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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1:59 minutes

Problem 40b

Textbook Question

Use hybrid orbitals to draw the following molecules.
(b)

Verified step by step guidance

Identify the central atom in the molecule and determine its steric number (the number of sigma bonds and lone pairs around the central atom). This will help determine the hybridization of the central atom.

Based on the steric number, assign the appropriate hybridization to the central atom. For example, a steric number of 2 corresponds to sp hybridization, 3 corresponds to sp², 4 corresponds to sp³, and so on.

Draw the molecule, showing the central atom with its hybrid orbitals. Represent sigma bonds as overlapping orbitals and indicate lone pairs (if any) in the appropriate hybrid orbitals.

For each bonded atom, determine its hybridization (if applicable) and represent its bonding orbitals. For example, hydrogen atoms use unhybridized 1s orbitals, while other atoms may use sp, sp², or sp³ hybrid orbitals depending on their bonding environment.

Combine all the information into a complete structural representation of the molecule, clearly showing the hybrid orbitals involved in bonding and any lone pairs on the central atom.

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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 process of combining atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of atoms in a molecule. This concept is crucial for understanding molecular geometry and bonding, as it explains how atoms can form equivalent bonds in various geometries, such as tetrahedral, trigonal planar, or linear arrangements.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the shape of the molecule. Understanding molecular geometry is essential for predicting the physical and chemical properties of substances.

Orbital Diagrams

Orbital diagrams visually represent the distribution of electrons in atomic and hybrid orbitals. They help illustrate how hybrid orbitals are formed and how they overlap to create bonds between atoms. By using orbital diagrams, one can better understand the electron configuration and bonding characteristics of molecules.

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Related Practice

Textbook Question

Predict the hybridization and geometry of the carbon and nitrogen atoms in the following molecules and ions. (Hint: Resonance.)

Textbook Question

Predict the hybridization and geometry of the carbon and nitrogen atoms in the following molecules and ions. (Hint: Resonance.)

Textbook Question

What orbitals contain the electrons represented as lone pairs in the structures of purine, and pyrimidine?

Textbook Question

Use hybrid orbitals to draw the following molecules.

(a)

Textbook Question

Use hybrid orbitals to draw the following molecules.

(c)

Textbook Question

Use hybrid orbitals to draw the following molecules.

(d)

Textbook Question

Draw the molecular orbital picture of the following molecules and ions. In each, how many electrons are in the p orbital on the central atom? (b) BH₃

Textbook Question

Draw the molecular orbital picture of the following molecules and ions. In each, how many electrons are in the p orbital on the central atom? (c) AlCl₃

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Use hybrid orbitals to draw the following molecules.(b)

Key Concepts

Hybridization

Molecular Geometry

Orbital Diagrams

Watch next

Use hybrid orbitals to draw the following molecules.
(b)