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 8, Problem 50PS
Compare the nitrogen-nitrogen bond in hydrazine, H2NNH2, with that in “laughing gas,” N2O. In which molecule is the nitrogen-nitrogen bond shorter? In which is the bond stronger?
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The formula of formic acid is HCO2H. One of the carbon-oxygen bond lengths in this molecule is 1.36 A while the other is 1.23 A .Draw the lewis structure of this molecule and label these bonds.
Consider peroxynitrite (chemical formula: ONOO−), a structural isomer of the nitrate anion. It is generated in the cell when nitric oxide (NO) reacts with the superoxide radical anion (O2-.). Peroxynitrite is a potent oxidant and nitrating agent and can lead to DNA and protein damage (this is the complete question)
Draw the correct Lewis structure for peroxynitrite and indicate approximate bond angles.
Tell how many molecular degrees of freedom of motion are present in peroxynitrite and what motions they correspond to.
Hydrazine, N2H4, burns in oxygen as follows:
N2H4 + O2 → N2 + 2H2O
[The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496]
Draw the chemical structures of the reactants and products and
give the formula to calculate enthalpy change in a reaction, ΔH.
Chapter 8 Solutions
Chemistry & Chemical Reactivity
Ch. 8.2 - Draw Lewis electron dot structures for CH3Cl...Ch. 8.2 - Prob. 2CYUCh. 8.2 - Prob. 3CYUCh. 8.2 - Prob. 4CYUCh. 8.2 - Prob. 1RCCh. 8.2 - 2. Which one of the species in the list below is...Ch. 8.2 - Prob. 3RCCh. 8.2 - Prob. 4RCCh. 8.3 - Prob. 1CYUCh. 8.3 - 1. What is the formal charge of the P atom in the...
Ch. 8.4 - Draw resonance structures for the bicarbonate ion,...Ch. 8.4 - 1. For which of the following species, SO32−, NO+,...Ch. 8.4 - Prob. 2RCCh. 8.5 - Sketch the Lewis structures for CIF2+ and CIF2....Ch. 8.5 - Prob. 1QCh. 8.5 - Prob. 2QCh. 8.5 - Prob. 1RCCh. 8.5 - Prob. 2RCCh. 8.6 - What is the shape of the dichloromethane (CH2C12)...Ch. 8.6 - Give the electron-pair geometry and molecular...Ch. 8.6 - Draw the Lewis structure for lCl2, and then decide...Ch. 8.6 - Prob. 4CYUCh. 8.6 - Which of the following species has...Ch. 8.6 - Prob. 2RCCh. 8.6 - What is the approximate ClCCl bond angle in...Ch. 8.6 - 4. What is the molecular geometry of N2O (where...Ch. 8.7 - Draw the resonance structures for SCN. What are...Ch. 8.7 - For each of the following molecules, decide...Ch. 8.7 - Prob. 1RCCh. 8.7 - 2. Which of the following best describes the...Ch. 8.7 - Three resonance forms can be drawn for the...Ch. 8.8 - The electrostatic potential surface for SOCl2 is...Ch. 8.8 - Using the bond dissociation enthalpies in Table...Ch. 8.8 - Prob. 1RCCh. 8.8 - Prob. 2RCCh. 8.9 - 1. Which of the following species has the longest...Ch. 8.9 - 2. Which of the following species has the largest...Ch. 8.9 - 3. Use bond dissociation enthalpies to estimate...Ch. 8 - Give the periodic group number and number of...Ch. 8 - Give the periodic group number and number of...Ch. 8 - For elements in Groups 4A-7A of the periodic...Ch. 8 - Prob. 4PSCh. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Show all possible resonance structures for each of...Ch. 8 - Show all possible resonance structures for each of...Ch. 8 - Prob. 11PSCh. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Prob. 18PSCh. 8 - Prob. 19PSCh. 8 - The following molecules or ions all have three...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Give approximate values for the indicated bond...Ch. 8 - Give approximate values for the indicated bond...Ch. 8 - Phenylalanine is one of the natural amino acids...Ch. 8 - Acetylacetone has the structure shown here....Ch. 8 - For each pair of bonds, indicate the more polar...Ch. 8 - For each of the bonds listed below, tell which...Ch. 8 - Urea, (NH2)2CO, is used in plastics and...Ch. 8 - Considering both formal charges and bond...Ch. 8 - Considering both formal charge and bond...Ch. 8 - Three resonance structures are possible for...Ch. 8 - Three resonance structures are possible for the...Ch. 8 - Compare the electron dot structures of the...Ch. 8 - Compare the electron dot structures of the...Ch. 8 - The chemistry of the nitrite ion and HNO2: (a) Two...Ch. 8 - Draw the resonance structures for the formate ion,...Ch. 8 - Prob. 39PSCh. 8 - Consider the following molecules: (a) CH4 (b)...Ch. 8 - Which of the following molecules is(are) polar?...Ch. 8 - Prob. 42PSCh. 8 - Give the bond order for each bond in the following...Ch. 8 - Prob. 44PSCh. 8 - In each pair of bonds, predict which is shorter....Ch. 8 - In each pair of bonds, predict which is shorter....Ch. 8 - Prob. 47PSCh. 8 - Compare the carbon-oxygen bond lengths in the...Ch. 8 - Consider the carbon-oxygen bond in formaldehyde...Ch. 8 - Compare the nitrogen-nitrogen bond in hydrazine,...Ch. 8 - Ethanol can be made by the reaction of ethylene...Ch. 8 - Methanol can be made by partial oxidation of...Ch. 8 - Hydrogenation reactions, which involve the...Ch. 8 - Phosgene, Cl2CO, is a highly toxic gas that was...Ch. 8 - The compound oxygen difluoride is quite reactive,...Ch. 8 - Oxygen atoms can combine with ozone to form...Ch. 8 - Prob. 57GQCh. 8 - Prob. 58GQCh. 8 - Which of the following compounds or ions do not...Ch. 8 - Prob. 60GQCh. 8 - Draw resonance structures for the formate ion,...Ch. 8 - Prob. 62GQCh. 8 - Prob. 63GQCh. 8 - What is the principle of electroneutrality? Use...Ch. 8 - Prob. 65GQCh. 8 - Draw resonance structures for the SO2 molecule,...Ch. 8 - What are the orders of the NO bonds in NO2 and...Ch. 8 - Which has the greater ONO bond angle, NO2 or NO2+?...Ch. 8 - Compare the FClF angles in CIF2+ and ClF2. Using...Ch. 8 - Draw an electron dot structure for the cyanide...Ch. 8 - Draw the electron dot structure for the sulfite...Ch. 8 - Dinitrogen monoxide, N2O, can decompose to...Ch. 8 - The equation for the combustion of gaseous...Ch. 8 - The cyanate ion, OCN, has the least...Ch. 8 - Vanillin is the flavoring agent in vanilla extract...Ch. 8 - Explain why (a) XeF2 has a linear molecular...Ch. 8 - The formula for nitryl chloride is ClNO2 (in which...Ch. 8 - Hydroxyproline is a less-common amino acid. (a)...Ch. 8 - Amides are an important class of organic...Ch. 8 - Prob. 81GQCh. 8 - The molecule shown here. 2-furylmelhanethiol, is...Ch. 8 - Dihydroxyacetone is a component of quick-tanning...Ch. 8 - It is possible to draw three resonance structures...Ch. 8 - Acrolein is used to make plastics. Suppose this...Ch. 8 - Molecules in space: (a) In addition to molecules...Ch. 8 - 1,2-Dichloroethylene can be synthesized by adding...Ch. 8 - The molecule pictured below is epinephrine, a...Ch. 8 - You are doing an experiment in the laboratory and...Ch. 8 - Prob. 90ILCh. 8 - A paper published in the research Journal Science...Ch. 8 - Uracil is one of the bases in RNA, a close...Ch. 8 - Prob. 93SCQCh. 8 - Prob. 94SCQCh. 8 - Bromine-containing species play a role in...Ch. 8 - Acrylamide, H2C=CHCONH2, is a known neurotoxin and...
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
- Write 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_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_forwardSulfuric acid is the industrial chemical produced in greatest quantity worldwide. About 90 billion pounds are produced each year in the United States alone. Write the Lewis structure for sulfuric acid, H2SO4, which has twooxygen atoms and two OH groups bonded to the sulfur.arrow_forward
- Which of the following bonds are polar: (a) P—O; (b) S—F; (c) Br—Br; (d) O—Cl? Which is the more electronegative atom in each polar bond?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_forward5. Consider the reaction between hydrazine and hydrogen to produce ammonia, N2H4(g)+H2(g)→2NH3(g)N2H4(g)+H2(g)→2NH3(g). Use enthalpies of formation and bond enthalpies to estimate the enthalpy of the nitrogen-nitrogen bond in N2H4N2H4. (Hint: In an N2H4N2H4 molecule, each NN atom has single bonds to the adjacent NN atom and two HH atoms. In an NH3NH3 molecule, the central NN atom has single bonds to three HH atoms.)arrow_forward
- In chemical reactions, heat is converted into chemical energy (the potential energy stored in chemical bonds) or vice versa. Bond energy is the energy required to break one mole of the bond in the gas phase. Since it takes energy to break a bond, bond energies are always positive. Conversely, energy is released when bonds are formed. Thus, the enthalpy change for a reaction can be approximated from Part A Calculate the bond energy per mole for breaking all the bonds in methane, CH4. ΔΗ Σ(ΔΗ breaking) + Σ(ΔΗ forming) Express your answer to four significant figures and include the appropriate units. where H represents bond energies for the breaking (positive bond energy) or forming (negative bond energy) of a bond and Hrxn represents the overall enthalpy for the • View Available Hint(s) reaction. Use the table to answer questions about bond energies. HẢ Bond energy Bond (kJ/mol ) Value Units AHCH, = C-C 347 C=C 611 Submit Сн 414 C-O 360 Part B C=OinCO2 799 O-0 142 Calculate the bond…arrow_forwardThe carbonate anion, CO32- , is a resonance hybrid. Draw all of the important resonance structures for this molecule. If an atom has a nonzero formal charge, be sure the formal charge is shown clearly in the structure. Use the resonance structures to calculate the average formal charge on each O atom (which are all equivalent in the "true" structure). [Note: all of the important contributing resonance structures have octets around each atom that desires an octet.]arrow_forwardWhen gaseous sulfur trioxide is dissolved in concentratedsulfuric acid, disulfuric acid forms:SO₃(g)+ H₂SO₄(l) →H₂S₂O₇(l) Use bond energies Table to determine ΔH°ᵣₓₙ. (The S atoms in H₂S₂O₇ are bonded through an O atom. Assume Lewis structures with zero formal charges; BE of SNO is 552 kJ/mol.)arrow_forward
- What's the molecular shape of CO2? What's the electron geometry of the cation ClF2+? what's the molecular shape of SF4?arrow_forward10.) The structural formula of a certain aldehyde (related to formaldehyde) is H3C-CH2-CHO. Draw a Lewis structure for this aldehyde and determine the number of bonds present. Note that a single or a double or a triple bond counts as one bond. Write the number, not the word.arrow_forwardAn carbon-to-oxygen single bond (i.e. C-O) has a bond energy of 358 kJ/mol and an carbon-to-oxygen double bond (i.e. C=O) has a bond energy of 749 kJ/mol. Estimate the value of the carbon-to-oxygen bond energy in the carbonate anion, CO32— . Hint: draw the Lewis structure of CO32— , consider resonance and determine which type of bonds it has. Because of the resonance, the bond between C and O will be somewhere in between the single and double bond. Group of answer choices 1107 kJ/mol 358 kJ/mol 488 kJ/mol 928 kJ/mol 1465 kJ/mol 618 kJ/mol 749 kJ/mol 554 kJ/molarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER
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