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

13. Alcohols and Carbonyl Compounds

Oxidizing and Reducing Agents

Organic Chemistry

13. Alcohols and Carbonyl Compounds

Oxidizing and Reducing Agents

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Problem 4c

Textbook Question

Determine the oxidation number of each carbon indicated by an arrow.
(c)

Verified step by step guidance

Identify the structure: The image shows a benzene ring, which is a six-membered carbon ring with alternating double bonds.

Determine the general rule for oxidation numbers: In organic chemistry, the oxidation number of carbon is determined by the number of electrons it 'owns' compared to its neutral state.

Assign electrons: In a C-C bond, each carbon gets one electron. In a C-H bond, carbon gets both electrons. In a C=C bond, each carbon gets one electron from the double bond.

Calculate the oxidation number: For the carbon indicated by the arrow, count the electrons it 'owns' and compare it to the number of valence electrons in a neutral carbon atom (which is 4).

Apply the formula: The oxidation number is calculated as the difference between the number of valence electrons in the neutral atom and the number of electrons 'owned' by the atom in the molecule.

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Key Concepts

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

Oxidation Number

The oxidation number, or oxidation state, is a theoretical charge assigned to an atom in a molecule, reflecting its degree of oxidation. It helps in understanding electron transfer in redox reactions. For carbon, common oxidation states range from -4 in methane (CH4) to +4 in carbon dioxide (CO2), depending on the number of bonds it forms with more electronegative elements.

Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a chemical bond. In determining oxidation numbers, the relative electronegativities of the atoms involved are crucial. For example, when carbon is bonded to more electronegative atoms like oxygen or chlorine, it typically has a higher oxidation state due to the electron pull from these atoms.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, which include: the oxidation number of an atom in its elemental form is zero, the oxidation number of a monoatomic ion is equal to its charge, and in compounds, the sum of oxidation numbers must equal the overall charge of the molecule. These rules guide the determination of oxidation states for each carbon in a given structure.

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