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.
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Ch.1 - Structure and Bonding
Wade9th EditionOrganic ChemistryISBN: 9780135213728
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Table of contents
- Ch.1 - Structure and Bonding107
- Ch. 2 - Acids and Bases; Functional Groups115
- Ch.3 - Structure and Stereochemistry of Alkanes100
- Ch.4 - The Study of Chemical Reactions99
- Ch.5 - Stereochemistry93
- Ch.6 - Alkyl Halides; Nucleophilic Substitution118
- Ch. 7 - Structure and Synthesis of Alkenes; Elimination158
- Ch.8 - Reactions of Alkenes171
- Ch.9 - Alkynes91
- Ch.10 - Structure and Synthesis of Alcohols143
- Ch.11 - Reactions of Alcohols104
- Ch. 12 - Infrared Spectroscopy and Mass Spectrometry22
- Ch. 13 - Nuclear Magnetic Resonance Spectroscopy45
- Ch. 14 - Ethers, Epoxides, and Thioethers72
- Ch. 15 - Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy89
- Ch. 16 - Aromatic Compounds74
- Ch. 17 - Reactions of Aromatic Compounds126
- Ch. 18 - Ketones and Aldehydes193
- Ch. 19 - Amines129
- Ch. 20 - Carboxylic Acids77
- Ch. 21 - Carboxylic Acid Derivatives141
- Ch. 22 - Condensations and Alpha Substitutions of Carbonyl Compounds175
- Ch. 23 - Carbohydrates and Nucleic Acids93
- Ch. 24 - Amino Acids, Peptides, and Proteins54
Chapter 1, Problem 14c
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 guidance1
Convert the percentage composition of each element to grams, assuming a 100 g sample. This gives you 25.6 g of C, 4.32 g of H, 15.0 g of N, and 37.9 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), N (14.01 g/mol), and Cl (35.45 g/mol).
Determine the simplest whole number ratio of moles of each element by dividing each mole value by the smallest number of moles calculated in the previous step.
Use the mole ratio to write the empirical formula. If necessary, multiply the ratios by a common factor to get whole numbers.
Calculate the molecular formula by comparing the empirical formula mass to the given molecular weight (93 g/mol). Multiply the subscripts in the empirical formula by the appropriate factor to match the molecular weight.
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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 percentage composition of each element in a sample and is crucial for understanding the basic composition of a substance without detailing the actual number of atoms present.
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Molecular Formula
The molecular formula provides the actual number of atoms of each element in a molecule of a compound. It can be a multiple of the empirical formula and is essential for determining the precise composition and structure of a compound, which is important for predicting its chemical behavior.
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Structural Representation
Structural representation involves depicting the arrangement of atoms within a molecule, including the types of bonds and the connectivity between atoms. This is vital for visualizing how the molecular formula translates into a specific three-dimensional structure, which influences the compound's properties and reactivity.
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Related Practice
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.
3
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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.
2
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Textbook Question
Draw line-angle structures for the compounds (a) through (h).
g. (CH3CH2)2CO
h. (CH3)3COH
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Textbook Question
Make a model of propane (C3H8), and draw this model using dashed lines and wedges to represent bonds going back and coming forward.
2
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Textbook Question
Predict the hybridization of the oxygen atom in water, H2O. Draw a picture of its three-dimensional structure, and explain why its bond angle is 104.5°.
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