Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 7, Problem 7.91QP
Chemists often represent benzene with the structure shown on the left. Explain why the structure on the left is a better representation of the benzene molecule than the one on the right.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Please envision this table like it was one long table. (I had to make it two because it hung out of the quiz
boundaries and was inaccessible.)
It is recommended that you draw the Lewis Structure of the molecules and then complete this table.
electronic
Molecular
Molecule
Geometry
Geometry
CH3F
tetrahedral
tetrahedral
NH3
tetrahedral
trigonal pyramidal
C2F4
trigonal planar
trigonal planar
CO2
linear
linear
main
dipole
Molecule
intermolecular
moment
force
CH3F
[ Select ]
yes
NH3
hydrogen bonding
yes
C2F4
[ Select )
no
CO2
( Select |
no
>
>
Explain what is wrong with each molecular geometry and provide the correct molecular geometry, given the numbers of lone pairs and bonding groups on the central
atom.
Match the words in the left column to the appropriate blanks in the sentences on the right.
a bent
a trigonal bipyramidal
an octahedral
a trigonal planar
a square planar
a trigonal pyramidal
a tetrahedral
a seesaw
a linear
In structure (a), four pairs of electrons give
cause lone pair-bonded pair repulsions and would have
Reset
electron geometry. The lone pair would
molecular geometry.
Help
In structure (b), five pairs of electrons give
electron geometry. The lone pair occupies an
equatorial position to minimize lone pair-bonded pair repulsions, and the molecule would have
molecular geometry.
In structure (c), six pairs of electrons give
electron geometry. The two lone pairs would
occupy opposite positions to minimize lone pair-lone pair repulsions, and the molecule would have
molecular geometry.
What
The previous lesson helped us understand the compositions of molecules and
their bonds through the Lewis structure theory. However, Lewis structures do not
demonstrate one of the most important features of molecules-their overall shapes.
The size and shapes of molecules are defined by the distances and angles between
the nuclei of the atoms involved. In this lesson, we learn how to portrait a molecule by
writing a two-dimensional structure for it and translating it to a three-dimensional
shape, and we examine the effects of molecular shape on molecular polarity.
What's New
Activity 1: Review on Geometry
Directions: Draw a two-dimensional or three-dimensional illustration of the following
geometries:
Example: Square Pyramidal:
1. Trigonal planar (2D)
2. Square Planar (3D)
3. Octahedral (3D)
4. Trigonal bipyramidal (3D)
5. Seesaw (3D)
13
Chapter 7 Solutions
Chemistry: Atoms First
Ch. 7.1 - Determine the shapes of (a) SO3 and (b) ICl4.Ch. 7.1 - Determine the shapes of (a) CO2 and (b) SCl2.Ch. 7.1 - (a) From what group must the terminal atoms come...Ch. 7.1 - These four models may represent molecules or...Ch. 7.1 - Acetic acid, the substance that gives vinegar its...Ch. 7.1 - Ethanolamine (HOCH2CH2NH2) has a smell similar to...Ch. 7.1 - The bond angle in NH3 is significantly smaller...Ch. 7.1 - Which of these models represents a species in...Ch. 7.1 - What are the electron-domain geometry and...Ch. 7.1 - What are the electron-domain geometry and...
Ch. 7.1 - Prob. 7.1.3SRCh. 7.1 - Prob. 7.1.4SRCh. 7.2 - Prob. 7.3WECh. 7.2 - Prob. 3PPACh. 7.2 - For each of the following hypothetical molecules,...Ch. 7.2 - Which of these models could represent a polar...Ch. 7.2 - Prob. 7.2.1SRCh. 7.2 - Prob. 7.2.2SRCh. 7.3 - Prob. 7.4WECh. 7.3 - Prob. 4PPACh. 7.3 - Prob. 4PPBCh. 7.3 - Prob. 4PPCCh. 7.3 - Prob. 7.3.1SRCh. 7.3 - Which of the following exhibits significant...Ch. 7.4 - Hydrogen selenide (H2Se) is a foul-smelling gas...Ch. 7.4 - Prob. 5PPACh. 7.4 - For which molecule(s) can we not use valence bond...Ch. 7.4 - Which of these models could represent a species...Ch. 7.4 - Prob. 7.4.1SRCh. 7.4 - Prob. 7.4.2SRCh. 7.5 - Prob. 7.6WECh. 7.5 - Use hybrid orbital theory to describe the bonding...Ch. 7.5 - Prob. 6PPBCh. 7.5 - Prob. 6PPCCh. 7.5 - Prob. 7.5.1SRCh. 7.5 - Prob. 7.5.2SRCh. 7.6 - Thalidomide (C13H10N2O4) is a sedative and...Ch. 7.6 - The active ingredient in Tylenol and a host of...Ch. 7.6 - Determine the total number of sigma and pi bonds...Ch. 7.6 - In terms of valence bond theory and hybrid...Ch. 7.6 - In addition to its rise in aqueous solution as a...Ch. 7.6 - Use valence bond theory and hybrid orbitals to...Ch. 7.6 - Use valence bond theory and hybrid orbitals to...Ch. 7.6 - Explain why hybrid orbitals are necessary to...Ch. 7.6 - Prob. 7.6.1SRCh. 7.6 - Prob. 7.6.2SRCh. 7.6 - Prob. 7.6.3SRCh. 7.6 - Prob. 7.6.4SRCh. 7.7 - Prob. 7.9WECh. 7.7 - Use molecular orbital theory to determine whether...Ch. 7.7 - Use molecular orbital theory to determine whether...Ch. 7.7 - For most of the homonuclear diatomic species shown...Ch. 7.7 - Calculate the bond order of N22+, and determine...Ch. 7.7 - Which of the following species is paramagnetic?...Ch. 7.7 - Prob. 7.7.3SRCh. 7.7 - Prob. 7.7.4SRCh. 7.8 - It takes three resonance structures to represent...Ch. 7.8 - Use a combination of valence bond theory and...Ch. 7.8 - Use a combination of valence bond theory and...Ch. 7.8 - Which of the following contain one or more...Ch. 7.8 - Which of the atoms in BCl3 need hybrid orbitals to...Ch. 7.8 - Which of the following can hybrid orbitals be used...Ch. 7.8 - Which of the following enables us to explain the...Ch. 7 - Prob. 7.1KSPCh. 7 - Which of the following species does not have...Ch. 7 - Prob. 7.3KSPCh. 7 - Prob. 7.4KSPCh. 7 - Prob. 7.1QPCh. 7 - Sketch the shape of a linear triatomic molecule, a...Ch. 7 - Prob. 7.3QPCh. 7 - Prob. 7.4QPCh. 7 - In the trigonal bipyramidal arrangement, why does...Ch. 7 - Prob. 7.6QPCh. 7 - Predict the geometry of the following molecules...Ch. 7 - Prob. 7.8QPCh. 7 - Predict the geometries of the following species...Ch. 7 - Predict the geometries of the following ions: (a)...Ch. 7 - Prob. 7.11QPCh. 7 - Prob. 7.12QPCh. 7 - Prob. 7.13QPCh. 7 - Describe the geometry about each of the central...Ch. 7 - Prob. 7.15QPCh. 7 - Prob. 7.16QPCh. 7 - Prob. 7.17QPCh. 7 - Prob. 7.18QPCh. 7 - Prob. 7.19QPCh. 7 - Prob. 7.20QPCh. 7 - Prob. 7.21QPCh. 7 - Prob. 7.22QPCh. 7 - Explain the term polarizability. What kind of...Ch. 7 - Prob. 7.24QPCh. 7 - What physical properties are determined by the...Ch. 7 - Prob. 7.26QPCh. 7 - Describe the types of intermolecular forces that...Ch. 7 - The compounds Br2 and ICl are isoelectronic (have...Ch. 7 - If you lived in Alaska, which of the following...Ch. 7 - The binary hydrogen compounds of the Group 4A...Ch. 7 - List the types of intermolecular forces that exist...Ch. 7 - Prob. 7.32QPCh. 7 - Prob. 7.33QPCh. 7 - Prob. 7.34QPCh. 7 - Diethyl ether has a boiling point of 34.5C, and...Ch. 7 - Prob. 7.36QPCh. 7 - Which substance in each of the following pairs...Ch. 7 - Prob. 7.38QPCh. 7 - What kind of attractive forces must be overcome to...Ch. 7 - Prob. 7.40QPCh. 7 - Prob. 7.41QPCh. 7 - The following compounds have the same molecular...Ch. 7 - Prob. 7.43QPCh. 7 - Prob. 7.44QPCh. 7 - Use valence bond theory to explain the bonding in...Ch. 7 - Prob. 7.46QPCh. 7 - Prob. 7.47QPCh. 7 - Prob. 7.48QPCh. 7 - Prob. 7.49QPCh. 7 - What is the hybridization of atomic orbitals? Why...Ch. 7 - Prob. 7.51QPCh. 7 - Prob. 7.52QPCh. 7 - Prob. 7.53QPCh. 7 - Describe the bonding scheme of the AsH3 molecule...Ch. 7 - Prob. 7.55QPCh. 7 - Prob. 7.56QPCh. 7 - Describe the hybridization of phosphorus in PF5.Ch. 7 - Prob. 7.58QPCh. 7 - Prob. 7.59QPCh. 7 - Prob. 7.1VCCh. 7 - Prob. 7.2VCCh. 7 - Prob. 7.3VCCh. 7 - Prob. 7.4VCCh. 7 - Prob. 7.60QPCh. 7 - Which of the following pairs of atomic orbitals of...Ch. 7 - Prob. 7.62QPCh. 7 - Prob. 7.63QPCh. 7 - Prob. 7.64QPCh. 7 - Prob. 7.65QPCh. 7 - Prob. 7.66QPCh. 7 - Prob. 7.67QPCh. 7 - Prob. 7.68QPCh. 7 - Benzo[a]pyrene is a potent carcinogen found in...Ch. 7 - What is molecular orbital theory? How does it...Ch. 7 - Define the following terms: bonding molecular...Ch. 7 - Prob. 7.73QPCh. 7 - Prob. 7.74QPCh. 7 - Prob. 7.75QPCh. 7 - Draw a molecular orbital energy level diagram for...Ch. 7 - Prob. 7.77QPCh. 7 - Prob. 7.78QPCh. 7 - Prob. 7.79QPCh. 7 - Acetylene (C2H2) has a tendency to lose two...Ch. 7 - Compare the Lewis and molecular orbital treatments...Ch. 7 - Prob. 7.82QPCh. 7 - Prob. 7.83QPCh. 7 - Prob. 7.84QPCh. 7 - Prob. 7.85QPCh. 7 - Draw the molecular orbital diagram for the cyanide...Ch. 7 - Given that BeO is diamagnetic, use a molecular...Ch. 7 - Prob. 7.88QPCh. 7 - Prob. 7.89QPCh. 7 - Both ethylene (C2H4) and benzene (C6H6) contain...Ch. 7 - Chemists often represent benzene with the...Ch. 7 - Determine which of these molecules has a more...Ch. 7 - Nitryl fluoride (FNO2) is used in rocket...Ch. 7 - Describe the bonding in the nitrate ion NO3 in...Ch. 7 - Prob. 7.95QPCh. 7 - Prob. 7.96QPCh. 7 - Prob. 7.97QPCh. 7 - Prob. 7.98QPCh. 7 - Prob. 7.99QPCh. 7 - Antimony pentafluoride (SbF5) combines with XeF4...Ch. 7 - Prob. 7.101QPCh. 7 - The molecular model of nicotine (a stimulant) is...Ch. 7 - Predict the bond angles for the following...Ch. 7 - The germanium pentafluoride anion (GeF5) has been...Ch. 7 - Draw Lewis structures and give the other...Ch. 7 - Which figure best illustrates the hybridization of...Ch. 7 - Prob. 7.107QPCh. 7 - Prob. 7.108QPCh. 7 - Prob. 7.109QPCh. 7 - Prob. 7.110QPCh. 7 - Prob. 7.111QPCh. 7 - Cyclopropane (C3H6) has the shape of a triangle in...Ch. 7 - The compound 1,2-dichloroethane (C2H4Cl2) is...Ch. 7 - Prob. 7.114QPCh. 7 - Prob. 7.115QPCh. 7 - Prob. 7.116QPCh. 7 - Prob. 7.117QPCh. 7 - Prob. 7.118QPCh. 7 - The amino acid selenocysteine is one of the...Ch. 7 - Prob. 7.120QPCh. 7 - Prob. 7.121QPCh. 7 - Prob. 7.122QPCh. 7 - Gaseous or highly volatile liquid anesthetics are...Ch. 7 - Prob. 7.124QPCh. 7 - Prob. 7.125QPCh. 7 - Two of the drugs that are prescribed for the...Ch. 7 - Prob. 7.127QPCh. 7 - Prob. 7.128QPCh. 7 - The BO+ ion is paramagnetic. Determine (a) whether...Ch. 7 - Use molecular orbital theory to explain the...Ch. 7 - Which best illustrates the change in geometry...Ch. 7 - Prob. 7.132QPCh. 7 - Prob. 7.133QPCh. 7 - Aluminum trichloride (AlCl3) is an...Ch. 7 - Prob. 7.135QPCh. 7 - Prob. 7.136QPCh. 7 - Prob. 7.137QPCh. 7 - Consider an N2 molecule in its first excited...Ch. 7 - The Lewis structure for O2 is Use molecular...Ch. 7 - Draw the Lewis structure of ketene (C2H2O) and...Ch. 7 - The compound TCDD, or...Ch. 7 - Name the kinds of attractive forces that must be...Ch. 7 - Carbon monoxide (CO) is a poisonous compound due...Ch. 7 - Prob. 7.144QPCh. 7 - Prob. 7.145QP
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 many central atoms does the molecule H2NCH3 have, and what is the shape about each?arrow_forwardIndicate which molecules are polar and which are nonpolar. (a) SeO2 (b) N2O (N is the central atom) (c) SCl4arrow_forwardIn each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.arrow_forward
- The structural formula for vitamin C is Give a molecular-level explanation why vitamin C is a water-soluble rather than a fat-soluble vitamin.arrow_forwardThe caffeine molecule is shown below. Indicate the electron geometry AND the molecular shape around each of the indicated atoms (six answers in total). Be aware that the angles may not be drawn correctly in this Lewis structure.arrow_forwardDepending on the protein under study, the bond angle of a drug molecule can become critical to successfully deactivating a viral protein. For this reason, chemists are frequently concerned with the 3D shape of their molecules and their bond angles. The oxygen atom shown in the structure has a tetrahedral electronic geometry, meaning we would predict that it would have 109.5° bond angles. However, the actual structure, the bond angles are smaller than 109.5°. Explain why this compression occurs. Make sure to discuss what’s happening around/what groups are present around the oxygen atom.arrow_forward
- Answer the questions in the table below about the shape of the sulfur hexabromide (SBr) molecule. How many electron groups are around the central sulfur atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central sulfur atom? (You may need to use the scrollbar to see all the choices.) (choose one) X Ś Um 0 Garrow_forwardConsider a hypothetical molecule with the formula X4Y2Z. The atoms X, Y, and Z have electronegativities of 2.5, 3.0, and 3.5, respectively. The molecule adopts a tetrahedral geometry with X atoms at the corners, Y atoms in the middle of the edges, and Z atoms at the center of the molecule. Explain the polarity of this molecule and the factors contributing to it.arrow_forwardUse VSEPR to predict the geometry (including bond angles) about each interior atom of methyl azide (CH3N3) and draw the molecule. Would you expect the bond angle between the two interior nitrogen atoms to be the same or different? Would you expect the two nitrogen–nitrogen bond lengths to be the same or different?arrow_forward
- ) Bean hexene is an odor compound used in cosmetics and cleaners. It is also known as leguminal. Its formula is: CH3CH2CHCHCH2CH2OCHCH2CH3 | OCH3 Please draw a Lewis structure for this compound with CORRECT GEOMETRY (use dashes and wedges!) Label all pi bonds in the molecule (if there are any) Indicate the bond angles for the red highlighted section of the molecule. (hint: you may want to keep the main carbon chain in-plane with the page for clarity) For this question, you don’t need to draw out the orbitals.arrow_forwardThe Lewis structure for SF6 is shown below. This sulfur S atom in this molecule has an expanded octet, and you are not expected to be familiar with the specific electron geometry and molecular geometry for expanded octets. Still, we can make some predictions with the knowledge that we have. Would you predict the electron geometry and molecular geometry for SF6 to be the same or to differ? Please briefly explain your answer.arrow_forwardConsider selenium oxychloride (SeOCl2): What is the elemental symbol of its central atom? How many valence electrons does this molecule contain? How many lone electron pairs surround the central atom? How many regions of electron density surround the central atom? For remaining items in this question, place the appropriate letter in the box: What is the electron geometry of this molecule? A = linear B = trigonal planar C = tetrahedral D = trigonal bipyramidal E = octahedral What is the molecular shape of this molecule? A = tetrahedral B = trigonal pyramid C = bent or angular D = T-shape E = Sawhorse or seesaw Is this a polar molecule? A = Yes B = No What is the hybridization of the central atom? A = sp B = sp2 C = sp3 D = sp3d E = sp3d2arrow_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 LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: 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
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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
Linear Combination of Atomic Orbitals LCAO; Author: Edmerls;https://www.youtube.com/watch?v=nq1zwrAIr4c;License: Standard YouTube License, CC-BY
Quantum Molecular Orbital Theory (PChem Lecture: LCAO and gerade ungerade orbitals); Author: Prof Melko;https://www.youtube.com/watch?v=l59CGEstSGU;License: Standard YouTube License, CC-BY