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What theoretical magnetic moment would be used to calculate [co(ox)]4-
Accepted Answer
To calculate the theoretical magnetic moment of [Co(ox)]4-, we need to consider the electronic configuration of the cobalt ion and the ligand field splitting. Here's how:
1. Determine the oxidation state of cobalt: In [Co(ox)]4-, oxalate (ox) has a -2 charge, and the overall complex has a -4 charge. Therefore, cobalt must be in the +2 oxidation state.
2. Write the electronic configuration of Co(II): The electronic configuration of Co(II) is [Ar] 3d7.
3. Consider the ligand field splitting: Oxalate is a weak-field ligand, meaning it causes a small splitting of the d orbitals. In an octahedral complex like [Co(ox)]4-, the d orbitals split into two sets: a lower energy set (t2g) and a higher energy set (eg).
4. Fill the d orbitals: Since oxalate is a weak-field ligand, the seven electrons of Co(II) will fill the t2g orbitals first, with one electron left to occupy one of the eg orbitals. This results in three unpaired electrons.
5. Calculate the magnetic moment: The spin-only magnetic moment (μs) can be calculated using the formula:
μs = √n(n+2) BM
where n is the number of unpaired electrons. In this case, n = 3, so:
μs = √3(3+2) BM = √15 BM ≈ 3.87 BM
Therefore, the theoretical magnetic moment of [Co(ox)]4- is approximately 3.87 Bohr magnetons.
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