ca: [Ar]4s^2#

However, an element's magnetic character does not depend solely on electron configuration, it depends on the empty orbitals that are next to the valence orbitals as well.

Notice that you have a vacant 3d-orbital very close in energy to the 4s-orbital. This sometimes can cause the transition of an electron from the 4s to the 3d-orbital, which causes two unpaired electrons to occupy the aforementioned orbitals and induce a paramagnetic character.

Another important aspect to take into consideration when discussing #Ca#'s paramagnetic or diamagnetic character is the fact that it has a metallic structure, which implies delocalized electrons.

Here's an answer detailing #Ca#'s metallic structure and its paramagnetic character posted by another contributor: