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: 757312
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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 Molecules
There are many ways to represent moleculesIf 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?
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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?
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Klein, Organic Chemistry 2e Slide4
2.1 Representing Molecules
To draw large molecules quickly, a different type of representation is neededConsider the antibiotic Amoxicillin. Its Lewis structure looks cluttered, and it would be very time consuming to draw
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2.2 Bond-line Structures
The Bond-line structure is easier to read and to drawCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
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2.2 Bond-line Structures
It may seem like a foreign language at first, because many of the atoms are not labeledThis type of representation is THE main way that chemists communicate, so it is a language you MUST master to be successful in organic chemistry
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2.2 Bond-line Structures
Like 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 anglesCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
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2.2 Bond-line Structures
Like Lewis structures, lines are drawn between atoms to show covalent bondsCarbon-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.
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2.2 Bond-line Structures
Practice identifying the location of and counting the number of carbon and hydrogen atoms in the structures below
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2.2 Bond-line Structures
Double bonds and triple bonds are represented as you might expectWhy is a triple bond written without zigzagging?Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
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2.2 Bond-line Structures
You should practice bond-line structures until it becomes natural for you to see all of the carbon and hydrogen atom locations. What’s the molecular formula of the following molecule?
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Klein, Organic Chemistry 2e Slide12
2.2 Bond-line Structures
If you are given a Lewis structure or condensed structure, you must also be able to draw the corresponding bond-line structureRepresent the bond angles with zigzagsFollow VSEPR and spread out the electron pairs on a central atom
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2.2 Bond-line Structures
Single bonds are axes of rotation, so be aware that they can rotateGive alternative bond-line structures for the molecule below
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Klein, Organic Chemistry 2e Slide14
2.2 Bond-line Structures
Heteroatoms (atoms other than C and H) should be labeled with all hydrogen atoms and lone pairs attachedNEVER draw a carbon with more than 4 bonds!!
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2.2 Bond-line Structures
Draw bond-line representations for the following Lewis structures
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Klein, Organic Chemistry 2e Slide16Slide17
2.2 Bond-line Structures
Draw bond-line representations for 3 possible isomers given the formula: C5H9ClODraw bond-line structures for 3 different rotational conformations for the molecule: CH2CH(CH2)4CH3
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Klein, Organic Chemistry 2e Slide18
2.3 Indentifying Functional Groups
Bond-line structures allow chemists to quickly examine how a chemical reaction has changed a moleculeCompare 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?
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2.3 Indentifying Functional Groups
When 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.
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2.3 Indentifying Functional Groups
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2.4 Bond-line Structures with Formal Charge
Formal charge (section 1.4) affects the stability and reactivity of molecules, so you must be able to identify formal charges in bond-line representationsLabel all of the formal charges in the following moleculePractice with conceptual checkpoints 2.12 and 2.13
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Klein, Organic Chemistry 2e Slide23
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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. In such cases, the carbon will only have 3 bonds.
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Klein, Organic Chemistry 2e Slide25
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. If carbon carries a charge in a molecule, the charge MUST be shown on the bond-line structure
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2.5 Bond-line Structures and Lone Pair Electrons
Sometimes 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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Klein, Organic Chemistry 2e Slide27
2.5 Bond-line Structures and Lone Pair Electrons
If the formal charge is indicated on an atom, you can determine how many lone pairs are presentTo 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)
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2.5 Bond-line Structures and Lone Pair Electrons
How 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.HOW many lone pairs should it have?
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2.5 Bond-line Structures and Lone Pair Electrons
You can also determine the formal charge on an O atom by matching its bonding pattern with its formal charge according to table 2.2Practice with SkillBuilder 2.4
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2.5 Bond-line Structures and Lone Pair Electrons
The 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 2.3Practice with SkillBuilder 2.5
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Klein, Organic Chemistry 2e Slide32
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2.6 3D Bond-line Structures
The vast majority of molecules are 3-dimensional, but it is difficult to represent a 3D molecule on a 2D piece of paper or blackboardWe 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 Slide34
2.6 3D Bond-line Structures
Here are some other ways to show 3D structure
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2.7 Resonance
Drawing lines between atoms inadequately represents covalent bonds in molecules with resonanceRemember 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?
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2.7 Resonance
Let’s look at the hybridization of the carbons in the allyl carbocationCalculate the steric number (# of σ bonds + lone pairs)When the steric number is 3, it is sp
2 hybridized
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Klein, Organic Chemistry 2e Slide37
2.7 Resonance
If 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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2.7 Resonance
How 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 Slide39
2.7 Resonance
Resonance makes a molecule MORE stableDelocalization of electronsElectrons 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 hybrid
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Klein, Organic Chemistry 2e Slide40
2.8 Curved Arrows in Resonance
Throughout Organic Chemistry, we will be using curved arrows to show electron movementCurved 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 Resonance
Rules for using curved arrows to show RESONANCEAvoid breaking a single bond
Resonance 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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Klein, Organic Chemistry 2e Slide42
2.8 Curved Arrows in Resonance
Rules for using curved arrows to show RESONANCENever exceed an octet for 2nd row elements (B, C, N, O, F)Atoms in the 2nd row can only have four 2
nd energy level orbitals holding a max. of 8 electronsExamples of arrows that violate rule 2.
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Klein, Organic Chemistry 2e Slide43
2.8 Curved Arrows in Resonance
Rules for using curved arrows to show RESONANCE2nd row elements (B, C, N, O, F) will rarely but sometimes have LESS than an octet
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2.9 Formal Charge in Resonance
When using curved arrows to show RESONANCE, often structures will carry a formal charge that must be shownDraw the resonance contributor indicated by the arrows belowAre any of the rules violated?Show any formal charges on the contributors
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Klein, Organic Chemistry 2e Slide46
2.9 Formal Charge in Resonance
In the resonance, the arrows tell us how to move the electrons to create the other contributorDraw 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
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2.10 Patterns in Resonance
There are 5 main bonding patterns in which resonance occurs. Recognize these patterns to predict when resonance will occurAllylic lone pairsAllylic positive chargeLone pair of electrons adjacent to a positive charge
A pi bond between two atoms with different electronegativitiesConjugated pi bonds in a ringWe will see many examples in the next few slides
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Klein, Organic Chemistry 2e Slide48
2.10 Patterns in Resonance
Vinyl and allyl refer to positions directly bonded to or one atom away from a C=C double bond
Label the vinylic chlorides and the allylic chlorides
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Klein, Organic Chemistry 2e Slide49
2.10 Patterns in Resonance
Identifying allylic lone pairs
Circle all of the allylic lone pairs
Draw arrows on each structure to show resonance
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2-49Klein, Organic Chemistry 2e Slide50
2.10 Patterns in Resonance
Identifying allylic lone pairsFor each, show the resulting resonance contributor and all formal charges
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Klein, Organic Chemistry 2e Slide51
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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 below
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Klein, Organic Chemistry 2e Slide54
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2-54Klein, Organic Chemistry 2e Slide55
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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2-55Klein, Organic Chemistry 2e Slide56
2.10 Patterns in Resonance
A lone pair adjacent to a positive chargeConsider the resonance in the NITRO groupDraw all possible resonance contributors
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Klein, Organic Chemistry 2e Slide57
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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
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Klein, Organic Chemistry 2e Slide59
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2-59Klein, Organic Chemistry 2e Slide60
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 neighbors
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2.10 Patterns in Resonance
Summary figure 2.5
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Klein, Organic Chemistry 2e Slide62
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2.12 Delocalized vs. Localized
Localized – electrons are NOT in resonanceDelocalized – 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 atomsTo be delocalized, electrons must be on an sp
or sp2 hybridized atom Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.
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Klein, Organic Chemistry 2e Slide66
2.12 Delocalized vs. Localized
Does the delocalization of the electrons in the amide create a more or less stable contributor?
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Klein, Organic Chemistry 2e Slide67
2.12 Delocalized vs. Localized
The sp2 hybridization of the nitrogen atom causes it to be trigonal planar rather than tetrahedral
To be delocalized, all three atoms involved MUST have p orbitals overlappingCopyright © 2015 John Wiley & Sons, Inc. All rights reserved.
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2.12 Delocalized vs. Localized
Generally, lone pars adjacent to a C=C double bond are capable of resonance, but not in this case.Copyright © 2015 John Wiley & Sons, Inc. All rights reserved.2-68
Klein, Organic Chemistry 2e Slide69
2.12 Delocalized vs. Localized
Recall that delocalized electrons must exist in an unhybridized p orbital overlapping with p orbitals on neighboring atoms
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Klein, Organic Chemistry 2e Slide70
Additional Practice Problems
How many carbon and hydrogen atoms are in the following molecule?
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Klein, Organic Chemistry 2e Slide71
Additional Practice Problems
Draw the bond-line structures from the following formulas: C(CH3)3CNCl2CH(CH2)5CO
2HCH3CHBrCH(NH2)C(CH3)3
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Klein, Organic Chemistry 2e Slide72
Additional Practice Problems
Fill in any necessary formal charge on the molecule below
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Klein, Organic Chemistry 2e Slide73
Additional Practice Problems
Fill in any necessary lone pairs in the structure below
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Klein, Organic Chemistry 2e Slide74
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