Carboxylic Acids (Chapter 19) Flashcards

1
Q

Why are carboxylic acid groups planar?

A

Conjugation (i.e. π-electron delocalization) between the carbonyl group and the hydroxyl group sets the entire carboxylic acid domain in the same plane.

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2
Q

Structure of Carboxylic Acid Groups

A

Planar

The carbonyl group and the hydroxyl group are in the same plane due to π-electron delocalization across the two functional groups.

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3
Q

Reagent Reactions with Carboxylic Acids

A
  • Nucleophile: Addition to Carbonyl Carbon
  • Base: Deprotonation of Hydroxyl Hydrogen
  • Acid: Protonation of Carbonyl Oxygen

The acidic protonation of the carbonyl oxygen is more favored than protonation of the hydroxyl oxygen. (The carbonyl oxygen will always be protonated before the hydroxyl oxygen.)

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4
Q

What determines the acidity of a carboxylic acid?

A

Stability of the (Carboxylic Acid’s) Conjugate Base

The acidity of a carboxylic acid increases as the stability of its conjugate base increases.

(Carboxylic acids with conjugate bases possessing a lower negative charge density are MORE STABLE than carboxylic acids with conjugate bases possessing a higher negative charge density.)

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5
Q

Carboxylate Anion

A

Deprotonated Form of Carboxylic Acid

—COO

The carboxylate anion is the conjugate base of the carboxylic acid.

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6
Q

Carboxylic Acid Acidity: Electron-Withdrawing Group

Electron-Withdrawing Group = EWG

A

Increases Acidity

The EWG stabilizes/delocalizes the negative charge of the carboxylate anion (through inductive effects), so the carboxylic acid is more prone to donating the H+ ion.

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7
Q

Carboxylic Acid Acidity: Electron-Donating Group

Electron-Donating Group = EDG

A

Decreases Acidity

The EDG destabilizes/increases the negative charge of the carboxylate anion (through inductive effects), so the carboxylic acid is less prone to donating the H+ ion.

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8
Q

Carboxylic Acid Acidity: Number of EWGs

Electron-Withdrawing Group = EWG

A

As the number of EWGs increases, the acidity of the carboxylic acid increases.

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9
Q

Carboxylic Acid Acidity: Number of EDGs

Electron-Donating Group = EDG

A

As the number of EDGs increases, the acidity of the carboxylic acid decreases.

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10
Q

Carboxylic Acid Acidity: Distance from EWG

Electron-Withdrawing Group = EWG

A

As the distance to the EWG(s) decreases, the acidity of the carboxylic acid increases.

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11
Q

Carboxylic Acid Acidity: Distance from EDG

Electron-Donating Group = EDG

A

As the distance to the EDG(s) decreases, the acidity of the carboxylic acid decreases.

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12
Q

Why is protonation of the carbonyl Oxygen more favorable than protonation of the hydroxyl Oxygen?

A

Protonation of the carbonyl Oxygen results in multiple cationic resonance structures (i.e. a greater delocalization of positive charge).

Protonation of the carbonyl Oxygen results in a single cationic resonance structure (i.e. no delocalization of positive charge).

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13
Q

Methods to Synthesize Carboxylic Acids

A
  • Oxidation of 1° Alcohols OR Aldehydes
  • Organometallic Addition to CO2
  • Hydrolysis of Nitriles
  • Synthesis of 2-Hydroxyl Carboxylic Acids
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14
Q

Electron-Donating Groups (EDGs)

A
  • —R (Akyl)
  • —OR (Ether)
  • —OCOR (Acyloxyl)
  • —OH (Hydroxyl)
  • —NHCOR (Amide)
  • —NR2 (Amine)
  • —NHR (Amine)
  • —NH2 (Amine)

EDGs decrease the acidity of carboxylic acids.

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15
Q

Electron-Withdrawing Groups (EWGs)

A
  • —X (Halide)
  • —COOH (Carboxylic Acid)
  • —COOR (Ester)
  • —COR (Ketone)
  • —CF3 (Trialkylfluoride)
  • —CN (Nitrile)
  • —SO3+H (Sulfonic Acid)
  • —NO2 (Nitro)
  • —NR3+ (Trialkylammonium)

EWGs increase the acidity of carboxylic acids.

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16
Q

1° Alcohol ⟶ Carboxylic Acid

A

Jones Oxidation

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17
Q

Aldehyde ⟶ Carboxylic Acid

No Intermediate

A

Jones Oxidation

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18
Q

Reagents: Jones Oxidation

A

Na2Cr2O7, H2SO4

  • CrO3, H2SO4
  • HNO3
  • KMnO4
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19
Q

Organometallic ⟶ Carboxylic Acid

Organometallic = Grignard or Organolithium

A

Organometallic Addition to CO2

The addition of an organometallic to CO2 results in a carboxylic acid compound with one more carbon than the organometallic reagent.

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20
Q

CO2 ⟶ Carboxylic Acid

A

Organometallic Addition to CO2

The addition of an organometallic to CO2 results in a carboxylic acid compound with one more carbon than the organometallic reagent.

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21
Q

Reagents: Organometallic Addition to CO2

Starting Material: Organometallic Compound

A
  1. CO2
  2. H3O+
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22
Q

Alkyl Halide ⟶ Carboxylic Acid

Grignard Intermediate

A
  1. Grignard Synthesis
  2. Organometallic Addition to CO2

This Grignard-intermediated synthesis reaction can occur with any alkyl halide compound.

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23
Q

Alkyl Halide ⟶ Carboxylic Acid

Nitrile Intermediate

A
  1. Nitrile Synthesis
  2. Nitrile Hydrolysis

This nitrile-intermediated synthesis reaction can only occur with 2°/1°/0° alkyl halides.

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24
Q

Alkyl Halide ⟶ Carboxylic Acid

Alcohol Intermediate

A
  1. OH Addition
  2. Jones Oxidation

This alcohol-intermediated synthesis reaction can ONLY occur with 1°/0° alkyl halides.

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25
Nitrile ⟶ Carboxylic Acid | **Nitrile =** —CN
Nitrile Hydrolysis
26
Alkyl Halide ⟶ Nitrile | **Nitrile =** —CN
SN2 Addition of CN to Alkyl Halide ## Footnote **NaCN =** CN
27
*Reagents:* Nitrile Hydrolysis
1. NaOH, Δ 2. H3O+ ## Footnote **Alternative:** H2SO4, H2O, Δ
28
Limitation of SN2 Nitrile Synthesis
SN2-mediated nitrile synthesis CANNOT occur with *3° alkyl halides*, *phenyl halides*, or *alkenyl halides*. ## Footnote SN2-mediated nitrile synthesis can ONLY occur with 2°/1°/0° alkyl halides.
29
Aldehyde ⟶ Carboxylic Acid | Cyanohydrin Intermediate
2-Hydroxyl Carboxylic Acid Synthesis
30
Cyanohydrin
A compound containing a *cyanide group* (—CN) and an *alcohol group* bonded to the *same* sp3-hybridized carbon atom.
31
*Reagents:* 2-Hydroxyl Carboxylic Acid Synthesis
1. NaCN, H2SO4 2. H2SO4, H2O, Δ
32
Mechanisms: Synthesis of Carboxylic Acid from Alkyl Halide
* **Jones Oxidation** (Alcohol Intermediate) * **Nitrile Synthesis-Hydrolysis** (Nitrile Intermediate) * **Organometallic Addition** (Carboxylate Intermediate) ## Footnote * The *Jones Oxidation* product contains the **same number** of carbons as the alkyl halide reagent. * The *Nitrile Synthesis-Hydrolysis* and *Organometallic Addition* products contain **one more** carbon than the alkyl halide reagent.
33
*Examples:* Carboxylic Acid Derivatives
* Acyl Halide * Anhydride * Ester * Amide
34
Anhydride
35
Acyl Halide
36
Amide
37
Ester
38
Carboxylic Acid ⟶ Ester
Fischer Esterification | Reversible ## Footnote * A catalytic acid (i.e. H2SO4, HCl) *must* be present for Fischer Esterification to occur. * The esterification process yields one molecule of byproduct H2O.
39
*Reagents:* Fischer Esterification | **Starting Material =** Carboxylic Acid
R—OH (Large Excess), H2SO4, Δ
40
Ester ⟶ Carboxylic Acid
Acid-Catalyzed Ester Hydrolysis | Reversible
41
*Reagents:* Acid-Catalyzed Ester Hydrolysis | **Starting Material =** Ether
H2O, H2SO4, Δ
42
Why must an *acid catalyst* be present for Fischer Esterification to occur?
The carbonyl Oxygen (of the carboxylic acid) must be protonated (by the acid catalyst) to increase the electrophilicity of the carboxylic acid compound. ## Footnote The unprotonated carboxylic acid compound is NOT sufficiently electrophilic to be attacked by the alcohol nucleophile.
43
*Mechanism:* Fischer Esterification
1. Protonation of Carbonyl Oxygen 2. Attack of Alcohol at Carbonyl Carbonyl 3. Elimination of Water ## Footnote The nucleophilic attack of the alcohol at the carbonyl Carbon results in an sp3-hybridized tetrahedral intermediate.
44
Hydroxycarbonic Acid
A carboxylic acid compound containing one (or more) hydroxyl groups.
45
Hydroxycarbonic Acid ⟶ Lactone
Intramolecular Esterification | Reversible
46
Lactone
Cyclic Ester ## Footnote Lactone are formed via the *intramolecular esterification* reaction.
47
Why does the *intramolecular esterification* reaction favor the lactone product?
Entropic Effects ## Footnote The hydroxycarbonic acid reagent is converted to a lactone compound *and* a water molecule.
48
*Reagents:* Intramolecular Esterification | **Starting Material =** Hydroxycarbonic Acid
H2SO4
49
*Reagents:* Lactone Hydrolysis
H2O, H2SO4
50
Lactone ⟶ Hydroxycarbonic Acid
Lactone Hydrolysis | Reversible
51
Carboxylic Acid ⟶ Amide
High-Temperature Amine Addition | Reversible ## Footnote The high-temperature amine addition reaction is an *addition-elimination mechanism* (that occurs slowly).
52
Carboxylic Acid ⟶ Ammonium-Salt
Low-Temperature Amine Addition | Reversible ## Footnote The low-temperature amine addition reaction is an *acid-base mechanism* (that occurs rapidly).
53
Ammonium-Salt Synthesis vs. Amide Synthesis | Carboxylic Acid Addition to Amines
* **Ammonium-Salt Synthesis:** Rapid Acid-Base Mechanism * **Amide Synthesis:** Slow Addition-Elimination Mechanism ## Footnote * The *ammonium salt* product is favored (i.e. the major product) at *low* reaction temperatures. * The *amide* product is favored (i.e. the major product) at *high* reaction temperatures.
54
*Conditions:* Ammonium-Salt Synthesis | Carboxylic Acid Addition to Amines
Amine at 0°C–100°C | Low Temperature
55
*Conditions:* Amide Synthesis | Carboxylic Acid Addition to Amines
Amine at >100°C | High Temperature
56
Why is *amine addition* an ineffective way to synthesize amide compounds? | Carboxylic Acid Addition to Amines
* High reaction temperatures create dangerous laboratory conditions. * Presence of competing reactions to form ammonium carboxylate salt.
57
Imide
58
Why is Imide Synthesis only possible with 0°/1° amines?
The imide synthesis mechanism requires the **double deprotonation** of the amine.
59
Dicarboxylic Acid ⟶ Imide
Imide Synthesis ## Footnote * The imide synthesis reaction requires the input of **heat**. * Imide Synthesis is *only* possible with **0°/1° amines**. (The synthesis processes requires the double deprotonation of the amine.)
60
*Reagents:* Imide Synthesis
2 NH3, Δ ## Footnote **Alternative:** 2 NRH2, Δ
61
Lactam
Cyclic Amide
62
Amino Acid ⟶ Lactam
Lactam Synthesis ## Footnote * The *lactam synthesis* reaction involves the cyclization of an amino acid. * **Heat** is required for the cyclization reaction to occur.
63
*Reagents:* Lactam Synthesis
1. Low Temperature 2. Δ
64
Lactone Classifications
* **3-Membered Ring:** α-Lactone * **4-Membered Ring:** β-Lactone * **5-Membered Ring:** γ-Lactone * **6-Membered Ring:** δ-Lactone
65
Carboxylic Acid ⟶ Acyl Chloride
SOCl2-Faciliated Chloride Substitution ## Footnote The *hydroxyl group* (of the carboxylic acid) is substituted for a *chloride* to yield an acyl chloride.
66
Carboxylic Acid ⟶ Acyl Bromide
PBr3-Faciliated Bromide Substitution ## Footnote The *hydroxyl group* (of the carboxylic acid) is substituted for a *bromide* to yield an acyl bromide.
67
*Mechanism:* SOCl2-Faciliated Chloride Substitution | **Starting Material =** Carboxylic Acid
1. Nucleophilic Attack of SOCl2 to Yield Inorganic Ester 2. Protonation by H—Cl to Yield Oxocarbenium Intermediate 3. Nucleophilic Attack of Cl to Yield Tetrahedral Intermediate 4. π-Electron Rearrangement to Eliminate SO2 and Cl
68
*Mechanism:* PBr3-Faciliated Bromide Substitution | **Starting Material =** Carboxylic Acid
1. Nucleophilic Attack of PBr3 to Yield Inorganic Ester 2. Protonation by H—Br to Yield Oxocarbenium Intermediate 3. Nucleophilic Attack of Br to Yield Tetrahedral Intermediate 4. π-Electron Rearrangement to Eliminate PBr2OH
69
*Reagents:* SOCl2 Substitution vs. PBr3 Substitution | **Starting Material =** Carboxylic Acid
* **SOCl2 Substitution:** SOCl2, Δ * **PBr3 Substitution:** PBr3
70
*Elimination Step:* SOCl2 Substitution vs. PBr3 Substitution | Carboxylic Acid Substitution
* **SOCl2 Substitution:** Hydroxyl oxygen π-electron rearrangement eliminates SO2 and Cl *without additional protonation*. * **PBr3 Substitution:** *Protonation of ether oyxgen* is required for hydroxyl oxygen π-electron rearrangement to eliminate PBr2OH.
71
Why should acid catalysts *NOT* be used in the amine-nucleophile addition to carboxylic acids?
* The acid catalyst could potentially protonate the amine nucleopile, which would *eliminate the amine's nucleophilic character*.
72
Carboylic Acid ⟶ 1° Alcohol
LiAlH4 Reduction ## Footnote The reduction of carboxylic acids to 1° alcohols can occur ONLY with LiAlH4. (NaBH4 is a *weaker reductant* than LiAlH4, so it cannot reduce carboxylic acids.)
73
*Reagents:* LiAlH4 Reduction
1. LiAlH4 2. H3O+
74
What factors determine the reactivity/electrophilicy of carboxylic acid derivates?
* Magnitude of Partial Positive Charge on Carbonyl Carbon. * Stabiity of Leaving Group (i.e. Strength of C—LG Bond). | **LG =** Leaving Group
75
*Reactivity:* Partial Positive Charge on Carbonyl Carbon | Carboxylic Acid Derivates
As the carbonyl carbon becomes *more partially positive*, the carboxylic acid derivative becomes *more reactive*. ## Footnote A *greater* partial positive charge on the carbonyl carbon *increases* the derivative's susceptibility to nucleophilic attack.
76
*Reactivity:* Stability of Leaving Group | Carboxylic Acid Derivates
As the stability of the leaving group *increases*, the carboxylic acid derivative becomes *more reactive*. ## Footnote A *more stable* leaving group denotes a *weaker* (i.e. more easily broken) C—LG bond.
77
What detemines the *strength* of the Carbon—LG bond? | Nucleophilic Attack of Carboxylic Acid Derivatives
The *extent of conjugation* between the carbonyl group and the adjacent heteroatom. ## Footnote If the adjacent heteroatom is a *weaker π-electron donor*, the C—LG bond is *weaker* (due to a lower degree of conjugation between the carbonyl group and heteroatom).
78
Strength of CCarbonyl—X Bond
The CCarbonyl—X bond is *weaker* due to the halogen being a *weak π-electron donor*. ## Footnote The *weak conjugation* between the carbonyl group and the halogen atom *increases* reactivity of the acyl halide.
79
Strength of CCarbonyl—N Bond
The CCarbonyl—N bond is *stronger* due to the nitrogen being a *strong π-electron donor*. ## Footnote The *strong conjugation* between the carbonyl group and the nitrogen atom *decreases* reactivity of the amide.
80
Reactivity of Acyl Halides | Carboxylic Acid Derivates
Acyl halides are *highly reactive* due to the (1) the halide's electron-withdrawing character and (2) the *weak* CCarbonyl—X bond.
81
Reactivity of Amides | Carboxylic Acid Derivates
Amides are relatively *unreactive* due to the (1) the nitrogen's electron-donating character and (2) the *strong* CCarbonyl—N bond.
82
Why is the CCarbonyl—N bond *shorter* than typical C—N bonds?
Conjugation between the carbonyl group and the nitrogen atom *increases the strength* of the CCarbonyl—N bond.
83
Why is rotation of the CCarbonyl—N bond slow?
Rotation about the CCarbonyl—N bond requires breaking the carbonyl-nitrogen conjugation across the amide, which is highly *enthalpically unfavorable* (at room temperature).
84
What determines the *basicity* of carboxylic acid derivatives? | Basicity of Carbonyl Oxygen
Stability of the (Derivative's) Conjugate Acid
85
What determines the *acidity* of carboxylic acid derivatives? | Acidity of α-Hydrogen
Stability of the (Derivative's) Conjugate Base
86
What factors dictate the *basicity* of carboxylic acid derivatives? | Basicity of Carbonyl Oxygen
* Positive-Charge Density of Conjugate Acid * Positive-Charge Compatibility in Conjugate Acid ## Footnote * If there is a *smaller* positive charge on the conjugate acid's hydroxyl oxygen, the derivative is *more basic*. * If the conjugate acid's resonance structures place the positive charge on *less electronegative* atoms, the derivative is *more basic*.
87
What factor dictates the *acidity* of carboxylic acid derivatives? | Acidity of α-Hydrogen
Negative-Charge Density of Base ## Footnote If there is a *smaller* negative charge on the conjugate base's α-Carbon, the derivative is *more acidic*.
88
*EWGs:* Acidity of Carboxylic Acid Derivatives
Increased Acidity ## Footnote EWGs delocalize the negative charge of the enolate conjugate base, which results in a *more stable* anionic compound.
89
*EWGs:* Basicity of Carboxylic Acid Derivatives
Decreased Basicity ## Footnote EWGs concentrate the positive charge on the conjugate acid's hydroxyl oxygen, which results in a *less stable* cationic compound.
90
*EDGs:* Acidity of Carboxylic Acid Derivatives
Decreased Acidity ## Footnote EDGs concentrates the negative charge of the enolate conjugate base, which results in a *less stable* anionic compound.
91
*EDGs:* Basicity of Carboxylic Acid Derivatives
Increased Acidity ## Footnote EDGs delocalize the positive charge on the conjugate acid's hydroxyl oxygen, which results in a *more stable* cationic compound.
92
Alkyl Halide ⟶ Carboxylic Acid
* **Same # of Carbons:** Jones Oxidation * **One Additional Carbon:** [Grigard + CO2] OR [Nitrile Hydrolysis]
93
Why is Imide Synthesis only possible with 0°/1° amines?
94
**Four Differences:** Carboxylic Acid Esterification vs. Carboxylic Acid Amidification
1. Initial Protonation to "Activate" Carbonyl Carbon 2. Proton Transfer to Form Neutral Tetrahedral Intermediate 3. Proton Acquisition to Eliminate H2O 4. Deprotonation of Carbonyl Oxygen to Yield Neutral Carbonyl ## Footnote * In Carboxylic Acid Esterification, the proton transfer processes involve external-internal exchanges (due to the presence of an **acid catalyst**). * In Carboxylic Acid Amidification, the proton transfer processes involve intramolecular exchanges (due to there being **no** acid catalyst).