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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4:09 minutes

Problem 39d

Textbook Question

Describe the orbitals used in bonding and the bond angles in the following compounds:
d. N₂

Verified step by step guidance

Identify the type of bonding in N₂: Nitrogen (N) forms a triple bond with another nitrogen atom in N₂. This triple bond consists of one sigma (σ) bond and two pi (π) bonds.

Determine the orbitals involved in the sigma bond: The sigma bond is formed by the head-on overlap of two sp-hybridized orbitals, one from each nitrogen atom.

Determine the orbitals involved in the pi bonds: The two pi bonds are formed by the side-by-side overlap of unhybridized p orbitals (px and py) from each nitrogen atom.

Analyze the bond angles: Since the nitrogen atoms in N₂ are sp-hybridized, the molecule is linear, and the bond angle is 180°.

Summarize the bonding and geometry: N₂ has a triple bond (1 σ bond and 2 π bonds), and the molecule is linear with a bond angle of 180° due to sp hybridization.

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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 of combining atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of nitrogen (N2), the two nitrogen atoms undergo sp hybridization, resulting in the formation of two sp hybrid orbitals that are used to create a triple bond between them.

Bond Angles

Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the hybridization of the orbitals involved. For N2, the bond angle is not applicable in the traditional sense since it is a diatomic molecule with a linear geometry, resulting in a bond angle of 180 degrees between the two nitrogen atoms.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. In N2, the linear geometry arises from the sp hybridization of the nitrogen atoms, leading to a straight-line arrangement that maximizes the distance between the bonding electrons, thereby minimizing repulsion and stabilizing the molecule.