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Q. Example of octahedral complexes?
Let us now turn our attention to the complexes having transition metal ion with d2 or d3 electrons. With these configurations, there are enough of vacant orbitals available to accept the pairs of elements from four or six ligands to form tetrahedral, square planar or octahedral compound. The magnetic moment of the complex will be the same as free ion value as shown in the diagram given below:
When the number of d electrons is greater than three and up to six as in d2, d6 systems, there is still a possibility of forming octahedral complexes using d2sp3 hybridised orbitals by forcing some of the electrons to pair up.
If a mole were to have 1*10^24 particles what is the weight of one mole of oxygen molecule and 1 molecule of oxygen Ans) Since the gram molecular mass remains the similar...weig
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why is density of interstitial compounds less than that of parent metal ?
Molecule in itself is electrically stable so it cant act as ligand So that it can acts as the negative and pasitive ligand.
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Express the concentration of a 2.0 M NaOH solution as a mass/volume percent. Can you please explain HOW to get the answer?
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Why is the total energy of a many-electron atom not equivalent to the sum of the orbital energies for every electron?
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