Explain the rotation and vibration spectra of molecules in their fundamental electronic state.

3. Predict the ground electronic state for each of the following molecules: (a). C₂ (b). N₂ (c). N₂O (d). F₂* (e). BF3

From the ground-state electron configurations of B2 andC2, predict which molecule should have the greater dissociation energy.

Use VSEPR theory to predict the shape of this molecule (POC13) and indicate any deviation from the bond angle(s) expected from a regular arrangement of repulsion axes. Show all the steps took to arrive at answer 4 to five sentences

What orbitals are used to form each of the C–C and C – H bonds in CH3CH2CH3 (propane)? How many s bonds arepresent in this molecule?

For each of the following molecules, identify whether it is a valid Lewis structure and if not, explain why. Then, regardless of whether it is a valid structure or not, use VSEPR to identify the expected 3-D structure.

A research student used a new software package to calibrate the electronic map using a material containing only gallium and bromine bonds, Ga and Br. On which atoms might you expect to see the highest electron density?

Which of the following non-linear molecules should be modeled as an asymmetric rigid top for its rotational energy levels? (The VSEPR configuration about the central atom is indicated in parentheses.) OBCI 3 (trigonal planar) O CHCl3 (tetrahedral) OCH3CI (tetrahedral) O CH₂Cl₂ (tetrahedral) OCCl4 (tetrahedral)

Given the molecule CH2CHCN Please draw a Lewis structure for this compound with CORRECT GEOMETRY and label all sigma and pi bonds with the orbitals it is made from (what orbitals are overlapping to form the bond). You may draw the hybridized sigma orbitals as sticks and the unhybridized p-orbitals as lobes for clarity. For this question, you DO need to draw out the orbitals.

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