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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5:45 minutes

Problem 39c

Textbook Question

Describe the orbitals used in bonding and the bond angles in the following compounds:
c. H₂CO

Verified step by step guidance

Identify the central atom in the molecule H₂CO. In this case, the central atom is carbon (C).

Determine the hybridization of the central atom. Carbon in H₂CO forms a double bond with oxygen and two single bonds with hydrogen atoms. This indicates sp² hybridization, as one s orbital and two p orbitals mix to form three sp² hybrid orbitals.

Describe the orbitals involved in bonding. The carbon atom uses its sp² hybrid orbitals to form sigma (σ) bonds with the two hydrogen atoms and one sigma bond with the oxygen atom. The remaining unhybridized p orbital on carbon overlaps with a p orbital on oxygen to form a pi (π) bond, completing the double bond.

Explain the bond angles. In sp² hybridization, the three sp² orbitals are arranged in a trigonal planar geometry around the central atom, resulting in bond angles of approximately 120°.

Summarize the bonding and geometry. The molecule H₂CO has a trigonal planar geometry around the carbon atom, with sp² hybrid orbitals forming sigma bonds and a p orbital forming a pi bond in the double bond with oxygen.

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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 H2CO (formaldehyde), the central carbon atom undergoes sp2 hybridization, resulting in three equivalent sp2 hybrid orbitals that are arranged in a trigonal planar geometry.

Bond Angles

Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the arrangement of hybrid orbitals. In H2CO, the bond angles around the carbon atom are approximately 120 degrees due to its sp2 hybridization, reflecting the trigonal planar structure of the molecule.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. For H2CO, the molecular geometry is trigonal planar, which is characterized by the carbon atom at the center with two hydrogen atoms and one oxygen atom bonded to it, leading to a flat structure that affects the molecule's reactivity and properties.