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

Intro to Organic Chemistry

Organic Chemistry

1. A Review of General Chemistry

Intro to Organic Chemistry

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6:13 minutes

Problem 14d

Textbook Question

Compute the empirical and molecular formulas for each of the following elemental analyses. In each case, propose at least one structure that fits the molecular formula.

Verified step by step guidance

Convert the percentage composition of each element to grams, assuming a 100 g sample. This gives 38.4 g of C, 4.8 g of H, and 56.8 g of Cl.

Convert the mass of each element to moles by dividing by their respective atomic masses: C (12.01 g/mol), H (1.008 g/mol), and Cl (35.45 g/mol).

Determine the simplest whole number ratio of moles of each element by dividing each by the smallest number of moles calculated in the previous step.

Use the whole number ratio to write the empirical formula of the compound.

Calculate the molecular formula by comparing the empirical formula mass to the given molecular weight (125 g/mol) and multiplying the subscripts in the empirical formula by the appropriate factor.

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Key Concepts

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

Empirical Formula

The empirical formula represents the simplest whole-number ratio of atoms of each element in a compound. It is derived from the elemental analysis data, which provides the mass percentages of each element present. For example, if a compound contains 40% carbon and 60% oxygen, the empirical formula can be determined by converting these percentages to moles and simplifying the ratio.

Molecular Formula

The molecular formula indicates the actual number of atoms of each element in a molecule of a compound. It can be derived from the empirical formula by multiplying the subscripts by a whole number, known as the molecular weight factor. For instance, if the empirical formula is CH2 and the molecular weight is 28 g/mol, the molecular formula would be C2H4, as it corresponds to a molecular weight of 28 g/mol.

Structural Representation

Structural representation involves depicting the arrangement of atoms within a molecule, which can be illustrated through various formats such as Lewis structures, condensed formulas, or skeletal structures. This representation is crucial for understanding the chemical behavior and properties of the compound. For example, knowing the molecular formula C2H4 allows for the proposal of structures like ethylene, which has a double bond between the carbon atoms.

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Related Practice

Textbook Question

In 1934, Edward A. Doisy of Washington University extracted 3000 lb of hog ovaries to isolate a few milligrams of pure estradiol, a potent female hormone. Doisy burned 5.00 mg of this precious sample in oxygen and found that 14.54 mg of CO₂ and 3.97 mg of H₂O were generated.

a. Determine the empirical formula of estradiol.

Textbook Question

Compute the empirical and molecular formulas for each of the following elemental analyses. In each case, propose at least one structure that fits the molecular formula.

Textbook Question

Compute the empirical and molecular formulas for each of the following elemental analyses. In each case, propose at least one structure that fits the molecular formula.

Textbook Question

Compute the empirical and molecular formulas for each of the following elemental analyses. In each case, propose at least one structure that fits the molecular formula.

Multiple Choice

How does photosynthesis benefit heterotrophs in the context of organic chemistry?

Multiple Choice

Which of the following best describes disruptive selection in the context of organic chemistry?

Multiple Choice

Which pattern in the fossil record supports the conclusion that species go extinct?

Multiple Choice

Why are yeast considered good model organisms for studying natural selection in organic chemistry?

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