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

Previous problemNext problem

2: minutes

Problem 65a

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

Verified step by step guidance

Step 1: Analyze the structure of the molecule CH3C≡CH. The molecule consists of three carbons: one in the methyl group (CH3), one in the triple bond (C≡), and one in the terminal alkyne (CH).

Step 2: Determine the hybridization of each carbon atom. The carbon in the CH3 group is bonded to three hydrogens and one other carbon, making it sp³ hybridized. The carbon in the triple bond (C≡) is bonded to one other carbon and one hydrogen, making it sp hybridized. The terminal carbon (CH) is also sp hybridized due to its triple bond.

Step 3: Recall the bond angles associated with each hybridization. For sp³ hybridized carbons, the bond angles are approximately 109.5° (tetrahedral geometry). For sp hybridized carbons, the bond angles are approximately 180° (linear geometry).

Step 4: Assign the bond angles to each carbon. The CH3 carbon has bond angles of approximately 109.5°. The C≡ carbon and the terminal CH carbon both have bond angles of approximately 180° due to their linear geometry.

Step 5: Summarize the findings. The CH3 carbon is sp³ hybridized with bond angles of 109.5°. The C≡ carbon and the terminal CH carbon are sp hybridized with bond angles of 180°.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above

Video duration:

Play a video:

Was this helpful?

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. In organic chemistry, carbon typically undergoes sp, sp², or sp³ hybridization, depending on its bonding environment. For example, sp hybridization occurs when a carbon atom forms two sigma bonds and has two unhybridized p orbitals, as seen in alkynes.

Bond Angles

Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the hybridization of the atoms involved. In sp hybridized carbon, the bond angles are approximately 180 degrees due to the linear arrangement of the bonds. Understanding bond angles is crucial for predicting the geometry and reactivity of organic molecules.

Alkynes

Alkynes are a class of hydrocarbons characterized by at least one carbon-carbon triple bond. The presence of a triple bond leads to sp hybridization of the carbon atoms involved, resulting in a linear geometry. In the case of CH3C≡CH, the terminal carbon atoms are sp hybridized, while the central carbon is also sp hybridized, contributing to the overall linear structure of the molecule.

Watch next

Master Molecular Geometry Explained. with a bite sized video explanation from Johnny

Start learning

Related Videos

Related Practice

Textbook Question

Predict the hybridization, geometry, and bond angles for the central atoms in

b. CH₃CH=NH

Textbook Question

Predict the hybridization, geometry, and bond angles for the central atoms in

a. but-2-ene, CH₃CH=CHCH₃

Textbook Question

a. Which of the species have bond angles of 109.5°?

b. Which of the species have bond angles of 120°?

H₂O H₃O⁺ ⁺CH₃ BF₃

Textbook Question

Do the sp² carbons and the indicated sp³ carbons lie in the same plane?

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

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

e. BF₃

Show more practices

Download the Mobile app

Privacy

Do not sell my personal information

Accessibility

Patent notice

Sitemap

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

Key Concepts

Hybridization

Bond Angles

Alkynes

Watch next

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