Organic Chemistry (6th Edition)
6th Edition
ISBN: 9781260119107
Author: Janice Gorzynski Smith
Publisher: McGraw Hill Education
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Textbook Question
Chapter 1, Problem 81P
a. What is the predicted hybridization and geometry around each carbon atom?
b. Two electrostatic potential plots are drawn for these species. Which ion corresponds to which diagram and why?
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CH3+ and CH3− are two highly reactive carbon species.
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Chapter 1 Solutions
Organic Chemistry (6th Edition)
Ch. 1.1 - While the most common isotope of nitrogen has a...Ch. 1.2 - Label each bond in the following compounds as...Ch. 1.3 - Draw a valid Lewis structure for each species. a....Ch. 1.3 - Prob. 9PCh. 1.4 - Draw Lewis structures for each molecular formula....Ch. 1.6 - Classify each pair of compounds as isomers or...Ch. 1.6 - Prob. 12PCh. 1.6 - Prob. 13PCh. 1.6 - Prob. 14PCh. 1.6 - Prob. 16P
Ch. 1.6 - Prob. 17PCh. 1.7 - Prob. 18PCh. 1.7 - Prob. 19PCh. 1.7 - Using the principles of VSEPR theory, you can...Ch. 1.8 - Convert each condensed formula to a Lewis...Ch. 1.8 - Prob. 22PCh. 1.8 - Prob. 23PCh. 1.8 - Convert each skeletal structure to a complete...Ch. 1 - Citric acid is responsible for the tartness of...Ch. 1 - Zingerone gives ginger its pungent taste. a.What...Ch. 1 - Assign formal charges to each and atom in the...Ch. 1 - Prob. 44PCh. 1 - Prob. 46PCh. 1 - Draw all possible isomers for each molecular...Ch. 1 - 1.45 Draw Lewis structures for the nine isomers...Ch. 1 - Prob. 52PCh. 1 - Prob. 53PCh. 1 - Prob. 54PCh. 1 - Consider compounds A-D, which contain both a...Ch. 1 - Draw in all the carbon and hydrogen atoms in each...Ch. 1 - 1.61 Convert each molecule into a skeletal...Ch. 1 - Prob. 65PCh. 1 - Predict the hybridization and geometry around each...Ch. 1 - Prob. 68PCh. 1 - Ketene, , is an unusual organic molecule that has...Ch. 1 - Rank the following bonds in order of increasing...Ch. 1 - Two useful organic compounds that contain Cl atoms...Ch. 1 - Use the symbols + and to indicate the polarity of...Ch. 1 - Prob. 74PCh. 1 - Anacin is an over-the-counter pain reliever that...Ch. 1 - 1.77 Stalevo is the trade name for a medication...Ch. 1 - 1.78 and are two highly reactive carbon...Ch. 1 - 1.79 The N atom in (acetamide) is hybridized,...Ch. 1 - Prob. 83PCh. 1 - Prob. 84PCh. 1 - Prob. 85PCh. 1 - Prob. 86PCh. 1 - Prob. 87PCh. 1 - Prob. 88P
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- Use the VSEPR model to predict the bond angles around each central atom in the following Lewis structures (benzene rings are frequently pictured as hexagons, without the letter for the carbon atom at each vertex). Note that the drawings do not necessarily depict the bond angles correctly.arrow_forwarda Carbonyl fluoride, COF2, is an extremely poisonous gas used in organofluorine synthesis. Give the valence bond description of the carbonyl fluoride molecule. (Both fluorine atoms are attached to the carbon atom.) b Nitrogen, N2, makes up about 80% of the earths atmosphere. Give the valence bond description of this molecule.arrow_forwardFor each of the following molecules, state the bond angle (or bond angles, as appropriate) that you would expect to see on the central atom based on the simple VSEPR model. Would you expect the actual bond angles to be greater or less than this? a CCl4 b SCl2 c COCl2 d AsH3arrow_forward
- In Chapter 6, we study a group of organic cations called carbocations. Following is the structure of one such carbocation, the tert-butyl cation. (a) How many electrons are in the valence shell of the carbon bearing the positive charge? (b) Using VSEPR, predict the bond angles about this carbon. (c) Given the bond angle you predicted in (b), what hybridization do you predict for this carbon?arrow_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_forwardWhich of the following factors contribute to the tetrahedral shape of the above molecule? Group of answer choices A. the shape of the two p orbitals in the carbon atom B. the shape of the one s orbital in the carbon atom C. the shape of the sp3 hybrid orbitals of the electrons shared between the carbon and hydrogen atoms D. hydrogen bonding configurations between the carbon and hydrogen atomsarrow_forward
- B. Answer the next two questions about the Lewis structure of XYZ shown below. メー三 -YEz: I. What is the hybridization of the central atom? II. For all covalent bonds, specify the type of bond (o vs. T) and the atomic orbitals that overlap to form the bond. For example, in a molecule of H2, the only bond is o: H(s)-H(s).arrow_forward1.You have made structures of NH3 and H2CO molecules in the Part A of your lab report.Both NH3 and H2CO molecules have three electron groups around the central atom.However, their molecular geometries are not the same. Explain this difference. 2. Draw the Lewis electron dot structure for SCl2 and discuss its molecular geometry. IsSCl2 molecule polar or nonpolar? Explain your answer.arrow_forwardDraw the 2D and the 3D Lewis structure for each molecule. You do not need to show resonance structures here. Determine the electron pair geometry (EPG), the molecular geometry (MG), the bond angle (BA) around the central atom, and the hybridization of the central or bold atom. Circle the formula of any polar molecule. For molecules with more than one central atom (e.g. CHCH20H) give the structure around the bold atom.arrow_forward
- 2. Complete the table for the indicated compounds Molecule C2H2 SF5- NO3- Lewis structure include lone pairs & formal charges on each atom Resonance structures don't have to include lone pairs; write N/A if there are none Electron Geometry Hybridization on central atom Overlapping orbitals include value of n in the orbital name (e.g. 1s, not s). Write N/A if that kind of bond is not present in the molecule T: Molecular Geometry Bond angle(s) include < as necessary 3D structure and polarity don't have to include lone pairs; draw the |dipole arrow on the molecule or write "non- polar"arrow_forward5. The element sulfur (S) bonds with element T. Element I is has 7 valence electrons and needs 8 electrons for a stable octet. Element T has a lower electronegativity than sulfur Draw the 3D lewis structure (perspective) for ST| | b. What is the VSEPR molecular geometry? | c. Indicate whether the molecule is polar or non polar. Explain how you know а.arrow_forward2. From the models of SF4, BrF3, and XeF4, deduce whether different atom arrangement, called geometrical isomers, are possible; if so, sketch them below. Indicate the preferred geometry for each case and suggest a reason for your choice. Indicate which structures have dipole moments and show their direction, Preferred Molecular Compound Electron Dipole Reason Geometry Moment (Polarity) geometry SF4 BRF3 XeF4 3. Using the Lewis structure predict the geometrical structures of the following ions and state the hybridization of the central atom. Ion Electron Geometry Molecular Formal Charge Central Atom Geometry of Central Hybridization Atom CO32- NO3- BF4arrow_forward
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