Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Chapter 2, Problem 15E
Interpretation Introduction
Interpretation:An example for a molecule with exception to the octet rule should be given.
Concept introduction:Octet rule explains that in a molecule the number of valence electrons around the atoms of N, O, C & F should be equals to 8.
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Which atoms in this formula have not achieved Lewis octets? Redraw this formula by changing nonbonding electrons into bonding electrons and giving each atom a Lewis octet..
Read the following statements. Which ones are correct? Be sure to explain how you know.
BF3 and PFs are examples of exceptions to the octet rule.
II. BF,¯ and BFg-NH3 are examples of violations of the octet rule.
III. Expanded valence shells occur most often when the central atom is bonded to a small, electronegative element.
IV. The central atoms most capable of having expanded valence shells come from rows 3, 4, and 5 of the periodic table.
With regard to resonance structures that are drawn for a real species, which of
the following statements is NOT TRUE?
Select one:
O A. Resonance structures are not real; they are only drawn structures.
O B. The real species rapidly oscillates between the resonance structures,
O C. Resonance structures differ in the location of their electrons, not the
positions of their atoms.
O D. Resonance structures all have electron localized structures, while the
real species that is described by them has delocalized electrons..
Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 2 - Prob. 1CTQCh. 2 - The valence shell of an atom in a legitimate Lewis...Ch. 2 - Prob. 3CTQCh. 2 - Prob. 4CTQCh. 2 - Prob. 5CTQCh. 2 - It is impossible to draw a legitimate Lewis...Ch. 2 - Describe how to calculate the total number of...Ch. 2 - Prob. 8CTQCh. 2 - Prob. 9CTQCh. 2 - Prob. 10CTQ
Ch. 2 - Prob. 11CTQCh. 2 - Prob. 12CTQCh. 2 - A complete Lewis structure must show all nonzero...Ch. 2 - Prob. 14CTQCh. 2 - Prob. 15CTQCh. 2 - Prob. 16CTQCh. 2 - Prob. 17CTQCh. 2 - Prob. 18CTQCh. 2 - Complete the rest of the table for N, O or X by...Ch. 2 - Prob. 20CTQCh. 2 - Prob. 21CTQCh. 2 - Make a checklist that can be used to determine if...Ch. 2 - Prob. 2ECh. 2 - Prob. 3ECh. 2 - Draw the Lewis structure of a neutral molecule...Ch. 2 - Prob. 5ECh. 2 - For each element, predict (and draw a Lewis...Ch. 2 - Predict which of the following species is least...Ch. 2 - The molecules BH3 and SF6 and the ion SO42 exist...Ch. 2 - These are NOTlegitimate Lewisstructures (and...Ch. 2 - Fill in missing formal charges where needed (all...Ch. 2 - Below each structure in the previous question is a...Ch. 2 - Prob. 12ECh. 2 - Carbon monoxide (CO) is an example of an overall...Ch. 2 - Explain why this Lewis structure for CO is not as...Ch. 2 - Prob. 15ECh. 2 - Prob. 16ECh. 2 - Prob. 17ECh. 2 - Prob. 18ECh. 2 - Prob. 19E
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- What is the maximum number of atoms to which a central atom in a molecule can bond and still conform to the octet rule? What is the minimum number?arrow_forwardIn the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.arrow_forwardExplain why nonmetal atoms in Period 3 and beyond can accommodate greater than an octet of electrons and those in Period 2 cannot do so.arrow_forward
- On the basis of the electronegativity values given in Fig. 12.3. indicate which is the more polar bond in each of the following pairs. msp;a.OClorOBrc.PSorPOb.NOorNFd.HOorHNarrow_forwardChloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.arrow_forwardThese are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.arrow_forward
- The molecules BH3 and SF6 and the ion SO42 exist and are stable. Draw a Lewis structure of each,and comment on whether they are exceptions to Lewis’ octet rule.arrow_forwardSulfur and oxygen form a series of 2 anions including sulfite, SO32, and sulfate, SO42. In addition to these, there are three other more complex anionsdithionite, S2O42, dithionate, S2O62, and tetrathionate, S4O62. Write correct Lewis structures for dithionite, dithionate, and tetrathionate ions.arrow_forwardthe formal charges on all the atoms in the following Lewis diagrams. Which one would best represent bonding in the molecule Cl2O ?arrow_forward
- The “Chemistry in Focus" segment Hiding Carbon Dioxide- discusses attempts at sequestering (storing) underground CO2produced at power plants so as to diminish the: greenhouse effect. Draw all resonance structures of the CO2molecule.arrow_forwardI'm having trouble trying to figure out where to move the doule bond, bc wherever I place it seems like it would violate the octet rule. can someone explain simply?arrow_forwardWhich if the following cannot exceed the octet in a molecule? S, l, N, or Parrow_forward
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