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

Hybridization

Organic Chemistry

1. A Review of General Chemistry

Hybridization

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4:09 minutes

Problem 70c,d

Textbook Question

Predict the hybridization of all non-hydrogen atoms.
(c)
(d)

Verified step by step guidance

Step 1: Identify all non-hydrogen atoms in the molecule. In the given structure, the non-hydrogen atoms are carbon (C) and oxygen (O).

Step 2: Determine the number of regions of electron density (bonds and lone pairs) around each non-hydrogen atom. For example, the first carbon (C) in the double bond has three regions of electron density: one double bond and two single bonds.

Step 3: Use the number of regions of electron density to predict the hybridization. For three regions of electron density, the hybridization is sp². For four regions of electron density, the hybridization is sp³.

Step 4: Analyze the oxygen atom. The oxygen atom has two lone pairs and two bonds (one double bond and one single bond), making a total of four regions of electron density. Therefore, its hybridization is sp³.

Step 5: Repeat the process for all other non-hydrogen atoms in the molecule, ensuring to count lone pairs and bonds accurately to determine their hybridization.

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Key Concepts

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

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of atoms in a molecule. It helps predict the geometry and bonding properties of molecules. For example, sp3 hybridization involves one s and three p orbitals, resulting in a tetrahedral shape, while sp2 hybridization involves one s and two p orbitals, leading to a trigonal planar shape.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They provide a visual representation of the arrangement of electrons and help in predicting molecular geometry and reactivity. Understanding how to draw and interpret Lewis structures is essential for determining hybridization and molecular shape.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

VSEPR theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to this theory, electron pairs will arrange themselves as far apart as possible to minimize repulsion, which directly influences the hybridization and shape of the molecule. This theory is crucial for understanding the spatial arrangement of atoms in a molecule.