Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Textbook Question
Chapter 9, Problem 62SCQ
What is the connection between bond order, bond length, and bond energy? Use ethane (C2H6), ethylene (C2H4), and acetylene (C2H2) as examples.
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Chapter 9 Solutions
Chemistry & Chemical Reactivity
Ch. 9.1 - Use valence bond theory to describe the bonding in...Ch. 9.1 - Identify the hybridization of each underlined atom...Ch. 9.1 - Use valence bond theory to describe the bonding in...Ch. 9.2 - What is the electron configuration of the H2+ ion?...Ch. 9.2 - Could the anion Li2 exist? What is the ions bond...Ch. 9.2 - The cations O2+ and N2+ are formed when molecules...Ch. 9.3 - Photoelectron spectroscopy is s1milar to the...Ch. 9.3 - What is the energy of a photon with a wavelength...Ch. 9.3 - Using the accompanying figure, state which...Ch. 9.3 - The kinetic energy of an electron ejected from the...
Ch. 9.3 - The N2+ ions that are formed when electrons with...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. 2.3ACPCh. 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 - 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 - Calcium carbide, CaC2, contains the acetylide ion,...Ch. 9 - Platinum hexafluoride is an extremely strong...Ch. 9 - When sodium and oxygen react, one of the products...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...
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- Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.arrow_forwardConsider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?arrow_forwardGiven the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?arrow_forward
- A toxic cloud covered Bhopal, India, in December 1984 when water leaked into a tank of methyl isocyanate, and the product escaped into the atmosphere. Methyl isocyanate is used in the production of many pesticides. Draw the Lewis structures for methyl isocyanate, CH3NCO, including resonance forms. The skeletal structure isarrow_forwardFormamide, HC(O)NH2, is prepared at high pressures from carbon monoxide and ammonia, and serves as an industrial solvent (the parentheses around the O indicate that it is bonded only to the carbon atom and that the carbon atom is also bonded to the H and the N atoms). Two resonance forms (one with formal charges) can be written for formamide. Write both resonance structures, and predict the bond angles about the carbon and nitrogen atoms for each resonance form. Are they the same? Describe how the experimental determination of the HNH bond angle could be used to indicate which resonance form is more important.arrow_forwardThe equation for the combustion of gaseous methanol is 2 CH3OH(g) + 3 O2(g) 2 CO2(g) + 4 H2O(g) (a) Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy change for this reaction. What is the enthalpy of combustion of one mole of gaseous methanol? (b) Compare your answer in part (a) with the value of tHcalculated using enthalpies of formation data.arrow_forward
- The study of carbon-containing compounds and their properties is called organic chemistry. Besides carbon atoms, organic compounds also can contain hydrogen, oxygen, and nitrogen atoms (as well as other types of atoms). A common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called histidine (an amino acid), which is one of the building blocks of proteins found in our bodies: Draw a complete Lewis structure for histidine in which all atoms have a formal charge of zero.arrow_forwardWrite all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardAcetylene gas (ethyne; HC≡CH) burns with oxygen in an oxyacetylene torch to produce carbon dioxide, water vapor, and the heat needed to weld metals. The heat of combustion for acetylene is −1259 kJ/mol. Calculate the C≡C bond energy. The average bond energies (kJ/mol) C―H 413 C―C 347 C═C 620 H―H 436 O―O 142 O═O 498 H―O 467 C―O 351 C═O 799arrow_forward
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