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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O 13
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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_forwardWhat are the angles a and b in the actual molecule of which this is a Lewis structure? H H C H a H C ^ b C a = 11° b=0° H -H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. X 3arrow_forward
- Which 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_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_forwardHydrogen selenide is one of nature's most foul-smelling substances. Molecules of H2Se have H-Se-H bond angles very close to 90°. How would VB theory explain the bonding in H2Se? Select the correct sketch of the orbital diagram to show how the bonds are formed. (In all choices, x stands for an electron being shared by hydrogen.) 4s 4p 1x 4s 4p 111 XX 4s 4p 11 XX 4s 4parrow_forward
- 12abarrow_forwardHere'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_forward10. Each ball-and-stick model below shows the electron-pair and molecular geometry of a generic molecule. Explain what is wrong with each molecular geometry and provide the correct molecular geometry based on the number of lone and bonding pairs around the central atom. (a) (b) (c) 11. Draw the Lewis structure for acetamide (CH3CONH2) and determine the geometry about each interior atom. Experiments show that the geometry about the N atom in acetamide is nearly planar. Draw a resonance structure that can account for the planar geometry about the N atom.arrow_forward
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