Essential Organic Chemistry (3rd Edition)
3rd Edition
ISBN: 9780321937711
Author: Paula Yurkanis Bruice
Publisher: PEARSON
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Textbook Question
Chapter 1, Problem 60P
- a. Why is a H 8 H bond (0.74 Å) shorter than a C 8 C bond (1.54 Å)?
- b. Predict the length of a C 8 H bond.
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Chapter 1 Solutions
Essential Organic Chemistry (3rd Edition)
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.2 - Prob. 2PCh. 1.2 - How many valence electrons do chlorine, bromine,...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar?Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...Ch. 1.3 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...
Ch. 1.4 - Prob. 12PCh. 1.4 - a. Draw two Lewis structures for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 16PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 18PCh. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.9 - Put a number in each of the blanks: a. ___ s...Ch. 1.11 - Predict the approximate bond angles in a. the...Ch. 1.11 - According to the potential map for the ammonium...Ch. 1.12 - Prob. 25PCh. 1.13 - a. Predict the relative lengths and strengths of...Ch. 1.13 - Prob. 28PCh. 1.14 - Which of the bonds in a carbonoxygen double bond...Ch. 1.14 - Caffeine is a natural insecticide, found in the...Ch. 1.14 - a. What is the hybridization of each of the carbon...Ch. 1.14 - Prob. 33PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Account for the difference in the shape and color...Ch. 1.15 - Which of the following molecules would you expect...Ch. 1 - Draw a Lewis structure for each of the following...Ch. 1 - Prob. 38PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Prob. 40PCh. 1 - Draw the condensed structure of a compound that...Ch. 1 - Prob. 42PCh. 1 - Prob. 43PCh. 1 - Draw a Lewis structure for each of the following...Ch. 1 - Prob. 45PCh. 1 - List the bonds in order from most polar to least...Ch. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Write the Kekul structure for each of the...Ch. 1 - Assign the missing formal charges.Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 51PCh. 1 - a. Which of the indicated bonds in each compound...Ch. 1 - In which orbitals are the lone pairs in nicotine?...Ch. 1 - Draw the missing lone-pair electrons and assign...Ch. 1 - Rank the following compounds from highest dipole...Ch. 1 - Prob. 56PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 58PCh. 1 - Sodium methoxide (CH3ONa) has both ionic and...Ch. 1 - a. Why is a H 8 H bond (0.74 ) shorter than a C 8...Ch. 1 - Which compound has a larger dipole moment, CHCl3...Ch. 1 - Which compound has a longer C 8 Cl bond?Ch. 1 - Prob. 63PCh. 1 - The following compound has two isomers. One isomer...
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- The oxygen oxygen bond in O2 is 112 pm and in O2 is 121 pm. Explain why the bond length in O2+ is shorter than in O2. Would you expect the bond length in O2 to be longer or shorter than that in O2? Why?arrow_forwardComplete the following resonance structures for POCl3. a. Would you predict the same molecular structure from each resonance structure? b. What is the hybridization of P in each structure? c. What orbitals can the P atom use to form the bond in structure B? d. Which resonance structure would be favored on the basis of formal charges?arrow_forward4.Examine the model and real structures for SO2. A.In what way does the central atom violate the octet rule? When is it possible for molecules to have this exception to the octet rule? B.Calculate the difference in the bond angle between the real and model structure? Is this difference larger or smaller than the difference observed for H2O? Why is the deviation between the real and model structure different for SO2compared to H2O? The deviation for H2O is 5 degreesarrow_forward
- An important starting material for the manufacture ofpolyphosphazenes is the cyclic molecule (NPCl₂)₃. The mol-ecule has a symmetrical six-membered ring of alternating N and P atoms, with the Cl atoms bonded to the P atoms. The nitrogen-phosphorus bond length is significantly less than that expectedfor an N−P single bond.(a) Draw a likely Lewis structure for the molecule.(b) How many lone pairs of electrons do the ring atoms have?(c) What is the order of the nitrogen-phosphorus bond?arrow_forwardThe nitrogennitrogen bond distance in N2 is 109 pm. On the basis of bond orders, would you expect the bond distance in N2+ to be less than or greater than 109 pm? Answer the same question for N2.arrow_forwardLight of appropriate wavelength can break chemical bonds. Light having λ < 240 nm can dissociate gaseous O2. It requires light with λ < 819 nm to dissociate gaseous H2O2 to 2 OH. Assume that all of the photon energy is used solely for these dissociations. (a) Calculate the energy required to dissociate (i) O2 and (ii) H2O2. (b) Consider the results of part (a). How well do they correlate with the Lewis structures of O2 and H2O2? Explain your answer.arrow_forward
- Explain why CF4 and Xef4 are nonpolar compounds (have no net dipole moments) while SF4 is polar (has a net dipo le moment). Is CO2 polar? What about COS?arrow_forwardDescribe the type of bonding that exists in die F2(g) molecule. How does this type of bonding differ from that found in the HF(g) molecule? How is it similar?arrow_forwardWhich of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments? (a) CIF5 (b) CIO2 (c) TeCI42 (d) PCl3 (e) SeF4 (f) PH2 (g) XeF2arrow_forward
- 7.97 Consider the structure shown below for as well as any other important resonance structures. (a) What is the expected O—N—O bond angle in this structure? (b) The molecule contains N—O bonds of two different lengths. How many sborter N—O bonds would be present?arrow_forwardThe three NO bonds in NO3 are all equivalent in length and strength. How is this explained even though any valid Lewis structure for NO3 has one double bond and two single bonds to nitrogen?arrow_forwardThe formula for nitryl chloride is ClNO2 (in which N is the central atom). (a) Draw the Lewis structure for the molecule, including all resonance structures. (b) What is the NO bond order? (c) Describe the electron-pair and molecular geometries, and give values for all bond angles. (d) What is the most polar bond in the molecule? Is the molecule polar? (e) The computer program used to calculate electrostatic potential surfaces gave the following charges on atoms in the molecule: A = 0.03, B = 0.26, and C = +0.56. Identify the atoms A, B, and C. Are these calculated charges in accord with your predictions?arrow_forward
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