Organic Chemistry (8th Edition)
8th Edition
ISBN: 9780134042282
Author: Paula Yurkanis Bruice
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 1.16, Problem 46P
What of the following molecules would you expect to have a dipole moment of zero? To answer parts g and h, you may need to review the Problem Solving Strategy on p. 39.
- a. CH3CH3
- b. CH2Cl2
- c. NH3
- d. BeCl2
- e. BF3
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Which compound below could have a dipole moment equal to zero?
a) PtCl2F2
b)SCl2F2
c)CClF2
d)CuCl2F2
which one of the figures below has every sp3 hybridized atom circled?
9.13 (a) An AB2 molecule is linear. How many nonbonding electronpairs are around the A atom from this information?(b) How many nonbonding electrons surround the Xe inXeF2? (c) Is XeF2 linear?
Chapter 1 Solutions
Organic Chemistry (8th Edition)
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.1 - a. How many protons do the following species...Ch. 1.1 - Chlorine has two isotopes, 35Cl and 37Cl; 75.77%...Ch. 1.2 - Prob. 4PCh. 1.2 - a. Write the ground-state electronic configuration...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar? a. b. c. d.Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...
Ch. 1.3 - Explain why HCL has a smaller dipole moment than...Ch. 1.3 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...Ch. 1.4 - Prob. 16PCh. 1.4 - a. Draw two Lewis structure for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 20PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 22PCh. 1.4 - Prob. 23PCh. 1.5 - Draw the following orbitals: a. 3s orbital b. 4s...Ch. 1.6 - Prob. 25PCh. 1.6 - Indicate the kind of molecular orbital (, , , or )...Ch. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.7 - Explain why a bond formed by overlap of s orbital...Ch. 1.9 - Put n number in each of the blanks: a. __ s...Ch. 1.9 - For each of the given species: a. Draw its Lewis...Ch. 1.11 - Predict the approximate bond angles in a. the...Ch. 1.11 - According to the potential map for the ammonium...Ch. 1.12 - Prob. 35PCh. 1.13 - a. What are the relative lengths and strengths of...Ch. 1.13 - Prob. 38PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Which of the bond in a carbon-oxygen double bond...Ch. 1.15 - Would you expect a CC bond formed by sp2sp2...Ch. 1.15 - Caffeine is a natural insecticide found in the...Ch. 1.15 - a. What is the hybridization of each of the carbon...Ch. 1.15 - Predict the approximate bond angles for a. the CNC...Ch. 1.16 - What of the following molecules would you expect...Ch. 1.16 - Account for the difference in the shape and color...Ch. 1.16 - If the dipole moment of CH3F is 1.847 D and the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 50PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Draw the condensed structure of a compound that...Ch. 1 - Predict the approximate bond angles: a. the CNH...Ch. 1 - Prob. 54PCh. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - What is the hybridization of each of the carbon...Ch. 1 - Rank the bonds from most polar. a. CO, CF, CN b....Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 59PCh. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 62PCh. 1 - Draw the missing lone-pair electrons and assigns...Ch. 1 - a. Which of the indicated bonds in each molecule...Ch. 1 - For each of the following molecules, indicate the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 67PCh. 1 - Rank the following compounds from highest dipole...Ch. 1 - In which orbitals are the lone pairs in nicotine?Ch. 1 - Prob. 70PCh. 1 - Prob. 71PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 73PCh. 1 - Which compound has a larger dipole moment: CH3Cl...Ch. 1 - Prob. 75PCh. 1 - Explain why CH3Cl has a greater dipole moment than...Ch. 1 - a. Draw a Lewis structure for each of the...Ch. 1 - There are three isomers with molecular formula...
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
- How can sigma bonds in molecules be source of electrons? (Include a drawing in the explanation as needed)arrow_forwardcan someone explain why this counts as fully conjugated? does the pos charge count as conjugation? I thought conjugation was sigma bond, pi bond, sigma bond, etc...arrow_forwardHow many sp, sp2, and sp3 carbons are present in a Capsaicin? What is the hybridization around N atom? How many pi bonds are present over the whole molecule (Capsaicin)? sp: sp2: sp3: N: pi bonds: Note: The image below contains a Capsaicin Lewis Structure for the question above. Thank you.arrow_forward
- ______ do not have a net dipole moment. (a) CS2 (b) SO3 (c) H2S (d) SO2arrow_forwardThis bond is made of an sp3 orbital from a carbon atom to a 1s orbital from the H atom. The correct orbital overlap is sp3-s. What type(s) of orbital overlap is(are) indicated on the following structure: -sp3-sp -sp2-s -sp3-s -p-p -sp3-sp2arrow_forwardCan someone help me this this? The question is: Determine the orbital in which the indicated non-bonding electrons reside. Candidates include atomic orbitals (s and p), hybrid orbitals (sp, sp2, and sp3), and molecular orbitals (s, s*, p, p*). Here is the picture for itarrow_forward
- Which is the correct electron configuration for B2+ according to the molecular orbital theory? (5B) A. σ1s2 σ*1s2 σ2s2 σ*2s2 σ2pz2 B. σ1s2 σ*1s2 σ2s2 σ*2s2 π2px1 C. σ1s2 σ*1s2 σ2s2 σ*2s2 σ2pz1 D. σ1s2 σ*1s2 σ2s2 σ*2s2 π2px1π2py1arrow_forwardhow is molecular orbital (MO) theory an improvement of valence bond theory? A.) valence bond theory is an oversimplification because it uses atomic orbitals in a molecular context MO theory corrects for this B.) valence bond theory is too complicated because the orbital overlap is hard to draw, MO theory is easier. C.) MO theory is not an improvement because it requires too much math. OR D.) MO theory allows us to directly solve schrodingers equation for a moleculearrow_forwardBe sure to answer all parts. Predict the geometry of the following species using the VSEPR model. Electron DomainGeometry MolecularGeometry (a) PCl3 (b) CHCl3 (c) SiH4 (d) TeCl4arrow_forward
- 1.8 One of the following molecules has a net dipole moment: Page 3 of 12 FINAL EXAMINATIONS (2021) - WALTER SISULU UNIVERSITY DEGREE EXAMINATIONS: CHEIIMI/ CHE 15MI A. CO₂, B. CCL4; C CO, D. AICI; E CHA,arrow_forwardTetrachloroethene (CCl2=CCl2) does not have a dipole moment. Explain this fact on the basis of theshape of CCl2=CCl2.arrow_forwardConsider the incomplete orbital representation of O2 , below right. a. Identify which lobes are hybrid orbitals (identify the type) and which lobes arep orbitals. b. Use dotted lines to show any bonds. c. Use up or down arrows to show electron occupation of each hybrid orbital or bond.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning
Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Organic Chemistry: A Guided Inquiry
Chemistry
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Cengage Learning
Chemistry for Today: General, Organic, and Bioche...
Chemistry
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9781305580350
Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
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