Chapter 6, Problem 6.46P

7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?

Consider a ring system made up of 8 atoms (each one contributing a p atomic orbital to make 8 pi molecular orbitals). If the system is filled with 6 orbitals containing single, electrons, there will 6 orbitals containing pairs of electrons and 1 unpaired electrons. Hint: Use a Frost Circle. Use numbers rather than text for your answers.

Sketch an orbital picture of ethylene, H2C = CH2, and highlight the orbitals that overlap to formeach σ and π bond. Identify the orbitals from each atom that overlap to form the σ and π bonds. Why isthe C⎯ C π bond weaker than the C⎯ C σ bond? Use orbital structure as part of your explanation.

Represent the bonding in each molecule or ion by drawing the orbitals (hybridized and unhybridized) of each atom in the bond. Label the σ and π bonds and label each bond by the orbitals that it is made from. For instance, the C–H bond in CH4 would be made from the overlap of: C (sp3) – H (1 s). You may draw the hybridized sigma orbitals as sticks and the unhybridized p-orbitals as lobes for clairity and ease. a. HONO b. CH3 CCH c. C3 H4 d. C2 O4 2-

Like many of the molecules we have studied in this class, propene (structure shown below) can be thought of as a particle in a box. There are three t-electrons. Since I can put two electrons in each energy level, the highest-energy electron is in the n = 2 state (the HOMO). What does the wave for this electron look like? n = 3 lowest unoccupie molecular orbital (LUMO) n = 2 highest occupiedi molecular orbital (НОМО) . n = 1 Select one: Оа. O b. О с. O d. None of these shapes are right.

This question will explore bonding in OH and OH- using molecular orbital theory a) Explain any differences in energy between atomic orbitals of O vs. the atomic orbital of H. b) Taking into account your response to part a, draw a molecular orbital diagram for the valence electrons in the neutral diatomic OH. Include a sketch of the molecular orbitals in your sketch. The relevant molecular orbitals listed in order of increasing energy are σ2s(1 orbital), σ2p(1 orbital), π2p (2 orbitals), σ2p∗(1 orbital). (Hint: the 2s atomic orbital of the O atom to not interact with the 1s atomic orbitals on the H atom). c) How do you expect the bond length in OH to compare to that of the OH- anion? Justify your answer by calculating the bond order of each species.

For the following molecule, write the Lewis structure, predict the molecular structure (including bond angles), give the expected hybrid orbitals on the central atom, and predict the overall polarity. KrF2:

Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

The structure of the visual pigment retinal is shown in (1). Label each atom with its state of hybridization and specify the composition of each of the different type of bond.