Organic Chemistry (9th Edition)
9th Edition
ISBN: 9780321971371
Author: Leroy G. Wade, Jan W. Simek
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 1, Problem 1.34SP
Draw Lewis structures for
- a. two compounds of formula C4H10
- b. two compounds of formula C2H6O
- c. two compounds of formula C2H7N
- d. three compounds of formula C2H7NO
- e. three compounds of formula C2H8O2
- f. three compounds of formula C2H4O
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
5. Draw Lewis structures for each molecular formula.
H
A. C₂H4Cl₂ (two isomers)
B. C3H8O (three isomers)
C. C6H14 (five isomers)
C-H-C-H-CI-CI
C-H-C-H-CI-CI
Draw the Lewis structure for each organic compound from its condensed structural formula.a. C2H4 b. CH3NH2 c. HCHOd. CH3CH2OH e. HCOOH
Draw Lewis structures for each molecular formula.
a. C2H4Cl2 (two isomers)
b. C3H8O (three isomers)
c.C3H6 (two isomers)
Chapter 1 Solutions
Organic Chemistry (9th Edition)
Ch. 1.2C - a. Nitrogen has relatively stable isotopes...Ch. 1.4 - Draw Lewis structures for the following compounds....Ch. 1.5 - Write Lewis structures for the following molecular...Ch. 1.5 - Circle any lone pairs (pairs of nonbonding...Ch. 1.6 - Use electronegativities to predict the direction...Ch. 1.8 - Prob. 1.6PCh. 1.9B - Draw the important resonance forms for the...Ch. 1.9B - Prob. 1.8PCh. 1.9B - Prob. 1.9PCh. 1.9B - Use resonance structures to identify the areas of...
Ch. 1.10A - Draw complete Lewis structures for the following...Ch. 1.10B - Give Lewis structures corresponding to the...Ch. 1.10B - Prob. 1.13PCh. 1.11 - Compute the empirical and molecular formulas for...Ch. 1.16 - a. Use your molecular models to make ethane, and...Ch. 1.17 - a. Predict the hybridization of the oxygen atom in...Ch. 1.17 - Predict the hybridization geometry and bond angles...Ch. 1.17 - Predict the hybridization, geometry, and bond...Ch. 1.17 - Prob. 1.19PCh. 1.17 - Allene, CH2=C=CH2, has the structure shown below...Ch. 1.17 - 1. Draw the important resonance forms for each...Ch. 1.18B - Prob. 1.22PCh. 1.18B - Two compounds with the formula CH3CH=NCH3 are...Ch. 1.19B - Prob. 1.24PCh. 1.19B - Give the relationship between the following pairs...Ch. 1 - a. Draw the resonance forms for SO2 (bonded OSO)....Ch. 1 - Name the element that corresponds to each...Ch. 1 - Prob. 1.28SPCh. 1 - For each compound, state whether its bonding is...Ch. 1 - a. Both PCl3 and PCl5 are stable compounds Draw...Ch. 1 - Draw a Lewis structure for each species a. N2H4 b....Ch. 1 - Prob. 1.32SPCh. 1 - Prob. 1.33SPCh. 1 - Draw Lewis structures for a. two compounds of...Ch. 1 - Prob. 1.35SPCh. 1 - Some of the following molecular formulas...Ch. 1 - Prob. 1.37SPCh. 1 - Give the molecular formula of each compound shown...Ch. 1 - 1. From what you remember of electronegativities,...Ch. 1 - For each of the following structures, 1. Draw a...Ch. 1 - Prob. 1.41SPCh. 1 - Prob. 1.42SPCh. 1 - Prob. 1.43SPCh. 1 - Prob. 1.44SPCh. 1 - For each pair of ions, determine which on is more...Ch. 1 - Use resonance structures to identify the areas of...Ch. 1 - Prob. 1.47SPCh. 1 - In 1934, Edward A. Doisy of Washington University...Ch. 1 - If the carbon atom in CH2Cl2 were fat. there would...Ch. 1 - Cyclopropane (C3H6, a three-membered ring) is more...Ch. 1 - Prob. 1.51SPCh. 1 - Prob. 1.52SPCh. 1 - In most amines, the nitrogen atom is sp3...Ch. 1 - Predict the hybridization and geometry of the...Ch. 1 - Draw orbital pictures of the pi bonding in the...Ch. 1 - Prob. 1.56SPCh. 1 - Prob. 1.57SPCh. 1 - Which of the following compounds show cis-trans...Ch. 1 - Give the relationships between the following pairs...Ch. 1 - Dimethyl sulfoxide (DMSO) has been used as an...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Draw a Lewis structure for each ion. a. CH3O− b. HC2− c. (CH3NH3)+ d. (CH3NH)−arrow_forwardDraw Lewis structures for tye following molecules. a.) Atom "X" has 4 valence electrons and Atom "Y" has 6 valence electrons. Draw the Lewis structure for the molecule XY2, showing all lone pairs and formal charges when necessary b.) Atom "M" has 5 valence electrons and Atom "L" has 7 valence electrons. Draw the Lewis structure for the molecule M2L4, showing all lone pairs and formal charges when necessaryarrow_forward1. Convert the condensed formulas to Lewis structures (show all atoms, bonds, lone pairs) a. CH3(CH₂)4OH b. CH3(CH₂)4CH(CH3)2 C. (CH3)2CHO(CH2)4CH3 d. (CH3)2CHCHOarrow_forward
- Draw Lewis structures for each molecular formula. a. C2H,Cl, (two isomers) b. C3H3O (three isomers) c. C3H6 (two isomers)arrow_forwardThe Structure of Hydrocarbons 1. Draw the four carbon bonding patterns commonly seen in hydrocarbons and all other organic compounds. Construct the Lewis structures of the following compounds by combining the carbon atoms with the appropriate bonding patterns and the required number of hydrogen atoms. 2. a. hexane: CH,CH,CH,CH,CH,CH, b. 3-hexene: CH,CH,CH=CHCH,CH, c. 2-hexyne: CH,C=CCH,CH,CH, 3. There are three distinct bond angles formed in the four bonding patterns of carbon. What are they and in which bonding pattern(s) is each seen?arrow_forwardDraw the Lewis structure for each organic compound from its condensed structural formula.a. C3H8 b. CH3OCH3 c. CH3COCH3d. CH3COOH e. CH3CHOarrow_forward
- Give the total number of valence electrons in the following molecule. a. N₂O5 b. H₂S c. C₂H6 d. SO2 valence electrons valence electrons valence electrons valence electronsarrow_forwarda. Draw two Lewis structures for C2H6O. b. Draw three Lewis structures for C3H8O.arrow_forward1.44 Draw one valid Lewis structure for each compound. Assume the atoms are arranged as drawn. H HCC NO H a. CH₂N₂ HCNN H H b. CH₂NO₂ HCNO HO C. CH3CNO d. (CH₂CN) HC CN H 1.45 Draw an acceptable Lewis structure from each condensed structure, such that all atoms have zero formal charge. a. diethyl ether, (CH3CH₂)2O, the first general anesthetic used in medical procedures b. acrylonitrile, CH₂CHCN, starting material used to manufacture synthetic Orlon fibers c. dihydroxyacetone, (HOCH₂)₂CO, an ingredient in sunless tanning products d. acetic anhydride, (CH3CO)2O, a reagent used to synthesize aspirinarrow_forward
- Draw the Lewis structure for each compound.a. Cl2O7 (no Cl¬Cl bond)b. H3PO3 (two OH bonds)c. H3AsO4arrow_forwardWrite the correct Lewis structures for CH4CH4. All hydrogen atoms must be shown.arrow_forwardPROVISIONAL LEWIS STRUCTURES T01/S01 For each provisional structure, identify if it is the correct Lewis structure (C) or if it needs to be modified according to procedure MA or MB to obtain the correct Lewis structure. MA. Form multiple bonds to the central atom using lone pair on the terminal atom(s) until the central atom has an octet (or septet). MB. Form multiple bonds to the central atom using lone pair on the terminal atom(s) until the central atom has a formal charge of zero (0) or until two double bonds are formed. A provisional structure has the valence electrons distributed in order as (1) a bond between each pair of atoms, (2) an octet for each ligand (terminal) atom or ligand group (CH3, NH2 or OH) and (3) any remaining electrons on the central atom.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY