3.- Based on the molecular orbitals of hydrogen, and the hybridized orbitals of single, double and triple bonded-carbon, assign the type of interaction for the following bonds (HINT: all answers must be expressed in "orbitai-orbital" format, review the double and triple bond slides form your ppt). H. H- H--c-H H' CC--H Blue= Red= Green= Orange= Purple=

3.- Based on the molecular orbitals of hydrogen, and the hybridized orbitals of single, double and triple bonded-carbon, assign the type of interaction for the following bonds (HINT: all answers must be expressed in "orbitai-orbital" format, review the double and triple bond slides form your ppt). H. H- H--c-H H' CC--H Blue= Red= Green= Orange= Purple=

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter17: Conjugation And Molecular Orbital (mo) Theory

Section: Chapter Questions

Problem 8CTQ

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Similar questions

For each molecule or molecular ion below, calculate the bond order: N2, N2-, O2 and O2+. In this calculation, show which specifically bonding and anti-bonding molecular orbitals were used in the calculation. Please label molecular orbitals with appropriate “g” (“gerade”) and “u” (“ungerade”) subscripts.
Please help me with the organic chemistry question below. The solutions are linked, as it is one question with 2 parts: 1. A. Draw a molecular orbital diagram for (2E,4E)hexa-2,4-diene and ethene below. Make sure to label orbitals, HOMO, LUMO, nodes, antibonding/bonding, and fill correctly with electrons. 1. B. Use the orbitals drawn in the previous problem to determine if a cycloadditon would occur between the two compounds mentioned and if so, would it be suprafacial or antarafacial. Be sure to specify which orbitals you are using and use those orbitals to demonstrate your answer.
Compare the bonding in formic acid (HCOOH) with that in its conjugate base formate ion (HCOO). Each molecule has a central carbon atom bonded to the two oxygen atoms and to a hydrogen atom. Draw Lewis diagrams, determine the steric numbers and hybridization of the central carbon atom, and give the molecular geometries. How do the orbitals differ in formic acid and the formate molecular ion? The bond lengths of the CO bonds in HCOOH are 1.23 (for the bond to the lone oxygen) and 1.36 (for the bond to the oxygen with a hydrogen atom attached). In what range of lengths do you predict the CO bond length in the formate ion to lie?
Three of the four molecular orbitals for cyclobutadiene are pictured here. Place them in order of increasing energy. (See Figures 9.13, 9.15, 9.16, and 9.18 and the relation of orbital energy and nodes.)
Explain why 1g is the ground state for H2+ . By combining your answer with the answer to Problem 5, what conclusions can you draw about the molecular orbital description of the bond in H2+ ?
The molecular ion HeH+ has an equilibrium bond length of 0.774 Å. Draw an electron correlation diagram for this ion, indicating the occupied MOs. Is HeH+ paramagnetic? When HeH+ dissociates, is a lower energy state reached by forming He+H+ or He++H ?
Explain the difference between the and MOs for homonuclear diatomic molecules. How are bonding and antibonding orbitals different? Why are there two MOs and one MO? Why are the MOs degenerate?
The pyridine molecule (C5H5N) is obtained by replacing one CH group in benzene with a nitrogen atom. Because nitrogen is more electronegative than the CH group, orbitals with electron density on nitrogen are lower in energy. How do you expect the MOs and energy levels of pyridine to differ from those of benzene?
Why is the following molecule a proof thathybridisation must exist? What would have beendifferent if there was no hybridisation?
How would you draw a molecular orbital diagram of butadiene showing the energies and occupancy ofthe orbitals in the ground state? How would you estimate the total pi binding energy of the molecule?
(a) Using only the valence atomic orbitals of a hydrogenatom and a fluorine atom, and following the model ofFigure 9.46, how many MOs would you expect for the HFmolecule? (b) How many of the MOs from part (a) would beoccupied by electrons? (c) It turns out that the difference inenergies between the valence atomic orbitals of H and F aresufficiently different that we can neglect the interaction ofthe 1s orbital of hydrogen with the 2s orbital of fluorine.The 1s orbital of hydrogen will mix only with one 2p orbitalof fluorine. Draw pictures showing the proper orientationof all three 2p orbitals on F interacting with a 1s orbitalon H. Which of the 2p orbitals can actually make a bondwith a 1s orbital, assuming that the atoms lie on the z-axis?(d) In the most accepted picture of HF, all the other atomicorbitals on fluorine move over at the same energy into themolecular orbital energy-level diagram for HF. These arecalled “nonbonding orbitals.” Sketch the energy-level diagramfor HF using…
Hydrofluoric acid (HF) forms strong bonds with other HF molecules to form a zigzag chain-like structure in its liquid form, as shown in the schematic below: a) Draw the molecular orbital diagram for HF. Be sure to clearly label orbitalsymmetries and indicate which orbitals are occupied by electrons. b) Identify and sketch the spatial representation of the HOMO and LUMO for the HF molecule. c) Based on your MO diagram, briefly explain why HF adopts a zigzag structure.