is F2 +2 ion diamagnetic or paramagnetic? I think its diamagnetic because it loses 2 electrons and it still has no unpaired pairs...i think...thanks.

Fe+2? Generally, its magnetic effects will depend on those atoms in the same lattice, how all are aligned.

Isolated...you are probably right.

You are correct! The F2 +2 ion is indeed diamagnetic. To determine whether an ion or a molecule is diamagnetic or paramagnetic, you need to consider its electron configuration.

The F2 +2 ion is formed by removing two electrons from the F2 molecule. The electron configuration of a neutral fluorine atom (F) is 1s2 2s2 2p5, where the superscripts represent the number of electrons in each orbital.

When two electrons are removed from F2 to form F2 +2, it results in a loss of one electron from the 2s orbital and one from the 2p orbital. Therefore, the electron configuration of F2 +2 becomes 1s2 2s1 2p4.

To determine if the ion is diamagnetic or paramagnetic, we need to check if there are any unpaired electrons. In the case of F2 +2, there are no unpaired electrons because all the 4 electrons occupy the orbitals in pairs (2s1 and 2p4).

Since there are no unpaired electrons, the F2 +2 ion is diamagnetic. Diamagnetic substances are those that have all their electrons paired up, and as a result, they are weakly repelled by a magnetic field.

Therefore, you were correct in identifying F2 +2 as diamagnetic because it has no unpaired electrons.

You are correct! The F2+2 ion is indeed diamagnetic.

To determine whether an ion is diamagnetic or paramagnetic, you need to consider its electron configuration. The F2+2 ion is formed by removing two electrons from a neutral F2 molecule.

The electron configuration of a neutral F2 molecule is 1s2 2s2 2px2 2py2 2pz2, where each letter (e.g., 2s2) represents a specific atomic orbital and the superscript number specifies the number of electrons in that orbital.

When two electrons are removed to form F2+2, the electron configuration becomes 1s2 2s2 2px2 2py0 2pz0. Since all the electrons are now paired (no unpaired electrons), the F2+2 ion is diamagnetic.

Therefore, your conclusion that the F2+2 ion is diamagnetic because it has no unpaired electrons is correct. Well done!