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

Molecular Orbitals

Organic Chemistry

1. A Review of General Chemistry

Molecular Orbitals

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Problem 24

Textbook Question

Draw the following orbitals:
a. 3s orbital
b. 4s orbital
c. 3p orbital

Verified step by step guidance

Understand that orbitals are regions in space where there is a high probability of finding an electron. The shapes of orbitals are determined by quantum numbers, and each type of orbital (s, p, d, etc.) has a characteristic shape.

For the 3s orbital: The 's' orbitals are spherical in shape. The 3s orbital will have three radial nodes (regions where the probability of finding an electron is zero). To draw it, sketch a sphere with concentric spherical shells representing the nodes.

For the 4s orbital: Similar to the 3s orbital, the 4s orbital is also spherical but larger in size. It will have four radial nodes. Draw a larger sphere with concentric spherical shells to represent the nodes.

For the 3p orbital: The 'p' orbitals are dumbbell-shaped and oriented along the x, y, or z axes. The 3p orbital will have two lobes with a single nodal plane passing through the nucleus. To draw it, sketch a dumbbell shape with a plane cutting through the center, and label it as 3p.

Label each orbital clearly in your drawing to indicate whether it is 3s, 4s, or 3p. Ensure that the relative sizes and nodal structures are consistent with the quantum mechanical descriptions of these orbitals.

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Key Concepts

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

Atomic Orbitals

Atomic orbitals are regions in an atom where there is a high probability of finding electrons. They are defined by quantum numbers and come in various shapes, including s, p, d, and f orbitals. The shape and size of these orbitals are crucial for understanding electron configurations and chemical bonding.

Quantum Numbers

Quantum numbers are numerical values that describe the energy levels and shapes of atomic orbitals. The principal quantum number (n) indicates the energy level, while the angular momentum quantum number (l) defines the shape of the orbital. For example, s orbitals have l=0 (spherical shape), and p orbitals have l=1 (dumbbell shape).

Orbital Diagrams

Orbital diagrams visually represent the arrangement of electrons in an atom's orbitals. They illustrate the shape and orientation of orbitals, helping to understand electron distribution. Drawing these diagrams for specific orbitals, like 3s, 4s, and 3p, aids in visualizing their spatial characteristics and energy levels.

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Textbook Question

Draw orbital pictures of the pi bonding in the following compounds:

f. CH₃CH=NCH=C=O

Textbook Question

In this, and previous, chapters, we have seen 1,2-alkyl and 1,2-hydride shifts. If both are possible, as in the carbocation shown, which would you expect to occur? Explain your answer.

Textbook Question

Draw orbital pictures of the pi bonding in the following compounds:

a. CH₃COCH₃

b. HCN

Textbook Question

Indicate the kind of molecular orbital (σ, σ*, π, or π*) that results when the two atomic orbitals are combined:

a. <IMAGE>

b. <IMAGE>

Textbook Question

A molecular orbital diagram is shown for the C―Cl bond in chloromethane. If two more electrons were added to chloromethane, where would the electrons go?

<IMAGE>

Textbook Question

There is free rotation around the C―C bond in ethane. There is an extremely high barrier to rotation around the C=C bond in in ethene. Explain.

Textbook Question

Looking ahead in Chapter 4, we explain that molecules like CH₃⁺ are Lewis acids or electron pair acceptors. Into which orbital would the new electron pair go?

Textbook Question

Draw the molecular orbital picture of trans-but-2-ene. Be sure to label all σ and π bonds. Is there free rotation around the C₂― C₃ bond? Why or why not?

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Draw the following orbitals:a. 3s orbitalb. 4s orbitalc. 3p orbital

Key Concepts

Atomic Orbitals

Quantum Numbers

Orbital Diagrams

Watch next

Draw the following orbitals:
a. 3s orbital
b. 4s orbital
c. 3p orbital