Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Chapter 1, Problem 10CTQ
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The average bond energy (enthalpy) for a C=CC=C double bond is 614 kJ/molkJ/mol and that of a C−CC−C single bond is 348 kJ/molkJ/mol. Estimate the energy needed to break only the ππ bond of the double bond of 2-butene.
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Chapter 1 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 1 - (E) What does the number (+Z) at the center of...Ch. 1 - Prob. 2CTQCh. 1 - Prob. 3CTQCh. 1 - Prob. 4CTQCh. 1 - Prob. 5CTQCh. 1 - Prob. 6CTQCh. 1 - Prob. 7CTQCh. 1 - You hear a student from a nearby group say that...Ch. 1 - Use VSEPR to explain why the HBH bond angle of BH3...Ch. 1 - Both the HCH and HCO bond angles of H2CO...
Ch. 1 - Prob. 11CTQCh. 1 - Consider the following flat drawing of methane...Ch. 1 - Use VSEPR to assign a value of (close to) 109.5,...Ch. 1 - A student draws the picture of ammonia (NH3) in...Ch. 1 - Prob. 15CTQCh. 1 - How many central atoms does the molecule H2NCH3...Ch. 1 - Indicate the bond angle and shape about each...Ch. 1 - Explain how there can be two kinds of bent:...Ch. 1 - A student makes the following statement: “The...Ch. 1 - A student who missed this class needs to know how...Ch. 1 - Prob. 1ECh. 1 - Prob. 2ECh. 1 - Consider the incomplete valence shell...Ch. 1 - How many valence electrons does a neutral a. K...Ch. 1 - Consider the molecules AlCl3 (aluminum chloride)...Ch. 1 - Draw an example of a bent molecule with a bond...Ch. 1 - Label each atom marked with an arrow with the...Ch. 1 - a model of each of the following molecules: a....
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- Formamide, 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_forwardCalculate the Enthalpy Change (ΔH) from average bond energies, which have been listed below in KJ/mol, for the following reaction and identify the nature of the reaction: CH3COOH + CH3OH → CH3COOCH3 + H2O [C‒H: 413; C‒C: 347; C=O: 745; C=C: 614; Cl‒Cl: 239, C‒O: 358; O‒H: 467]arrow_forwardExplain why acetic acid, CH3CO2H, Contains two distinct types of Carbon oxygen Bonds, Whereas the acetate ion, formed by loss of hydrogen ion from acetic acid, Only contains one type of carbon oxygen bondarrow_forward
- How would you describe the molecular geometry of C2H2F2, and what are its bond angles?arrow_forwardSelect the bonds in the 3D representation of methyl urethane below that are multiple bonds. (Hint: Consider the number of bonds attached to an atom in the image compared to the normal valence of that atom. In a valid structure, the number of bonds to an atom will equal the valence of that atom.) • Gray = C: white = H; red = 0; blue = N; dark green = Cl; brown = Br; light green = F; purple = 1; yellow = S: orange = P. • Double click to select bonds. You can zoom in and out using the mouse scroll wheel (or pinch to zoom on touch screens). ●arrow_forwardOne way of naming alcohols is to name the alkyl group that is attached to the −OH and add the word alcohol. Write bond-line formulas for (a.) propyl alcohol and (b.) isopropyl alcohol.arrow_forward
- Draw the line-bond structure of oleic acid (cis-9-octadecenoic acid), CH3(CH2)7CH=CH(CH2)7COOH, at physiological pH. You do not need to draw hydrogen atoms attached to carbon atoms.arrow_forwardThe carbon–carbon bond length in C2H2 is 1.20 Å, that in C2H4 is 1.34 Å, and that in C2H6 is 1.53 Å. Near which of these values would you predict the bond length of C2 to lie? Is the experimentally observed value, 1.31 Å, consistent with your prediction?arrow_forwardFormation of ammonia from nitrogen and hydrogen is an exothermic process. Which of the following statements is true about the bonds that are broken and formed during this reaction? N2(g) + 3H2(g) ---> 2NH3(g) a.) products have lower PE because product bonds are weaker than reactants b.) products have higher PE because product bonds are stronger than reactants c.) products have higher PE because product bonds are weaker than reactants d.) products have lower PE because product bonds are stronger than reactantsarrow_forward
- Methanal can be made through the partial oxidation of methane using O2 in the presence of a catalyst: CH4 (g) + O2 (g) → CH2O(g) + H,O(g) a. Use bond dissociation enthalpies to estimate the enthalpy change for this reaction. Bond ΔΗ (kJ/mol) C-H 413 O=0 498 O=C 745 0-H 463 Enthalpy change = kJ b. Calculate the enthalpy change for this reaction from enthalpies of formation. Substance A;H (kJ/mol) CH4 (g) -74.87 O2 (g) H2 O(g) -241.8 CH20(g) -115.9 Enthalpy change kJarrow_forwardEthylene, C₂H₄, and tetrafluoroethylene, C₂F₄, are used tomake the polymers polyethylene and polytetrafluoroethylene(Teflon), respectively.(a) Draw the Lewis structures for C₂H₄ and C₂F₄, and give theideal H-C-H and F-C-F bond angles.(b) The actual H-C-H and F-C-F bond angles are 117.4and 112.4, respectively. Explain these deviations.arrow_forwardTwo useful organic compounds that contain Cl atoms are vinyl chloride (CH2 = CHCI) and chloroethane (CH;CH;CI). Vinyl chloride is the starting material used to prepare poly (vinyl chloride), a plastic used in insulation, pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic. Why is the C – Cl bond of | vinyl chloride stronger than the C – Cl bond in chloroethane.arrow_forward
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