GRUPOS FUNCIONALES
Short Description
grupos funcionales...
Description
UNIDAD 3- GRUPOS FUNCIONALES II
MARCO ANTONIO HERRERA VILLAMIZAR-1098220373 DORA CASTILLO-63254972 LUD MILENA ORTIZ-1098221156 ORTIZ-1098221156 LAURAARID !AIMES LOPEZ-1100503696 LAD PATRICIA PATRICIA CAICEDO CO"OS-1096949223 CO"OS-109 6949223
GRUPO 100416#346
MARIA DEL CARMEN PARRA TUTOR
UNIVERSIDAD NACIONAL A"IERTA A DISTANCIA $UNAD% &UIMICA ORGANICA NOVIEM"RE 2016
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INTRODUCCION
En la química orgánica se puede decir que son muchos los procesos que se generan para que la vida del ser humano sea posible, y en este trabajo veremos cómo los grupos funcionales participan en una forma activa y directa en las reacciones rea cciones químicas que permiten la vida. Los grupos funcionales son cierto grupo de átomos comunes con una misma función y cuya presencia nos revela determinadas y parecidas propiedades en los cuerpos cuerp os que los poseen, en química orgánica un átomo o grupo de átomos unidos de manera característica determinan las propiedades del compuesto en el que estos se presentan. pre sentan. Los grupos funcionales ayudan a determinar los tipos de reacciones químicas en que participan los compuestos, la mayoría de estos grupos forman asociaciones con facilidad con otras moléculas por ejemplo enlaces iónicos y de hidrógenos.
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UNIDAD 3- GRUPOS FUNCIONALES II
ETERES' &UE SON' !on compuestos que resultan de la unión de dos radicales alquílicos o aromáticos a través de un puente de o"ígeno #$#.
N()*+,./. .. /** •
La
nomenclatura
de
los
éteres
seg%n
las re reco come mend ndac aciion ones es
de
&''( &' '( de de
la )*+)*+- actualmente actualmente en vigencia/ especifican que estos compuestos pertenecientes al grupo funcional o"igenado deben nombrarse como .,(.,.+(, es decir, como si fueran sustituyentes. !e debe especificar al grupo funcional éter como de menor prioridad frente a la mayoría de cadenas orgánicas. -ada radical éter será acompa0ado por el sufijo oxi . •
*n comp compue uest stoo senc sencil illo lo,, como como por por ejem ejempl ploo CH3-O-C6H5 seg%n seg%n las las no norm rmas as de la )*+- se llamaría
•
•
)*/(*+,*+( La nomenclatura tradicional o clásica también aceptada por la )*+- y válida para éteres simples/ especifica que se deben nombrar por orden alfabético los sustituyentes o restos alquílicos de la cadena orgánica al lado i1quierdo de la palabra éter. El compuesto anterior se llamaría seg%n las normas antiguas ya en desuso/ de esta manera
•
*+ )*/ /* Los éteres sencillos de cadena alifática o lineal pueden nombrarse a0adiendo al final de la palabra éter el sufijo -,( luego de los prefijos met#, et#, but#, etc. seg%n lo indique el n%mero de carbonos.
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La nomenclatura de los éteres resulta muy sencilla si tenemos en cuenta que para nombrarlos solamente tenemos que identificar los radicales unidos al o"ígeno y luego nombrarlos en orden de complejidad, terminando el nombre con la palabra eter.
REGLAS DE NOMENCLATURA' R*:. 1; Los éteres pueden nombrarse como alco"i derivados de alcanos nomenclatura )*+sustitutiva/. !e toma como cadena principal la de mayor longitud y se nombra el alcó"ido como un sustituyente.
R*:. 2; La nomenclatura funcional )*+-/ nombra los éteres como derivados de dos grupos alquilo, ordenados alfabéticamente, terminando el nombre en la palabra éter.
R*:. 3; Los éteres cíclicos se forman sustituyendo un #-23# por #$# en un ciclo. La numeración comien1a en el o"ígeno y se nombran con el prefijo o"a# seguido del nombre del ciclo.
R*:. 4; Los ésteres proceden de condensar ácidos con alcoholes y se nombran como sáles del ácido del que provienen. La nomenclatura )*+- cambia la terminación #oico del ácido por #oato, terminando con el nombre del grupo alquilo unido al o"ígeno.
R*:. 5; Los esteres son grupos prioritarios frente a aminas, alcoholes, cetonas, aldehídos, nitrilos, amidas y haluros de alcanoilo. Estos grupos se nombran como sustituyentes siendo el éster el grupo funcional.
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R*:. 7; -uando el grupo éster va unido a un ciclo, se nombra el ciclo como cadena principal y se emplea la terminación #carbo"ilato de alquilo para nombrar el éster.
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E!EMPLOS'
Los 5teres se designan mediante el interfijo 6#(#6 entre los radicales R y R 77
-2(8O8-238-2( 9 met(etano
En primer lugar se nombra el radical más peque0o de los dos y a continuación el más largo
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!i los dos radicale radicaless son iguales iguales ent entonc onces es el nombre comien1a comien1a por la locali1a locali1ació ciónn del #$# seguido del prefijo 6o"i#6
-2(#-23#-23#$#-23#-23#-2( 9 (,( o"ipropano
!i están presentes dos grupos #$# se nombra con el prefijo 6dio"a#6
-2(#O#-23#-23#O#-23#-2( 9 dio"aheptano
DITER-BUTIL ÉTER
ISOBUTIL METIL ÉTER
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ÉTER
NOMENCLATURA COMÚN IUPAC
CH3-O-CH3
Dimetiléter
Éter de petróle éter dimet!li"
CH3-CH%-OCH%-CH3
Dietiléter
éter diet!li"
CH3-O-CH%CH3
Met&iet'(
Etil metil éter
ORDEN DE PRIORIDAD
ESTRUCTURA GENERAL
#
R-O-R$
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Los carbonos a los cuales está unido el grupo =OH $>?(% rojos/ están a su ve1 unidos a un solo carbono a1ul/, por tanto son primarios.
SECUNDARIOS.# !on aquellos en los cuales el grupo =OH $>?(% está unido a un carbono secundario, o sea un carbono unido a dos átomos de carbono. Ejemplo
El carbono unido al :$2 rojo/ está enla1ado a dos carbonos a1ules/, por tanto es un carbono secundario.
TERCIARIOS.# !on aquellos en los cuales el grupo =OH $>?(% está unido a un carbono terciario, o sea un carbono unido a tres átomos de carbono.
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Estructuralmente los éteres pueden considerarse derivados del agua o alcoholes, en los que se han reempla1ado uno o dos hidrógenos, respectivamente, por restos carbonados.
Los éteres contienen enlaces sencillos en el átomo de carbono que soporta al grupo funcional, este carbono debe contener hibridación sp(, estructura tetraédrica. La estructura angular de los éteres se e"plica bien asumiendo una hibridación sp( en el o"ígeno, que posee dos pares de electrones no compartidos, no puede establecer enlaces de hidrógeno consigo mismo y sus puntos de ebullición y fusión son muchos más bajos que los alcoholes referibles.
F@RMULA GENERAL; ;#$#;<
LAS PROPIEDADES FISICAS &UIMICAS PROPIEDADES FSICAS; =ebido a que el ángulo del enlace -#o#- no es de &>?@, los momentos dipolares de los dos enlaces -#$ no se anulanA en consecuencia, los éteres presentan un peque0o momento dipolar neto. !us puntos de ebullición son menores que los alcoholes que lo formaron pero son similares a los
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PROPIEDADES &UMICAS; Los éteres tienen muy poca reactividad química, debido a la dificultad que presenta la ruptura del enlace -B$. +or ello, se utili1an mucho como disolventes inertes en reacciones orgánicas. En contacto con el aire sufren una lenta o"idación en la que se forman peró"idos muy inestables y poco volátiles. Estos constituyen un peligro cuando se destila un éter, pues se concentran en el residuo y pueden dar lugar a e"plosiones. Esto se evita guardando el éter con hilo de sodio o a0adiendo una peque0a cantidad de un reductor !$CDe, Li)2C/ antes de la destilación. Los éteres no son reactivos a e"cepción de los epó"idos. o tienen hidrógenos activos como en los casos de los alcoholes o ácidos. +or este motivo son inertes ante metales como el sodio o potasio o litio. ecesitan del calor para descomponerse y ahí si poder reaccionar con algunos metales.
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!us puntos de ebullición son más bajos que los alcoholes a pesar que tiene un peso molecular similar, esto se debe a las débiles fuer1as de atracción entre moléculas.
•
EP@BIDOS
Los E?( son ,()*/( (:+,( formados por un átomo de o"ígeno unido a dos átomos de carbono, que a su ve1 están unidos entre sí mediante un solo *+.,* ,(.*+/*. Los E?( son líquidos a temperatura ambiente, incoloro y soluble en otros compuestos orgánicos como alcoholes, éteres o bencenos.
•
Los epó"idos son éteres cíclicos de tres eslabones, se pueden obtener por reacción de
•
alquenos con pero"iácidos ;-$(2/. Los éteres cíclicos de tres átomos, contando el o"ígeno. +refijo $G/ y cicloalcano.
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E!EMPLOS
•
&,3Epo"iciclohe"ano
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2
$ -
2
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-2 3
-2( -23
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-is 3, ( epo"ipentano.
-2(
-23
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3,3 =ietil ( metiletilo"aciclopropano 2
$ -
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&,3 I"ido de ciclohe"eno epo"iciclohe"an o
PROPIEDADES FSICAS' !on compuestos polares con puntos de ebullición menores que los de los alcoholes y más altos que los éteresA son solubles en agua.
PROPIEDADES &UMICAS'
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;eacción con bases el epó"ido puede reaccionar con un reactivo básico y fuertemente nucleofílico como alcó"ido, fenó"ido, 2(.
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En química orgánica, un tiol es un compuesto que contiene el grupo funcional formado por un átomo de a1ufre y un átomo de hidrógeno #!2/. !iendo el a1ufre análogo de un grupo hidro"ilo #$2/, este grupo funcional es llamado grupo tiol o grupo sulfhidrilo. Hradicionalmente los tioles son denominados mercaptanos.
N()*+,./. /.?,(+. se nombra el .?,. al que va unido el grupo tiol y luesgo se a0ade la palabra 6)*,./.+(6
IUPAC
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•
-2(#-23#-23#!2 propanotiol
•
-23!2#-23#-23#-23#!2 butano#&,C#ditiol
4cido 3,( mercapto#pentanodioico
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-2( : -23 : -2 !2/ # -2( butano 3 tiol. 2$ : -23 : -23 : !2 3 mercaptoetanol
CH3SH metanotiol/
CH3#CH2#SH etanotiol/
CH3#CH2#CH#SH/#CH3 3#butanotiol/
CH3#CH2#CH2#SH &#propanotiol/
CH3#CH#SH/#CH3 3#propanotiol/
CH3#CH2#CH2#CH2#SH &#Putanotiol/
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La propiedad más representativa representativa de los tioles es su olor característico característico similar similar al ajo para el cual el ser human humanoo es muy sensi sensibl blee lle llega ga a detec detecta tarse rse en con concen centr traci acion ones es de &? entre entre &??? millones/. +or esta característica los tioles se a0aden al gas natural inodoro/ y a otros hidrocarburos para poder detectar su presencia. Hemperatura de ebullición debido a que los átomos de a1ufre son menos electronegativos que los del o"ígeno, forman por lo tanto enlaces intermoleculares más débiles que las moléculas que presentan el grupo #$2, resultando en unas un as temperaturas de ebullición más bajas.
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Los sulfuros son combinaciones de compuestos que se encuentran formados por a1ufre, con un estado de o"idación #3, junto a otro elemento químico o también, junto a un radical. 2ay compuestos del a1ufre, de tipo covalente, que también se consideran sulfuros como es el caso del sulfuro de hidrógeno, siendo éste, uno de los compuestos más importantes de éste tipo.
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!ulfuro de dietilo
;egla !e menciona la palabra S!ulfuroT, la proposición SdeT, el nombre del radical primero
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Hetrahidrotiofeno Hiolano
o sulfuro de
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general, se puede decir que, cuanto más noble sea un metal, más estables e insolubles serán los sulfuros que forme. Los sulfuros muy insolubles se podrán formar a cualquier p2 pero para que se formen los
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+ara tres o más grupos aldehídos se emplean el prefijo 6()#6
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AMINAS
REACCIONES DE LAS AMINAS CON JCIDO NITROSO N.NO2
R NH2 .)6+. 1Q
R N N C . ?* ?6.K(+6(
HC
NH2
N
N
C
N.NO2 HC OCH OCH3
OCH OCH3
Esta reacción de dia1otación solo la e"perimentan las aminas primarias y desde el punto de vista sintético solo tienen interés las sales de dia1onio aromáticas ya que las sales de dia1onio alifaticas se descomponen. R NH
R 1
.)+. .)+. 2Q 2 Q
N.NO2 HC
R
N
O
R 1 N-+/((.)+. R 2
R 2 R
N
N
N.NO2
R 1
R
HC
.)6+. .)6+. 3Q 3 Q
N
N
O
R 1 . ?* N-+6/((.)(+6(
Las sales de dia1onio se pueden utili1ar como punto de partida para la obtención de diferentes compuestos reempla1ando el grupo dia1onio por otros grupos funcionales.
HIDR@LISIS; A
N
N
C
NH2
H2SO4 H2O
N
N.NO2 HC
N
A
OH
G
N2
8*+( C
H2SO4 H2O
OH
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REACCI@N DE SANDMEER; En este reacción se reempla1a el grupo dia1onio por los grupos halógeno D, -l, Pr y )/ y el grupos ciano # -/. A
N
N
C0B
C
A
B
N2
G
$B CI "% NH2
N
N
C
N.NO2
"
C0"
HC OCH3
A
OCH OCH3
N
N
OCH3
C0CN
C
NH2
N
N
A
CN
G
C
N.NO2
N2 C
N
C0CN
HC OCH3
OCH OCH3
OCH3
REACCI@N CON H"F4 PARA FORMAR LOS FLUORUROS; A
N
N
C
NH2
H"F4
N
A
N
N2
C
N.NO2 HC
F
H"F4
OCH OC H3
F
OCH OC H3
OCH OC H3
REACCI@N CON NAI PARA FORMAR LOS ODUROS. A NH2
N
N
C
N. N.II
N
A N
C
I
G
N2 I
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REEMPLAZO DEL GRUPO DIAZONIO POR HIDR@GENO; A
N
N
H3PO2
C
NH2
N
N
N.NO2 HC
H
N2
C
H
H"F4
OCH OC H3
A
OCH OC H3
OCH OC H3
REACCI@N DE COPULACI@N. !e produce esta reacción entre una sal de dia1onio y un compuesto aromático activado. A
N
N
C
G
R
A
$R :0( .,/6E.+/*%
N
N
R
,()0*/(
#$o
CH3 H3CO
N
N
CH3
CH
C
H3CO
N
N
CH3 ,()0*/( #$o
CH3
REACCIONES REACCIONES DE CONVERSI@N CONVERSI@N A AMIDAS; AMIDAS; ^a hemos estudiado que las amidas reaccionan con los derivados reactivos de los ácidos carbo"ílicos dando las respectivas amidas.
O R
CH
O
C
C
G
R 1
NH2
R
C
NH
R 1
G
HC
REACCIONES CON ALDEHIDOS CETONAS PARA DAR "ASES DE SCHIFF. R C RP
O
G
H2N
R 1
H
R C
N
R 1
G
RP 7. * ?* ?* S%&i'' S%&i''
H2O
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AMIDAS
REACCI@N DE LAS AMIDAS CON EL JCIDO NITROSO; El ácido nitroso suele emplearse para convertir grupos amino en grupos hidro"ilo. sí, cuando las amidas primarias se tratan con ácido nitroso se forma el ácido orgánico correspondiente y se desprende nitrógeno gaseoso, de acuerdo a la siguiente reacción.
ELIMINACI@N DE HOFMANN
La pérdida de una trialquilamina y un átomo átomo de de hidrógeno hidrógeno en en respecto del nitrógeno a partir de una sal de amonio cuaternario conducen a un alqueno mediante la reacción conocida generalmente como eliminación de 2ofmann
La reacción transcurre normalmente por mecanismo E3 y sigue la preferencia estereoelectrónica para la eliminación anti. -uando e"isten dos tipos diferentes de hidrógenos en respecto al nitrógeno cuaternario, la eliminación conduce generalmente al ()*+o,iio +* #/0*o ,*o1 1012i20i+o. =e hecho, 2ofmann propuso su regla sobre la orientación de la eliminación en &>M& como consecuencia de sus estudios sobre eliminaciones a partir de sales de amonio cuaternario.
La eliminación puede conseguirse tratando una sal de amonio cuaternario con una base fuerte, si bien es más normal utili1ar el hidró"ido de amonio cuaternario como reactivo, con lo que se se requiere base e"terna. El rendimiento en alquenos es generalmente alto. La reacción posee utilidad limitada utilidad limitada para la síntesis síntesis de de alquenos, ya que a menudo es más fácil
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REDUCCI@N DE AMIDAS El hidruro de litio y aluminio convierte a las amidas en aminas. En este caso, la amina tiene igual n%mero de carbonos que la amida.
ELIMINACI@N PIROLTICA
-iertos precursores de alquenos no requieren un reactivo e"terno que promueva la eliminación. Los ésteres y los ó"idos de amina constituyen dos ejemplos de tales sustratos. En esos casos, la calefacción aporta suficiente energía para que el grupo grupo saliente saliente act%e como una base intermolecular. La ruptura térmica de una molécula se conoce como . -uando se calienta un éster (?? # ??@/, generalmente un acetato que contiene un átomo de hidrógeno en su porción alcohólica, se forman un alqueno y un ácido carbo"ílico. !e cree que la reacción transcurre de forma concertada a través de un estado estado de de transición cíclico de seis miembros. Hales reacciones de eliminación pirolítica se designan a menudo como Ei*i,i#%i3, interna. La reacción es estereoespecifica, el mecanismo cíclico intermolecular requiere %o(##)i+#+ 1i de los grupos que se pierden.
MECANISMO' DE LA PIR@LISIS DE STERES;
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método de de síntesis de alquenos muy LA PIR@LISIS DE @BIDOS DE AMINA es un método relacionado con la pirólisis de ésteres. El átomo de o"ígeno de un ó"ido de amina posee una carga negativa formal y puede actuar como una base interna.
cetato de treo#3#deuterio
#Estilbeno #Estilbeno trans/
E
#&,3#difeniletilo
cetato de Eritro#3#deuterio
#&#=euterioestilbeno #&#=euterioestilbeno trans/
E
#&,3#difeniletilo
El mecanismo de la reacción de -ope será estudiado en capítulo dedicado a las amina.
DESHALOGENACI@N
En las reacciones de &,3#eliminación más comunes, el protón es uno de los dos grupos que se pierde. -uando en un sustrato están presentes pres entes dos átomos de halógeno, la reacción reacc ión con base puede conducir a una doble deshidrohalogenación. desh idrohalogenación. El ciclohe"adieno se prepara de esta es ta manera a
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deshidrohalogenación. En esta reacción E3, la pérdida de los dos átomos de halógeno está sincroni1ada con la formación del doble enlace.
El ion yoduro y el cinc metálico son los reactivos más com%nmente utili1ados para la deshalogenación.
DESHIDROGENACI@N CATALTICA;
La eliminación de hidrógeno a partir de un hidrocarburo es un importante proceso industrial. La deshidrogenación se lleva a cabo a temperaturas elevadas sobre catali1adores compuestos normalmente de ó"idos metálicos. La tecnología de este tipo de procesos de procesos catalíticos continuos es muy sofisticada. Los factores críticos para controlar los rendimientos y los productos secundarios son la temperatura temperatura,, la composición del catali1ador y la velocidad de flujo a través del reactor. El vapor de agua y el nitrógeno son dos gases gases portadores portadores utili1ados para arrastrar los productos de partida y los productos de reacción entre entr e ellos hidrógeno/ a través del catali1ador. La naturale1a naturale1a y y concentración de estos gases 6inertes6 son a menudo variables importantes de la reacción.
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4; D*, . *. ?* .(./(( ?* /( ,( ),( **,/(,,( * *)/* . ?*+/,.,+ ?* ,.?. :( +,(+. $/** E?( T(* S( A?*>?( C*/(+. J,?( C.(,( ,()*/( N/(:*+.?(%;
PRUE"AS FSICAS La aplicación de pruebas de clasificación físicas son la determinación de
PUNTO DE E"ULLICI@N D*/*)+.,+ ?* +/( ?* *,+ ( . /,+,. ?* ),( *,.. !i el compuesto problema es un líquido, se determina su punto de ebullición mediante el siguiente procedimiento &. La muestra se pone en un tubo peque0o C " ?.M cm/ que contiene un tubo capilar sellado e invertido. 3. !e sujeta el tubo al termómetro con una ruedita de hule cortada de una manguera. (. El termómetro se pone, sujetándolo con una pin1a, en un vaso de precipitados de &? mL conteniendo aceite mineral. La muestra debe quedar sumergida en el aceite pero éste no debe tocar la liga. C. !e calienta lentamente con parrilla. M. El punto de ebullición es la temperatura a la que sale un rosario de burbujas de aire del capilar o, mejor a%n, la temperatura a la que salen las %ltimas burbujas y entra líquido al capilar cuando se suspende el calentamiento.
PUNTO DE FUSI@N
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(. -ontrole -ontrole la velocidad velocidad de de calentamient calentamientoo con la perill perilla. a. En la posición posición (?, (?, la temperatura se llegará a elevar muy lentamente al final/ hasta cerca de 3??@ -. !i el punto de fusión de la muestra es desconocido, desconoc ido, caliente más rápidamente para obtener un punto de fusión apro"imado y repita la determinación con una muestra nueva a la velocidad adecuada. La velocidad de calentamiento cercana al punto de fusión no debe ser mayor de 3@Zmin. C. l acabar acabar de fundir fundir la muestra muestra apague apague el aparato aparato y verifiqu verifiquee que la temperat temperatura ura no suba más de dos grados. !i el incremento es mayor, el punto de fusión determinado no es confiable, ya que la transferencia de calor a través del vidrio es lenta, por lo que la temperatura de la muestra al fundir no corresponde con la lectura del termómetro. M. ;egist ;egistre re los rangos rangos de fusió fusiónn en la hoja hoja de resulta resultados. dos.
COMPORTAMIENTO DE SOLU"ILIDAD L. ?*/*)+.,+ ?* . ,..,/*/,. ?* (?.? de un compuesto orgánico puede dar información valiosa respecto a su composición estructural. Esta información es especialmente %til si se correlaciona con los datos espectroscópicos del compuesto. !e han propuesto varios esquemas para clasificar a una sustancia de acuerdo a los grupos funcionales que contiene, y de acuerdo a la solubilidad en varios solventes. *na versión simplificada se discute a continuación. o hay una división definitiva para determinar si un compuesto es soluble o insoluble en un compuesto orgánico. !ugerimos que un compuesto sea clasificado como soluble si su solubilidad es mayor de &M mgZM?? `L de solvente. Las determinaciones de solubilidad se deben llevar a cabo a temperatura ambiente en tubos de ensaye peque0os. +ara hacer las pruebas, coloque &M mg de muestra en un tubo de ensaye y a0ada, con una pipeta beral, ?.M mL del solvente que se está probando, dividiéndolo en tres porciones. porc iones. =espués de
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3. !ólo si el compuesto es soluble en agua, determine la solubilidad en éter etílico. !i también es soluble en este solvente, la sustancia puede ser un alcohol, cetona, aldehído, éster, amida o nitrilo menor de cinco carbonos, o mayor, si es polifuncional. !i el compuesto orgánico problema es soluble en agua, pero insoluble en éter, probablemente se tratará de un a1%car, la sal de un ácido carbo"ílico o sulfónico, la sal de una amina o de un aminoácido. (. !i la sustancia es insoluble en agua, pruebe su solubilidad en una solución al M] de a$2. !i es soluble, determine la solubilidad del compuesto en una solución al M] de a2-$(. El uso de bicarbonato de sodio ayuda a distinguir entre ácidos carbo"ílicos más fuertes, solubles/ y fenoles más débiles, insolubles/.
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M. +ruebe los compuestos insolubles en 2-l al M] con 23!$C concentrado.
PRECAUCI@N' E/. *. * ?**+ >.,* ,(+ **,. ,?.?(; !i son solubles en sulf%rico, puede diferenciarse a%n más usando 2(+$C al >M] como se muestra en el esquema. $bserve que puede no ser necesario probar la solubilidad en cada uno de los solventes para clasificar una sustancia. !ólo lleve a cabo las pruebas necesarias que permitan la clasificación. 2aga sus observaciones con cuidado y siga el orden lógico indicado. +ara observar las pruebas de solubilidad en compuestos testigo, lleve a cabo el procedimiento con tolueno, he"ano, alcohol isopropílico, cloruro de t#butilo, 3#penteno, metiletilcetona, ácido ben1oico y trietilamina. ;egistre sus observaciones en la tabla de resultados.
RESULTADO DE LA IGNICI@N L. *. ?* :+,+ se lleva a cabo colocando mg de muestra en la punta de una espátula y calentándolos en un mechero. o coloque la muestra directamente en la flama, caliente la espátula como a un centímetro y acerque lentamente a la flama. Fientras se quema la muestra, debe hacer las siguientes observaciones 2 C.'l.ier 4./ió( e5ide("i' de /.0lim'"ió(6 l .e d' .(' ide' 'pr&im'd' del p.(t de 4./ió( pr l' temper't.r' (e"e/'ri' p'r' "'./'rl'
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+ara observar este tipo de comportamiento haga las siguientes pruebas &. +ara probar probar la naturale1a naturale1a de de los hidrocarbur hidrocarburos os alifáticos alifáticos y aromáticos/, aromáticos/, queme queme una peque0a muestra de tolueno aromático/ y he"ano he "ano alifático/. ;egistre sus observaciones en la tabla de resultados. 3. +ara probar probar la naturale1a naturale1a de de alcoholes, alcoholes, a1%cares a1%cares y compuesto compuestoss que dejan dejan residuos, residuos, queme por separado peque0as muestras de metanol o etanol, glucosa, tartrato de sodio, ferroceno residuo de fierro/, he"ametildisilo"ano residuo de !i$3/. ;egistre sus observaciones en la tabla de resultados. (. 2aga la prueba de ignició igniciónn con sus compuest compuestos os problema. problema. ;egistre ;egistre sus sus observaciones observaciones
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c/ +ara observar la prueba de Pelstein positiva, queme una peque0a muestra testigo de cloruro de tbutilo o de bromobenceno como se indicó. ;egistre sus observaciones en la tabla de resultados.
COLOR OLOR ^a que la mayoría de los compuestos orgánicos no tienen color, esta característica puede ser s er un dato importante para la identificación de la muestra. !in embargo, se debe interpretar con precaución, pues la presencia de peque0as pe que0as cantidades de impure1as puede colorear una muestra. +or ejemplo, la anilina recién destilada es incolora, pero después de un tiempo una peque0a fracción se o"ida y colorea a la muestra entera de un color café#roji1o que, con mayor envejecimiento, puede llegar hasta negro. Hambién el olor de la muestra puede dar algunos indicios sobre su naturale1a.
ASPECTO DE LA SUSTANCIA PRO"LEMA PRUE"AS &UMICAS
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TIOLES MERCAPTIDA DE PLOMO
0adir tiol a una solución saturada de acetato de plomo en etanolA precipitan mercaptidas de plomo amarillas. !i se forma un precipitado amarillo, la prueba es positiva, es decir, hay presencia de tioles.
ALDEHDOS CETONAS P*. ,(+ 24-?+/(*+>?.K+. $,.(+(%; =isolver cinco gotas de la muestra en 3.? mL de etanol, posteriormente anadir 3.? mL de reactivo de 3,C#dinitrofenilhidra1ina.
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N(/.' Esta prueba se usa generalmente para identificar a1%cares reductores. $tros compuestos como hidra1inas y paminofenol también hacen positiva la prueba.
PRUE"A DEL "ISULFITO DE SODIO $ALDEHDOS CETONAS METIL CETONAS ALIFJTICAS% 0ada apro"imadamente &.? mL de reactivo de bisulfito ( a M gotas/, por cada ?.( mL de muestra problema.
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COMPUESTOS NITROGENADOS 1; AMINAS Ensayo de 2insberg !uspender la sospechada amina en una disolución de hidró"ido sódico. l a0adir cloruro de benceno sulfonilo •
•
•
Las aminas primarias forman sulfonamidas que permanecen disueltas en la disolución fuertemente alcalina. l acidular, precipita la sulfonoamida sólida blanca. Las aminas secundarias forman sulfonoamidas que no quedan en la disolución sino que precipitan directamente como sólidos blancos a partir de la me1cla reaccionante rea ccionante alcalina, insolubles en agua, alcalís y ácidos diluidos. Las aminas terciarias no reaccionan, permanecen sin disolver y se disuelven al acidular
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5; CO CONC NCLU LUSI@ SI@N N GR GRUP UPA AL
En este trabajo que acabamos de concluir, adquirimos los conocimientos y recopilamos la información necesaria dando a conocer grupos funcionales, su uso, la presencia de ellos en nuestro entorno, reglas que se aplican para su nomenclatura, nombre iupac, las estructura, algunos ejemplos de estos grupos y las características físico químicas, también los procesos y cambio a los que son sometidos por la e"perimentación en el laboratorio, como la halogenacion,
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REFERENCIAS "I"LIOGRAFICAS
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Her(7(de86 L H6 *lre/6 R R6 9 Arr'8l'6 D * D M :%;; ?2 @ 2
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