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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.
how many solid state are there?
Molecule in itself is electrically stable so it cant act as ligand So that it can acts as the negative and pasitive ligand.
What is the maximum number of electrons which can be accommodated in an atom in which the highest principal quantum number value is 4: (1) 10 (2) 18 (3) 32
According to Bohr's principle, the relation between principle quantum number and radius of orbit is: (1) r ∞ n (2) r ∞ n 2 (3) ∞1/n (4) r∞ 1/ n 2 Ans: r
5
why ionisation energy of Al is greater than Ga?
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In the discussion it asks, what is a possible extension that can be cinsidered, can u please help me , thanks :)
Number of nodal centres for 2s orbital: (1) 1 (2) 0 (3) 4 (4) 3 Ans: 1
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