Name: how aliphatic amines act as bases
Uploaded: 2023-04-30T10:38:56.000Z
Duration: 1 min 21 s
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Las alquilaminas alifáticas reaccionan como bases de Brønsted-Lowry, es decir, como aceptores de protones, para formar el ácido conjugado, los iones alquilamonio.
El valor de pKa del ion alquilamonio indica la basicidad relativa de la amina; un valor de pKa más alto significa un ácido conjugado más débil y una base más fuerte correspondiente. Por lo tanto, las alquilaminas son bases más fuertes que el amoníaco.
La mayor basicidad de las alquilaminas se debe a los efectos inductivos de los grupos alquilo y a los efectos de solvatación que estabilizan los iones de amonio correspondientes mediante enlaces de hidrógeno.
Los grupos alquilo donantes de electrones estabilizan el ion amonio mediante la deslocalización parcial de la carga positiva, aumentando así su valor pKa.
Sin embargo, el valor de pKa no aumenta como se esperaba de los iones alquilamonio secundarios a terciarios debido al efecto de solvatación reducido.
El aumento del obstáculo estérico en el ion alquilamonio terciario disminuye la viabilidad de la solvatación.
Como los efectos inductivos y de solvatación estabilizan por igual el ion alquilamonio secundario, su valor de pKa es mayor que el de los iones primario y terciario correspondientes.

basicidad de las aminas alifáticas

Basicity of Aliphatic Amines

Las aminas pueden comportarse como bases de Brønsted-Lowry al aceptar un protón del ácido para formar los ácidos conjugados correspondientes. Debido a un par solitario de electrones no enlazantes, las aminas alifáticas también pueden actuar como bases de Lewis formando un enlace covalente con un electrófilo.


 Para medir la basicidad de las aminas, generalmente se utilizan dos convenciones. El primero define K_b como la constante de basicidad para la reacción de desprotonación del agua por la amina, como se presenta en la Figura 1. Convencionalmente, una K_b más baja indica una mayor basicidad de la amina. Por ejemplo, el amoníaco y la metilamina tienen constantes de basicidad de 4,7 y 3,3, respectivamente.

<img alt="Figure1" src="/files/ftp_upload/12526/12526-PT_Figure_2.svg" style="text-align: center; height: 65px;">
Figura 1. La desprotonación del agua por una amina.

 La otra convención correlaciona la basicidad de las aminas con la acidez del ácido conjugado correspondiente. Cuanto mayor sea la constante de acidez, pK_a, del ácido conjugado, mayor será la basicidad de la amina a partir de la cual se formó el ácido conjugado. Por ejemplo, como se muestra en la Figura 2, los ácidos conjugados de amoníaco, metilamina y etilamina tienen valores de pK_a de 9,26, 10,64 y 10,75, respectivamente. Esto indica la mayor basicidad de la etilamina, seguida de la metilamina y el amoníaco.

<img alt="Figure2" src="/files/ftp_upload/12526/12526-PT_Figure_3.svg" style="text-align: center; height: 100px;">
Figura 2. Los valores de pK_a de varias aminas.

 Las aminas alifáticas son más básicas que el amoníaco debido a la capacidad de liberación de electrones de los grupos alquilo unidos al átomo de N. El grupo alquilo estabiliza el ácido conjugado dispersando su carga positiva; como resultado, mejora la basicidad de las aminas. Podría anticiparse que las aminas terciarias, que tienen tres grupos alquilo, deberían ser más básicas que las aminas primarias que tienen sólo un grupo alquilo. Sin embargo, esto sólo es cierto en la fase gaseosa, donde vemos la acidez de los ácidos conjugados de amoníaco, metilamina, dimetilamina y trimetilamina en el orden que se indica a continuación.


 [NH_4]^+ &gt; [MeNH_3]^+ &gt; [Me_2NH_2]^+ &gt; [Me_3NH]^+


 Por lo tanto, el amoníaco es la base más débil y la trimetilamina es la base más fuerte en la fase gaseosa. Sin embargo, la basicidad de las aminas en la fase acuosa también se ve influenciada por la solvatación de los ácidos conjugados correspondientes en agua. Por lo tanto, a pesar de tener tres grupos alquilo unidos al átomo de N, los ácidos conjugados de aminas terciarias tienen solo un átomo de H para ser donado para el enlace de H intermolecular con agua. Por el contrario, los ácidos conjugados de aminas primarias tienen tres átomos de H para formar enlaces de hidrógeno intermoleculares con agua. Por lo tanto, los valores de pK_a de los ácidos conjugados de aminas en una solución acuosa son como se muestra en la Figura 3.

<img alt="Figure3" src="/files/ftp_upload/12526/12526-PT_Figure_5.svg" style="text-align: center; height: 100px;">
Figura 3. Valores de pK_a de ácidos conjugados de aminas.

 Los ácidos conjugados de aminas secundarias disfrutan de un equilibrio óptimo entre la capacidad de liberación de electrones de los grupos alquilo y la capacidad de solvatación con agua.

Basicidad de las aminas alifáticas

Las aminas pueden comportarse como bases de Brønsted-Lowry aceptando un protón del ácido para formar los ácidos conjugados correspondientes. Debido a un solo par de ...

Education

Educación

JoVE Core

Organic Chemistry

Química Orgánica

Unit 1

Unidad 1

Amines

Aminas

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

how aliphatic amines act as bases

Aliphatic amines act as bases because the nitrogen atom can accept a proton from an acid. They can also behave as Lewis bases, since the nitrogen lone pair can form a covalent bond with an electrophile. These properties make amines useful examples of basic behavior in organic chemistry.

Amine basicity is commonly described in two ways. One method uses the basicity constant, K b, for the reaction in which the amine removes a proton from water. A lower K b means a stronger base. By this measure, methylamine is more basic than ammonia, with K b values of 3.3 and 4.7, respectively.

A second method compares the p K a values of the conjugate acids of amines. In this case, a higher p K a means the original amine is more basic. The conjugate acids of ammonia, methylamine, and ethylamine have p K a values of 9.26, 10.64, and 10.75. This shows that ethylamine is the most basic of the three, followed by methylamine and then ammonia.

Aliphatic amines are more basic than ammonia because alkyl groups push electron density toward the nitrogen atom. This effect helps stabilize the conjugate acid by spreading out its positive charge. It is easy to expect tertiary amines to be the most basic, since they have three alkyl groups, but that trend is only true in the gas phase.

In the gas phase, the conjugate acids follow the order [NH4]+ &gt; [MeNH3]+ &gt; [Me2NH2]+ &gt; [Me3NH]+ in acidity. That means ammonia is the weakest base and trimethylamine is the strongest base there. In water, however, solvation changes the trend. Tertiary amine conjugate acids have only one hydrogen for hydrogen bonding with water, while primary amine conjugate acids have three.

Because of this, aqueous basicity follows a different order from the gas phase. The conjugate acids of amines in water show p K a values that reflect the balance between alkyl electron donation and solvation. Secondary amines often show the best balance of these two effects.

How Aliphatic Amines Act as Bases

amines: introduction

Amines: Types and Classifications

Amines are organic derivatives of ammonia. They form when one or more ammonia protons are replaced by alkyl or aryl groups. Chemists sort amines by the number of organyl groups attached to the nitrogen atom. Primary amines have one organyl group on nitrogen. Secondary amines have two, and tertiary amines have three. If a fourth organyl group is present, the nitrogen carries a formal positive charge. These compounds are called quaternary ammonium salts. Amines are also grouped as aliphatic or...

nomenclature of primary amines

Naming Primary Amines in Organic Chemistry

Primary amines are named by following a few clear organic chemistry rules. These rules help identify the amino group, written as –NH2, and show how it connects to the carbon chain. Common names for primary amines use the alkyl group name plus the suffix -amine. In IUPAC naming, the final -e of the parent alkane is changed to -amine, which gives an alkanamine name. The longest carbon chain attached to the amine nitrogen is chosen, and the carbon bonded to nitrogen gets the lowest locant. Any...

nomenclature of secondary and tertiary amines

nomenclature-of-secondary-and-tertiary-amines

Naming Secondary, Tertiary, and Quaternary Amines

Secondary and tertiary amines are ammonia derivatives with two or three hydrogen atoms replaced by alkyl groups. They may be symmetrical, with the same alkyl groups attached to nitrogen, or unsymmetrical, with more than one kind of alkyl group present. These compounds are often named as alkylamines in standard naming. For symmetrical secondary and tertiary amines, the prefixes di- and tri- are used. For unsymmetrical amines, each substituent is named and listed in alphabetical order. IUPAC...

nomenclature of aryl and heterocyclic amines

nomenclature-of-aryl-and-heterocyclic-amines

Naming Aniline and Ring Amine Derivatives

Naming aniline and ring amine derivatives follows clear rules for aromatic and heterocyclic amines. The simplest aromatic amine is phenylamine, which has an –NH2 group directly attached to an aromatic ring. The common name for this skeleton is aniline. Functionalized anilines often use the prefixes ortho-, meta-, and para- to show where a substituent is placed on the ring. Many of these compounds also have trivial, or common, names. For systematic naming, the ring is numbered from the carbon...

structure of amines

Amines: Shape, Bonding, and Chirality

Amines have a nitrogen atom with a lone pair of electrons. That lone pair affects the shape of the molecule, the bond angles, and the bond lengths around nitrogen. In most amines, nitrogen is hybridized and attached to three substituents. The bond angle is about 108°, which is a little less than the 109.5° tetrahedral angle. The C–N–H bond angle is slightly larger at 112°, and the carbon-nitrogen bond length is 147 pm. This bond is longer than the carbon-oxygen bond in alcohols, which is 143...

physical properties of amines

Amines: Smell, Solubility, and Boiling Points

Amines show clear physical properties that depend on molecular size and structure. Low molecular weight amines are usually gases at room temperature, while higher molecular weight amines are often liquids or solids. Many low molecular weight amines also have a rotten fish-like smell, and diamines usually have a pungent odor. Amines are polar molecules, so they can take part in intermolecular hydrogen bonding. Primary and secondary amines have N–H bonds that allow these interactions. Because of...

basicity of aliphatic amines

Aliphatic amines act as bases because the nitrogen atom can accept a proton from an acid. They can also behave as Lewis bases, since the nitrogen lone pair can form a covalent bond with an electrophile. These properties make amines useful examples of basic behavior in organic chemistry. Amine basicity is commonly described in two ways. One method uses the basicity constant, K b, for the reaction in which the amine removes a proton from water. A lower K b means a stronger base. By this measure,...

basicity of aromatic amines

Why Aromatic Amines Are Less Basic

Aromatic amines are less basic than aliphatic amines because the nitrogen lone pair can share electrons with the aryl ring through resonance. When the lone pair is delocalized, it is less available to accept a proton, so the amine shows weaker basicity. Substituents on the aryl ring can change this effect. Electron-donating groups increase electron density on the ring and raise the basicity of the amine. Electron-withdrawing groups have the opposite effect and can lower basicity sharply. A...

basicity of heterocyclic aromatic amines

Why Ring Nitrogen Changes Amine Basicity

Heterocyclic amines can show very different basicity depending on where the nitrogen atom sits in the ring. When nitrogen is part of an alicyclic ring, the amine behaves much like an alkylamine. When nitrogen is part of an aromatic ring, the compound is usually much less basic than its alicyclic counterpart. Piperidine and pyridine show this difference clearly. Piperidine is significantly more basic than pyridine, with pKb values of 2.8 and 8.8, respectively. The reason is the orbital that...

nmr spectroscopy of amines

Amines in NMR: Key Signal Patterns

Amines in NMR spectroscopy show clear signal patterns that help identify their structure. In proton NMR, primary amines and secondary amines give a broad N–H signal between δ 0.5 and 5 ppm. The exact position can change with sample concentration, hydrogen bonding, and the solvent used. The N–H protons in amines are labile, which means they exchange quickly in solution. Because of this fast proton exchange, they do not split with nearby protons. Their peak stays broad and does not reveal the...

mass spectrometry of amines

Amines in Mass Spectra

Amines in mass spectra show a clear pattern that helps identify them. Their parent ions often have odd molecular weights, which follows the nitrogen rule. That rule says a molecule with an odd number of nitrogen atoms gives a molecular ion with an odd molecular weight. Amines also break apart in a characteristic way during alpha cleavage. Alpha cleavage means the bond next to the nitrogen atom splits. This forms nitrogen-containing cations called iminium ions and alkyl radicals. The molecular...

preparation of amines: alkylation of ammonia and amines

preparation-of-amines-alkylation-of-ammonia-and-amines

Alkylation of Ammonia to Make Amines

To make only primary amines, chemists use specific reaction conditions such as excess ammonia. Ammonia is the most common substrate because it is cheap and readily available. Tertiary alkyl halides are not the best choice for alkylation because they are too hindered. Secondary alkyl halides can react, but they are also less preferred because they tend to undergo elimination reactions.

preparation of 1&deg; amines: azide synthesis

Azide Route to Primary Amines

Azide synthesis is a useful route to primary amines. It helps avoid the polyalkylation that can happen when ammonia is alkylated directly. In that direct reaction, unwanted polyalkylated amines and a quaternary ammonium salt can form. In the azide method, azide ions act as strong nucleophiles. A nucleophile is a species that donates an electron pair in a reaction. They react with unhindered alkyl halides to make alkyl azides. Alkyl azides do not take part in more nucleophilic substitution...

preparation of 1&deg; amines: gabriel synthesis

preparation-of-1-amines-gabriel-synthesis

Gabriel Synthesis for Primary Amines

Gabriel synthesis is a selective way to make primary amines. It avoids direct alkylation, which can create polyalkylated products. For that reason, it is a preferred method when the goal is to make only one alkylated amine product. The reaction starts with phthalimide, which holds nitrogen in a protected form. A strong base such as NaOH or KOH removes a hydrogen from phthalimide and forms an anion. This anion acts as a nucleophile and attacks an alkyl halide, giving N-alkylphthalimide. The...

preparation of amines: reduction of oximes and nitro compounds

preparation-of-amines-reduction-of-oximes-and-nitro-compounds

Routes to Amines from Oximes and Nitro Groups

Oximes and nitro compounds can both be converted into primary amines. Oximes are reduced by catalytic hydrogenation, hydride reduction, or sodium metal reduction. A primary amine is an amine with one carbon group attached to nitrogen, so this step is an important way to build nitrogen-containing molecules. Nitro compounds follow a similar path to primary amines. Aliphatic and aromatic nitro compounds can be reduced by catalytic hydrogenation or by active metals such as Fe, Zn, and Sn in the...

preparation of amines: reduction of amides and nitriles

preparation-of-amines-reduction-of-amides-and-nitriles

Making Amines from Nitriles and Amides

Nitriles and amides can both be turned into amines by reduction. Nitriles are reduced to primary amines with reducing agents such as lithium aluminum hydride or by catalytic hydrogenation. In this reaction, the amino group is added with one extra carbon in the chain. Nitriles are often made first from alkyl halides and sodium cyanide. This step follows an S N 2 mechanism, and primary alkyl halides are the best substrates for preparing nitriles. The nitrile can then be reduced to the primary...

preparation of amines: reductive amination of aldehydes and ketones

preparation-of-amines-reductive-amination-of-aldehydes-and-ketones

Making Amines with Reductive Amination

Reductive amination is a way to make amines from carbonyl compounds and primary amines. A carbonyl compound is a molecule with a carbon-oxygen double bond. The reaction first forms an imine, and then the same mixture is reduced to give a secondary amine. Selective reducing agents make this step work. Sodium cyanoborohydride and sodium triacetoxyborohydride are commonly used because they reduce the imine without reacting too aggressively. Reductive amination with sodium cyanoborohydride is...

preparation of 1&deg; amines: hofmann and curtius rearrangement overview

preparation-of-1-amines-hofmann-and-curtius-rearrangement-overview

Carbon-Loss Routes to Primary Amines

Carbon-loss reactions can turn certain amides into primary amines. The Hofmann rearrangement uses an aqueous base and a halogen to remove the carbonyl group as carbon dioxide and form a primary amine. It often gives aryl and alkyl primary amines in high yield, and the products are free of secondary and tertiary amine contamination. The Curtius rearrangement follows a similar goal but starts from an acyl azide. When heated, the acyl azide converts into a primary amine and releases nitrogen gas...

preparation of 1&deg; amines: hofmann and curtius rearrangement mechanism

preparation-of-1-amines-hofmann-and-curtius-rearrangement-mechanism

Primary Amine Synthesis by Rearrangement

Hofmann and Curtius rearrangements are used to make primary amines from carboxylic acid derivatives. In the Hofmann rearrangement, a primary amide is treated with a base and then halogenated to form an N-haloamide. A second proton loss gives a stable anionic species that rearranges to an isocyanate after an alkyl group migrates from the carbonyl carbon to the nearby nitrogen. The isocyanate then reacts with water to form carbamic acid. Carbamic acid breaks down on its own to release carbon...

amines to amides: acylation of amines

Using Acylation to Modify Amines

Amines can be modified by acylation to form amides. In this reaction, a carboxylic acid derivative such as an acid chloride, ester, or anhydride provides the acyl group. The process uses two equivalents of amine, and each one has a different job. The first amine acts as a nucleophile. It attacks the carbonyl carbon and forms a tetrahedral intermediate. The leaving group then leaves, and the C=O bond is restored. The second amine acts as a Brønsted base, meaning it removes a proton from the...

amines to alkenes: hofmann elimination

Hofmann Elimination and Alkene Formation

Hofmann elimination turns an amine into an alkene through an E2 elimination. The amine is first changed into a good leaving group. A quaternary ammonium salt is formed by treating the amine with an excess of alkyl halide, which gives a halide salt. Next, the halide salt is converted into a hydroxide salt. This hydroxide salt acts as a base during the elimination. With heat, the hydroxide removes a proton from the beta carbon. At the same time, an alkene forms and a neutral amine molecule...

amines to alkenes: cope elimination

Syn Elimination in Cope Reaction

The Cope elimination reaction converts tertiary amines into alkenes. It uses hydrogen peroxide and heat. The process starts with oxidation of the tertiary amine to form an amine oxide. The amine oxide then acts as a base during the elimination step. The reaction follows syn stereochemistry, which means the groups leave from the same side. It also proceeds through a cyclic transition state. The N,N-dimethyl hydroxylamine group is formed as the leaving group. The major product is usually the...

1&deg; amines to diazonium or aryldiazonium salts: diazotization with nano2 overview

1-amines-to-diazonium-or-aryldiazonium-salts-diazotization-with-nano2

Nitrous Acid Reactions with Amines

Nitrous acid reacts with amines in acidic conditions, and the products depend on the type of amine. It is a key nitrogen-containing acid, but it is weaker than nitric acid. Nitrous acid has a pKa of 3.37, so it ionizes in water to form nitrite ion and hydronium ion. Nitrous acid is unstable, so it is made in situ, or formed in the reaction mixture as needed. A sodium nitrite solution is combined with a cold aqueous acid such as hydrochloric acid or sulfuric acid. In acid, the –OH group of...

1&deg; amines to diazonium or aryldiazonium salts: diazotization with nano2 mechanism

Diazotizing Primary Amines with Nitrous Acid

Diazotizing primary amines with nitrous acid forms diazonium salts. The reaction begins with nitrous acid, a weak and unstable acid made in situ from sodium nitrite and cold, dilute hydrochloric acid. In acidic solution, nitrous acid is protonated and loses water to form the nitrosonium ion, which acts as the electrophile. Primary amines react with the nitrosonium ion to start diazotization. The amine serves as the nucleophile and attacks the electrophile. After deprotonation, an N-nitrosamine...

2&deg; amines to n-nitrosamines: reaction with nano2

2-amines-to-n-nitrosamines-reaction-with-nano2

Nitrosamine Formation from Secondary Amines

Secondary amines can form N-nitrosamines when they react with nitrous acid. Nitrous acid is weak and unstable, so it is made in the reaction mixture from sodium nitrite and a strong acid such as hydrochloric acid or sulfuric acid. The reaction is carried out in cold conditions. In acid, nitrous acid becomes protonated. It then loses water and forms the nitrosonium ion, a reactive electrophile. The secondary amine acts as a nucleophile and attacks this ion. That step gives an N-nitrosammonium...

diazonium group substitution with halogens and cyanide: sandmeyer and schiemann reactions

diazonium-group-substitution-with-halogens-cyanide-sandmeyer

Making Aryl Halides from Diazonium Salts

Arenediazonium salts can be used to make substituted aromatic compounds. In these reactions, the diazonium group is replaced by other functional groups such as halides, hydroxyl, and nitrile. The transcript focuses on how this chemistry is used to form aryl chlorides, bromides, fluorides, iodides, and nitriles. When arenediazonium salts react with copper(I) salts of chloride, bromide, or cyanide, they form the corresponding aryl chloride, aryl bromide, or aryl nitrile. These are called...

diazonium group substitution: &ndash;oh and &ndash;h

Arenediazonium Salt Reactions: Phenols and H

Arenediazonium salt reactions show how a diazonium group can be replaced by other functional groups. These reactions begin with diazotization, the formation of an arenediazonium salt from a primary arylamine. The process uses nitrous acid, which is made in situ from sodium nitrite and a strong acid under cold conditions. In acidic solution, nitrous acid breaks down to form nitrosonium ions. A primary arylamine then attacks the nitrosonium ion. This first step leads to an N-nitrosoaminium ion...

aryldiazonium salts to azo dyes: diazo coupling

aryldiazonium-salts-to-azo-dyes-diazo-coupling

Diazo Coupling and Azo Dye Formation

Diazo coupling is the reaction that forms azo dyes from aryldiazonium salts and highly activated aromatic compounds. The product contains an —N=N— azo linkage, and the nitrogen atoms from the diazonium salt remain in the product. Phenols and arylamines are common activated partners for this reaction. The coupling usually takes place at the para position on the aromatic ring. If the para position is already occupied, the reaction shifts to the ortho position instead. The mechanism is an...

amines to sulfonamides: the hinsberg test

Amines and the Hinsberg Reagent Test

The Hinsberg test identifies primary, secondary, and tertiary amines by their reaction with benzenesulfonyl chloride, also called the Hinsberg reagent. It is named after Oscar Hinsberg. The test uses excess aqueous base, and the mixture is then acidified to show different results for each amine type. A primary amine reacts with the Hinsberg reagent to form an N-substituted benzenesulfonamide. The sulfonyl group pulls electron density away and makes the N-H proton acidic. Because of this, base...

key terms and concepts

Learn how aliphatic amines act as Brønsted-Lowry and Lewis bases, and compare their basicity using Kb and conjugate-acid pKa values.

How Aliphatic Amines Act as Bases | JoVE K12

organic chemistry

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How Aliphatic Amines Act as Bases

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