Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 9.3, Problem 1PPC
Practice ProblemCONCEPTUALIZE
Which of these models could represent a species for which
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
What molecular geometries contain a central atom with 5 electron groups connected to it?
[Select all that apply]
T-shape
square pyramidal
linear
see-saw
Figure
3 of 3
Which of the following clusters of orbitals would form the shape shown here (Figure 3) either through the formation of a single molecule or
by bonding to another atom of similar electronic geometry and results in an arrangement of orbitals that is possible within the valence shell
of an atom?
Check all that apply.
► View Available Hint(s)
two sp orbitals and two p orbitals
six sp³ d² orbitals
three sp orbitals
two sp orbitals and four p orbitals
three p orbitals
six sp³ d orbitals
six sp³ orbitals
one sp orbital and two p orbitals
Which of the following are true statements regarding hybridization of atomic orbitals? (Select all that apply)
Group of answer choices
A hybrid orbital represents a volume of space that is likely to contain an electron.
Hybridization is the mixing of 2 or more atomic orbitals to form a new set of hybrid orbitals.
Hybrid orbitals can overlap other hybrid orbitals to form covalent bonds.
Hybridization of atomic orbitals requires energy.
Hybrid orbitals have the same shape as the original atomic orbitals.
Chapter 9 Solutions
Chemistry
Ch. 9.1 - Practice Problem ATTEMPT
Determine the shapes of...Ch. 9.1 - Prob. 1PPBCh. 9.1 - Prob. 1PPCCh. 9.1 - 9.1.1 What are the electron-domain geometry and...Ch. 9.1 - What are the electron-domain geometry and...Ch. 9.1 - Prob. 3CPCh. 9.1 - Prob. 4CPCh. 9.1 - Prob. 5CPCh. 9.2 - Practice Problem ATTEMPT
Ethanolamine has a...Ch. 9.2 - Practice Problem BUILD
The bond angle in is...
Ch. 9.2 - Practice ProblemCONCEPTUALIZE Which of these...Ch. 9.2 - 9.2.1 Identify the polar molecules in the...Ch. 9.2 - Identify the nonpolar molecules in the following...Ch. 9.3 - Practice ProblemATTEMPT Use valence bond theory to...Ch. 9.3 - Practice ProblemBUILD For which molecule(s) can we...Ch. 9.3 - Practice ProblemCONCEPTUALIZE Which of these...Ch. 9.3 - Which of the following atoms, in its ground state,...Ch. 9.3 - According to valence bond theory, how many bonds...Ch. 9.4 - Practice Problem ATTEMPT Use hybrid orbital theory...Ch. 9.4 - Practice ProblemBUILD Use hybrid orbital theory to...Ch. 9.4 - Prob. 1PPCCh. 9.4 - How many orbitals does a set of s p 2 hybrid...Ch. 9.4 - How many p atomic orbitals are required to...Ch. 9.5 - Practice Problem ATTEMPT
The active ingredient in...Ch. 9.5 - Practice ProblemBUILD Determine the total number...Ch. 9.5 - Practice ProblemCONCEPTUALIZE In terms of valence...Ch. 9.5 - Which of the following molecules contain one or...Ch. 9.5 - 9.5.2 From left to right, give the hybridization...Ch. 9.5 - Which of the following pairs of atomic orbitals on...Ch. 9.5 - 9.5.4 Which of the following pairs of atomic...Ch. 9.6 - Practice ProblemATTEMPT Use valence bond theory...Ch. 9.6 - Prob. 1PPBCh. 9.6 - Prob. 1PPCCh. 9.6 - Prob. 1CPCh. 9.6 - Prob. 2CPCh. 9.6 - Prob. 3CPCh. 9.6 - Prob. 4CPCh. 9.7 - Prob. 1PPACh. 9.7 - Prob. 1PPBCh. 9.7 - Prob. 1PPCCh. 9.7 - Prob. 1CPCh. 9.7 - Prob. 2CPCh. 9.7 - Prob. 3CPCh. 9.7 - Prob. 4CPCh. 9.8 - Practice ProblemATTEMPT Use a combination of...Ch. 9.8 - Practice ProblemBUILD Use a combination of valence...Ch. 9.8 - Prob. 1PPCCh. 9 - Prob. 1KSPCh. 9 - Which of the following species does not have...Ch. 9 - 9.3
Which of the following species is polar?
Ch. 9 - Which of the following species is nonpolar (a) IC1...Ch. 9 - How is the geometry of a molecule defined, and why...Ch. 9 - 9.2 Sketch the shape of a linear triatomic...Ch. 9 - How many atoms are directly bonded to the central...Ch. 9 - Discuss the basic features of the VSEPR model....Ch. 9 - In the trigonal bipyramidal arrangement, why does...Ch. 9 - 9.6 Explain why the molecule is not square...Ch. 9 - Predict the geometries of the following species...Ch. 9 - Predict the geometries of the following species: (...Ch. 9 - Predict the geometry of the following molecules...Ch. 9 - Predict the geometry of the following molecules...Ch. 9 - Predict the geometry of the following ions using...Ch. 9 - 9.12 Predict the geometries of the following ions:...Ch. 9 - Describe the geometry around each of the three...Ch. 9 - 9.14 Which of the following species are...Ch. 9 - Prob. 15QPCh. 9 - The bonds in beryllium hydride ( BeH 2 ) molecules...Ch. 9 - Determine whether (a) BrF 5 and (b) BCl 3 are...Ch. 9 - Determine whether (a) OCS and (b) XeF 4 are polar.Ch. 9 - Prob. 19QPCh. 9 - Prob. 20QPCh. 9 - Prob. 21QPCh. 9 - Use valence bond theory to explain the bonding in...Ch. 9 - Prob. 23QPCh. 9 - Prob. 24QPCh. 9 - 9.25 What is the hybridization of atomic orbitals?...Ch. 9 - Prob. 26QPCh. 9 - 9.27 What is the angle between the following two...Ch. 9 - Prob. 28QPCh. 9 - Prob. 29QPCh. 9 - Prob. 30QPCh. 9 - Prob. 31QPCh. 9 - Prob. 32QPCh. 9 - Prob. 33QPCh. 9 - Prob. 34QPCh. 9 - Which of the following pairs of atomic orbitals of...Ch. 9 - Prob. 36QPCh. 9 - 9.37 Specify which hybrid orbitals are used by...Ch. 9 - The allene molecule ( H 2 C=C=CH 2 ) is linear...Ch. 9 - Prob. 39QPCh. 9 - Prob. 40QPCh. 9 - How many pi bonds and sigma bonds are there in the...Ch. 9 - Prob. 42QPCh. 9 - Benzo(a)pyrene is a potent carcinogen found in...Ch. 9 - What is molecular orbital theory? How does it...Ch. 9 - 9.45 Define the following terms: bonding molecular...Ch. 9 - Sketch the shapes of the following molecular...Ch. 9 - Explain the significance of bond order. Can bond...Ch. 9 - Explain in molecular orbital terms the changes in...Ch. 9 - 9.49 The formation of from two atoms is an...Ch. 9 - 9.50 Draw a molecular orbital energy level diagram...Ch. 9 - Prob. 51QPCh. 9 - Prob. 52QPCh. 9 - Which of these species has a longer bond, B 2 or B...Ch. 9 - Prob. 54QPCh. 9 - 9.55 Compare the Lewis and molecular orbital...Ch. 9 - Prob. 56QPCh. 9 - Prob. 57QPCh. 9 - Prob. 58QPCh. 9 - A single bond is almost always a sigma bond, and a...Ch. 9 - Prob. 60QPCh. 9 - In Chapter 8, we saw that the resonance concept is...Ch. 9 - Prob. 62QPCh. 9 - Prob. 63QPCh. 9 - Prob. 64QPCh. 9 - Nitryl fluoride ( FNO 2 ) is very reactive...Ch. 9 - Prob. 66QPCh. 9 - Prob. 67QPCh. 9 - Which of the following species is not likely to...Ch. 9 - Prob. 69APCh. 9 - Although both carbon and silicon are in Group 4A,...Ch. 9 - Predict the geometry of sulfur dichloride ( SCl 2...Ch. 9 - Antimony pentafluoride ( sbF 5 ) reacts with XeF 4...Ch. 9 - Prob. 73APCh. 9 - Prob. 74APCh. 9 - Predict the bond angles for the following...Ch. 9 - Briefly compare the VSEPR and hybridization...Ch. 9 - 9.77 Draw Lewis structures and give the other...Ch. 9 - Prob. 78APCh. 9 - Determine whether (a) PCl 5 and (b) H 2 CO (C...Ch. 9 - Prob. 80APCh. 9 - 9.81 Which of the following molecules are linear:...Ch. 9 - Prob. 82APCh. 9 - 9.83 The molecule can exist in either of the...Ch. 9 - Cyclopropane ( C 3 H 6 ) has the shape of a...Ch. 9 - Determine whether (a) CH 2 Cl 2 and (b) XeF 4 are...Ch. 9 - 9.86 Does the following molecule have a dipole...Ch. 9 - For which molecular geometries (linear, bent,...Ch. 9 - Prob. 88APCh. 9 - 9.89 Carbon suboxide is a colorless...Ch. 9 - The following molecules ( AX 4 Y 2 ) all have an...Ch. 9 - Prob. 91APCh. 9 - Write the ground-state electron configuration for...Ch. 9 - 9.93 What is the hybridization of C and of N in...Ch. 9 - The stable allotropic form of phosphorus is P 4 ,...Ch. 9 - Prob. 95APCh. 9 - Use molecular orbital theory to explain the...Ch. 9 - Carbon dioxide has a linear geometry and is...Ch. 9 - Draw three Lewis structures for compounds with the...Ch. 9 - Prob. 99APCh. 9 - Prob. 100APCh. 9 - Prob. 101APCh. 9 - Draw the Lewis structure of ketene ( C 2 H 2 O )...Ch. 9 - Prob. 103APCh. 9 - Which of the following ions possess a dipole...Ch. 9 - Prob. 105APCh. 9 - Prob. 106APCh. 9 - The compound TCDD, or...Ch. 9 - Progesterone is a hormone responsible for female...Ch. 9 - 9.109 Carbon monoxide is a poisonous compound due...Ch. 9 - Prob. 110APCh. 9 - Prob. 111APCh. 9 - Prob. 112APCh. 9 - 9.113 The compound 1,2-dichloroethane is...Ch. 9 - Consider an N 2 molecule in its first excited...Ch. 9 - Prob. 115APCh. 9 - Prob. 1SEPPCh. 9 - Prob. 2SEPPCh. 9 - These questions are not based on a descriptive...Ch. 9 - These questions are not based on a descriptive...
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 of the following molecules have at least one atom that has tetrahedral electronic geometry? Consider only non-terminal atoms. Select all that apply. a) e CH3 b) O c) NH4 Но HOH d) HCN e) e CC3 f) g) NH3 BF3arrow_forwardDraw the Molecular Orbital Energy Diagrams for the diatomic molecules, O2, OF and F2. Which of the following statement is (are) true? (Select all that apply.) Of these three molecules, O2 has the highest stability None of these statements are true. O2 and OF are paramagnetic and F2 is diamagnetic. Of these three molecules, F2 has the longest bond. The bond order of OF is 1.5. Of these three molecules, F2 has the highest bond order.arrow_forward2. Which of the following configurations are paramagnetic (select all that apply)?arrow_forward
- arch Consider a molecule AB3, where element A and B both have 6 valence electrons. If the AEn for A=2.4 and the AEn for B = 3.0, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) Steric Number of the molecule b) name of shape (based on the VSEPR names) c) bond hybridization d) bond polarity (polar or non-polar) e) molecular polarity (polar or non-polar) A/ Ai 3 O % 5 H N Marrow_forwardO ELECTRONIC STRUCTURE AND CHEMICAL BONDING Identifying hybridization in a small molecule What is the hybridization of the central atom in the orthotellurate (TeO ) anion? Explanation Check Type here to search 近 IIarrow_forwardWhich of the following compounds do not have an overall molecular dipole moment at all? Select all that apply Select one or more: CO HCI CF4 CHF3 BH3 CO₂ 0arrow_forward
- Determine which of the following molecules have a net dipole moment. Select all that apply.arrow_forwardwhat bond angle is predicted for a liners molecule? which molecules were linear, did the molecular mechanics calculation product the correct bond angle list includes, CH4, CO2, H2CO, HCN, NH3, H2O, C2H4arrow_forwardAnswer the questions below for the diatomic species A) CN+2 B) CN- C) CN-² What is the bond order for the CN+2 ion? Bond Order = Which of the species has the shortest bond? ◆ How many of the above molecules/ions are diamagnetic?arrow_forward
- Which of the following molecule(s) are polar? Select all that apply: O Secla ICI5 AsCl5 OSICI4arrow_forwardExample 6 An imine is a molecule that contains a carbon – nitrogen double bond. Describe the bonding of the simplest possible imine, H₂CNH, by sketching the σ and л bonding systems.arrow_forwardConsider the MO diagrams for these diatomic species. Rank the following diatomic species in order of bond dissociation energy (from smallest to largest). A) CN⁺ < CN < CN⁻ B) CN⁻ < CN < CN⁺ C) CN < CN⁻ < CN⁺ D) CN⁻ < CN⁺ < CNarrow_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