Second Edition Chapter 2 Molecular Representations David Klein Copyright 2015 John Wiley amp Sons Inc All rights reserved Klein Organic Chemistry 2e 21 Representing Molecules There are many ways to represent molecules ID: 623706
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Slide1
Organic Chemistry
Second Edition
Chapter 2Molecular Representations
David Klein
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
Klein, Organic Chemistry 2e Slide2
2.1 Representing MoleculesThere are many ways to represent molecules
If you were representing a large molecule with 20 or more atoms, which structure would be most time consuming to draw?Which structures give you the most information about the structure?
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-2Klein, Organic Chemistry 2e Slide3
2.1 Representing Molecules
Given that there are three isomers of propanol (below), which structures above are adequate to represent only isopropanol and not its isomers?Practice with SkillBuilder 2.1
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-3
Klein, Organic Chemistry 2e Slide4
2.1 Representing MoleculesTo draw large molecules quickly, a different type of representation is needed
Consider the antibiotic Amoxicillin. Its Lewis structure looks cluttered, and it would be very time consuming to drawCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-4Klein, Organic Chemistry 2e Slide5
2.2 Bond-line StructuresThe Bond-line structure is easier to read and to draw
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-5Klein, Organic Chemistry 2e Slide6
2.2 Bond-line StructuresIt may seem like a foreign language at first, because many of the atoms are not labeled
This type of representation is THE main way that chemists communicate, so it is a language you MUST master to be successful in organic chemistryCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-6Klein, Organic Chemistry 2e Slide7
2.2 Bond-line StructuresLike Lewis structures, lines are drawn between atoms to show covalent bonds
Atoms are bonded at angles (zigzag) that represent the actual geometry of the bond anglesWhat is the bond angle for sp3 hybridized carbon?Carbon atoms are not labeled, but a carbon is assumed to be located at every corner or endpoint on the zigzag.
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-7Klein, Organic Chemistry 2e Slide8
2.2 Bond-line StructuresLike Lewis structures, lines are drawn between atoms to show covalent bonds
Carbon-Hydrogen bonds are omitted. WHY?If the H atoms are omitted, how will we know how many H atoms are attached to a carbon?Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-8Klein, Organic Chemistry 2e Slide9
2.2 Bond-line StructuresPractice identifying the location of and counting the number of carbon atoms in the structures below
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2-9Klein, Organic Chemistry 2e Slide10
2.2 Bond-line StructuresDouble bonds and triple bonds are represented as you might expect
Why is a triple bond written without zigzagging?
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Klein, Organic Chemistry 2e Slide11
2.2 Bond-line StructuresYou must also be able to use the bond-line structure language to interpret the number and location of H atoms in a molecule
H atoms are not shown, but we can assume there are enough to complete the octet (4 bonds) for each carbon
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-11
Klein, Organic Chemistry 2e Slide12
2.2 Bond-line StructuresYou should practice bond-line structures until it becomes natural for you to see all of the carbon and hydrogen atom locations.
How many carbon and hydrogen atoms are in the following molecule?Practice with SkillBuilder 2.2
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-12Klein, Organic Chemistry 2e Slide13
2.2 Bond-line StructuresIf you are given a Lewis structure or condensed structure, you must also be able to draw the corresponding bond-line structure
Represent the bond angles with zigzagsFollow VSEPR and spread out the electron pairs on a central atom
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Klein, Organic Chemistry 2e Slide14
2.2 Bond-line StructuresIf you are given a Lewis structure or condensed structure, you must also be able to draw the corresponding bond-line structure
Single bonds are axes of rotation, so be aware that they can rotateGive alternative bond-line structures for the molecule below
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-14Klein, Organic Chemistry 2e Slide15
2.2 Bond-line StructuresIf you are given a Lewis structure or condensed structure, you must also be able to draw the corresponding bond-line structure
Heteroatoms (atoms other than C and H) should be labeled with all hydrogen atoms and lone pairs attached
NEVER draw a carbon with more than 4 bonds!!Practice with SkillBuilder 2.3Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
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Klein, Organic Chemistry 2e Slide16
2.2 Bond-line StructuresDraw bond-line representations for the following Lewis structures
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-16Klein, Organic Chemistry 2e Slide17
2.2 Bond-line StructuresDraw bond-line representations for 3 possible isomers given the formula: C5
H9ClODraw bond-line structures for 3 different rotational conformations for the molecule: CH2CH(CH2)4CH3Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-17Klein, Organic Chemistry 2e Slide18
2.3 Indentifying Functional GroupsBond-line structures allow chemists to quickly examine how a chemical reaction has changed a molecule
Compare the condensed formula with the bond-line structure below for the same reactionWhich representation makes it more apparent that the H2 is reacting to convert the double bond to a single bond?
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-18Klein, Organic Chemistry 2e Slide19
2.3 Indentifying Functional GroupsWhen certain atoms are bonded together in specific arrangements, they undergo specific chemical reactions
Such arrangements of atoms are called functional groups
. WHY are such groups called FUNCTIONAL?Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-19Klein, Organic Chemistry 2e Slide20
2.3 Indentifying Functional Groups
More functional groups are listed in table 2.1Practice with conceptual checkpoint 2.11
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-20Klein, Organic Chemistry 2e Slide21
2.4 Bond-line Structures with Formal ChargeFormal charge (section 1.4) affects the stability and reactivity of molecules, so you must be able to identify formal charges in bond-line representations
Label all of the formal charges in the following moleculePractice with conceptual checkpoints 2.12 and 2.13
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-21
Klein, Organic Chemistry 2e Slide22
2.4 Bond-line Structures with Formal ChargeMost carbon atoms will have 4 covalent bonds and no lone pairs to avoid carrying a formal charge
Sometimes carbon will have a +1 charge. In such cases, the carbon will only have 3 bonds.Is there anything especially unstable about CARBOCATIONS?
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-22Klein, Organic Chemistry 2e Slide23
2.4 Bond-line Structures with Formal Charge
Most carbon atoms will have 4 covalent bonds and no lone pairs to avoid carrying a formal chargeSometimes carbon will have a -1 charge. Is there anything especially unstable about CARBANIONS?If carbon carries a charge in a molecule, the charge MUST be shown on the bond-line structure
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Klein, Organic Chemistry 2e Slide24
2.5 Bond-line Structures and Lone Pair ElectronsSometimes lone pairs are omitted from bond-line structures.
For example…You can’t determine the formal charge on the N atom unless you know how many electrons there are on the NIt could be…You must ALWAYS draw formal charges on a bond-line structure to eliminate confusion
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2.5 Bond-line Structures and Lone Pair ElectronsIf the formal charge is indicated on an atom, you can determine how many lone pairs are present
To calculate the number of lone pair electrons for an atom, compare the number of valence electrons that should be associated with the atom to the number of valence electrons that are actually associated with an atom (section 1.4)Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-25Klein, Organic Chemistry 2e Slide26
2.5 Bond-line Structures and Lone Pair ElectronsHow many lone pairs are on the oxygen atom below?
Oxygen should have 6 valence e-s assigned to it, because it is in group VIA on the periodic table.It is carrying a -1 charge, so it must actually have one additional electron (6+1=7) assigned1 electron is assigned to the oxygen from its bond with carbon. WHY?HOW many lone pairs should it have?
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-26
Klein, Organic Chemistry 2e Slide27
2.5 Bond-line Structures and Lone Pair ElectronsYou can also determine the formal charge on an O atom by matching its bonding pattern with its formal charge according to table 2.2
Practice with SkillBuilder 2.4
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-27Klein, Organic Chemistry 2e Slide28
2.5 Bond-line Structures and Lone Pair ElectronsThe formal charge on a N atoms can be calculated the same way or by matching its bonding pattern with its formal charge according to table 2.3
Practice with SkillBuilder 2.5
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-28Klein, Organic Chemistry 2e Slide29
2.6 3D Bond-line StructuresThe vast majority of molecules are 3-dimensional, but it is difficult to represent a 3D molecule on a 2D piece of paper or blackboard
We will use dashed and solid wedges to show groups that point back into the paper or out of the paper
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Klein, Organic Chemistry 2e Slide30
2.6 3D Bond-line StructuresImagine the thin lines as being flat in the plane of the board/paper
Dashed and solid wedges to show groups that point back into the paper or out of the paper
We will focus on this type of representation in Chapter 5Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-30Klein, Organic Chemistry 2e Slide31
2.6 3D Bond-line StructuresHere are some other ways to show 3D structure
Read the “Medically Speaking” section of Chapter 2 to see one example of how 3D structure is important
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Klein, Organic Chemistry 2e Slide32
2.7 ResonanceDrawing lines between atoms inadequately represents covalent bonds in molecules with resonance
Remember from General Chemistry, what is resonance?Consider the allyl carbocation:How is the bond-line structure inadequate in representing the allyl carbocation’s TRUE structure?
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-32Klein, Organic Chemistry 2e Slide33
2.7 ResonanceLet’s look at the hybridization of the carbons in the allyl carbocation
Calculate the steric number (# of σ bonds + lone pairs)When the steric number is 3, it is sp2 hybridized
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Klein, Organic Chemistry 2e Slide34
2.7 ResonanceIf all of the carbons have unhybridized
p orbitals, they can overlapAll three overlapping
p orbitals allow the electrons to move throughout the overlapping area simultaneouslyThat’s RESONANCE
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Klein, Organic Chemistry 2e Slide35
2.7 ResonanceFrom a molecular orbital point of view, when the THREE unhybridized p orbitals overlap, THREE new MOs are formed
How many electrons are in each of the MOs for the allyl carbocation?
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-35Klein, Organic Chemistry 2e Slide36
2.7 ResonanceThe allyl
carbocation has a charge of +1. Which MO is the missing electron missing from?Where is the positive charge located?
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-36Klein, Organic Chemistry 2e Slide37
2.7 ResonanceHow do we represent the
complete picture of the allyl carbocation provided by valence orbital and MO theories using a bond-line structure?The pi electrons can exist on both sides of the molecule, so we can use two resonance contributors to represent the structure
The brackets indicate that both resonance contributors exist simultaneously
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Klein, Organic Chemistry 2e Slide38
2.7 ResonanceBecause neither of the contributors exists (look at MOs), the average or hybrid is much more appropriate
vs. δ+ δ+ two contributors resonance hybridHow is a resonance arrow different from equilibrium?Analogy: a nectarine is a hybrid formed by mixing a peach and a plum. A nectarine is NOT sometimes a peach and sometimes a plum.
It is always a nectarine.
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-38
Klein, Organic Chemistry 2e Slide39
2.7 ResonanceResonance makes a molecule MORE stableDelocalization of electrons
Electrons exist in orbitals that span a greater distance giving the electrons more freedom minimizing repulsionsElectrons spend time close to multiple nuclei all at once maximizing attractionsDelocalization of chargeThe charge is spread out over more than one atom. The resulting partial charges are more stable than a full +1 charge. δ+ δ+
resonance hybridCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-39Klein, Organic Chemistry 2e Slide40
2.8 Curved Arrows in ResonanceThroughout Organic Chemistry, we will be using curved arrows to show electron movement
The sooner you master this skill, the easier the course will beCurved arrows generally show electron movement for pairs of electronsThe arrow starts where the electrons are currently locatedThe arrow ends where the electrons will end up after the electron movementWe will explore curved arrows to show other reactions in Chapter 3
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Klein, Organic Chemistry 2e Slide41
2.8 Curved Arrows in ResonanceRules for using curved arrows to show RESONANCE
Avoid breaking a single bond
Single bonds can break, but NOT in RESONANCEResonance occurs for electrons existing in overlapping p orbitals, while electrons in single bonds are overlapping sp, sp2, or sp3 (sigma) orbitals.
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41Klein, Organic Chemistry 2e Slide42
2.8 Curved Arrows in ResonanceRules for using curved arrows to show RESONANCE
Never exceed an octet for 2nd row elements (B, C, N, O, F)Atoms in the 2nd row can only have four 2nd energy level orbitals holding a max. of 8 electrons
Examples of arrows that violate rule 2.How does this arrow look?
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Klein, Organic Chemistry 2e Slide43
2.8 Curved Arrows in ResonanceRules for using curved arrows to show RESONANCE
2nd row elements (B, C, N, O, F) will rarely but sometimes have LESS than an octet
What will the resonance hybrid look like for this structure?Practice with SkillBuilder
2.6
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43Klein, Organic Chemistry 2e Slide44
2.9 Formal Charge in ResonanceWhen using curved arrows to show RESONANCE, often structures will carry a formal charge that must be shown
Draw the resonance contributor indicated by the arrows belowAre any of the rules violated?Show any formal charges on the contributors
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-44Klein, Organic Chemistry 2e Slide45
2.9 Formal Charge in ResonanceIn the resonance, the arrows tell us how to move the electrons to create the other contributor
Draw arrows showing the resonance in the reverse directionYou can also think of the arrows as showing the direction that charge will flowPractice with SkillBuilder 2.7
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-45Klein, Organic Chemistry 2e Slide46
2.10 Patterns in ResonanceThere are 5 main bonding patterns in which resonance occurs. Recognize these patterns to predict when resonance will occur
Allylic lone pairsAllylic positive chargeLone pair of electrons adjacent to a positive chargeA pi bond between two atoms with different
electronegativitiesConjugated pi bonds in a ringWe will see many examples in the next few slidesCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-46Klein, Organic Chemistry 2e Slide47
2.10 Patterns in ResonanceVinyl and
allyl refer to positions directly bonded to or one atom away from a C=C double bondLabel the vinylic chlorides and the allylic chlorides
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Klein, Organic Chemistry 2e Slide48
2.10 Patterns in Resonance
Identifying allylic lone pairsCircle all of the allylic lone pairs
Draw arrows on each structure to show resonance
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48Klein, Organic Chemistry 2e Slide49
2.10 Patterns in Resonance
Identifying allylic lone pairsFor each, show the resulting resonance contributor and all formal charges
Practice with conceptual check point 2.25
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Klein, Organic Chemistry 2e Slide50
2.10 Patterns in Resonance
Dealing with allylic positive chargeOnly one curved arrow is needed
If there are multiple double bonds (conjugated), then multiple contributors are possible. Show the resonance contributors and curved arrows belowDraw a resonance hybridPractice with conceptual checkpoint 2.26
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Klein, Organic Chemistry 2e Slide51
2.10 Patterns in Resonance
A lone pair adjacent to a positive chargeOnly one arrow is neededExplain how the formal charges are affected by the electron movement in the following examples
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Klein, Organic Chemistry 2e Slide52
2.10 Patterns in Resonance
A lone pair adjacent to a positive chargeConsider the resonance in the NITRO groupWhy can’t ONE arrow be used to cancel out the formal charge and create a resonance contributor?Draw all possible resonance contributors
Practice with conceptual checkpoint 2.27
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Klein, Organic Chemistry 2e Slide53
2.10 Patterns in Resonance
A pi bond between atoms of different electronegativityThe pi electrons will be more attracted to the more electronegative atomExplain how the formal charges are created by the electron movement in the following examples
Practice with conceptual checkpoint 2.28
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53Klein, Organic Chemistry 2e Slide54
2.10 Patterns in Resonance
Conjugated pi bonds in a ringEach atom in the ring MUST have an unhybridized p orbital that can overlap with its neighborsElectrons can be shown to move clockwise or counterclockwise
What type of motion do the electrons actually have?Practice with conceptual checkpoint 2.31
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Klein, Organic Chemistry 2e Slide55
2.10 Patterns in ResonanceSummary figure 2.5
Practice with conceptual checkpoint 2.32
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Klein, Organic Chemistry 2e Slide56
2.10 Patterns in Resonance
Show all of the resonance contributors for the following molecule
Notice that carbons with 4 bonds (sp3
) isolate areas of resonance from one another
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Klein, Organic Chemistry 2e Slide57
2.11 Stability of Contributors
Remember our nectarine analogy. Is a nectarine more like a peach or more like a plum?What if we made a fruit that was 65% peach, 34% plum, and 1% kiwi? How would that look?Similarly, there are many molecules that have multiple resonance contributors where not all resonance structures contribute equallyThe resonance hybrid will most resemble the more stable contributor(s)
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-57Klein, Organic Chemistry 2e Slide58
2.11 Stability of Contributors
How do we assess the stability of resonance contributors?Formal charge generally DECREASES stability, especially a +1 charge on an
electronegative atom or -1 on a low electronegativity atom
COMPLETE OCTETS INCREASE stabilityDraw the three resonance contributors for acetic acid
Assess the stability of each contributor, and draw a resonance hybrid
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Klein, Organic Chemistry 2e Slide59
2.11 Stability of Contributors
Formal charge generally DECREASES stabilityA +1 charge on an electronegative atom or -1 on a low electronegativity atom is especially unstable
COMPLETE OCTETS INCREASE stabilityDraw the three resonance contributors for the acetate ionAssess the stability of each contributor, and draw a resonance hybrid
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Klein, Organic Chemistry 2e Slide60
2.11 Stability of Contributors
Formal charge generally DECREASES stabilityA +1 charge on an electronegative atom or -1 on a low electronegativity atom is especially unstableCOMPLETE OCTETS INCREASE stability
Draw the resonance contributors for the following moleculeAssess the stability of each contributor, and draw a resonance hybrid
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Klein, Organic Chemistry 2e Slide61
2.11 Stability of Contributors
The octet rule is usually a bigger factor than formal charge when assessing stabilityFor each structure, assess the stability of each contributor, and draw a resonance hybrid
Practice with SkillBuilder 2.8
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Klein, Organic Chemistry 2e Slide62
2.12 Delocalized vs. LocalizedLocalized – electrons are NOT in resonance
Delocalized – electrons ARE in resonanceDelocalization increases stabilityThere are a couple ways to recognize electrons that are delocalized through resonance?To be delocalized, electrons must exist in an unhybridized p orbital that can overlap with p orbitals on neighboring atoms
To be delocalized, electrons must be on an sp or sp2 hybridized atom Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-
62Klein, Organic Chemistry 2e Slide63
2.12 Delocalized vs. LocalizedDoes the delocalization of the electrons in the amide create a more or less stable contributor?
Delocalization must be a very stabilizing force if it can favor sp
2 hybridization over sp3 even when the delocalization doesn’t involve two equally stable contributorsCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
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Klein, Organic Chemistry 2e Slide64
2.12 Delocalized vs. LocalizedTo allow for delocalization (resonance), some atoms that would normally be sp
3 will become sp2 hybridizedCalculate the steric number and predict the hybridization for Nitrogen atom of an amideIf the Nitrogen atom were sp3, its lone pair
of electrons couldn’t engage in resonanceThe Nitrogen of an amide will be sp2 hybridizedIn this case, the stability of the delocalization outweighs the stability difference between sp
2 and sp3 Why is sp
2 generally less stable than sp3 ?
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Klein, Organic Chemistry 2e Slide65
2.12 Delocalized vs. Localized
The sp2 hybridization of the nitrogen atom causes it to be trigonal planar rather than tetrahedralTo be delocalized, all three atoms involved MUST have p orbitals overlapping
Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-65Klein, Organic Chemistry 2e Slide66
2.12 Delocalized vs. Localized
Generally, lone pars adjacent to a C=C double bond are capable of resonance, but not in this case.
The electron movement above does not violate any of our rules, so why can’t the Nitrogen’s lone pairs be delocalized? - see next slideCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-
66Klein, Organic Chemistry 2e Slide67
2.12 Delocalized vs. LocalizedRecall that delocalized electrons must
exist in an unhybridized p orbital overlapping with p orbitals on neighboring atoms
The Nitrogen’s lone pair is positioned perpendicular to the plane where the other pi electrons residePractice with SkillBuilder 2.9Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-
67Klein, Organic Chemistry 2e Slide68
Additional Practice ProblemsHow many carbon and hydrogen atoms are in the following molecule?
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68Klein, Organic Chemistry 2e Slide69
Additional Practice ProblemsDraw the bond-line structures from the following formulas: C(CH
3)3CNCl2CH(CH2)5CO2H
CH3CHBrCH(NH2)C(CH3)3Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-
69Klein, Organic Chemistry 2e Slide70
Additional Practice ProblemsFill in any necessary formal charge on the molecule below
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70Klein, Organic Chemistry 2e Slide71
Additional Practice ProblemsFill in any necessary lone pairs in the structure below
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71Klein, Organic Chemistry 2e Slide72
Additional Practice Problems
Show all of the resonance contributors for the following molecule and draw the resonance hybridCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
2-72Klein, Organic Chemistry 2e