Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Sigma and Pi Bonds

Organic Chemistry

1. A Review of General Chemistry

Sigma and Pi Bonds

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4:31 minutes

Problem 75c

Textbook Question

For the following partial structures, the bond is shown. Add the indicated number of bonds, being sure to specify the orientation (that is, x, y, or z axis) of the p orbitals used.
(c)

Verified step by step guidance

Examine the given partial structure and identify the atoms involved in the bond where the π bond is to be added. Recall that π bonds are formed by the sideways overlap of p orbitals.

Determine the orientation of the p orbitals that will overlap to form the π bond. The orientation can be along the x, y, or z axis, depending on the spatial arrangement of the atoms in the molecule.

Ensure that the p orbitals involved in the π bond are unhybridized. For example, in sp² hybridized atoms, one p orbital remains unhybridized and is available for π bonding.

Add the π bond by specifying the overlap of the unhybridized p orbitals. For instance, if the p orbitals overlap along the y-axis, the π bond is oriented in the y direction.

Verify that the addition of the π bond does not violate the octet rule or any other bonding rules for the atoms involved. Ensure the structure remains chemically valid.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Pi Bonds

A pi bond is a type of covalent bond that occurs when two lobes of an orbital on one atom overlap with two lobes of an orbital on another atom. This bond is formed from the side-to-side overlap of p orbitals, which allows for the sharing of electrons. Pi bonds are typically found in double and triple bonds, where they accompany sigma bonds, and they play a crucial role in the geometry and reactivity of organic molecules.

Orbital Orientation

The orientation of orbitals refers to the spatial arrangement of atomic orbitals in relation to each other. In the context of pi bonds, p orbitals can align along different axes (x, y, or z) to form the bond. Understanding the orientation is essential for predicting molecular geometry and the resulting physical and chemical properties of the compound.

Hybridization

Hybridization is the concept of mixing atomic orbitals to create new hybrid orbitals that can form bonds with specific geometries. In organic chemistry, hybridization helps explain the bonding and shape of molecules. For example, sp2 hybridization involves one s and two p orbitals, leading to the formation of a trigonal planar structure, which is relevant when considering the formation of pi bonds in alkenes.

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