1/25/2024 0 Comments Cobalt ii chloride formulaAs in the case of the hexacyanoferrate(II) ion, the strong field of the ammonia ligands splits the d orbitals and allows all electrons to pair. Hexaamminecobalt(III) chloride is not attracted to the poles of the magnet. The d orbitals in the iron(II) ions are split by the strong crystal field of the cyanide ligands, allowing all six electrons to pair. Potassium hexacyanoferrate(II) is shown to be diamagnetic. Since the d subshell in zinc(II) ion is full, there are no unpaired electrons and it is diamagnetic. When zinc(II) sulfate heptahydrate is brought near the poles of the magnet there is no attraction. Nickel(II) ions have two unpaired electrons. When nickel(II) sulfate hexahydrate is brought near the poles of the magnet, it appears to have about the same attraction as the cobalt(II) chloride, perhaps slightly less. Cobalt(II) ions have three unpaired electrons. Iron(II) ions have four unpaired electrons.Ĭobalt(II) chloride hexahydrate can be brought closer to the poles than the iron (II) sulfate or the manganese(II) sulfate before it swings toward the magnet. This compound is not as strongly paramagnetic as the manganese(II) sulfate. Iron(II) sulfate pentahydrate can be brought closer to the magnet than the manganese(II) sulfate monohydrate, but eventually it swings toward the magnet. Manganese ions in manganese(II) sulfate monohydrate have five unpaired electrons. Manganese(II) sulfate monohydrate is strongly attracted by the magnet, which shows that it is paramagnetic. There are no unpaired electrons in sodium chloride and sodium chloride is diamagnetic. There is no attraction of the sodium chloride to the magnet, even when the vial strikes the magnet. Water is not attracted to the magnet poles water is diamagnetic. Salts of these ions that have strong-field ligands are diamagnetic. But strong-field ligands can split the energy levels of the d orbitals so that they are no longer degenerate. These metal ions have unpaired electrons in degenerate d orbitals as predicted by Hund's rule and thus exhibit paramagnetism. Paramagnetism is most easily observed in the salts of some of the first row transition metals (manganese through nickel). It occurs when there are unpaired electrons in the substance. Paramagnetism is when a substance is weakly attracted to a magnetic field.
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