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ISOMERISM
The acorance of more than one compounds of same molecular formula is calledisomerism and such compounds are known as isomers.
eg CH3 – O – CH3 and CH3 – CH2 – OH
(C2H6O) O
CH3CH2 – CHO and CH3 – C – CH3
(C3H6O)
ince isomers are different compounds the! ha"e different ph!sical and chemical
properties. tructural tereo # pace
Or constituitional configratinal # conformational
Chain
$ositional ⇒ %eometrical
&ing chain
'unctional
etamers ⇒ Optical
Tantomers
→ tructural "ersus stereo isom. somers differing in connecti"it! of atom are calledstructral isomers.
eg CH3 – CH – CH3 and CH3 – CH2 – CH2 – OHOH
CH3 – O – CH3 and CH3 – CH2 – OH
somers ha"e same connecti"it! of atom *ut different spetial arrangement of atom or
group a*out a centre or *ond are called stereo isomers.
Cl
CH2 – CH2 and CH2 – CH2
CH3 CH3 CH3 H
C + C and C + C etc.H H H CH3
Chain isomers, str. iso. -iffering in chains of C – atom.
eg CH3 – CH2 – CH2 – CH2 – CH3 and CH3 – CH – CH2 – CH3
CH3
Positional isomers: differing in position of an atom # group.
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CH3 – CH – CH3 and CH3 – CH2 – CH2
OH OH
/ctuall! onl! those
tr. will chain isomers in which parants chain are different otherwise positional isomers.
eg () CH3 – CH2 – CH2 – CH2 – CH2 − CH2 – CH3
(2) CH3 – CH2 – CH – CH2 – CH2 – CH3
CH3
(3) CH3 – CH – CH2 – CH2 – CH2 – CH3
CH3
(0) CH3 – CH – CH – CH2 – CH3
CH3 CH3
() s the chain isomer of all (2) is chain isomer of (i) and (i") *ut positional isomer of
(iii).
Ring – chain isomers: f one isomer has ring str. while the other has open chain str. then the!
CH3 – CH + CH2 or1
CH2 + CH – OH or1
CH3 and1 CH – CH2 – CH3
CH3 oth howe"er can ha"e ring *ut then the sie of
rings is should *e different.
Functional : 'unctional group differ.
eg O O
CH3 – C and H – C – OCH3
OH
CH3 CH2 OH CH3 – C – CH3
O
CH3 – CH2 CHO CH3 – C – CH3
*** Metamers : functional group not mono"alant. f no. of C – atom differ either side at
the functional group.
eg CH3 – CH2 – O – CH2 – CH3 and CH3 – O – CH2 – CH2 – CH3
444 Tautomers, → &eadil! inter con"erti*le structural isomers.
2
CH3
OH
CH3
OH
CH3
OH
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O O
CH3 – C and CH3 – CH2 – C
CH3 . H
O OHCH3 – C CH2 + C
CH3 CH3
O .
CH2 – C
H CH3
.
and one not are intercon"erti*le therefore and are tautomers of each other.
→ Tautomers are different compels therefore the! ha"e different ph!sical and chemical properties. 5"en then it is "er! difficult to separate then. This is *ecause tautomers eist
in a state of d!namic e7uilm. Howe"er separation is possi*le speciall! when all tautomersare in good proportions and emplo!ed techni7ue does not allow enter con"ersion.
O OH
CH3 – C CH2 + C
889 CH3 9 CH3
∴ con:t *e separate
f we take1O O OH O
CH3 – C – CH2 – C – CH3 CH3 – C + CH – C – CH3
;9 H – release.. 829
∴ can *e separate.
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O
4 $H – C – H
O
4 $H – C – $HCH3 – CH + >H2 CH2 + CH – >H2
O
CH3 – CH2 – CH2 – C – H
444 $ercentage enol content, → $ercentage enol content depend upon
(a) ta*lit! of enol ? $5C ∝ sta* of enol
(*) /cidit! of enolia*le H ? greater is the acidit! higher will *e 5C.
(c) ol"ent (d) Temparature,
Stability factor: O OH
CH3 – C – CH3 CH2 + C – CH3
C + O C + O
C – H O – H
4 ( 5 C + O @ 5 C – H) A (5C + C1 5 O – H) therefore in this case ketoform is moresta*le than enol form.
O O OH O
CH3 C CH2 C CH3 CH3 C CH C CH3
/cet!l acetone,
ta*iliation energ! C + O C + C 1 OH H – *ond etended resonance.
C – H
n case of acet!l acetone enol form is more sta*le then ketoform.
O O OCH3 C CH3 CH3 C CH2 C CH3
.
∴ enol content A .
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. $H C CH2 C $H C + CH – C – CH3
O O O O
. CH3 O C CH2 C CH3 − C – CH3 A − C – OCH3
O O
B. CH3O – C – CH2 – C – OCH3
enol content ? A A A B.
(2)
. .
enol content A .
(3) CH3 CH3
C + O C + O C + O
H CH3 CH3
.
enol content A A .
(0)
enol content A A
5noliation? enoliation can *e either acid # *one catal!sed
/cid catal!sed process?
O H@ OH OH
CH3 C CH3 CH2 C CH3 CH2 + C – CH3 – H
H
H@ protonates car*o!lic O: and thus clea"age C + O and C – H *ond *ecomes "er!
eas!.
ase catal!sed process.
O OH− O
CH2 C CH3 CH2 – C CH3
↓
O H – OH ↓
CH2 + C – CH3
O
D
OO
O OOH
δ−δ−
δ−
δ−
O O O
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CH2 + C CH3 @ OH
O O O
CH3 C CH2 – CH3 CH3 C CH2 C CH3
H@ OH H@ OH−
OH OH O
OH CH2 + C CH2 – CH3 CH3 – C + CH – C CH3
CH3 – C CH – CH3 .
is more sta*le than . *ecame more su*stituted (+) is more sta*le.
CH3
C + CH2 A CH3 – C + CH2
CH3
n acid catal!sed process sta*ilit! of enol is dri"ing force *ut in *ase catal!sed pro"es
acidit! of enolia*le – H is the dri"ing force.
444 sotope echange
& – OH → O D2 & – O-.
CH3COOH → O D2 CH3COO-.
echanism , − & O HOδ@
& Hδ−
Oδ−
-δ@ – Oδ−
-δ@
&
O @H
- O
-
T.. O#H *ond can *e echange *ut not C – H *ecause in C – H *ond H is not protic.
O O
$H C CH3 → )(2 excessO D $H – C C-3
$ropose mechanism E
O O – H O – -
6
OH-2O
-
O
O
H
-
&
-
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$H C CH3 $H – C + CH2 → O D2 $H – C CH2
O – - O – H O
$H – C CH ← O D2 $H – C CH $H – C CH2
- - -
O O – H
$H – C C-2 $H – C C-2 → O D2
H
O O – -
$H – C C-3 $H – C C-2
⇒ Effect of temperature on enol content:
O O OH O
CH3 C CH2 C CH3 CH3 C CH C CH3
2DoC 9
3DoC ! 9
0DoC 9
A ! A . /t high temperature H – *ond *reaks therefore enol content decreases.
⇒ Solvent effect on enol content:
O O OH O
CH3 C CH2 C CH3 CH3 C CH – C – CH3 %as phase 9
in H2O ! 9 F A !G
n water keto form makes H – *ond with water molecules1 therefore need to go in enol
form decreases.
O OH
CH3 C CH3 CH2 + C CH3
3DoC 9
Do
C ! 9 F A !G⇒ onfigurational verses conformational isomers:
f stereo isomers cannot *e inter con"erted without clea"ing an! *ond then the! are calledconfugrational isomers on the other *and if this intercon"ersion is possi*le without
clea"ing an! *ond then the! are called conformational isomers.
Cl
CH2 – CH2 CH2 – CH2 conform.
I
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r Cl r
CH3 CH3
C + C configraH H
/ *ond has to *e clea"ed
CH3 H
C + C
CH3 H
⇒ !eometrical isomers:
Configrational isomerism arising due to different spetial arrangement of atoms or groups
a*out a *ond along which rotation is restricted is called geometrical isomerism these *onds on *e multiple *ond or single *onds of ring.
"# %eometrical isomers is possi*le along which of the following multiple *onds.
(a) C + C (*) C ≡ C (c) C + > (d) C + O (e) > + >
>ote – that two isomers can *e geometrical isomers onl! if the! differ in spetial distance
*etween the groups.
"# %eometrical isomers occur with , −
(a) /lkene (*) /lk!ne (c) imines (d) ketones (e) h!dragone.
(i) case of C + C *onds, − geometrical isomers a*out C + C *ond will *e possi*le onl! if each C: of the dou*le *onds *ears two different groups.
a l a a
C + C C + C
* m * *
a *
C + C
a *
CH3 – CH + CH – CH2 – CH3 CH3CH2 – CH + CH – CH2 – CH2 – CH3
CH2 + CH – CH + CH2
CH2 + CH – CH + CH – CH3
CH2 – CH + CH – CH + CH – CH3
ase of $ bon% in ring :
;
H
H
•
•
H2
H2
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>o geometrical isomers *ecause trans configuration is not possi*le. Howe"er it *ecomes
possi*le from ; – mem*ered ring onwards.CH3 – CH + C + CH – CH3
CH3 – CH + C + C + CH – CH3 CH3 CH3
C + C + C
H H
umelens
(i) 5"en no. of C + C *ond
→ geometrical isomers isomerism(ii) Odd no. of C + C *ond
→ geometrical isomers occurs if each and *ears two different JJJJJJJJJJJJJJJJJJ.→ Ca*in – ngold – prelog se7uence rule, − () The group ha"ing first atom of high atomic no (atJwt) will *e of higher priorit!.
eg − CH3 1 − OH 1 − >H2 1 − Cl1 − HC O > Cl H
− Cl A OH A − >H2 A − CH3 A −H.(2) f frist atom same then appl! a*o"e rule on second atoms
CH3
eg −CH31 − CH2 – CH31 − CH 1 − CH2 – rCH3
− CCl3 1 − CHr 2 respecti"el! 3H 2H1 C ? H1 2C? 2H? r ? 3Cl ? H1 2r H C r Cl ?r A Cl A Cl A C A H
CH3
K − CHr 2 A − CH2r A − CCl3 A A − CH2 – CH3 A CH3 CH3 O
eg CHO ⇒ − C – O
− C + O H C
H
⇒ − CHO ? − COOH ? − CH2OH ? − C ≡ > ? − CH2 – >H2
O1 O1 O ⇓ H H H > C H H H
O − C – >
− C – O C > C
OH O1O1O
∴ COOH A CHO A CH2OH A C> A − CH2 >H2
CH3
"# − CH + CH2 1 − C ≡ CH 1 C – CH3 1 − $H ?
8
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CH3
⇒ CisJtrans >omencl.
This method is applied when *oth atom of C + C contain at least one identical group.
CH3 – C + C – CH3 CH3 – C + C – C2 HD
H H H H
f identical group lie on the same side of the C + C *ond then it is called cisJisomer
otherwise trans isomer.
CH3 – CH + CH – C2 HD → 2 – pentene.
CH3 C2 HD CH3 H
C + C C + C
H H H C2 HD
Cis Trans
r Cl r r
C + C C + C
Cl r Cl Cl
Trans Cis
r
C + C sol"ed *! following method.
Cl '
5#L – nomenclature, Top priorit! groups are on the same side then it is called L – isomer
otherwise 5 isomer
r r '
C + C C + C
Cl ' Cl
(L) (5)
This method can *e appl! in all cases of geometrical isomerism.
CH3 CH3 CH3 H
C + C C + C
H H H CH3
Cis#2 Trans#5
H
C + C ⇒ C + C
Cl Cl Cl
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>um*er of geometrical isomers + 2n where n + the no. of C + C *onds. Howe"er if no. of
C + C *ond is e7ual to then no. of geometrical isomers is alwa!s two1 *ut if no. of C +C *ond is more than then no. of geo – isomer ma! *e 2n or M 2n.
i.e C + C + ? %. + 2
C + C A 2 ? %. ≤ 2n
t will *e 2n when num*ering of $.C is not possi*le from either side. On the other hand it
will *e less than 2n1 when num*ering $.C possi*le from either side.
(i) CH3 – CH + CH – CH3 (geo.)
(ii) Cis (iii) trans. + 2.
Cis1 trans Cis1 trans.
↑ ↑
(ii) CH3 – CH + CH – CH + CH – CH 2 – CH2 >o. of geom – isom + (0) sincenum*ering is possi*le onl! from left.
() Cis – Cis () Cis – trans () trans – Cis B ↑ − ↑.
(i) H H (ii) CH3 H
C + C C2HD C + C H
C2HD C + C H C + C
H H H C2HD
Cis – Cis Trans – trans.
H H CH3 H
C + C H C + C C2HD
C2HD C + C H C + C
H C2HD H H
Cis – trans Trans – Cis.
(ii) CH3 – CH + CH – CH + CH – CH3
H H CH3 H
C + C CH3 C + C H
CH3 C + C Cis – Cis H C + C . TransJtrans
H H H CH3
H H CH3 H
C + C H C + C CH3
CH3 C + C . CisJtrans H C + C B TransJCis.
H CH3 H H
and B are identical
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∴ >o. of geo.Jisomer + 3.
(iii) CH3 – CH + CH – CH – CH + CH – CH3
→ C C C
→ T T T
a) C – C – C C – C – C
*) C – C – T T – C – C
c) C – T – C C – T – C
d) C – T – T T – T – C
e) T – C – C C – C – T
f) T – C – T T – C – T
g) T – C – T C – T – T
h) T – T – T T – T – T
∴ >o. of geom – isomers + 6
yclic cases: %eometrical isom. also occurs in rings. ince rotation a*out C – C single *ond of
ring is also restricted.
CH2 – CH – CH – CH3
C2HD C2HD
Howe"er it will *e possi*le onl! if ring *ears at least two groups same or different at
different position.
() (2)
(3) (0) (D)
(6) (I) (;)
(8) ()
(3) or1 ? or1
2
CH
CH3
CH3
CH3 CH3
CH3
CH3
CH3
r
CH3
H
H r
CH3
r
r
r
CH3
CH3
r
r
Cl r
r
r
r
CH3
O
CH3
CH3
CH3
r
H
H
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(D)
oth are identical1 therefore1 no geometrical isomerism in this case.
(I) or1
d + d2
∴ >ote geo – isomers1 since spetial distance does not charge.
Cis Trans.
Cis Trans
***"# ∴ >o. of geo – isomers + 0.
(i) CH3 CH3 OH
C + > ⇒ C + >
C2HD (L) OH C2HD
(Oime)
!neth!l or antimeth!l K %eomJisomers are possi*le.
4 Choose w.r.t hea"ier group.
(ii) CH3 – > + > – CH3 CH3 > + >
↑ ↑ > + > CH3 CH3
CH3
Trans#/nti (∈) Cis s!n(2)
⇒ ntercon"ersion of geometrical isomers , −
3
CH3
CH3
CH3
H
CH3
CH3
CH3
H
CH3 CH3
O(sp2)
HH
HCH3
O
O
p3
H
H
H
H
H H H
H
r
r
r
r
r r r
r
(C#T) r
CH + CH – CH3(C#T)
sp2 sp2
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ince rotation a*out C + C is restricted. ntercon"ersion of geometrical isomers is
possi*le onl! if π − *ond is cleare. This can *e done either *! heating or with the help of catal!st. Nhich can *e an acid or *ase or radicals.
CH3 CH3 / + homo or1 heterol!sis.
(i) (cis) C + C
H H
CH3 CH3 H CH3
C − C C + C
H H CH3 H
CH3 CH3 CH3 CH3
(ii) C + C C + CH H H o H
CH3 CH3 CH3 CH3
C − C C − C – H
H H H
H CH3 CH3
C − C C − C – H
CH3 H H H CH3
H CH3 H CH3
C − C @ H@ C − C @ o
CH3 H CH3 CH3
H.N $ropose mechanism for *ase catah!sed rean
→ ta*ilit! of geometrical isomers, −
That geometrical isomers will *e more sta*le in which steric – repulsion is less.
CH3 H CH3 CH3
C C
H CH3 H H
Trans Cis
CH3 CH3
0
• •
H@
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H C
H C2HD C + C CH3
C + C CH3 C2HD C2HD
C2HD C
CH3 CH3 Trans M Cis
→ elting point of geometrical isomers
'2()1 Cl2()1 r 2()1 2 (δ)
i.e intermolecular force of attraction
2 A r 2 A Cl2 A '2
$olarisation of e− clad.
eg C + O
C OH
CH3 – CH2 – CH2 – CH2 – CH3
CH3 – CH2 – CH2 – CH2 – CH3 n pentane ntermolecular "ander walls force of alterationis more in n – pantane that in new pentane
ntermolecular "ander walls force of alteration (for single molecule) is more in neoJpent.
Than in n – pertane. Therefore newJpentane is more sta*le than nJpentane.
CH3 CH3
CH3 – C – CH3 CH3 – C – CH3 >eoJpentane
CH3 CH3
CH3 CH3 CH3 H
C + C C + C
H H H CH3
(Cis) ⇓ ⇓ (Trans)
CH3 CH3 CH3 – CH + CH – CH3
CH + CH map
map
D
δ@
δ@δ−
δ−
δ@ δ−
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intermolecular "ander walls force of attraction is more in trans isomer than in cis.
Therefore map of trans 2 – *utane is more straight than that of cis.
Solubility
CH3 – OH
OH H
H
CH0. O
H
olu*ilit! of cis – isomer is more then that of trans – isomer.
Optical isomerism:
$lane – polarised light, Ordinar! light "i*rates in all dir n1 when pass to a nicol prism
(ade up of CalO3)1 it *egins to "i*rate in onl! one dir n
. Then it is called plane polariedlight.
>o effect or. Compd (inacti"e) /cti"e(opticall!)
Optical isomerism is the isomerism which deals with opticall! alti"e compds. Howe"er either all optical isomers will *e opticall! acti"e or some ma! *e acti"e and some
inacti"e.
/s!mmetric centre # chiral centre
The C – atom *earing for different group is called as!mmetric or chiral centre.
CH3 – CH – CH2 – CH3 CH3 – CH2 – CH – CH2 – CH2 – CH3
r 4 C + . r
6
H2OH2O
OH2
H2OH2O
H2O
OH2
>a@
OH2
Cl
OH2
H2OH2OH2O
H2O
H2O
>icol prism
ample tesle containing
Org. compd.
&ight ward
detro. lea"o.
left ward
Compd
OptJacti"e Opt –inacti"e
-etrorotator!
d or (@)
ea"orotator!
l or (−)
∗ ∗
∗∗
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CH3 – CH – CH – CH3 CH3 – CH – CH – CH3
r r r Cl
4 C + 2 (imilar) 4 C + 2 (dissimilar)
r
CH3 CH H C + C C + C
H H H CH3
cis trans 4 C + .
4 C + . 4 C + O 4 C + O 4 C + O 4 C + .
4 C + 2 (similar) (C4 + 2) C4 + O.
→ $resentation of as!mmetric C – centre and configuration.
(i) 'ischer pro=ection formula, −
COOH COOH CH3
CH3 – CH – C2HD CH3 C H ≡ CH3 H ⇒ HOOC C2HD
COOH C2HD C2HD H
to 3 "ia – 2 H CH3
Clock wise – & C2HD COOH H C2HD
/nti clock – . CH3 COOH
>ote, That this str. ha"ing same configuration on all respecti"e ass!metric centre will *eidentical.
CH3 CH3
H OH OH H
H OH H OH
C2HD . C2HD
H H
I
∗
OH OH OHOH
O
∗
OH
O
CH3
∗∗
CH3 ∗
∗
CH3
CH3 CH
3
CH3
2
3
&
&
&
&
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OH OH CH3 H
OH C2HD C2HD OH
H B OH
and are identical
and are identical and are identical
and are identical
and B are identical
and B are identical
CH3 CH3
(i) H OH (ii) HO H
H OH H OH
C2HD C2HD
CH3 Cl CH3 Cl
H OH H OH HO H H OH
Cl C2HD Cl C2HD
OH OH H OH
Cl CH3 C2HD Cl Cl C2HD C2HD Cl
H H OH H
H H CH3
() OH CH3 HO CH3 Cl H
OH C2HD Cl OH
H
H Cl
CH3 OH ⇒ HO CH3
Cl HCOOH COOCH3
2 H OH H OH
H OH H OH
COOCH3 COOH
OH
;
&
&
&
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COOH OH − CH
H OH Cl COOH ? COOCH3
Cl H O
C O
OH C
oth are non – identical.
In 'e%ge formula:
CH3 – CH – COOH
OH
H CH3 COOH OH CH3 C2HD
C ⇒ ?
OH COOH CH3 H OH H
In sa'horse formula:
This formula is written it molecule has two#more ass!m. centre
CH3 – CH – CH – C2HD
OH OH
CH3 H OH
H
OH C2HD
H C2HD
Cl OH "ertical *ond ⇒ OH Cl
C2HD H
CH3 C2HD CH3
CH3 OH ? OH CH3 Cl
H H H OH
H OH CH3 Cl
Cl OH
CH3 H
8
CH
OC
∗
∗ ∗
s&
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OH C2HD H
and &
H CH3 OH
Plane of Symmetry:
f molecule can *e di"ided with two e7ual portions – One portion *eing the mirror image
of the other portion then it is said to ha"e plane of s!mmetr!.
/ molecule without plane of s!mmetr! is called diss!mmetric. >ote that all the
s!mmetric molecules are opticall! inacti"e.
CH3 ∴ Has plane of s!mmetr!
H OH ∴ opticall! inacti"e.
H OHCH3
CH3 → >a plane of s!mmetr!
H OH ∴ olecule is diss!mmetric and thus opticall! acti"e.
HO H
CH3
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)onsuper impossible Super impossible
→ /ll diss!mmetric molecules ha"e → /ll s!mmetric molecules ha"e super
nonJsuper impossi*le mirror image impossi*le mirror image
→ There structures will *e non – super impossi*le mirror image of each other in which
configurations are opposite on all respecti"e as!mmetric centres.CH3 CH3 CH3 OH
H OH HO H H OH H CH3
H r r H H r r H
CH3 CH3 CH3 CH3
-iss!mmetric
∴ P one nonJsuper impossi*le mirror ∴ oth nonJsuper impossi*le mirror
image of each other image of each other.
→ Condition for optical isomers, −
(i) $resence of s!mmetric centres, −
f a molecule at s!mmetric centre then optical isomerism certainl! occurs. Howe"er there
are molecules which do not ha"e an! as!mmetric centres *ut ehi*it optical isomerism.
(ii) presence of diss!mmetr!, −
olecule with diss!mmetr! are alwa!s opticall! acti"e therefore ha"ing diss!mmetr! is
the compulsor! condition to ehi*it optical isomerism
>o. of optical isomerism + 2n
Nhere n + no. of ass!m. centre
Howe"er in some cases no. of optical isomerism will *e less than 2 n. These cases will *e
the cases of similar as!mmetric centres.
∴ C4 + – >o. of optical isomer + 21
dissimilar C4 + 2 similar
>o. of isomer + 0 >o. of isom + 3
CH3 – CH – COOH
OH
COOH COOH
H OH OH H
CH3 CH3
oth are acti"e and called enantiomers.
CH3 – CH – CH – CH3
OH r
2
&
&
∗
∗ ∗
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CH3 CH3
H OH HO H / pair of enantiomers.
H r r H
I CH3 II CH3
CH3 CH3 HO H H OH / pair of enantiomers.
H r r H
III CH3 I+ CH3
>o. of optical isomers + 0.
is diastereomers of – and B.
is diastereomers of and .
CH3 – CH – CH – CH3
r r
CH3 CH3
H r r H and → identical called
H r r H mesomer.
CH3 CH3
CH3 CH3
r H H r >O. of isomer + 3 *ecause
H r r H and are identical
CH3 CH3
oth are pair of enantiomers.
⇒ 'eatures of enantiomers, −
(i) Those two str. are enantiomers of each other which are non – super – impossi*le mirror
image of each other.
(ii) Those two structure are enantiomers of each other which ha"e opposite configuration on
all respecti"e centres.
(iii) 5nantiomers are alwa!s diss!mmetric and there opticall! acti"e. One will *e
detrorotator! while other lea"o. *! same magnitude.
COOH COOH
H OH HO H
CH3 CH3
@ 2o − 2o
− 0Do @ 0Do
22
∗∗
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(i") /n e7uimolar miture of enantiomer is called recemic miture1 recemic mi are
opticall! inacti"e due to eternal compensations.
(")
Mesomer:
(i) Opticall! inacti"e isomers is called mesomers
(ii) t is found onl! in cases of two or more similar as!mmetric centres.
(iii) That isomer will *e mesomers which has plane of s!mmetr! conse7uentl!1 its mirror image will *e super impossi*le.
(i") That str. will *e mesomer in which configuration are opposite on similar as!mmetric
centres within the molecules.
This is the reason that mesomers are opticall! inacti"e.
CH3 CH3
H r r H
C2HD C2HD
(@ 3) (− 3)
CH3 @ 0o
H OH
H OH
CH3 − 0o
esomers are opticall! inacti"e is detro while other half is lea"o *! same magnitude.
,iastereomers:
→ Those isomers are diastereomers which are not mirror image of each other.
→ The two str. which are neither identical nor non enantiomers are diastereomes
→ /ll chemical and ph!sical prop. of diastereomes are different.
On the other land enantiomers ha"e all ph!sical properties same ecept their entraction
with plane polaried light which in e7ual and opposite.
The! all chemical properties of enantiomers are same ecept their reacti"it! with chiralreagents.
→ %eometrical diastereomer.
C2HD C2HD r r
H r r H H C2HD C2HD H
23
&
&
&
&
&
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H OH CH3 HO HO CH3 HO CH3
CH3 H H H
B
P – P B → enantiomer
P – P – P B → diastereomes P B – identical.
". COOH COOH
H CH3 CH3 H
C2HD C2HD
enantiomers.
This order doesn:t match with eperimental order. Howe"er onl! the position of
c!cloheane is delocated i.e theor! faith of c!cloheane cense of this failure is the
assumption that all rings are planer. ut c!cloheane is not planer. t eist in chair and *oat form mainl!.
h!pothetical Chair oat
form /ll age form + 8o 2;:
∴ /s + O
mp + mp ? p + p
solu*ilit! + solu*ilit!& + & .
*ut @2o − 2o # − 2o @ 2o
COOH COOCH3
H r H r
CH3 CH3
and
COOH COOCH3
r H r H
CH3 CH2
∴ Q + Q 2
f reagent is chiral such as
CH3
HO H then Q ≠ Q 2
20
Q
CH3OH#H@
Q 2
CH3OH#H@
2o
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O
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% + 2 % + 2 % + 2 % + O + 0 O + 3 O + 0 O + 2
& m + & m + 2 & m +
eso +
Trans dl – pair Cis dl – pair
-# – configuration, −
CHO CHO
H OH OH H
CH2OH CH2OH
- # (@) %l!cerol # (−) %l!cerol
i.e (@) %l!cerol is assigned - – configuration while (−) %l!cerol is assigned – configuration assignment is ar*itrar!
!lyceric (ci% :
CH2 – CH – COOH
OH OH
f - – gl!cerol is o*tained then configuration is gi"en gl!ceric acid was - and it –
gl!cerol o*tained then configuration in gl!ceric acid was li.
!lycerol : similar configuration &etension # n"ersion in configuration.
&etension occurs if reagent attack from the front side and in"ersion occurs if reagent
attacks. 'rom the *ack side.
CH3 CH3 CH3
H r → −OH H OH @ OH H
C2HD CH3 C2HD
&etension prd n"ersion prd.
Inversion also calle% -al%en.s inversion Erythro – threo nomenclature:
26
CH3
CH3
CH3
C2H
D
CH3
H
H
C2H
D
CH3
H
HC2H
D
CH3
H
H C2H
D
CH3
H
HC2H
D
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This nomenclature is applied when molecule has two dissimilar ass!metric car*on atom
containing two similar group.
CH3 – CH – CH – C2HD. CH3 – CH – CH – C2HD
OH r OH OH
f similar group are same side in fisher pro=ection formula then it is called sr!thro isomer
otherwise threo isomers.
CH2 CH3
H OH HO H
H OH HO H
C2HD C2HD
5r!thro – dl – pairs
CH3 CH3
H OH HO H
HO H H OH
C2HD C2HD
Threo – dl – pair
⇒ Optical isomerism without C4
Case of cumulenes
CH3 CH3
C + C + C
H H >onJplaner
The molecule is dis – s!mmetric therefore opticall! acti"e.
>o. of optical isomers + 2
CH3 CH3 (planer) s!mmetric
C + C + C + C (>o opticall! acti"e)
H H
CH3 H not planer s!mmetric
C + C + C >o optical acti"it!.
H H
umulenes
→ 5"en no. of C + C optical isomerism → Odd no. of C + C geometrical isom.
occurs and if each *ears two different occurs if each and e"er! *ears two
2I
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groups different groups.
ase of biphenyles:
iphen!l ehi*its optical isomerism if ortho su*stituent are present and *oth ring are
opticall! diss!mmetric.
dis!metric opticall!acti"e O + 2
!mmetric >O. O – .
Resolution: eperation of enantioment or recemic mi is called resolution
That since ph!.prop of enantiomers are same the! can not *e separate *! ordinar!methods like fractional distillation or c!otellisation. Howe"er it is possi*le throughcon"ersion cnto diastereomers.
CH3 C2HD
H COOH ? H COOH
C2HD CH3
$HH@ HO H
-
O $H C2HD O $H
H C – O H ? H C – O H
O CH3 -
H3O@ H3O
@
- -2
'ractional distillation
CH3 $H
- + H COOH @ HO H
C2HD -
C2HD $H
-2 + H COOH @ HO H
2;
r r
r
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CH3 -
O
4 &COOH @ CH3OH → + )( H & – C – CH3 G H3O
@
↓
&COOH @ CH3OH
⇒ Conformational isomerism, −
>ew man pro=ection formula , −
>ew man taggred form
5lips formula
4 -ihedral angle , − interplaner angle is called dihedral angle defined *!
-ihedral angle tg. eclipsed
H – C – C – ' – ; 2
H – C – C – r – 6 2
H – C – C – Cl – 6
Condition for conformational iso.
28
a
a
*
*c
c
c c
l l m m
n
n
a
* c
l
mn
'
Cl r
OHH
'
OH
HCl r
a – * – c – d
a
d
*
c
a
d c
*
;o
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olecule must ha"e an unit like a – * – c – d and rotation should *e free. >o. of
conformers will *e infinite and a d!namic state of egutn. The! are not *e separated.
>H3 H H
>
H
H2O H H
CH3OH C + C
H H
H – O – O – H
CH3 – CH3 CH2 + CH – CH2 – CH3
Conformational anal!sis of ethno.
taggred form 5clipsed form
>o. .$1 prepulsion, $ – $ – repulsion
2 . 6 Qcal # mol
&otation # di"edral angle.
4 Heat of com*ustion is sta*ilit!.
&H @ O1 → CO2 @ H2O @ Heat
Rsing heat of com*ustion relati"e sta*ilit! can *e deri"ed if molecular formula is same
CH3 – CH2 – CH2 – CH3 2
.3O2 → HCO2 @ QCal#mol
CH3 – CH – CH3 @2
.3O2 → HCO2 @ 3H2O @ !QCal#mol
CH3 F A !G
Therefore iso*utene is more sta*le than H – *utane
→ &ule is that *ranched alkane is more sta*le than un*ranched.
∆H#CH2
3
H
H H
H
HH
H
H H
HH H
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66.6 DI.0
60.
D;.I
,eyer.s strain theory :
/ngle strain +2
S2;H8 eactualangl o − P sta*ilit! ∝ #angle strain
/ngle strain1 +2
6HS.;.H8 −o
+ 20o00′
+ S0082
8HS2;H8 oo
=−
+ S002
H;S2;H8 =− oo
+ S00D2
H;S2;H8 oo
−=−
∴ sta*ilit! order on the *asis of angle strain is
This order doesn:t match with eperimental order. Howe"er onl! the position of
c!cloheane is delocated. t means that this theor! fails at c!cloheane cause of failure isthe eemption that all! ring are planer. ut c!cloheane is not planer. it eist in chair and
*oat forms mainl!
H!pothetical ? /ll angle + 8o 2;′
train + .
** onformation analysis of butane – /0 – /& – /0
() /nti form () $artiall! eclipsed.
3
2o
H
H H
H
H
HH
6o
6o
CH3
CH3CH3
CH3
H
CH3
CH3
H
HHH
CH3
CH3
H HH
H
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() %auche (B) 'ull! eclipsed.
() /nti form , − >o $ – -$ repulsion >o steric # "enderwall repulsion ? (ost sta*le)
() $artiall! eclipsed , −
→ $ – $ repulsion
→ ome "enderwall repulsion
() >o $ – -$ repulsion some steric repulsion
(B) -$ – $ repulsion on man steric repulsion
Stability or%er :
/nti A %auche A $artiall! eclipsed A full!ed
5nerg! profile , −
Subtituent effects:
u*stituent /cidit!
The atom or group which itself doesn:t participate inren *ut effect reacti"it! of themolecule is su*stituent and its effect is called su*stituent effect.
-epending upon the modes of transmittance su*stituent effect is classifies as
u*stituent effect nducti"e steric
32
/nti /nti%auche
'ull! eclipsed
$artiall! eclipsed
-ihedral angle
$5
OH OH
>O2
>O2
>a@ >a@O− O−
@H2O@H2O
− &eadil!.
>aOH >aOH
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→ mesomeric
→ H!percon=ugation
→ electromeric
/ypercon1ugation :
Transmittance of su*stituent effect through σ − π con=ugation is known ash!percon=ugation. t occurs in
(a) /lkenes. (*) /lk!nes. (c) Cations. (d) &adicals.
$ro"ided that – there is at least one h!drogen at the con=ugated position.
p3 CH2 – CH + CH2 ≡ H2C CH – CH2
H p2 p3
CH2 – CH – CH2
H@ ≡ CH2 – CH – CH2
⇒ Nrite structures in all and h!percon=ugation, −
CH2 + CH2
CH3 – CH + CH – CH3
CH3
C + CH – CH2 – CH3
CH3
CH3
CH3 – CH2 ↔ CH2 – CH2 ↔ CH2 + CH2
H H
CH3 – CH – CH2 – CH3
CH3 – CH2 CH2 – CH2 ↔ CH2 + CH2
H H
CH3 – CH – CH3
→ n the structure arising from h!per con=ugation are C – H *ond is clea"ed. That is wh!h!per con=ugation is also called no *ond – resonance.
→ Total no. of structures will *e e7ual to no. of h!per con=uga*le H atom @ .
33
Hσs
H@
••
• •
•
•••
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Howe"er these structures are imaginar! or real.
Ha
H * C – CH + CH2 → CH2 + CH – CH2
Hc Ha
CH2 + CH – CH2 CH + CH – CH2
Hc H *
Haδ@
H *δ@ C – CH – CH2
δ−
Hcδ@ H!*rid.
/s shown C – H *ond is actuall! not clea"ed *ut elongated such that C – H *ond pair electron are shifted more towards car*on.
Therefore h!per is a method of electro – donation n other words an alk!l group donates
electron *! wa! of h!per and this e−
− donating power is directl! proportional to no. of h!per con=uga*le H – atoms.
CH3 CH3
− CH3 A − CH2 CH3 A − CH A − C CH3
o 2o CH3 CH3
(Lero no. of H – atom)
CH3
CH2 + CH – C CH3 → (+) *ond is added
CH3
Therefore in general1 electron donating power of alk!l groups through h!per con=ugation
is
− CH3 A o & A 2o & A 3o &.
ince h!per con=ugation in"ol"es delocalisation of e− it increases sta*ilit! of the
molecules
CH2 + CH2 H
CH3 – CH + CH2 3 H
CH3 – CH + CH – CH3 6 H
B CH3
C + CH – CH3 8 H
30
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CH3
B. CH3 CH3
C + C 2 H
CH3 CH3
ta*ilit! B A B A A A &ule is that more su*stituted alkene is more sta*le than less su*stituted alkene.
/ypercon1ugation is heat of hy%rogenation :
5tent of heat of h!drogenation ∝ #etent of h!percon=ugation
∴ Order of heat of h!drogenation is
A A A B A B.
CH3 – CH3 – CH2 – '
⇒ agnitude of – effects
@ − O
− COO – CH2 – -
(i) − O A − COO A − CH3 A -
(ii) − >O2 A − '
(iii) − A − OH
O
C AAA > → O ?3
+
NH A − >O2
444 / general order of − : magnitude – >H3 A − >O2 A − C> A − COOH A − ' − Cl A − r A − A OH.
− CH3 @ – effect.
CH3 CH3
− CH2 – CH3 − C(CH3)3 A − CH A − CH − CH2 – CH3 A − CH3
3o CH3 2o CH3
o
CH3
− C – CH3
CH3
∴ %en. order of magnitude of @ effect among alk!l group is 3o A 2o A o CH3
)ote : that this order is =ust opposite to the order of e− donating power through h!percon=ugation
which is ml A o A o A 3o.
3D
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⇒ esomeric effect or (&esonance effect)
Transmittance of su*stituent effect through π − *ond is called mesomeric effect (#& – effect) therefore this effect operates onl! in molecules undergoing &esonance.
CH2 + CH – O CH3 → su*stituent.
CH2 – CH + OCH3
– effect
( @ ) (− )
→ f su*sti. donates a pair of e− → f su*sti. withdraw π − e− in
in resonance. uch grps one called π − donar resonance. uch grps are called π − accepter
eg , − O CH3 ( @ 1 − )
− >H2 (− 1 @ )
− >O2 (− 1 − )
− (− # @ )
− C> (− # − )
− COOH (− # − ) ? − CHO (− # − )
− CH + CH2 @ # − − ? − >O
− COCl (− # − ) − N + O
− COCl (− # − ) @ − # − .
− COO& (− # − )
− C ≡ CH − @ # − # −
− $H @ # − # − .
eg ,
@ # − ≡ E
@ A A
− A A .
eg, O
O CH3 1 – O – C − CH3 1 – O – CH + CH2
36
>O2 O CH3
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@ − A A
O CH3 A − $H ? − CH + O A $H
@ @ − −
O O O
− C – H − C – >H2 − C − O CH3
− ? A A .
!roups
− # − @ 1 @ (−O) − # @
i.e σ − accepter as well as π −accepter
/ccepter
i.e σ − donar as well as π −donar i.e donar σ − accepter π − donar *otheffectance operating then
mesomeric effect is fa"ouredtherefore such groups
effecti"el! acts as donar
: Electromeric effect :
$olarisation of π − *ond caused *! the approach of reagent
eg. CH2 + CH2 → / non – polar *ond.⇓ H@
@CH2 – CH2
H
Therefore this effect is temporar! and operates onl! in ecited state.
: (l2one :
3I
COOH
OCH3− # @ ∴π − donar
COOH
>O2 − # − /ccepter
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Preparation :
() C + C → 2,# NH N C – C @ ∆H
− C ≡ C – → SS C – C @ ∆H2
E3othermic :
C + C → 2 H C – C @ ∆H (wrong)
5act of h!drogenation + high so a catal!st is regd to lower the eact
atalyst
/omogeneous
&hCl ($$H3) chlorotris – triphen!l plusphine
rhodium1 or willkinson catal!st.
/eterogeneous
&ame! >i1 pt1 pd (p – 2) lindlar catal!st
Alloy
Al Ni )( + worom
agNaOH → &ane! >i &a! – >i finall!
di"ided into >i – $articles
→ p – 2 is >i2 (>ickel *oride)
B NiOAC Nieborohydrid sod
NaBH
aectate Nickel 2
).()(2
0)( →
→ indlar:s cat. is pd#aO0#
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C + O →
U CH – OH
& &
O
& – C – O & ′ → &CH2 – OH @ & ′ − OH
& – C> →
U &CH2 >H2
& – COCl →
U & CH2OH
& &
C + > – OH →
U CH – >H2
& &
& – CH + O
H ↓ H
& CH2 – OH
O
& – C – O – & ′ → 2# H Ni
& CH2
OH @ & ′OH O
& – CH – O& ′ → & – CH + O@ @ & ′OH
>i#H2
& – CH2 – OH
OH
C → C + >H @ H2O
>H2
O OH
& – C – >H2 → NI H #2 & – CH – 2
..
H N
& – CH2 – >H2 ← 2# H Ni & CH + >H ←
+− H & – CH + >H2
/n ester , −
(i) ester E → Ni H #2 OH + CH3 – CH – CH3
o OH
38
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O
/ns $H – C CH3
O – CH
CH3
(ii) ester E → Ni H #2
C + O
mp. O
& – C – O & ′ → o # 2o # 3o
& CH2OH onl! o (alwa!s)
E How man! esters → 2# H Ni CH3 OH @ C2HDOH
o o
/ns O O
H – C – O C2HD # CH3 – C – O – CH3
E How man! h!drocar*ons for2I
2#
H C For
H Ni →
/ns
→ H!drogenation → s!n radical addition
C + C
H H
catal!st cis1 meso onl!
&eacti"it! !ne A ene:
JJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJ
CH3
(ii) CH2 + CH2 A C + CH2
CH3
0
OH
OH
2o
o
OO
CH3
CCCC
CH3
CH3
CH3
CH3
H
H
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SE4E5I+I56
(willkinson:s cat)
& – C ≡ C – &
↓ p – 2
& – CH2 – CH2 – & & &
C + C
H H
(onl! cis) so *oth p – 2 and – cat are selecti"e rid – agent of ≡ # +.
44 & – C ≡ C – &
(nice) echanism , − i → i⊕ @ e−
& – C ≡ C – &
↓ &
& – C + C – & ≡ C + C
&
JJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJ
& H
C + C
&
↓ >H3
& H
C + C
H &
→ ! di"ide (H> + >H)
(h!drogine) >H2 – >H2 → 22O H H> + >H (di"ide)
H H
> + H onl! cis di"ide is used for h!drogenation
0
CH + O CH2OHCH2OH
>aH0 >i#H2
CHOo1 wiliumson:s
aplnopriste forgenation of
cat (wc) is selecti"e
h!dro C + C *onds.
>i#H2
indlar:s catal!st
C + C (Trans)&
H &
H
C + C (cis )
&
H H
&indlar:s
Catal!st
#>H3
•
•
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→ ! h!dro*oration ,− H2C + CH2
↓ H3 , TH' (T H ')
ech
CH3 – CH2 CH2 + CH2
H –
→ 5lectrophilic addition.
→ arkonico" rule is o*e!ed.
→ !n addition.
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Called irch reduction which gi"es 1 0 c!cloheadiene not 1 3 c!cloheadiene e"en
though ca*er is more sta*le than former. Came (not clear)
→ Qol*e – electrol!sis
& – COO>a → is Electrolys & – &
mech
O
& – C – O− >a@ O
/node , & – C – O• @ e−
Cathode , >a@ @ e− → >a
>a @ H2O → >aOn @ V H2↑
O
& – C – O → & • @ CO2
2& • → & – &.
/s reacn mo"e pH of soln inc. due to the formation of >aOH.
CH3COO>a → −e CH3 – CH3
→ -ecar*o!lation of fatl! acids.
CH3COO>a >aOH # CaO # odaline
O
∆ ↓ sodaline CH3 – C → CH3 @ CO2 → )( 2O H CH0 .
CH0 C
Car*anion is the intermediate therefore e− withdrawing grp. increases the ease of
decar*o!lation
. CH3 – COOH
. CH3 – CH2 – COOH
. CH3
CH – COOH
CH3
ease , A A .
Qe!, Wust remo"e CO2 ↑ from compd.
O O O
CH3 – C C – OH → ∆ CH3 – C – CH3
CH2
CH2 – COOH → ∆ CH3 – COOH →
sodaline C – H6
03
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ech, O O O
CH3 – C C – OH → CH3 – C – CH2 @ CO2 CH2
O H – O
CH3 – C C + O O CH3
CH2 C
∆ ↓ OH CH3
CH3 – C + CH2 @ CO2
O
COOH C
CH2 → CH2 O
COOH H
C + O
OH O – H O
CH2 + C @ CO2 → CH3 – C – OH
OH
→ Nurt reaction , & – ∆ → ether Na #
& – &.
ech , & – → Na & >a @ >a
& – → & – & @ >a
o 1 2o 1 3o halide undergo this reacn. >ot 3o due to JJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJ
CH3 CH2 – H CH3
CH3 – C – → Na CH3 – C → C + CH2
CH3 CH3 CH3
n wurt reacn onl! that alkane is formed in good !ield which re7uires onl! one & –
which is net 3o.
CH3 – @ CH3 – CH2 –
↓ >a
CH3 – CH2 – CH3 @ CH3 – CH3 @ CH3 – CH2 CH2 CH3
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CH3 – CH2 – CH2 – CH2 – CH2 – CH3
CH3 CH3
CH3 – C – C – CH3
CH3 CH3
→ 'rankland reacn
,− ller as wurt ecept >a is replaced *! Ln.& – → Zn & – Ln – → − I & – & @ Ln2
↓Ln
& – &
→ Core! house alkane s!nthens ,−
→ *etterthan wurt.
& – → !i & i
↓ Cu
& – & ′ ← & 2Culi @ & ′
eg CH3 – CH – CH2 – → CuliCH CH 223 )( CH3 (CH2)3CH3
→ 'rom %rignard reagent & – → ∆ Ethen Na # & – g – (%J&)
44 own & – g –
i.e compd H O H → 2
relearning H@ H NH → 3
will gi"e &–H H OH CH → −3
with %J& H NH − → − 2
H COOH CH − → 3
D DiO →
() CH3 – CH + O + → H
"gx
.2
.
CH3 – CH – OH
&
CH3 CH3 OH
(2) C + O+
→ H
"gx
.2
.
C
CH3 CH3 &
O
(3) CH3 – C – OCH3 + → H excess "gx )(
CH3 – C – &
&
0D
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(0) +
→ H
"gx
.2
.
O O
(D) $H – C – OCH3 ).( g "gx → $H – C – &
own nfact %& @ H@ → alk.
o in reacn not add
& H@ or multiple *ond for product
H0 Cl
OH
C2HD – C – $h @ CH3OH
$h
/ns /ns O
CH3 – CH2 – C – OCH3
CH3
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O OH
& – C – OCH3 −−−−−−−−
→ .2
. 3 "gBr CH & – C – CH3 @ CH3
O
& – C – O& ′
OH CH3OH
& – C – CH3
CH3
mp. O
& – C – O& ′
3o alc. o1 2o1 3o
>ote, That %.& can:t *e prepared from i.e. dilalids. added to this it can:t *e prepared if molecule contains one or more reacti*le group.
r r
CH2 – CH2 CH2 – CH2
r ↓ mg g
CH2 + CH2
eng!ne.
H0Cl ↓ CH3 g r (ecess)
OH
CH3 OH @ CH3 – CH – CH3
/ns O
H – C – O CH3
→
∴
0I
r
r
r
r
g
>H2Cl
>a>H2
Cl
>H2
or1 p2
H
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→ Clemenson and wolf kishner reduction
(ket or ald.)
&
mech, (w.k red) (i) C + O @ 3 H N
&
& OH & O
C C
& 2..
H N & >H3
& &
C + >H2 C + >H
& &
)ote, − C& – acidic med. oth are complementar! to each other
wk – *asic med.
i.e t ketone # ald gas acid JJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJ
carried at1 it *ase semiti"e then C& is carried out
& H &
(ii) C + O @ > – >H2 → C – H2
& H (h!draine) &
& &
C + > – >H2 @ H2O C – H @ >2
& ↓ QOH &
& &
C + > – 2 H N − CH – > + > @ H2O
& & ↑ QOH
& &
C – > + >H → O H 2 CH – > + >H
& &
0;
Ln#HgA CH
2
A CH2∆ >2H0QOH (N.Q)
C + O
pure
(an!)
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Properties :
/alogenation :
& – H @ 2 → heat !ight # & – @ H
mech,− – → ∆ 2 • (i)
• @ H – & → sd r .. H @ & • (ii)
& • @ – → & @ • (iii)
&elati"it! of 2 → '2 A Cl2 A r 2 A 2
&elati"it! of H – atom 3o H A 2o H A o Cl
K 3o & A 2o & A o &
electi"it! , CH3 – CH2 – CH3
↓ Cl2 # light
CH3 – CH – CH3 @ CH3 – CH2 – CH2
Cl D69 (ma=) 009 Cl (min)
electi"it! ratio + &eacti"it! × pro*a* ratio
3o H 2o H o H
Cl2 D , 3.; ,
r 2 6 , ;.2 ,
electi"it! ratio + .#326.3
;.3
6
2
;.3 II ===×
@ + 9
∴ 9 + D69 9 + 009
CH3 – CH2 – CH3 → light Br #2 CH3 – CH – CH3 @ CH3 – CH2 – CH2 – r
08
Ln # H
Conc HCl
>2H
0#OH
O
OH
Cl
Cl
>2H
0#conc QOH
Ln # H
conc HCl
O
OH
OH
Cl
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r 869 09
/ll H – atom of alk. Can *e replaced
CH0 → ∆#2Cl CH3Cl → CH2Cl2 → CHCl3 → Cl
CH3Cl (e=)
CH0 (5l.) @ Cl2 (ee)
CCl0 (a=)
"# CH3 – CH3 → ∆#2Cl How man! prd.
/ns + 8.
ombustion : Heating alkanes in atm. Of O2
CH0 @ 2O2 → ∆ CO2 @ H2O @ heat
CH3 – CH3 @ 8#2 O2 → 8 2CO2 @ 3H2O @ heat
n asscence of sufficient amount of O2 in complete com*ustion occurs
CH0 @ 3#2 O2 → CO @ 2H2O
CH0 @ 3O2 → C @ 2H2O
amp *lack.
Pyrolysis: Heating alkanes in total a*sence of O 2 is called p!rol!sis or cracking which
produces lower alkanes from higher ones
CH3 – CH3 → 2 . CH3
↓ DoC
CH0
(47E)E
Preparation:
() 'rom alcohol,
〉 C + C 〈 +
←orH
$O H 02 〉 CH – C 〈 → HCl 〉 CH – C 〈
OH Cl
Case, − Cl− is much *etter nu than HO0−
mech, 〉 CH – C 〈
OH
↓ conc H2O0
H
〉 C – C 〈
5 OH 52
D
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〉 C – C 〈 〉 C + C 〈
HO0 H → 〉 C + C 〈 @ H2O0.
o alc follow 52 pathwa!1 while 2o and 3o alcohol follow 5 pathwa!.
Cause , o C is not so sta*le.
CH3 – CH2 – CH2 – CH2 – OH
∆ ↓ H2O0
CH3 – CH2 – CH + CH2 CH3 – CH + CH – CH3 CH3 – CH2 – CH2 – CH3
↓ H (a=or) ↓
CH3 – CH2 – CH – CH3 CH3 – CH2 – CH – CH3
How man! products
JJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJ
CH3
CH3 – C – CH + CH2 @
CH3
CH3 CH3
CH3 – C + C @ CH2 + C – CH – CH3
CH3 CH3 CH3
OH → ∆+ # H @ a=or
: Pinacol – pinacolone rearrangement :O
& – CH – CH – & → $O H 2 & – C – CH2 – &
ech, H
& – CH – CH – & → ⊕
H & – C – CH – &
OH OH OH OH2
O H
& – C – CH2 – & ← ⊕
H & – C – CH – &
O – H
mp. igrator! aptitude,
H A $H3 A 3o & A 2o & A o & A CH3
$H CH3 $H O
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o C@ ion rearrangement
→ Laise" rule is followed for orientation
→ t is not re"ersi*le *ecause H is neutralied *! *ase.
5, 'ind the ma=or product
CH3 – CH – CH2 – CH3 ∆
→ kon Alc.
CH3 – CH + CH – CH3
r
r
CH3 – CH – CH – CH3
CH3 ↓ /lc. con1 ∆
D2
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CH3
rkon
Alc → C + CH – CH3 (a=)
CH3
ecause path is 52 in which there is no C@ rearrangement.
: ,ehalogehation :
r
Ln 〉 C – C 〈 Q
r ↓ g
〉 C – C 〈 〉 C + C 〈 (a=) 〉 C – C 〈
@ Lnr 2 @ gr 2
echanism , −
r r r
〉 C – C 〈 〉 C – C 〈 〉 C – C 〈
r r r
↓ Ln ↓ g − ↓
r r r
〉 C – C 〈 〉 C – C 〈 〉 C + C 〈
Ln r ↓ g r @ r @ Qr.
〉 C + C 〈 @ Ln r 〉 C + C 〈 @ g r 2
Imp# r
〉 C + C 〈 *ut 〉 C – C 〈 → 〉 C + C 〈 @ 2
r (sta*le) (not sta*le)
r
"# CH + CH – r → Zn HC ≡ CH
r → Zn
r r
→ Zn
r
mp.
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C + C
$H r
$H
↓ Ln C + C$H
$H – C ≡ C – $H
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Case, H is strongest acid and − is a good >u−
Cl
CH3 – CH – CH + CH2 → HCl
CH3 – C – C2HD *oth enahtiomer
CH3 CH3
Cl
and CH3 – CH – CH – CH3 (a=or)
CH3
9PERO8I,E EFFE5
CH3 – CH – CH3 ← HBr CH3 – CH + CH2
22O
HBr → CH3 – CH2 – CH2
r r arkon – addition /ntimark – addition
& – O – O – & → ∆ 2&O•
&O• H – r → &OH @ r •
CH3 – CH + CH2
(2) ↓ r • ()
CH3 – CH – CH2 () CH3 – CH – CH2• (.)
r H r r
CH3 – CH2 – CH2 @ r •
r
$eroide effect works onl! on Hr not on HCl and H.
Cause, oth step () and (2) are eothermic in case of Hr not in case of H and HCl now peroide effect separates also on other t!pes of molecules like CCl01 CHCl3. Cr 3 etc.
5,J Cl
CH3 – CH + CH2 OCCl → 0
CH3 – CH – CH2 (not formed)
↓ CCl0 . peroide
CH3 – CH – CH2 – CCl3.
Cl
Cause,J first • CCl3 attacks
& – O• @ Cl – CH3 → & – OCl @ • CCl3
DD
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& – O – CCl3 @ Cl• → >ot permici*le
Cl – CCl3
H – CCl3 → 'irst attacking fran7uent
– Cr 3
: /alogenation :
r
〉 C + C 〈 .# 02
tem' oom
CCl Br → 〉 C – C 〈
→ 5lectrophilic addition
→ Occurs through. ech, J 〉 C + C 〈
c!clic *romoaion c!clic *romination ↓ r – r
intermediate *ecame 〉 C – C 〈
it is more sta*le than C⊕ r ⊕
r
〉 C – C 〈 〉 C – C 〈 〉 C – C 〈
r () ↓ r (.) r
Complete octet of n complete octet /nti addition due to c!clicintessmer
all 3 – atoms octet of can*on.
"# -rite the pro%uct:
Cl CH3 – CH + CH2 r 2#H2O
↓ >aCl#r 2
Cl OH
CH3 – CHJ CH2 CH3 – CH – CH2 CH3 – CH – CH2 (a=)
Cl (a=) r r
CH3 – CH – CH2 – r CH3 – CH – CH2
r r
2. → 2 Br (Trans onl! oth ehantiomer)
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r CH3 H r H CH3
CH3 CH3
H r H r
i.e ehantiomers (/cti"e) es
CH3 CH3 CH3
H r r H H r
r H H r H r
CH3 CH3 CH3
/y%ration
CH3 – CH + CH2 OH
→ + O H H 2# CH3 – CH – CH3
0
22
.2
#)(.
BaBH
O H OAC Hg → CH3 – CH – CH3
OH
OH
− → OH O H
H B
#.2
.
22
62
CH3 – CH2 – CH2
(ci% catalyse hy%ration:
() CH3 – CH + CH2 → CH3 – CH – CH3
→ 5lectrophilic addition OH
→ arkohikott:s rule followed. CH3 – CH – CH3
→ C – interus. o rearrangement is possi*le. OH2
CH3 – CH – CH2
OH
(a) CH3 – CH – CH + CH2
CH3 ↓ H2O0#H2O
OH
CH3 – C – CH2 – CH3 ↓ H@ # H2O
CH3 (a=or)
@ CH3 – CH – CH – CH3
CH3 OH (inor)
→ Bia o!mercuration # demercunation.
CH3 – CH + CH2 CH3 – CH – CH3
DI
CH3
CH3
CH3 (a=)
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Hg(O/C)2 ↓ o!mercuration. OH
JJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJJ
ech, CH3 – CH + CH2 O/C
Hg
O/C
→ 5lectrophilic addition H2O
→ – "alue followed CH3 – CH – CH2
→ >o C@ − ion rearrangement. Hg
↓ O/C
OH
CH3 – C – CH2
Hg O/C.
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D8
CH3 CH3
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6