Question

Part A

Choose the paramagnetic species from below.
O He
O Te
O T14+
O All of the above are paramagnetic.
None of the above is paramagnetic.

Answer 1

Among the given options (He, Te, Ti4+), none is paramagnetic because all have paired electrons in their electron configurations. Paramagnetic species require one or more unpaired electrons, which none of these species have.

Step-by-step explanation:

To determine the paramagnetic species among the given options, we must look at the electron configurations of helium (He), tellurium (Te), and ion Ti4+. A species is considered paramagnetic if it contains one or more unpaired electrons, which are attracted to magnetic fields due to their magnetic dipole moments. In contrast, a species with all electrons paired is diamagnetic and will not be attracted to a magnetic field; it might be slightly repelled.

Helium (He) has a complete valence shell with no unpaired electrons, making it diamagnetic. Tellurium (Te) has a ground-state electron configuration that results in paired electrons in its orbitals, making it diamagnetic as well. Lastly, Ti4+ has a configuration where all its 3d electrons are removed, leading to no unpaired electrons and thus it is also diamagnetic. Hence, none of the above options are paramagnetic.