Organic Chemistry
8th Edition
ISBN: 9781305580350
Author: William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 1, Problem 1.40P
Use VSEPR to predict the geometry of these ions.
- (a) NH2–
- (b) NO2–
- (c) NO2+
- (d) NO3–
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
1.
Draw the Lewis structures for each of the following ions or molecules. For each, give (i) the
molecular shape, (ii) the electron pair geometry at the central atom, and (iii) the hybridization of the central
atom.
(a) POF3
(b) XeO₂F3+
(c) BrCl₂
(d) N3 (the central atom is N; two other N's are bonded to it)
(e) PF3
The Lewis structure of BH2Cl
(a) Is the molecule polar or nonpolar?
(b) What is the hybridization of the carbon atom?
(c) What is the geometric shape of the molecule?
What are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(a) ClF5(b) ClO2−(c) TeCl42−(d) PCl3(e) SeF4(f) PH2−
Chapter 1 Solutions
Organic Chemistry
Ch. 1.1 - Prob. 1.1PCh. 1.2 - Prob. 1.2PCh. 1.2 - Judging from their relative positions in the...Ch. 1.2 - Classify each bond as nonpolar covalent or polar...Ch. 1.2 - Using the symbols and +, indicate the direction...Ch. 1.2 - Draw Lewis structures showing all valence...Ch. 1.2 - Draw Lewis structures for these ions and show...Ch. 1.3 - Draw Lewis structures and condensed structural...Ch. 1.3 - Prob. 1.9PCh. 1.3 - Prob. 1.10P
Ch. 1.3 - Prob. 1.11PCh. 1.3 - Prob. 1.12PCh. 1.4 - Predict all bond angles for these molecules. (a)...Ch. 1.5 - The geometry of carbon in diamond is tetrahedral,...Ch. 1.5 - Because of their spherical shape, C60 molecules...Ch. 1.5 - What best describes the CCC bond angles in C60? 1....Ch. 1.5 - Prob. 1.14PCh. 1.7 - Describe the bonding in these molecules in terms...Ch. 1.8 - Prob. 1.16PCh. 1.8 - Prob. 1.17PCh. 1.8 - Prob. 1.18PCh. 1.9 - Draw three contributing structures of the...Ch. 1.9 - What is the hybridization state of the circled...Ch. 1.9 - The molecule shown on the right in the example in...Ch. 1.9 - Prob. CQCh. 1.9 - The following structure is called imidazolium....Ch. 1 - Write the ground-state electron configuration for...Ch. 1 - Identify the atom that has each ground-state...Ch. 1 - Define valence shell and valence electron.Ch. 1 - How many electrons are in the valence shell of...Ch. 1 - Prob. 1.24PCh. 1 - Prob. 1.25PCh. 1 - Prob. 1.26PCh. 1 - Write Lewis structures for these compounds. Show...Ch. 1 - Write Lewis structures for these ions. Show all...Ch. 1 - Prob. 1.29PCh. 1 - Some of these structural formulas are incorrect...Ch. 1 - Following the rule that each atom of carbon,...Ch. 1 - Following are several Lewis structures showing all...Ch. 1 - Which statements are true about electronegativity?...Ch. 1 - Why does fluorine, the element in the upper right...Ch. 1 - Arrange the single covalent bonds within each set...Ch. 1 - Using the values of electronegativity given in...Ch. 1 - Prob. 1.37PCh. 1 - Use VSEPR to predict bond angles about each...Ch. 1 - Use VSEPR to predict bond angles about each atom...Ch. 1 - Use VSEPR to predict the geometry of these ions....Ch. 1 - Prob. 1.41PCh. 1 - Prob. 1.42PCh. 1 - What is the meaning of the term tertiary (3) when...Ch. 1 - What is the meaning of the term tertiary (3) when...Ch. 1 - Draw structural formulas for (a) The four primary...Ch. 1 - Draw structural formulas for the three tertiary...Ch. 1 - Prob. 1.47PCh. 1 - Identify the functional groups in each compound.Ch. 1 - Draw a three-dimensional representation for each...Ch. 1 - Tetrafluoroethylene, C2F4, is the starting...Ch. 1 - Which statements are true about resonance...Ch. 1 - Prob. 1.52PCh. 1 - Prob. 1.53PCh. 1 - Prob. 1.54PCh. 1 - Are the structures in each set valid contributing...Ch. 1 - State the orbital hybridization of each...Ch. 1 - Describe each highlighted bond in terms of the...Ch. 1 - Following is a structural formula of the...Ch. 1 - Draw a Lewis structure for methyl isocyanate,...Ch. 1 - What is the hybridization of the highlighted atoms...Ch. 1 - Using cartoon representations, draw a molecular...Ch. 1 - In what kind of orbitals do the lone-pair...Ch. 1 - Draw the delocalized molecular orbitals for the...Ch. 1 - Prob. 1.64APCh. 1 - Each compound contains both ions and covalent...Ch. 1 - Predict whether the carbon-metal bond in these...Ch. 1 - Prob. 1.67APCh. 1 - Phosphorus is immediately under nitrogen in the...Ch. 1 - Draw a Lewis structure for the azide ion, N3. (The...Ch. 1 - Cyanic acid, HOCN, and isocyanic acid, HNCO,...Ch. 1 - In Chapter 6, we study a group of organic cations...Ch. 1 - Many reactions involve a change in hybridization...Ch. 1 - Following is a structural formula of benzene,...Ch. 1 - Following are three contributing structures for...Ch. 1 - (a) Draw a Lewis structure for the ozone molecule,...Ch. 1 - The following two compounds are isomers; that is,...Ch. 1 - In future chapters, we will encounter...Ch. 1 - Prob. 1.78AP
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
- Give the Lewis structure, molecular structure, and hybridization of the oxygen atom for OF2. Would you expect OF2 to be a strong oxidizing agent like O2F2 discussed in Exercise 61?arrow_forwardWhich of these molecules has a linear molecular geometry and the molecule is polar? (A) CO2 (B) Cl2O (C) N2O (D) SO2arrow_forwardPredict the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) SF6(b) PCl5(c) BeH2(d) CH3+arrow_forward
- Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) IF6+(b) CF4(c) BF3(d) SiF5−(e) BeCl2arrow_forwardDetermine the electron-group arrangement, molecular shape, and ideal bond angle(s) for each of the following:(a) SO₄²⁻(b) NO₂⁻(c) PHarrow_forward(a) Why do stable xenon fluorides have an even number of F atoms? (b) Why do the ionic species XeF₃⁺ and XeF₇⁻ have odd numbers of F atoms? (c) Predict the shape of XeF₃⁺ .arrow_forward
- HCI VIO 4. Draw the Lewis structures for the following: (a) K (b) Cl (d) Ca2 (c) O2 nolar and which U he T0IIOWINO would you preoarrow_forward. Assume that the third-period element phosphorus forms a diatomic molecule, P2, in an analogous way as nitrogen does to form N2. (a) Write the electronic configuration for P2. Use [Ne2] to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?arrow_forwardGive the hybridization of the metalloid and the molecular geometry for each of the following compounds or ions. (a) GeH4(b) SbF3(c) Te(OH)6(d) H2Te(e) GeF2(f) TeCl4(g) SiF62−(h) SbCl5(i) TeF6arrow_forward
- Draw the Lewis structures for CO2 and CO, and predict the number of σ and π bonds for each molecule.(a) CO2(b) COarrow_forwardChemical species are said to be isoelectronic if they have the same Lewis structure (regardless of charge). Consider these ions and write a Lewis structure for a neutral molecule that is isoelectronic with them. (a) CN–, (b) NH4+ (c) CO3 2–arrow_forwardIn addition to Al₂Cl₆, aluminum forms other specieswith bridging halide ions to two aluminum atoms. One suchspecies is the ion Al₂Cl₇. The ion is symmetrical, with a 180° Al−Cl−Al bond angle.(a) What orbitals does Al use to bond with the Cl atoms?(b) What is the shape around each Al?(c) What is the hybridization of the central Cl?(d) What do the shape and hybridization suggest about the pres-ence of lone pairs of electrons on the central Cl?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
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
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
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
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