MOLECULAR ORBITAL THEORY 1. Explain the main difference between Molecular Orbital and Valence Bond Theory.

7. The bond angels of NH3 have been experimentally determined to be 107°. According to valence bond theory, what are the expected bond angles? According to hybridization theory, what are the expected bond angles? If they are not the same, which model is the best match?

What is a property of diamond that can be explained using valence bond theory? It is sp2 hybridized through its structure. It is extremely hard. It conducts electricity readily. It exists in a trigonal pyramid shape. It is highly expensive.

What are the angles a and b in the actual molecule of which this is a Lewis structure? H H H C H a a = C b = ⁰ C H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. H X

2) a) Consider the following molecule . Given what you have learned about hybridization theory, draw an image or images explaining the bonding situation in this molecule. I want you to draw out all of the orbitals, hybrid orbitals and how they overlap to form the bonds in the molecule. Indicate the % s or p character in the given atomic and hybrid orbitals. Which C-C bond or bonds are the longest? In a paragraph or so explain the image or images you just drew. b) Lastly, consider the molecule below. Indicate the Molecular formula, the molar mass, label the hybridization of each atom except for hydrogen, indicate any chiral centers with a *, which bond or bonds are the shortest, identify by name of each functional group with an arrow pointing to the group.

I dont understand this. Determine the hybridization of the central atom in the compound PCl5.A. sp3dB. sp3C. sp3d2D. sp2

Determine the covalent bonding of methane (CH4) using Valence Bond and Molecular Orbital models.

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