Concept explainers
Interpretation:
The orbital interaction that would be necessary to generate each sp hybrid orbital from pure AOs is to be drawn by considering the given pair of sp hybrid orbitals.
Concept introduction:
Any sp-hybridized atom has two sp hybrid orbitals and two unhybridized p orbitals. The two sp hybrid orbitals are aligned along the same axis and point in opposite directions. Mixing of the lobe with the same phase leads to constructive interference, thus increasing the size of the lobe. The other lobe of p orbital having an opposite phase as s orbital leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The larger lobe shows the overlapping of s and p orbitals with the same phase. The smaller lobe is often omitted entirely for simplicity.
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Organic Chemistry: Principles and Mechanisms (Second Edition)
- 4. ,A: Briefly describe why the p orbital can contain a positive charge and hybridized orbital cannot. Use pictures in your answer. B: Briefly explain why a hybridized orbital can contain a negative charge, and P-orbital cannot. Use pictures in your answer.arrow_forwardCircle all the isolated (not conjugated) pi bond(s).arrow_forwardOne of the orbital interactions we did not consider in this chapter is that between an s AO from one atom and a p AO from another atom in the fashion shown. These orbitals will not interact while in this orientation. Explain why.arrow_forward
- 3 Consider this compound when answering the questions below. OH How many units of unsaturation does this compound have? type your answer... How many atoms are sp² hybridized? type your answer... How many bent atoms are there? type your answer... Previousarrow_forwardTo preview the image Click Here t A) For the indicated Carbon atom, give its hybridization and a list of all hybridized and unhybridized atomic orbitals and how each orbital is used for this atom. B) REDRAW the structure on your paper. Directly ON TOP of the structure, draw pictorial representation of the T for the localized bonding molecular orbitals for the bond that is indicated in the following structure. State the atomic orbitals that are used to build the molecular orbitals. Part B CEC-H Part A pointing to this carbonarrow_forward2. Which of followings represents a hybrid orbital?arrow_forward
- What is the molecular formula?For each heteroatom (not C or H), indicate the hybridization. Also note whether each lone pair is localized (on the atom) or delocalized (through resonance).arrow_forwardCould we cut just one bond in the "starting" molecule shown in the drawing area below to create this "target" molecule? The target molecule. If so, highlight the bond to be cut. If not, check the box under the drawing area that says Not possible. Note: it's OK if cutting the bond creates more than one molecule, as long as one of them is the target molecule. Xarrow_forwardConsider a carbon atom that is sp hybridized. Indicate how many of each orbital exist on this carbon atom by sorting each orbital type. Consider the outer valence only.arrow_forward
- 3) Combine any Atomic orbitals to form Molecular orbitals assuming they fulfill the phase and energy requirement. Construct MO diagram (include AOs, MOs, pictures of each, electrons, HOMO, LUMO, B.O., and comparative energies, etc.). REMOVE an ELECTRON to form CATION Please only do part 3. The first image shows the problemarrow_forwardAmong the resonance structures that occur in the structure below, please tell us a resonance structure that does not actually contribute to a resonance hybrid. I want the reason to be detailed.arrow_forwardA triple bond occurs when between two atoms that each have: Group of answer choices one hybridized orbital and two p orbitals. three hybridized orbitals and one p orbital. one hybridized orbital and three p orbitals. two hybridized orbitals and two p orbitals.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning