Ch. 16 - Conjugated SystemsWorksheetSee all chapters
All Chapters
Ch. 1 - A Review of General Chemistry
Ch. 2 - Molecular Representations
Ch. 3 - Acids and Bases
Ch. 4 - Alkanes and Cycloalkanes
Ch. 5 - Chirality
Ch. 6 - Thermodynamics and Kinetics
Ch. 7 - Substitution Reactions
Ch. 8 - Elimination Reactions
Ch. 9 - Alkenes and Alkynes
Ch. 10 - Addition Reactions
Ch. 11 - Radical Reactions
Ch. 12 - Alcohols, Ethers, Epoxides and Thiols
Ch. 13 - Alcohols and Carbonyl Compounds
Ch. 14 - Synthetic Techniques
Ch. 15 - Analytical Techniques: IR, NMR, Mass Spect
Ch. 16 - Conjugated Systems
Ch. 17 - Aromaticity
Ch. 18 - Reactions of Aromatics: EAS and Beyond
Ch. 19 - Aldehydes and Ketones: Nucleophilic Addition
Ch. 20 - Carboxylic Acid Derivatives: NAS
Ch. 21 - Enolate Chemistry: Reactions at the Alpha-Carbon
Ch. 22 - Condensation Chemistry
Ch. 23 - Amines
Ch. 24 - Carbohydrates
Ch. 25 - Phenols
Ch. 26 - Amino Acids, Peptides, and Proteins
Sections
Conjugation Chemistry
Stability of Conjugated Intermediates
Allylic Halogenation
Conjugated Hydrohalogenation (1,2 vs 1,4 addition)
Diels-Alder Reaction
Diels-Alder Forming Bridged Products
Diels-Alder Retrosynthesis
Molecular Orbital Theory
Drawing Atomic Orbitals
Drawing Molecular Orbitals
HOMO LUMO
Orbital Diagram: 3-atoms- Allylic Ions
Orbital Diagram: 4-atoms- 1,3-butadiene
Orbital Diagram: 5-atoms- Allylic Ions
Orbital Diagram: 6-atoms- 1,3,5-hexatriene
Orbital Diagram: Excited States
Pericyclic Reaction
Thermal Cycloaddition Reactions
Photochemical Cycloaddition Reactions
Thermal Electrocyclic Reactions
Photochemical Electrocyclic Reactions
Cumulative Electrocyclic Problems
Sigmatropic Rearrangement
Cope Rearrangement
Claisen Rearrangement
Additional Practice
Conjugated Halogenation
Diels-Alder Inductive Effects
Diels-Alder Regiospecficity
Diels-Alder Asymmetric Induction
Diels-Alder Synthesis
Allylic SN1 and SN2
Cumulative Orbital Diagram Problems
Cumulative Cycloaddition Reactions
Cumulative Sigmatropic Problems
UV-Vis Spect Basics
UV-Vis Spect Beer's Law
Molecular Electronic Transition Therory
Woodward-Fieser Rules
Additional Guides
Diene

Get out your pencil (and eraser) because we are about to learn how to draw atomic orbitals.

 

Two Rules:

  1.  The # of atomic orbitals = the # of conjugated atoms
  2. You need to know what type of pi electron contribution each type of non-bonding orbital will have

Concept #1: Two Rules of Drawing Atomic Orbitals

Transcript

Now that we understand a little bit about how atomic orbitals can blend together into molecular orbitals I want to go back to the beginning and make sure that we all understand how to draw atomic orbitals correctly. So, let's get started.

So, thankfully transforming a conjugated molecule into atomic orbitals only requires two steps and they're super easy. So, this lesson should be very easy for you. So, rule number one, the number of atomic orbitals that you have in your molecule should be equal to the number of conjugated atoms that you have, so the rule basically states that you should have one atomic orbital drawn per conjugated atom, so notice that in this molecule that I have drawn it's an anion, I actually have 4 atoms 1, 2, 3, 4, good? But let's look again, how many of those atoms actually have nonbonding orbitals? have orbitals that are not bonded to atoms, well, it turns out that one doesn't count because it only has orbitals that are attached to atoms, so that would not be a conjugated atom, the other ones are conjugated though because we know that 2 has an orbital with an electron, 3 has an orbital with an electron and then an anion, anytime you see an anion that means it's a lone pair with a negative charge. So, those are nonbonding orbitals and for every nonbonding orbital or conjugated atom you would have one atomic orbital, so that means that then I would just put 3 atomic orbitals and this would just basically be for atom 2, atom 3 and atom 4 easy enough, right? So then, rule number 2 says you need to know what type of pi electron contribution each type of nonbonding orbital will have. So, remember, we went over the nonbonding orbitals and we said that there's different types, right? So, let's just start from the beginning, empty orbitals and carbocations donate 0 electrons because and 0 electrons inside, right? Pi bonds and radicals donate one each because in each situation there's one electron that's possible to be conjugated, okay? And then finally a lone pair and an anion. Notice that they have two electrons in the orbitals, they donate to each, okay? So, what you would do is you would count up the number of atomic orbitals that you have, line them up and then you would add in the number of pi electrons that are being contributed, okay? So, in the following examples, we're going to go over some molecules and we're going to try to draw the atomic orbitals for them.

Example #1: Supply Atomic Orbitals

Example #2: Supply Atomic Orbitals

Example #3: Supply Atomic Orbitals