Magnetic properties diamagnetism

Magnetic properties Diamagnetic Paramagnetic Diamagnetic Paramagnetic Diamagnetic Diamagnetic... 

Assume that the third-period element phosphorus forms a diatomic molecule, P2, in an analogous way as nitrogen does to form N2. (a) Write the electronic configuration for P2. Use [Ne2] to represent the electron configuration for the first two periods, (b) Calculate its bond order, (c) What are its magnetic properties (diamagnetic or paramagnetic) ... 

A major weakness of valence bond theory has been its inability to predict the magnetic properties of molecules. We mentioned this problem in Chapter 7 with regard to the 02 molecule, which is paramagnetic, even though it has an even number (12) of valence electrons. The octet rule, or valence bond theory, would predict that all the electrons in 02 should be paired, which would make it diamagnetic. 

The magnetic properties of Pu(CeHe)2 (=Pu(C0T)2), Pu(C2HsC0T)2 and Pu(CifH9C0T)2 were measured by Karraker (17,18). All compounds proved to be diamagnetic at room temperature near the theoretically calculated diamagnetic value. At low temperature they showed strong temperature dependent diamagnetism from -5,000 x 10-6 emu at 4 K to -900 x 10 6 emu at 45 K. 

As we can see, the diffuse orbitals play a dramatic part in the description of the magnetic properties of BeH not less two sets of these orbitals (basis set III) are necessary to obtain an accurate and converging value of the susceptibility. The BeH-anion should be diamagnetic and its mean susceptibility is of the order of -2.10- erg.G-2.mol"L Note that the use of a single set of supplementary diffuse orbitals is not sufficient to bring to light this magnetic property. 

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