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

Lewis Structure

Organic Chemistry

1. A Review of General Chemistry

Lewis Structure

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3:06 minutes

Problem 62v

Textbook Question

Draw the Lewis structure for the following molecular formulas.
(v) CH₅N

Verified step by step guidance

Step 1: Count the total number of valence electrons in the molecule. Carbon (C) has 4 valence electrons, hydrogen (H) has 1 valence electron each (5 hydrogens contribute 5 electrons), and nitrogen (N) has 5 valence electrons. Add these together to determine the total number of valence electrons available for the Lewis structure.

Step 2: Identify the central atom. In this case, carbon (C) is typically the central atom because it can form the most bonds. Nitrogen (N) will likely be bonded to carbon, and the hydrogens (H) will be distributed around the structure.

Step 3: Arrange the atoms and form single bonds. Place carbon (C) in the center, bond it to nitrogen (N) with a single bond, and attach the hydrogens (H) to the remaining available bonding sites on carbon and nitrogen. Each single bond represents 2 electrons.

Step 4: Distribute the remaining valence electrons to satisfy the octet rule (or duet rule for hydrogen). Start by completing the octet for nitrogen (N) by adding lone pairs if necessary. Ensure that all hydrogens have 2 electrons (a full duet).

Step 5: Verify the structure. Check that the total number of valence electrons used matches the total calculated in Step 1. Also, confirm that all atoms (except hydrogen) satisfy the octet rule and that the structure is stable.

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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 use dots to represent valence electrons and lines to indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the molecule's structure and stability. For example, in CH₅N, carbon has four, hydrogen has one, and nitrogen has five valence electrons, which must be accounted for when constructing the Lewis structure.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom, which can affect the molecule's physical and chemical properties. Understanding molecular geometry helps in predicting the shape of the molecule formed by CH₅N, which is important for its reactivity and interactions.

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