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 Geometry

Organic Chemistry

1. A Review of General Chemistry

Molecular Geometry

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3:51 minutes

Problem 39e

Textbook Question

Describe the orbitals used in bonding and the bond angles in the following compounds:
e. BF₃

Verified step by step guidance

Identify the central atom in BF3. Boron (B) is the central atom, as it is less electronegative than fluorine (F) and can form three bonds.

Determine the hybridization of the central atom. Boron in BF3 forms three sigma bonds with fluorine atoms. To achieve this, boron undergoes sp² hybridization, which involves mixing one s orbital and two p orbitals to form three equivalent sp² hybrid orbitals.

Describe the geometry of the molecule. The sp² hybridization results in a trigonal planar geometry, where the three sp² hybrid orbitals are arranged 120° apart in a plane to minimize electron pair repulsion.

Explain the bond angles. In a trigonal planar geometry, the bond angles between the fluorine atoms are approximately 120°.

Discuss the orbitals involved in bonding. Each B-F bond is formed by the overlap of a boron sp² hybrid orbital with a fluorine p orbital, resulting in a sigma bond.

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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 by which atomic orbitals mix to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In BF3, the boron atom undergoes sp2 hybridization, resulting in three equivalent sp2 hybrid orbitals that are oriented in a planar arrangement.

Bond Angles

Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the arrangement of electron pairs around the central atom. In BF3, the bond angles are approximately 120 degrees due to the trigonal planar geometry resulting from the sp2 hybridization of boron.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. BF3 has a trigonal planar geometry, which arises from the arrangement of the three fluorine atoms around the central boron atom, minimizing electron pair repulsion according to VSEPR theory.

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Related Practice

Textbook Question

For each of the following molecules, indicate the hybridization of each carbon and give the approximate values of all the bond angles:

a. CH₃C≡CH

Textbook Question

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

Textbook Question

In most amines, the nitrogen atom is sp³ hybridized, with a pyramidal structure and bond angles close to 109°. In urea, both nitrogen atoms are found to be planar, with bond angles close to 120°. Explain this surprising finding. (Hint: Consider resonance forms and the overlap needed in them.)

Textbook Question

Predict the hybridization, geometry, and bond angles for the carbon and nitrogen atoms in acetonitrile (CH₃–C≡N:).

Textbook Question

Predict the approximate bond angles in

a. the methyl cation.

b. the methyl radical.

c. the methyl anion.

Textbook Question

Predict the approximate bond angles for the following:

c. the C—C—N bond angle in CH₃C≡N

d. the C—C—N bond angle in CH₃CH₂NH₂

Textbook Question