HW Key _7 part b - S22. Use the MO model to explain the...

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S22. Use the MO model to explain the bonding in BeH 2 . When constructing the MO energy level diagram, assume that the Be 1s electrons are not involved in bond formation. We start explaining the bonding of BeH 2 by determining the Lewis structure. The Lewis dot structure is H–Be–H. Since there are two regions of electron density around the Be atom. This means that according to VSEPR the molecular geometry is linear, which requires sp hybridized orbitals on the Be atom to obtain the correct geometry. The molecular orbitals for BeH 2 are formed from the two hydrogen 1s orbitals and the two sp orbitals from beryllium. The two 1s hydrogen orbitals that combine with the two sp orbitals form two sigma bonding orbitals and two sigma antibonding orbitals. Using the z axis as the intermolecular axis, this means that we used the 2p z orbital to create the sp orbital. This leaves two p orbitals on Be that are not involved in bonding; the 2p x and 2p y orbitals are nonbonding orbitals since they don't have proper symmetry necessary to overlap with 1s orbitals. The MO diagram for BeH2 is: Bond Order = (4 - 0)/2 = 2; The MO diagram predicts BeH 2 to be a stable species and also predicts that BeH 2 is diamagnetic. Note: The MOs are not localized
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This note was uploaded on 02/01/2011 for the course CHEM 111 taught by Professor Owens,g during the Fall '08 term at University of Utah.

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HW Key _7 part b - S22. Use the MO model to explain the...

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