What is the spin magnetic moment of chromium in hexaquachromium(ll)

To determine the spin magnetic moment of chromium in hexaquachromium(ll), we need to consider the electron configuration of chromium in its +2 oxidation state.

1. Start by writing the electron configuration of chromium. The atomic number of chromium is 24, so the electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^4.

2. In hexaquachromium(ll), there are six water molecules (H2O) coordinated to the chromium ion. Each water molecule donates a lone pair of electrons to the chromium ion, resulting in six ligand donor electrons.

3. The coordination complex has a d^4 electron configuration, meaning there are four unpaired electrons in the 3d orbitals of the chromium ion.

4. The spin magnetic moment (μs) is given by the formula μs = √(n(n+2)) where n is the number of unpaired electrons.

5. Plugging in the value of n = 4 into the formula, we get μs = √(4(4+2)) = √(4*6) = √24.

6. Simplifying further, μs = √(4*6) = √(24) = 2√6.

Therefore, the spin magnetic moment of chromium in hexaquachromium(ll) is 2√6.