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

Previous problemNext problem

1:53 minutes

Problem 40c

Textbook Question

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

Verified step by step guidance

Step 1: Understand the concept of hybrid orbitals. Hybrid orbitals are formed by the mixing of atomic orbitals (such as s, p, and sometimes d orbitals) to create new orbitals that are better suited for bonding in molecules. Common types include sp, sp², and sp³ hybridization.

Step 2: Determine the central atom in the molecule and its steric number. The steric number is calculated as the sum of the number of bonded atoms and lone pairs around the central atom. This will help identify the type of hybridization.

Step 3: Assign the hybridization based on the steric number. For example: steric number 2 corresponds to sp hybridization, steric number 3 corresponds to sp² hybridization, and steric number 4 corresponds to sp³ hybridization.

Step 4: Draw the molecule using the hybrid orbitals. Represent the central atom with its hybrid orbitals and show the bonds formed with other atoms. Use appropriate bond angles based on the hybridization (e.g., 180° for sp, 120° for sp², and 109.5° for sp³).

Step 5: Include lone pairs and pi bonds if applicable. Lone pairs occupy hybrid orbitals, while pi bonds are formed by unhybridized p orbitals overlapping sideways. Ensure the drawing reflects the correct geometry and bonding.

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 process of combining atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of a molecule. This concept is crucial for understanding molecular geometry and bonding properties, as it explains how atoms can form equivalent bonds in molecules. For example, in methane (CH4), the carbon atom undergoes sp3 hybridization, resulting in four equivalent bonds with hydrogen atoms.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the types of hybrid orbitals involved and the number of electron pairs around the central atom. Understanding molecular geometry is essential for predicting the shape and reactivity of molecules, as seen in the tetrahedral shape of methane due to sp3 hybridization.

Bonding and Lone Pairs

In molecular structures, bonding pairs of electrons are shared between atoms, while lone pairs are non-bonding electrons localized on a single atom. The presence of lone pairs affects the geometry and angles between bonds, as they occupy space and repel bonding pairs. For instance, in water (H2O), the two lone pairs on oxygen lead to a bent molecular shape, deviating from the ideal tetrahedral angle.

Watch next

Master How carbon creates 4 partially-filled orbitals. with a bite sized video explanation from Johnny

Start learning

Related Videos

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

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.

(b)

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

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.

Show more practices

Download the Mobile app

Privacy

Do not sell my personal information

Accessibility

Patent notice

Sitemap

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

Key Concepts

Hybridization

Molecular Geometry

Bonding and Lone Pairs

Watch next

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