Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 9, Problem 56IL
Carbon dioxide (CO2), dinitrogen monoxide (N2O), the azide ion (N3–), and the cyanate ion (OCN–) have the same geometry* and the same number of valence shell electrons. However, there are significant differences in their electronic structures.
- (a) What hybridization is assigned to the central atom in each species? Which orbitals overlap to form the bonds between atoms in each structure.
- (b) Evaluate the resonance structures of these four species. Which most closely describe the bonding in these species? Comment on the differences in bond lengths and bond orders that you expect to see based on the resonance structures.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The structure of caffeine is shown below.
(a) Complete the Lewis structure.
(b) How many pi bonds are present in caffeine? How many sigma bonds?
(c) Identify the hybridization of the carbon atoms.
(d) What is the value of the O-C-N angle?
Butadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths:
(a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.
Consider the reaction BF3 + NH3 -> F3B-NH3
(a) Describe the changes in hybridization of the B and N atoms as a result of this reaction.
(b) Describe the shapes of all the reactant molecules with their bond angles.
(c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms.
(d) What is the name of the bond between B and N.
(e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.
Chapter 9 Solutions
Chemistry & Chemical Reactivity
Ch. 9.2 - Use valence bond theory to describe the bonding in...Ch. 9.2 - Identify the hybridization of each underlined atom...Ch. 9.2 - Use valence bond theory to describe the bonding in...Ch. 9.2 - What is the hybridization of the S atom (the...Ch. 9.2 - 2. Which of the following is incorrect?
The...Ch. 9.2 - Prob. 3RCCh. 9.2 - Prob. 4RCCh. 9.3 - What is the electron configuration of the H2+ ion?...Ch. 9.3 - Could the anion Li2 exist? What is the ions bond...Ch. 9.3 - The cations O2+ and N2+ are formed when molecules...
Ch. 9.3 - What is the NO bond order in nitrogen monoxide,...Ch. 9.3 - Prob. 2RCCh. 9.3 - Prob. 3RCCh. 9.3 - 4. Among the known dioxygen species (O2+, O2, O2−...Ch. 9.3 - What is the empirical formula of Tynan purple?Ch. 9.3 - Butter yellow absorbs light with a wavelength of...Ch. 9.3 - Prob. 3CSCh. 9.A - Photoelectron spectroscopy is s1milar to the...Ch. 9.A - What is the energy of a photon with a wavelength...Ch. 9.A - Using the accompanying figure, state which...Ch. 9.A - The kinetic energy of an electron ejected from the...Ch. 9.A - The N2+ ions that are formed when electrons with...Ch. 9 - Draw the Lewis structure for chloroform, CHCl3....Ch. 9 - Draw the Lewis structure for NF3. What are its...Ch. 9 - Draw the Lewis structure for hydroxylamine, H2NOH....Ch. 9 - Draw the Lewis structure for 1,...Ch. 9 - Draw the Lewis structure for carbonyl fluoride,...Ch. 9 - Draw the Lewis structure for acetamide, CH3CONH2....Ch. 9 - Specify the electron-pair and molecular geometry...Ch. 9 - Specify the electron-pair and molecular geometry...Ch. 9 - Prob. 9PSCh. 9 - What is the hybrid orbital set used by each of the...Ch. 9 - Draw the Lewis structures of the acid HPO2F2 and...Ch. 9 - Draw the Lewis structures of the arid HSO3F and...Ch. 9 - What is the hybridization of the carbon atom in...Ch. 9 - What is the hybridization of the carbon atoms in...Ch. 9 - What is the electron-pair and molecular geometry...Ch. 9 - Prob. 17PSCh. 9 - For each compound below, decide whether cis and...Ch. 9 - Molecular Orbital Theory (See Examples 9.49.6.)...Ch. 9 - Give the electron configurations for the ions Li2+...Ch. 9 - Platinum hexafluoride is an extremely strong...Ch. 9 - When potassium and oxygen react, one of the...Ch. 9 - Among the following, which has the shortest bond...Ch. 9 - Consider the following list of small molecules and...Ch. 9 - Prob. 27PSCh. 9 - The nitrosyl ion. NO+, has an interesting...Ch. 9 - These questions are not designated as to type or...Ch. 9 - What is the OSO angle and the hybrid orbital set...Ch. 9 - Sketch the resonance structures for the nitrite...Ch. 9 - Sketch the resonance structures for the nitrate...Ch. 9 - Sketch the resonance structures for the N2O...Ch. 9 - Compare the structure and bonding in CO2 and CO32...Ch. 9 - Numerous molecules are detected in deep space....Ch. 9 - Acrolein, a component of photochemical smog, has a...Ch. 9 - The organic compound below is a member of a class...Ch. 9 - The compound sketched below is acetylsalicylic...Ch. 9 - Phosphoserine is a less-common amino acid. (a)...Ch. 9 - Lactic acid is a natural compound found in sour...Ch. 9 - Cinnamaldehyde ocaus naturally in cinnamon oil....Ch. 9 - The ion Si2 was reported in a laboratory...Ch. 9 - The simple valence bond picture of O2 does not...Ch. 9 - Nitrogen, N2, can ionize to form N2+ or add an...Ch. 9 - Which of the homonuclear, diatomic molecules of...Ch. 9 - Which of the following molecules or ions are...Ch. 9 - Prob. 47GQCh. 9 - The structure of amphetamine, a stimulant, is...Ch. 9 - Menthol is used in soaps, perfumes, and foods. It...Ch. 9 - Prob. 50GQCh. 9 - Suppose you carry out the following reaction of...Ch. 9 - Ethylene oxide is an intermediate in the...Ch. 9 - The sulfamate ion, H2NSO3, can be thought of as...Ch. 9 - The compound whose structure is shown here is...Ch. 9 - Prob. 55ILCh. 9 - Carbon dioxide (CO2), dinitrogen monoxide (N2O),...Ch. 9 - Draw the two resonance structures that describe...Ch. 9 - Draw a Lewis structure for diimide, HNNH. Then,...Ch. 9 - Prob. 59SCQCh. 9 - Consider the three fluorides BF4, SiF4, and SF4....Ch. 9 - When two amino acids react with each other, they...Ch. 9 - What is the connection between bond order, bond...Ch. 9 - When is it desirable to use MO theory rather than...Ch. 9 - Show how valence bond theory and molecular orbital...Ch. 9 - Three of the four molecular orbitals for...Ch. 9 - Lets look more closely at the process of...Ch. 9 - Borax has the molecular formula Na2B4O5(OH)4. The...Ch. 9 - A model of the organic compound allene is shown...Ch. 9 - Prob. 69SCQCh. 9 - Prob. 70SCQCh. 9 - Bromine forms a number of oxides of varying...Ch. 9 - Prob. 72SCQCh. 9 - Urea reacts with malonic acid to produce...
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
- For each of the following molecule: (i) draw the correct Lewis structure; (ii) determine the molecular geometry and the type of hybridization on the central atom, and (iii) predict whether the molecule is polar or nonpolar. (a) BrCl5arrow_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_forward2(a) Provide the Lewis structures for both CH3OH and C2H3Cl. 2(b) What is the largest bond angle among all the bond angles in CH3OH and C2H3Cl? Listthe three atoms making this largest bond angle, and estimate the value of the angle.2(c) What intermolecular forces are present(i) between CH3OH molecules?(ii) between C2H3Cl molecules?arrow_forward
- A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H3CCN. It is present in paint strippers.(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.(b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form σ bonds.(c) Describe the atomic orbitals that form the π bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.arrow_forward7. Nitrogen is the central atom in each of the species given. (a) Draw the Lewis electron-dot structure for each of the species. + NO₂ NO₂ NO₂ (b) List the species in order of increasing bond angle. Justify your answer. (c) For NO₂ and NO₂, give the hybridization of the nitrogen atom in it. (d) Identify the only one of the species that dimerizes and explain what causes it to do so.arrow_forwardAmmonia, NH3, reacts with incredibly strong bases to producethe amide ion, NH2-. Ammonia can also react with acidsto produce the ammonium ion, NH4+. (a) Which species(amide ion, ammonia, or ammonium ion) has the largestH¬N¬H bond angle? (b) Which species has the smallestH¬N¬H bond angle?arrow_forward
- If an electron is removed from a fluorine molecule, an F+2molecular ion forms.(a) Give the molecular electron configurations for F2 and F+2 (for the MOs constructed from valence AOs).(b) Give the bond order of each species.(c) Predict which species should be paramagnetic.(d) Predict which species has the greater bond dissociation energy.arrow_forwardPropylene, C3H6, is a gas that is used to form the importantpolymer called polypropylene. Its Lewis structure is given. (a) What is the total number of valence electrons in the propylenemolecule? (b) How many valence electrons are usedto make σ bonds in the molecule? (c) How many valenceelectrons are used to make π bonds in the molecule? (d) Howmany valence electrons remain in nonbonding pairs in themolecule? (e) What is the hybridization at each carbon atomin the molecule?arrow_forwardDraw the molecular orbital energy diagrams for the valence electrons in the following diatomic molecules. Calculate the bond order and indicate if each of them is diamagnetic or paramagnetic. (а) В> (b) С. (c) CO (d) NO (е) Оzarrow_forward
- (a) Complete the Lewis structure for the molecule shown below. How many lone pairs are there? H-C H 1 H (b) Give the hybridizations of the following atoms in the structure: (i) Ca; (ii) Ob (c) Give approximate values of the following bond angles: (i) O a-Ca-Ob; (ii) С a -О b-Сbarrow_forwardAzo dyes are organic dyes that are used for many applications,such as the coloring of fabrics. Many azo dyes arederivatives of the organic substance azobenzene, C12H10N2.A closely related substance is hydrazobenzene, C12H12N2.The Lewis structures of these two substances are given (Recall the shorthand notation used for benzene.)(a) What is the hybridization at the N atom in each of thesubstances? (b) How many unhybridized atomic orbitalsare there on the N and the C atoms in each of the substances?(c) Predict the N—N—C angles in each of thesubstances. (d) Azobenzene is said to have greater delocalizationof its π electrons than hydrazobenzene. Discussthis statement in light of your answers to (a) and (b). (e) Allthe atoms of azobenzene lie in one plane, whereas thoseof hydrazobenzene do not. Is this observation consistentwith the statement in part (d)? (f) Azobenzene is an intensered-orange color, whereas hydrazobenzene is nearly colorless.Which molecule would be a better one to use in…arrow_forward(a) Write a single Lewis structure for SO3 , and determine the hybridization at the S atom. (b) Are there other equivalent Lewis structures for the molecule? (c) Would you expect SO3 to exhibit delocalized π bonding?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
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