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

Electronegativity

Organic Chemistry

1. A Review of General Chemistry

Electronegativity

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1:38 minutes

Problem 77(3)

Textbook Question

a. Draw a Lewis structure for each of the following:
b. Draw a structure for each of the species that shows approximate bond angles.
c. Which species have no dipole moment?
3. N₃⁻

Verified step by step guidance

Step 1: For part A, start by determining the total number of valence electrons for the N₃⁻ ion. Nitrogen has 5 valence electrons, and there are three nitrogen atoms. Additionally, the negative charge adds one extra electron. Use the formula: \( \text{Total valence electrons} = 3(5) + 1 = 16 \).

Step 2: Arrange the three nitrogen atoms in a linear structure (as N₃⁻ is known to be linear). Place a single bond between each pair of nitrogen atoms. Distribute the remaining electrons as lone pairs to satisfy the octet rule for each atom, starting with the outer atoms.

Step 3: For part B, determine the approximate bond angles in the N₃⁻ ion. Since the molecule is linear, the bond angle between the nitrogen atoms is approximately \( 180^\circ \). Draw the structure with this bond angle clearly indicated.

Step 4: For part C, analyze the dipole moment of the N₃⁻ ion. Since the molecule is linear and symmetric, the dipoles from the bonds cancel out, resulting in no net dipole moment. Conclude that N₃⁻ has no dipole moment.

Step 5: Summarize the findings: (1) Draw the Lewis structure with lone pairs and formal charges, (2) indicate the linear geometry with \( 180^\circ \) bond angles, and (3) confirm that N₃⁻ has no dipole moment due to its symmetry.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They help visualize the arrangement of electrons and the connectivity of atoms, which is crucial for understanding molecular geometry and reactivity. In the case of N3−, the Lewis structure will illustrate how the nitrogen atoms are bonded and how the negative charge is distributed.

Molecular Geometry and Bond Angles

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule, which influences its physical and chemical properties. The VSEPR (Valence Shell Electron Pair Repulsion) theory is often used to predict bond angles based on the repulsion between electron pairs. Understanding the geometry of species like N3− is essential for determining the approximate bond angles and the overall shape of the molecule.

Dipole Moment

A dipole moment is a measure of the separation of positive and negative charges in a molecule, indicating its polarity. Molecules with an uneven distribution of electron density exhibit a dipole moment, while symmetrical molecules may not. Identifying species with no dipole moment involves analyzing their symmetry and the arrangement of polar bonds, which is key to understanding their behavior in electric fields and interactions with other molecules.

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