Describe the bonding in the methanol molecule, CH30H, using valence bond theory.

Draw the Lewis Structures for boron trifluoride (BF3), phosphorous trichloride (PCI3), oxygen difluroide (OF2), nitrogen trichloride (NCI3) and meth (CH4). Which do you expect to be the most polar? (Hint: which will have the greatest molecular dipole?) O boron trifluoride O phosphorous trichloride O methane O oxygen difluroide O nitrogen trichloride

Determine the electron geometry (eg) and molecular geometry (mg) of NO2-, the nitrite anion.

Write the two resonances formula for benzene, C6H6, (note the carbon atoms are all bonded to each other forming a ring.). What is the geometry about any one of the carbon atoms? What hybridization would be used in valence bond theory to describe the bonding? The ∆Hf for C6H6(g) is actually -83 kJ/mol. What is the equation for the standard molar enthalpy of formation form benzene? Use the standard enthalpy of formation equation and ∆Hf for C(g) 715 kJ/mol and H2(g) is 0 kJ/mol. Calculate the estimate enthalpy of formation of benzene. Then calculate the resonance energy of benzene. The resonance energy is defined as ∆Hf (estimated) – ∆Hf (actual).