Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Chapter 3, Problem 11E
Draw orbital representations of bonding in water and methane
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Electrons in bonds are negatively charged and therefore repel each other. If you had are a molecule of formula AB 3 , with A being the central atom, what would you predict the 3D shape to be to allow maximum distance between the three B atoms bonded to A ? A tripod-like or pyramidal -the shape, with A being the tip of the tripod and the B atoms being the " feet" of the tripod distanced less than 120° from each other A triangular shape, with A in the middle and all B atoms at 120° from each other AT shape, with A in the middle and the tip of the "".
Electrons in bonds are negatively charged and therefore repel each other. If you had a molecule of formula AB 4 , with A being the central atom, what would you predict the 3D shape to be to allow maximum distance between the four B atoms bonded to A? Some kind of tridimensional shape with A in the middle and B-A-B bond angles bigger than 90° A bidmensional shape like a "" sign where the B - A - B bond angles ate exactly 90 degrees
There are
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Chapter 3 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 3 - Prob. 1CTQCh. 3 - What neutral atom is represented by the electron...Ch. 3 - Prob. 3CTQCh. 3 - Consider any one of the four identical hybrid...Ch. 3 - Prob. 5CTQCh. 3 - Prob. 6CTQCh. 3 - Prob. 7CTQCh. 3 - Prob. 8CTQCh. 3 - Prob. 9CTQCh. 3 - Prob. 10CTQ
Ch. 3 - On the left side of Figure 3.6, label the areas...Ch. 3 - Prob. 12CTQCh. 3 - Prob. 13CTQCh. 3 - Prob. 14CTQCh. 3 - Prob. 15CTQCh. 3 - Now consider the fully formed molecule on the...Ch. 3 - Prob. 1ECh. 3 - Explain why the two molecules below cannot...Ch. 3 - Prob. 3ECh. 3 - Consider the incomplete orbital representation of...Ch. 3 - Consider the following orbital representation of...Ch. 3 - Summarize how one determines the hybridization...Ch. 3 - Explain what is wrong with each of the following...Ch. 3 - Prob. 8ECh. 3 - Prob. 9ECh. 3 - Complete the following tables, and memorize their...Ch. 3 - Draw orbital representations of bonding in water...Ch. 3 - Draw electron configuration diagrams for carbon in...Ch. 3 - Prob. 13E
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- Best Lewis Formula and Molecular Geometry A student writes the Lewis electron-dot formula for the carbonate anion, CO32, as a Does this Lewis formula obey the octet rule? Explain. What are the formal charges on the atoms? Try describing the bonding for this formula in valence bond terms. Do you have any difficulty doing this? b Does this Lewis formula give a reasonable description of the electron structure, or is there a better one? If there is a better Lewis formula, write it down and explain why it is better. c The same student writes the following resonance description for CO2: Is there something wrong with this description? (What would you predict as the geometries of these formulas?) d Is one or the other formula a better description? Could a value for the dipole moment help you decide? e Can you write a Lewis formula that gives an even better description of CO2? Explain your answer.arrow_forwardConsider the following molecules: SiH4, PH3, H2S. In each case, a central atom is surrounded by four electron pairs. In which of these molecules would you expect the bond angle to be less than 109.5? Explain your reasoning.arrow_forwardhow do i solve this problemarrow_forward
- Draw a Lewis structure for the C3Hg molecule using the connectivity shown in the spacefilling model in the window. • Gray C; white = H; red = 0; blue = N; dark green= Cl; brown = Br; light green = F; purple I; yellow = S; orange = P. Use your drawing to answer the following questions. The total number of electrons in C-H bonds = The number of C-C single bonds = Previous Use your drawing to answer the following questions. The total number of electrons in C-H bonds = The number of C-C single bonds = The number of C=C double bonds = The total number of unshared pairs = Nextarrow_forwardWhich statement about the charge-minimized Lewis structure of the cyanate anion (OCN) is true? (Charges not shown in the Lewis structure.) N=3=O There are two o-bonds oriented at 180° to one another. There are two л-bonds oriented at 180° to one another. There are two formal negative charges. The central carbon is sp2-hybridized.arrow_forward[Review Topics] [References] Use the References to access important values if needed for this question. Draw a Lewis structure for the C₂H6O molecule, using the connectivity shown in the spacefilling model in the window. (Gray = C; white = H; red = 0; blue = N; dark green = Cl; brown = Br; light green= F; purple = I; yellow = S; orange = P.) The number of C-H bonds = Submitted The number of O-H bonds = 20 The number of C-C single bonds = The number of C-O single bonds = The total number of lone pairs = $ 4 R F 288 V %6 5 PA T Cengage Learning Cengage Technical Support 6 I G MacBook Air B pe Y H & 7 N F7 U J H 8 1 M ( 9 K V 1 ) O L P Previous ¡ Email Instructor Save and Exit Next [ 11 1 Darrow_forward
- Given the values of bond length, arranged in DECREASING order of intramolecular force:(1) C=O 133;(2) C—O 143;and (3) CΞN 116 3 < 1 < 2 2 < 1 < 3 1 < 2 < 3 3 < 2 < 1 None of the abovearrow_forwardUse VSEPR theory to predict the geometry (including bond angles) about each interior atom of methyl azide (CH3N3), and make a sketch of the molecule. Would you expect the bond angle between the two interior nitrogen atoms to be the same or different? Would you expect the two nitrogen–nitrogen bond lengths to be the same or different?arrow_forward12abarrow_forward
- Here's a wild molecule: disulfur dinitride (S2N2). It can be isolated as a crystalline solid, but it is unstable (explosive). Therefore, it must to be handled carefully in an inert atmosphere free of oxygen. X-ray diffraction measurements of the crystalline solid indicate the atoms are arranged in a square with the sulfur atoms on opposite corners and the nitrogen atoms on the remaining opposite corners. Consider the bonding in this unusual molecule. a. Determine the best Lewis structure representation for S2N2. Include the formal charges on each atom in the structure. b. Determine the valence bonding theory predictions for hybridization at each atom in S2N2. The bond angles in S2N2 have been measured by X-ray diffraction and are all approximately 90°. Does valence bond theory do a good job of predicting this observation? Consider the geometry and bonding of S2N2 computed using molecular orbital theory. The results are shown below. Identify the orbital character of the HOMO(-2),…arrow_forwardThe 3rd Nitrogen from the left has 3 sigma bonds and a lone pair. Isn't that sp3?arrow_forwardDraw the Lewis dot structure for acetic acid (HC2H3O2, CH3COOH). Determine the optimum formal charge structure. Determine the VSEPR domain and molecular geometries for the central carbon atoms. Determine the hybridization of the carbons and oxygens. Determine the polarity of the molecule; show the polarity arrows and partial charges for the molecule. (Electronegativities: H 2.1,C 2.5, O 3.5)arrow_forward
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