Organic Chemistry, 12e Binder Ready Version Study Guide / Student Solutions Manual
12th Edition
ISBN: 9781119077336
Author: T. W. Graham Solomons, Craig B. Fryhle, Scott A. Snyder
Publisher: WILEY
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 1, Problem 43P
Consider a chemical species (either a molecule or an ion) in which a carbon atom forms three single bonds to three hydrogen at-oms and in which the carbon atom possesses no other valence electrons. (a) What formal charge would the carbon atom have? (b) What total charge would the species have? (c) What shape would you expect this species to have? (d) What would you expect the hybridization state of the carbon atom to be?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Identify the name of the Following bond line-structures.
The O¬H bond lengths in the water molecule 1H2O2 are0.96 Å, and the H¬O¬H angle is 104.5°. The dipole momentof the water molecule is 1.85 D. (a) In what directionsdo the bond dipoles of the O¬H bonds point? In what directiondoes the dipole moment vector of the water moleculepoint? (b) Calculate the magnitude of the bond dipoleof the O¬H bonds. (Note: You will need to use vector addition to do this.) (c) Compare your answer from part (b)to the dipole moments of the hydrogen halides (Table 8.3).Is your answer in accord with the relative electronegativityof oxygen?
Which whould you expect to be more polar a C-O or a C-F bond?. Explain please
Chapter 1 Solutions
Organic Chemistry, 12e Binder Ready Version Study Guide / Student Solutions Manual
Ch. 1 - Prob. 1PPCh. 1 - Prob. 2PPCh. 1 - Prob. 3PPCh. 1 - Prob. 4PPCh. 1 - Prob. 5PPCh. 1 - Prob. 6PPCh. 1 - Prob. 7PPCh. 1 - Prob. 8PPCh. 1 - Prob. 9PPCh. 1 - Prob. 10PP
Ch. 1 - Prob. 11PPCh. 1 - Prob. 12PPCh. 1 - Prob. 13PPCh. 1 - Prob. 14PPCh. 1 - Prob. 15PPCh. 1 - Prob. 16PPCh. 1 - Prob. 17PPCh. 1 - Prob. 18PPCh. 1 - Prob. 19PPCh. 1 - Prob. 20PPCh. 1 - Prob. 21PPCh. 1 - Practice Problem 1.22 Which of the following...Ch. 1 - Prob. 23PPCh. 1 - Prob. 24PPCh. 1 - Practice Problem 1.25
What do the bond angles of...Ch. 1 - Prob. 26PPCh. 1 - Practice Problem 1.27
Use VSEPR theory to predict...Ch. 1 - Practice Problem 1.28 Predict the bond angles of...Ch. 1 - 1.29 Which of the following ions possess the...Ch. 1 - 1.30 Write a Lewis structure for each of the...Ch. 1 - Prob. 31PCh. 1 - Add any unshared electrons to give each element an...Ch. 1 - Prob. 33PCh. 1 - What is the molecular formula for each of the...Ch. 1 - Prob. 35PCh. 1 - Prob. 36PCh. 1 - 1.37 Write bond-line formulas for all of the...Ch. 1 - Prob. 38PCh. 1 - Prob. 39PCh. 1 - Prob. 40PCh. 1 - Prob. 41PCh. 1 - (a) Cyanic acid (HOCN) and isocyanic acid (HN=C=O)...Ch. 1 - Consider a chemical species (either a molecule or...Ch. 1 - 1.44 Consider a chemical species like the one in...Ch. 1 - 1.45 Consider another chemical species like the...Ch. 1 - Draw a three-dimensional orbital representation...Ch. 1 - Ozone (O3) is found in the upper atmosphere where...Ch. 1 - Write resonance structures for the azide ion, N3....Ch. 1 - Write structural formulas of the type indicated:...Ch. 1 - Prob. 50PCh. 1 - 1.51 In Chapter 15 we shall learn how the...Ch. 1 - Prob. 52PCh. 1 - (a) Consider a carbon atom in its ground state....Ch. 1 - Open computer molecular models for dimethyl ether,...Ch. 1 - Boron is a group IIIA element. Open the molecular...Ch. 1 - 1.56 There are two contributing resonance...Ch. 1 - Prob. 1LGPCh. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Prob. 7LGPCh. 1 - Prob. 8LGP
Additional Science Textbook Solutions
Find more solutions based on key concepts
Determine the de Brogue wavelength of a. an electron moving at 1/10 the speed of light. b. a 400 g Frisbee movi...
Inorganic Chemistry
2. A schedule of experiments for a laboratory indicates that the 1-bromobutane preparation is paired with the p...
The Organic Chem Lab Survival Manual: A Student's Guide to Techniques
The electronic configuration for an element with known group number needs to be predicted. Concept introduction...
Living By Chemistry: First Edition Textbook
The specific heat of an unknown metal is to be calculated for a given amount and rise in temperature. Concept i...
Chemistry: Matter and Change
39. What are the units of k for each type of reaction?
a. first-order reaction
b. second-order reaction
c...
Chemistry: Structure and Properties (2nd Edition)
Refer to figure 10.2 to find the electronegativity different between each of elements; then refer to Table 10.2...
Introductory Chemistry (6th Edition)
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
- Carbon dioxide, dinitrogen monoxide, the azide ion N3-, and cynate ion OCN- have the same arrangement of atoms and the ame number of valence shell electrons. Howeer, there are significant differences in the electronic structures. What hybridization should be assigned to the central atom in each species? Are there any resonance structures associated with these molecules and/or ions? If so, descrie them. Estimate the bond lengths and bond orders of each atom in these molecules and ions.arrow_forwardAssign hybridization state of each carbon, nitrogen, oxygen, halogen, and boron atom indicated with arrows in the molecules below.arrow_forwardFrom models of SF4, BrF3, and XeF4, deduce whether differentatom arrangements, called geometrical isomers, are possible, and,if so, sketch them below.Indicate the preferred geometry foreach case and suggest a reason for your choice.Indicatewhich structures have dipole moments, and show their direction. Molecule Dipole Moment Preferred Geometry SF4 BrF3 XeF4arrow_forward
- Draw three contributing structures of the following compound (called guanidine) and state the hybridization of the four highlighted atoms. In which orbitals do the three lone pairs drawn reside?arrow_forwardAspartame is a compound that is 200 times sweeter than sugar and is used extensively (under the trade name NutraSweet) in diet soft drinks. The skeleton structure of the atoms in aspartame is (a) Complete the Lewis structure and give the number of and bonds in aspartame. (b) What is the hybridization about each carbon atom that forms a double bond with an oxygen atom? (c) What is the hybridization about each nitrogen atom?arrow_forwardBoth the HCH and HCO bond angles of H2CO (formaldehyde) are very close to 120°, but oneis slightly smaller than the other. Predict which is smaller, and explain your reasoning.arrow_forward
- Calcium carbide (CaC2) is an intermediate in the manufacturing of acetylene (C2H2) . It is the calcium salt of the carbide (also called acetylide) ion (C22) . What is the electron configuration of this molecular ion? What is its bond order?arrow_forwardAll carbon-to-carbon bond lengths are identical in benzene. Does this argue for or against the presence of C=C bonds in benzene? Explain.arrow_forwardBenzene is commonly regarded as a resonance hybrid of the two Kekule structures, but other possible structures can also contribute. Draw three other structures in which there are only covalent π bonds (allowing for bonding between some non-adjacent C atoms) and two st ructu res in which there is one ionic bond. Why may these structures be ignored in simple descriptions of the molecule?arrow_forward
- Draw the line-bond structure formula of the following:arrow_forwardHow many hybrid orbitals are represented in the picture, hoe many s,p,d atomic orbitals corresponding to what hybridization, what electron pair, and what bond angle(s)?arrow_forwardWhich of the following molecules contains a nitrogen atom with linear geometry?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Organic Chemistry: A Guided Inquiry
Chemistry
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9781305580350
Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher:Cengage Learning
INTRODUCTION TO MOLECULAR QUANTUM MECHANICS -Valence bond theory - 1; Author: AGK Chemistry;https://www.youtube.com/watch?v=U8kPBPqDIwM;License: Standard YouTube License, CC-BY