hich of these ions are likely to be paramagnetic?I. Ti3+II. Cr3+III. Fe3+A. I and II onlyB. I and III onlyC. II and III onlyD. I, II and II

To answer this question, we need to understand what paramagnetism is. Paramagnetism refers to the magnetic state of an atom or ion that has unpaired electrons. This means that the atom or ion is attracted to a magnetic field due to the spin of its unpaired electrons.

Now, let's examine each ion:

I. Ti3+ (Titanium 3+) The electron configuration of a neutral titanium atom is [Ar] 3d2 4s2. When it loses three electrons to become Ti3+, it loses the two 4s electrons and one of the 3d electrons, leaving it with one unpaired electron in the 3d orbital. Therefore, Ti3+ is paramagnetic.

II. Cr3+ (Chromium 3+) The electron configuration of a neutral chromium atom is [Ar] 3d5 4s1. When it loses three electrons to become Cr3+, it loses the 4s electron and two of the 3d electrons, leaving it with three unpaired electrons in the 3d orbital. Therefore, Cr3+ is also paramagnetic.

III. Fe3+ (Iron 3+) The electron configuration of a neutral iron atom is [Ar] 3d6 4s2. When it loses three electrons to become Fe3+, it loses the two 4s electrons and one of the 3d electrons, leaving it with five paired electrons in the 3d orbital. Therefore, Fe3+ is not paramagnetic.

So, the answer is A. I and II only.