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 4g

Textbook Question

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

Verified step by step guidance

Identify the structure: The molecule shown is an ether, specifically diethyl ether, with the formula \( C_2H_5OC_2H_5 \). The arrow points to the carbon atom in one of the ethyl groups.

Determine the bonds: The carbon indicated by the arrow is bonded to two hydrogen atoms and one other carbon atom, as well as the oxygen atom in the ether linkage.

Assign oxidation numbers: In organic chemistry, the oxidation number of carbon is determined by considering the electronegativity of the atoms it is bonded to. Carbon is less electronegative than oxygen but more electronegative than hydrogen.

Calculate the oxidation number: For each bond to a more electronegative atom (oxygen), assign +1. For each bond to a less electronegative atom (hydrogen), assign -1. Bonds to other carbon atoms do not affect the oxidation number.

Apply the rules: The carbon atom has two bonds to hydrogen (each contributing -1) and one bond to oxygen (contributing +1). Therefore, the oxidation number of the carbon atom is calculated as \(-1 - 1 + 1 = -1\).

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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). Determining oxidation numbers involves analyzing the bonding and electronegativity of surrounding atoms.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how an atom bonds with others. For carbon, which has four valence electrons, this allows it to form four covalent bonds, influencing its oxidation state. Understanding the distribution of valence electrons is essential for calculating oxidation numbers, as it directly relates to the atom's bonding environment.

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 considered; more electronegative atoms will attract shared electrons more strongly, leading to a higher oxidation state for the less electronegative atom. This concept is vital for accurately assessing the oxidation states of carbon in various compounds.

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