Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 3, Problem 7E
Explain what is wrong with each of the following statements.
a. “A
b. “A
c. “A
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
For a homonuclear diatomic molecule, what type of molecular orbital does the
illustration shown below represent? Note: the
represents each nuclei.
a bonding o orbital formed from two p atomic orbitals.
a bonding o orbital formed from two s atomic orbitals.
a bonding o orbital formed from one p and one s atomic orbital.
a bonding n orbital formed from one s and one p atomic orbital.
a bonding n orbital formed from two p atomic orbitals.
Which bonds allow for a large, bonded network to be more directional and why?
1. Sigma bonds
2. Pi bonds
Because
1. The orbitals overlap side-to-side to hold the bond in place.
2. The orbitals overlap end-to-end in several different directions.
3. Multiple of these bonds result in delocalized electrons.
ο ο ο ο ο ο
O 2,1
O2,2
O 1,3
O 1,2
O2,3
O 1,1
lyr
a. One of the two known binary compounds of xenon and oxygen is XeO3. A Lewis structure is shown here, which may or may not be complete. How many lone pairs should be present on the central Xe atom?
b. What is the electron pair geometry around the Xe?
c. What is the molecular geometry of XeO3?
d. What hybrid orbitals does the Xe atom use?
Chapter 3 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 3 - Prob. 1CTQCh. 3 - What neutral atom is represented by the electron...Ch. 3 - Prob. 3CTQCh. 3 - Consider any one of the four identical hybrid...Ch. 3 - Prob. 5CTQCh. 3 - Prob. 6CTQCh. 3 - Prob. 7CTQCh. 3 - Prob. 8CTQCh. 3 - Prob. 9CTQCh. 3 - Prob. 10CTQ
Ch. 3 - On the left side of Figure 3.6, label the areas...Ch. 3 - Prob. 12CTQCh. 3 - Prob. 13CTQCh. 3 - Prob. 14CTQCh. 3 - Prob. 15CTQCh. 3 - Now consider the fully formed molecule on the...Ch. 3 - Prob. 1ECh. 3 - Explain why the two molecules below cannot...Ch. 3 - Prob. 3ECh. 3 - Consider the incomplete orbital representation of...Ch. 3 - Consider the following orbital representation of...Ch. 3 - Summarize how one determines the hybridization...Ch. 3 - Explain what is wrong with each of the following...Ch. 3 - Prob. 8ECh. 3 - Prob. 9ECh. 3 - Complete the following tables, and memorize their...Ch. 3 - Draw orbital representations of bonding in water...Ch. 3 - Draw electron configuration diagrams for carbon in...Ch. 3 - Prob. 13E
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
- Which statement is true concerning molecular orbital (MO) theory? A. Atomic orbitals overlap to form bonds B. Atomic orbitals combine to form both bonding and anti-bonding orbitals C. Atomic orbitals through VSEPR can determine the geometric shapes of molecules D. Atomic orbitals on the same atom combine with each other to make hybrid orbitals.arrow_forwardA. Sigma orbitals B. Bonding orbitals C. Antibonding orbitals D. Pi orbitals 26. A molecular orbital can contain how many electrons? A. One B. Two C. Three D. Four 27. It is the hybrid orbital in a carbon atom with the greatest "s character." A. sp3 B. sp2 C. sp D. sp4arrow_forwardWhich one of the following statements about molecular orbitals for homonuclear diatomic molecules is incorrect? a. Pi orbitals are symmetric to rotation about the internuclear axis. b. Sigma orbitals have a symmetrical distribution of electron density around the two nuclei. c. Sigma* orbitals are higher in energy than their corresponding sigma orbitals. d. Sigma orbitals can be formed from the overlap of s or p atomic orbitals. e. Pi orbitals have a planar node along the internuclear axis.arrow_forward
- This question is related to valence bond theory. a. Explain the assumptions made in bonding models under valence bond theory. What best describes bonding under these models? b. Draw the Lewis structure of SO2. Identify bonds in the moldule as either sigma or pi bonds. Draw orbital diagrams for ground state S and O atoms. Use these orbital diagrams determine the geometry of SO2 using valence bond theory (hint: SO2 must be descried using hybrid atomic orbitals. In other words, which orbitals on which atoms overlap to give rise to which bonds? C. d. Explain why valence bond theory does not adequately describe the bonding in SO2, even though it accurately predicts the geometry/bond angle.arrow_forward11. What is the electron-domain geometry of water molecule (H2O)? a. bent b. tetrahedral c. trigonal planar d. linear 12. Write the correct Lewis dot structure for O2. Which statement correctly describes the structure of the whole molecule? a. There is a double bond and four lone pairs. b. There is a double bond and six lone pairs. c. There is a single bond and six lone pairs. d. There is a single bond, a double bond, and six lone pairs. 13. If there are four (4) electron pairs around the central atom of a molecule, these electron pairs are in a/n a. trigonal planar b. trigonal pyramidal arrangement. C. octahedral d. tetrahedral 14 The molecular geometry of the molecule NF3 is a. linear b. trigonal pyramidal c. tetrahedral d. trigonal planar 15 Which of the following species will exhibit tetrahedral molecular geometry? d. PCI5 a. CCI4 b. CO2 C. O3arrow_forwardFour sp3 hybrid orbitals has what kind of arrangement of electron pair .A Octahedral Tetrahedral .B .C Linear .D Trigonal planararrow_forward
- List the correct electron and molecular geometries that correspond to each set of electron groups around the central atom of a molecule.a. four electron groups overall; three bonding groups and onelone pairb. four electron groups overall; two bonding groups and two lone pairsc. five electron groups overall; four bonding groups and one lone paird. five electron groups overall; three bonding groups and two lone pairse. five electron groups overall; two bonding groups and three lone pairsf. six electron groups overall; five bonding groups and one lone pairg. six electron groups overall; four bonding groups and two lone pairsarrow_forwardGive the correct electron and molecular geometries that correspond to each set of electron groups around the central atom of a molecule.a. four electron groups overall; three bonding groups and one lone pairb. four electron groups overall; two bonding groups and two lone pairsc. five electron groups overall; four bonding groups and one lone paird. five electron groups overall; three bonding groups and two lone pairse. five electron groups overall; two bonding groups and three lone pairsf. six electron groups overall; five bonding groups and one lone pairg. six electron groups overall; four bonding groups and two lone pairsarrow_forwarda.An s orbital and a p orbital can combine to form molecular orbitals in a couple different ways. Draw a sketch of the overlap between these two atomic orbitals that would produce each of the following molecular orbitals. A. a sigma bonding MO B. a sigma antibonding MO b. For each of the following molecules, make a list of the molecules that are (i) polar, (ii) nonpolar and (iii) ionic. A. NH 3 B. H2 O C. CH3 CH2 CH3 D. NH4 Cl E. Na2 SO 4 F. CH3 Cl G. C6H6OH H. CH3COOH I. LiNO3arrow_forward
- Which of the following descriptions of a sigma bond (according to valence bond theory) is NOT CORRECT? Select one: OA. A sigma bond is formed when two adjacent, parallel p orbitals overlap along their sides. O B. When a sigma bond is formed, a shared electron pair lies on the bond axis of adjacent, bonded atoms. OC. A sigma bond is formed between adjacent atoms when hybrid orbitals, co-linear with the bond axis, overlap. O D. A sigma bond is formed when an s orbital overlaps with a hybrid orbital.arrow_forwardIf an electron is added to H2 it would go into a A. σ*1s molecular orbital and strengthen the H—H bond. B. σ1s molecular orbital and strengthen the H—H bond. C. σ1s molecular orbital and weaken the H—H bond. D. σ*1s molecular orbital and weaken the H—H bond. AND How many molecular orbitals are produced in the valence shell when two fluorine atoms bond to form the F2 molecule?arrow_forwardWhich of the following correctly describes a pi bond according to valence bond theory? Select one: O A. A pi bond is formed between adjacent atoms when two p orbitals, co- linear with the bond axis, meet "head on". O B. A pi bond is formed when an s orbital overlaps with a hybrid orbital. O C. A pi bond is formed between adjacent atoms when hybrid orbitals, co- linear with the bond axis, overlap. O D. A pi bond is formed when two adjacent, parallel p orbitals overlap along their sides.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 Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles 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 Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary 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