Analyzing Organic Reactions Flashcards

1
Q
type of acid or base:
electron acceptor (in formation of a covalent bond), vacant p-orbitals or positively polarized atoms; tend to be electrophiles
A

Lewis acid

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2
Q
type of acid or base: 
electron donor (in formation of a covalent bond), lone pair of electrons that can be donated, are often anions; tend to be nuclephiles
A

Lewis base

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3
Q

created by interaction of Lewis acid and base

A

coordinate covalent bond

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4
Q

type of acid or base:

can donate a proton (H+)

A

Bronsted-Lowry acid

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5
Q

type of acid or base:

can accept a proton (H+)

A

Bronsted-Lowry base

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6
Q

molecule that can act as either a Bronsted-Lowry acid or base (like H2O)

A

amphoteric

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7
Q

measures strength of acid in solution

A

acid dissociation constant (Ka)

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8
Q

acid dissociation constant (Ka)

A

Ka = [H+] [A-] / [HA]

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9
Q

pKa

A

pKa = -log Ka

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10
Q

“nucleus-loving” species; has lone pairs or π bonds that can form new bonds to electrophiles; strength is based on relative rates of reaction with common electrophile

A

nucleophile

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11
Q

four major factors that determine nucleophilicity:

A

1) charge - nucleophilicity increases with increasing electron density (more negative charge)
2) electronegativity - neucleophilicity decreases as electronegativity increases because these atoms are less likely to share electron density
3) steric hindrance - bulkier molecules are less nucleophilic
4) solvent - protic solvents can hinder nucleophilicty by protonating the nucleophile or though H-bonding

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12
Q

“electron-loving” species; has positive charge or positively polarized atom than can accept an electron pair forming new bonds with a nucleophile; more positive compounds are more electrophilic

A

electrophile

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13
Q

a bond is broken and both electrons are given to one of the two products; essentially the opposite of a coordinate covalent polar bond formation

A

heterolytic reactions

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14
Q

molecular fragments that retain electrons after heterolysis; best groups will be able to stabalize extra electrons: weak bases (like I-, Br-, and Cl-) are good, H ions and alkanes are very bad

A

leaving group

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15
Q

a reaction where a nucleophile forms a bond with a substrate carbon and a leaving group leaves

A

nucleophilic substitution reaction

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16
Q

type of nucleophilic substitution reaction:
two steps: first, leaving group leaves forming carbocation, second, nucleophile attacks carbocation from either side; reactions prefer more substituted carbons because alkyl group can donate electron density and stabilize carbocation; rate depends on concentration of substrate

A

Sn1

17
Q

type of nucleophilic substitution reaction:
one step: nucleophile attacks from back (less sterics) as leaving group leaves; inversion of stereochemistry; reaction prefers less substituted carbons because less steric hindrance; rate depends on concentration of substrate and nucleophile

A

Sn2

18
Q

hypothetical charge an atom would have if all of its bonds were totally ionic; can be calculated from molecular formula

A

oxidation state

19
Q

most reduced form of carbon

A

CH4 : C = -4, each H = +1

20
Q

most oxidized form of carbon

A

CO2 : C = +4, each O = -2

21
Q

oxidation state of ions

A

equal to the charge

22
Q

an increase in oxidation state assisted by oxidizing agents

A

oxidation

23
Q

accept electrons and are reduced in process; have affinity for electrons or unusually high oxidation state, often contain metal and large number of oxygens

A

oxidizing agents

24
Q

common oxidizing agent(s)

A

PCC (pyridinium chlorochromate), CrO3 (chromium trioxide), Na2Cr2O7 or K2Cr2O7 (sodium or potassium dichromate)

25
Q

can be oxidized one level to aldehydes (by PCC) or two levels to carboxylic acids (by CrO3, Na2Cr2O7, or K2Cr2O7)

A

primary alcohols

26
Q

can be oxidized to ketones by most oxidizing agents

A

secondary alcohols

27
Q

can be oxidized to carboxylic acids by most oxidizing agents

A

aldehydes

28
Q

a decrease in oxidation state assisted by reducing agents

A

reduction

29
Q

donate electrons and are oxidized in process; have low electronegativity and ionization energy, often contain metal and large number of hydrides

A

reducing agents

30
Q

common reducing agent(s)

A

LAH (LiAlH4, lithium aluminum hydride)

31
Q

can be reduced to alcohols by LAH

A

aldehydes, ketones, and carboxylic acids

32
Q

can be reduced to amines by LAH

A

amides

33
Q

can be reduced to a pair of alcohols by LAH

A

esters

34
Q

the preferential reaction of one functional group in the presence of other functional groups; both nucleophile-electrophile and oxidation-reduction reactions tend to react at the highest priority (most oxidized) functional group

A

chemoselectivity

35
Q

refers to when bulky groups (such as protecting groups) can make it impossible for the nucleophile to reach the most reactive electrophile, making the nucleophile more likely to attack another region

A

steric protection

36
Q

Ka

A

Ka = 10^-pKa