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)
- To 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_forwardWhat is the hybridization at each of the carbon atoms? Drag the appropriate labels to their respective targets. Note: not all labels will be used. sp sp³ sp³ d sp³d²arrow_forwardCircle all the isolated (not conjugated) pi bond(s).arrow_forward
- Could 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_forwardCheck all statements which are not true. ☐Electrons placed in antibonding orbitals destabilize a species. ☐The total number of combining atomic orbitals and the total number of molecular orbitals formed is always the same. ☐One of the molecular orbitals formed by linear combination of two atomic orbitals (AOs) acquires lower energy than the combining AOs while the other molecular orbital acquires higher energy than the combining AOs. ☐A fractional bond order results in an unstable chemical bond. ☐Non-bonding molecular orbitals also sometimes contribute to the bond order.arrow_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 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_forwardThe next part of the problem is to draw the resonance hybrid. (Exclude formal charges) I’m not sure where to put the dotted resonance lines of the hybrid structure.arrow_forward3. Draw an orbital overlap model of the following molecule and indicate the most reactive electron pair. Explain your reasoning based on VB theory.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning