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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3:32 minutes

Problem 5c

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

Verified step by step guidance

Step 1: Identify the central atom in the molecule. In AlCl₃, aluminum (Al) is the central atom because it is less electronegative than chlorine (Cl) and can form bonds with three chlorine atoms.

Step 2: Determine the valence electrons of the central atom. Aluminum (Al) is in Group 13 of the periodic table, so it has 3 valence electrons.

Step 3: Analyze the bonding in AlCl₃. Each chlorine atom forms a single covalent bond with aluminum, using one of aluminum's valence electrons. This leaves no lone pairs on aluminum, and all three valence electrons are involved in bonding.

Step 4: Consider the molecular geometry. AlCl₃ has a trigonal planar geometry due to sp² hybridization of the aluminum atom. The p orbitals on aluminum are involved in forming the sigma bonds with chlorine atoms, leaving no unoccupied p orbitals.

Step 5: Conclude the number of electrons in the p orbital of the central atom. Since all p orbitals of aluminum are involved in bonding and there are no lone pairs, there are 0 electrons in the p orbital of the central aluminum atom in AlCl₃.

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Key Concepts

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

Molecular Orbital Theory

Molecular Orbital Theory describes how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons. In this theory, electrons are delocalized over the entire molecule rather than being localized around individual atoms. Understanding this concept is crucial for visualizing the electron distribution in molecules like AlCl₃ and determining the occupancy of p orbitals.

Hybridization

Hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In AlCl₃, the aluminum atom undergoes sp² hybridization, resulting in three equivalent hybrid orbitals that form sigma bonds with chlorine atoms. Recognizing the hybridization state helps in understanding the geometry and bonding characteristics of the molecule.

Electron Configuration

Electron configuration refers to the distribution of electrons in an atom's orbitals. For the central atom in AlCl₃, aluminum has an atomic number of 13, leading to a specific electron configuration. Analyzing the electron configuration allows us to determine how many electrons occupy the p orbitals, which is essential for answering the question regarding the p orbital occupancy in the molecule.

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Related Practice

Textbook Question

Use hybrid orbitals to draw the following molecules.

(b)

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

Explain why a σ bond formed by overlap of an s orbital with an sp³ orbital of carbon is stronger than a σ bond formed by overlap of an s orbital with a p orbital of carbon.