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 8, Problem 49PS
Consider the carbon-oxygen bond in formaldehyde (CH2O) and carbon monoxide (CO). In which molecule is the CO bond shorter? In which molecule is the CO bond stronger?
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The average bond energy (enthalpy) for a C=C double bond is 614 kJ/molkJ/mol and that of a C−C single bond is 348 kJ/molkJ/mol. If it takes
4.42×10−19
J/molecule
to break the C=C double bond. What is the longest wavelength λ of light that will provide photons of sufficient energy to break the π bond and cause the isomerization?
Express your answer numerically in nanometers.
5.
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.)
The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water:
OF2(g) + H2O(g) → O2(g) + 2HF(g)
ΔE°rxn = –318 kJ
Using bond energies, calculate the bond dissociation energy of the O–F bond in OF2.
Average Bond Energies (kJ/mol)
Picture
O–F bond dissociation energy = _____kJ/mol
Chapter 8 Solutions
Chemistry & Chemical Reactivity
Ch. 8.2 - Draw Lewis electron dot structures for CH3Cl...Ch. 8.2 - Prob. 8.2CYUCh. 8.2 - Prob. 8.3CYUCh. 8.2 - Prob. 8.4CYUCh. 8.3 - Prob. 8.5CYUCh. 8.4 - Draw resonance structures for the bicarbonate ion,...Ch. 8.5 - Sketch the Lewis structures for CIF2+ and CIF2....Ch. 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. 8.7 - For each of the following pairs of bonds, decide...Ch. 8.7 - Draw the resonance structures for SCN. What are...Ch. 8.8 - For each of the following molecules, decide...Ch. 8.8 - The electrostatic potential surface for SOCl2 is...Ch. 8.9 - Using the bond dissociation enthalpies in Table...Ch. 8.10 - Prob. 1.1ACPCh. 8.10 - Do any of the atoms in an ibuprofen molecule have...Ch. 8.10 - What is the most polar bond in the molecule?
Ch. 8.10 - Prob. 1.4ACPCh. 8.10 - Prob. 1.5ACPCh. 8.10 - Prob. 1.6ACPCh. 8.10 - Are there any 120° bond angles in ibuprofen? Any...Ch. 8.10 - Prob. 1.8ACPCh. 8.10 - Prob. 2.2ACPCh. 8.10 - Calculate the difference in electronegativity...Ch. 8.10 - Predict the bond dissociation enthalpy for a...Ch. 8.10 - Prob. 3.3ACPCh. 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 - Guanine is present in both DNA and RNA. (a) What...Ch. 8 - Prob. 94ILCh. 8 - Prob. 95SCQCh. 8 - Prob. 96SCQCh. 8 - Bromine-containing species play a role in...Ch. 8 - Acrylamide, H2C=CHCONH2, is a known neurotoxin and...
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- Which bond requires more energy to break: the carbon-oxygen bond in formaldehyde, H2CO, or the carbon-oxygen bond in carbon monoxide, CO?arrow_forward13) The average C−C bond dissociation energy (D) is 350 kJ/mol and the average C=C bond dissociation energy is 728 kJ/mol. Based on these values, which is stronger: a σ or a π bond?arrow_forwardThe element vibranium (Vb) reacts with pandemonium (Pn) to generate a covalent PnVb4 molecule. If a pandemonium atom has 8 valence electrons and each vibranium atom has 7 valence electrons, draw the Lewis structure of PbVb4. What is the molecular geometry of the PbVb4 molecule? Pn is the central atom.arrow_forward
- Hydrogen cyanide can be catalytically reduced with hydrogen to form methylamine. Use Lewis structures and bond energies to determine ΔH°rxn for HCN(g) + 2 H2(g) ⟶ CH3NH2(g)arrow_forwardConsider 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.arrow_forwardTwo useful organic compounds that contain Cl atoms are vinyl chloride (CH2=CHCl) and chloroethane (CH3CH2Cl). Vinyl chloride is the starting material used to prepare poly(vinyl chloride), a plastic in insulation, pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic. Why is the C–Cl bond in vinyl chloride stronger than the C–Cl bond in chloroethane?arrow_forward
- When 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_forwardSelenium tetrafluoride is produced from a reaction of elemental Se with chlorine trifluoride according to the balanced chemical equation: 3 Se(g) + 4 CIF3(g) → 3 SEF4(g) + 2 Cl2(g) AHrxn = -1874 kJ Using AHrxn and the table of bond energies below, determine the bond energy of the Se-F bonds in SeF4. Note that all bonds in the reactants and products are single bonds. Bond Bond Energy (k.J/mol) CI-F 253 CI-CI 243 The units are kJ/mol. Do not include units in your answer. Scientific notation is optional. To write scientific notation in Canvas, type "e" to replace "x 10". For example, "1 x 1014" is written "1e+14" in Canvas.arrow_forwardCompounds (1) C4H6Cl2 and (2) AlCl3. Explain the difference between them using the following categories. Types of bonding? The number of chlorine atom of each one?arrow_forward
- A chemist wants to observe the following reaction: 2H2 + O2 → 2H2O The chemist is standing inside a room with oxygen in the air and has a balloon filled with hydrogen. The chemist holds a small flame up to the hydrogen balloon. When the balloon pops, the hydrogen explodes in a ball of fire. Based on what you know about breaking and forming bonds, explain which part of the reaction is higher in energy (i.e., does it take more energy to break the bonds of the reactants, or is more energy given off when the product bonds are formed?). Defend your answer in three to five sentences.arrow_forwardConsider the compound XeO2F2. Draw the Lewis structure for this compound (on a separate piece of paper that you can refer to), and indicate the number of lone pairs of electrons on each atom in the molecule.arrow_forwardCarbon-carbon bonds form the “backbone” of nearly every organic and biological molecule. The average bond energy of the C¬C bond is 347 kJ/mol. Calculate the frequency and wavelength of the least energetic photon that can break an average C¬C bond. In what region of the electromagnetic spectrum is this radiation?arrow_forward
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