Textbook Question
Draw a complete structural formula and a condensed structural formula for
b. five compounds of formula C3H6O
1
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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 37a,b,c
Draw complete Lewis structures, including lone pairs, for the following compounds.
(a) 
(b) 
(c) 
Verified step by step guidance1
Identify the total number of valence electrons for each compound. For pyridine (C5H5N), count the valence electrons from carbon (4 each), hydrogen (1 each), and nitrogen (5).
Draw the skeletal structure for pyridine, ensuring that the nitrogen atom is part of the six-membered ring and alternating double bonds are present. Add lone pairs to the nitrogen atom to complete its octet.
For pyrrolidine (C4H9N), count the valence electrons from carbon, hydrogen, and nitrogen. Draw a five-membered ring with nitrogen, ensuring that nitrogen has a lone pair and a hydrogen atom attached to it.
For furan (C4H4O), count the valence electrons from carbon, hydrogen, and oxygen. Draw a five-membered ring with oxygen, ensuring that oxygen has two lone pairs and alternating double bonds are present in the ring.
Check each structure to ensure that all atoms have complete octets (except hydrogen, which should have a duet) and that the total number of valence electrons used matches the number calculated initially.
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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 of a molecule and the lone pairs of electrons that may exist. They are essential for visualizing the arrangement of electrons in molecules, showing how atoms are bonded and the presence of any lone pairs. This helps in predicting the geometry, reactivity, and properties of the molecule.
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04:12
Drawing the Lewis Structure for N2H4.
Heterocyclic Compounds
Heterocyclic compounds are cyclic compounds that have atoms of at least two different elements as members of their ring(s). In the given question, pyridine, pyrrolidine, and furan are examples of heterocycles containing nitrogen and oxygen atoms. Understanding the role of these heteroatoms is crucial as they influence the electronic structure and reactivity of the compounds.
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Lone Pairs and Formal Charge
Lone pairs are pairs of valence electrons that are not shared with another atom and are sometimes represented in Lewis structures. They can affect the shape and reactivity of molecules. Formal charge is a concept used to determine the charge distribution within a molecule, calculated by assuming equal sharing of electrons in bonds. Correctly assigning lone pairs and formal charges is vital for accurate Lewis structures.
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02:21Calculate the formal charges of ALL atoms.
Related Practice
Textbook Question
Draw a complete structural formula and a condensed structural formula for
a. three compounds of formula C3H8O
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Textbook Question
Give the molecular formula of each compound shown
(d)
(e)
(f)
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Textbook Question
Draw complete Lewis structures, including lone pairs, for the following compounds.
(g)
(h)
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Textbook Question
Some of the following molecular formulas correspond to stable compounds. When possible, draw a stable structure for each formula. Propose a general rule for the numbers of hydrogen atoms in stable hydrocarbons.
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Textbook Question
Give the molecular formula of each compound shown
(a)
(b)
(c)
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