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This article was downloaded by: [University of Cambridge]On: 11 November 2014, At: 04:48Publisher: Taylor & FrancisInforma Ltd Registered in England and Wales Registered Number:1072954 Registered office: Mortimer House, 37-41 Mortimer Street,London W1T 3JH, UK
Synthesis and Reactivity inInorganic and Metal-OrganicChemistryPublication details, including instructions forauthors and subscription information:http://www.tandfonline.com/loi/lsrt19
Oxo-Cation Complexes -Part XIII. Dioxouranium(VI),Oxovanadium(IV) andOxovanadiuti(V) Complexesof the Schiff Base (N,N′-2,2′-bis(aminoethyl)methylamine-bis(3-carboxysalicylideneimine))Kamalendu Dey a , Asoke Kumar Sinha Roy a ,Alok Kumar Mallick a & Kartik Kumar Nandi aa Department of Chemistry , University ofKalyani , Kalyani, 741 235, IndiaPublished online: 22 Nov 2011.
To cite this article: Kamalendu Dey , Asoke Kumar Sinha Roy , Alok Kumar Mallick& Kartik Kumar Nandi (1992) Oxo-Cation Complexes - Part XIII. Dioxouranium(VI),Oxovanadium(IV) and Oxovanadiuti(V) Complexes of the Schiff Base (N,N′-2,2′-bis(aminoethyl)methylamine-bis(3-carboxysalicylideneimine)), Synthesis andReactivity in Inorganic and Metal-Organic Chemistry, 22:2-3, 145-159, DOI:10.1080/00945719208021378
To link to this article: http://dx.doi.org/10.1080/00945719208021378
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SYNTH. REACT. INORG. MET.-ORG. CHEM., 2 2 ( 2 & 3 ) , 1 4 5 - 1 5 9 ( 1 9 9 2 )
0x0-CATION -m,zxss - PART XIII.
DIOXOIr3A':IUFT('v'I), OXOVLNADTJT( IV) 4 ,: O ~ O V A N 4 D I I J ? ? ( V ) C P P E X E S 0;. THE
SCFI?? BAS? (N,N1-2, 2'-BIS( UlINOC1HuL)!~T'YLA'I~~-~~S( 3-CAWOMSALICYLI-
D V T I T " 1%) )
Kamalendu DeyX, Asoke Kumar Sinha %y, Alok Kumar Mall ick
ar,d K a r t i k Kumar Nandi
'lepartment of Chemistry, Univers i ty of Kalyani , Kalyani - 7'41 235,India .
4ESTRACT
A ne.3. Sch if f base ( N , N -2,2' -b 1 s( am inoe thy1)nethylam ine-bis
( 3 - c a r h o x y s a l i c y l i d e n e ~ ~ e ) ) , abbreviated t3 Hqfsadien, h a s been
synthes ized f ?om 3-formylsal icyl ic ac id (H2f sa) ane die thylene t r iamine
( d i e n ) . The c h e l a t e s of t h i s l igand with UO:', V02+ and V03+ have a l s o
been synthesized and charac te r ized i:ith t h e h e l p of e lementa l a n a l y s i s ,
m o l a r conductance, n a p e t i c s u s c e p t i b i l i t y and v i s i b l e - W and 12
sue c t roscopie s.
II\T 3O?UCT I O N
3 - F o m y l s a l i c y l i c a c i d (H2fse) , and i t s Schi f f bases \;it- mono-
and d i - m i n e s a r e v e r s a t i l e l igands (F ig . 1 anc! 2 ) and t h e i r conplexes
wi th t r a n s i t i o n and non-tr?nsit.ion meta ls have been e x t e n s i v e l y s tud ied
i n r e c e n t years'-".
such a s d ie thylene t r iamine ( d i e n ) , t r i e t h y l e n e t e t r a n i n e ( t r i e n ) , e t c . ,
have not been much used a s l igands f o r complex foxmation. We have
Hc*,*ever, Schi f f bases of H2fsa with oolyvnines,
145
Copyright 0 1992 by Marcel Dekker. Inc
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146 DEY ET AL.
H C C- OH I I ' I 1 N OH 0 '
R
R=CHs,Et.Ph, -CHI -COOH
etc.
FIG. 1
therefore studied the
II I1 N OH 0
H
/
R \
N
H ,yJ- OH
FIG 2
C-OH II
C I1
H \
N OH 0 /
H 2C I
H2C, NH
HzC, N OH 0 I I I I I
H' c+Yc-OH kJ F I G . 3
( HGfsodien 1
t r a n s i t i o n and non-transition metal complexes
of Schiff bases derived from H2fsa with polyamines.
descr ibes the synthesis and charac te r i sa t ion of a new ?:?.iff base
( t i ,N'-2,Z1-bis( aminoethyl) methylmine-bis( 3-carboxysalicylideneimine)
derived from HZfsa anc? dien abbreviated t o H4fsadien) (Fig 3) and i t s
che la t e s with UO$ V02+ and V03+.
EXPERMENPAL
This paper
?ea;rent grade chemicals and solvents were used, an? they were
pu r i f i ed and dried whenever necessary by standard methods.
Data f o r charac te r i sa t ion of the new cmplexes were co l lec ted a s described ?reviously 11,12.
The Schiff base l i - a n ? , Hqfsadien was i so la ted i n the solid
s t a t e by t r ea t ing dien 0.02 rnol wi th H2fsa 0.04 mol in refluxing
m t h a n o l (200 ml) i n 65% yie ld , m.p. 208-21O0C(dec.).
0x0-cation complexes reported i n t h i s note, however, i so l a t ed
following an in-situ reaction procedure.
Most of the
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0x0-CATION COMPLEXES. XI11 147
Preparation of metal cauplexes
- /-(Hqfsadien)U02(N03)+7 (2) - H2fsa (4 m o l , 0.664 g) was dissolved in ethanol (15 ml) t o
which d i m ( 2 mmol, 0.226 g) i n ethanol (5 ml) was added dropwise while
s t i r r i n g . The mixture turned yellow and was heated under reflux on a
s t e m bath f o r 30 m i n .
6H20 was then added t o t h i s ho t solution of the lie;and, Hqfsadien while
s t i r r i n g .
1 h.
f i l t e r e d o f f , washed with ethanol and dried i n vacuo. Yield 80%.
An ethanol so lu t ion containing 2 mmol U02(1;03)2.
The whole mixture was then heated under gent le reflux f o r
During reflux a yellow compound was separated out , which was
The complex (2) is soluble i n W S O but insoluble in a l l other
ccmnon orEanic solvents. Rwever, it is appreciably soluble i n ho t
water. The canpound is diamagnetic.
- /-( H2f sadien)U0&7H20, (2)
Reaction of the d i sod im s a l t of the above Schiff base,
Na Y fsadien (prepared in-situ as described above, by the reaction of
H2fsa, deta and NaOH) with U02C12 ( 2 mmol; 0.682 g) in ethanol (70 ml)
gave t h i s yellow product i n about 75% yie ld .
ethanol and dried in a desiccator over fused CaC12.
2 2
It was washed with
The complex is soluble i n LMSO, but insoluble in other common
organic solvents. It is diamagnetic.
The complex ( a ) , when t rea ted with s t o i c h i m e t r i c mount of
NaOH i n aaueous ethanol, gave compound (2). - r ( H q f sadien)V0-7SOq, (2)
This d i r t y yellow compound was prepared by a method s h i l z r t o
th2 t employed for (A) us- a hot e thanol ic solution of V03Ob.H20(2 mmol;
0.362 g). It was washed with ethanol and dried i n vacuo. Yield a&.
Thz cmplex is highly soluble i n MSO, p a r t i a l l y so i n ho t water,
but insoluble i n othor organic solvents. It is paramagnetic ( P e f r =
1.67 B.M. a t room temp.).
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148 DEY ET AL.
- r ( H 2 f sadien)VO-mpO, (5) This grey yellow compound was prepared by a method s imi l a r t o
t h a t employed f o r (2) us- solid VO(CH3COO), ( 2 m o i , 0.37 g ) it
was washed with ethanol and dried in a desiccator over fused CaC12.
Y i e l d 75%.
The complex i s highly soluble in ITIS0 and moderately so in CMF.
It is paramagnetic ( Feff = 1.6s B.M. a t room temp.).
r ( H 2 f sadien)VO_f, ( 5 ) A suspension of Hqfsadien (2 -01, 0.8 g) i n ethanol (30 m l ) was
t r e a t e d v i t h a so lu t ion (18 r n l ) of sodium hydroxide (4 mmol, 0.16 g)
i n water-ethanol (3:5, v:v) mixture and heated on water bath for few
minutes t o ge t a yellow so lu t ion of t he sodium s a l t of the ligand.
Solid VO(CH3C02)2 ( 2 mmol; 0.37 g) w a s then aCdea t o t h i s so lu t ion
and then refluxed on a water bath f o r 30 min.
compound separated out. It was recrys ta l l ized from MF-EtOH mixture.
Yield 70%. MSO, LMF and dioxan and is parmagnet ic (
temp.).
while a grey granular
The complex (5) is hygroscopic. It is soluble in hot
= 1.70 B.M. a t room F e f f
The enhydrous canplex (2) can also be obtained from (i) on
keeping it is a vacuum des icca tor over conc. H2S04 for about a week.
r( Na2fsadien)V0-7, < 8) A suspension of Hqfsadien ( 2 mmol, 0.8 g) in alcohol (30 ml)
was t r ea t ed with a so lu t ion (18 ml) of so.’im hydroxide (4 m o l ,
0.16 g) i n water-ethanol (3:5, v:v) mixture and heated on water
bath f o r f e w m i n s . t o ge t a c l e a r yellow so lu t ion of t h e sod im s a l t
of the l igand.
( 2 mmol, 0.36 g) was added t o the r e su l t i ng so lu t ion a t the room
tem?erature while a voluminous brown compound separated out, f i l t e r e d
and washed with aqueous ethanol.
A c l e a r ethanol so lu t ion containing VOS04.H20
Yield 70%.
The complex is soluble i n water and a l so in coordinating
solvents. It is paramagnetic ( Peff = 1.73 a.br. at room temp.).
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0x0-CATION COMPLEXES. XIII 149
(!:a2fsadien)VO(OH), (2) p____._- ~
H2fsa ( I r mmol, 0.664 g) was d isso lved i n e thanol (15 ml) t o
which
while s t i r r i n g . The mixture turned yellow and was heated under
r e f l u x on steambath f o r about 20 a i n . T o t h e hot s o l u t i o n of t h e
l iyand Hqfsadien, sodium hy-’roxide ( 2 mmol, 0.08 g ) i n water - e t h a - o l (3:5, v/v) mixture was added t o make t h e r e a c t i o n mixture
a l k a l i n e (pF 9 ) . An e t h a n o l i c s o l u t i o n containing 2 mmol V03O4.H20
was t h e n aaded and the r c a c t i o n mixture wzs ref luxe2 f o r 1 h. A
d i r t y yellow conpound .hich was i s o l a t e < by f i l t r a t i o n was washed
(2 mmol, 0.206 g) i n e t h a n o l ( 5 ml) was added dropwise
e t h a n o l ane d r i e d i n vacuo. Yield 7m.
The complex i s s o l u b l e i n wzter and a l s o in csord ina t ing
so lvec ts . It i s diamagnetic.
RFXETS AND DISCUSSION
Synthes is . Depending on t h e r e a c t i o n conc‘itions t h e l izand
Hqfsadien r e a c t s with t h e salts of dioxo-uranium(V1) and oxo-
vmadium( IT!) i o n s a f f o r d i n e d i f f e r e n t 0x0-cation complexes. The
chemical composition of t h e i s o l a t e d complexes depend t o s m e e x t e n t
on t h e n a t u r e of t h e r e a c t a n t s , s o l v e n t s , t h e pH of t h e s o l u t i o n s
and t h e o t h e r condition:. of t h e r e a c t i o n s .
1) support t h e i r formulat ions.
E l e n e n t a l ana lyses (Table
Magnetic moments. A l l t h e 0x0-vanadium( IV) c m p l e x e s (2, 2, 2 anc $) are paramagnetic, t h e p e f f v a l u e s being in t h e range 1.67 - 1.73 B . M . , which a r e q u i t e c l o s e t o s p i n only value f o r one unpaired
e l e c t r o n a s is expected f o r 0x0-vanadium(1V) che la tes . These
approxim?tely normal mzpnetic moment v a l u e s i n d i c a t e t h a t t h e r e is no
s i g n i f i c a n t i n t e r a c t i o n between neighbouring vanadium( I V ) i o n s . On t h e o t h e r hand, t h e complex (2) is diamagnetic a t room temperature,
i n e i c a t i n g t h - t it c o n t a i n s 0x0-vanadim(V) species . The uranyl
complexes ( a ) and (2) a r e diamagnetic (Table 1) a s is expected f o r
t h e s e i o n s having do c o n f i g w a t i o n
10,11
10,ll
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TABL
E 1.
Ele
men
tal
an
aly
sis,
mag
pet ic
mom
ents
, co
lou
r an
d m
elti
ng
po
ints
of
som
e di
oxou
rani
um(V
I),
oxov
anad
ium
( Iv
) P*
(v)
com
plex
es.
Cm
ple
xa
Foun
d (C
alc.
) %
Iv
lngn
etic
m
omen
t beff
C
olou
r M
N C
H Na
(B .M. ) -
at
room t
emp.
-.
<..
" D
iam
agne
tic
[(H4f
sa
dien
)UO
J-b
Yel
low
30.9
8.7
29.8
2.4
-
I(
H2f
sad
ien)
U0,
+7H
20,
(2)
Yel
low
35.9
5.9
35.6
2.0
- (30.01)
(8.8)
(30.26)
(2.6)
(NO3)29 (2)
(34.74)
(6.13) (35.03)
(3.06)
[(H4fsadien)V0-7SOq,C(J)
Dirt
y 9.5
7.9
41.9
4.1
- ye
llow
(9
.06
) (7.47) (42.7)
(3.7)
r(H
2fsa
dien
)VO
-7H
20,
(9)
Gre
y 10,l
8.9
50.2
4.7
- [(
H2f
sadi
en)V
0-7,
(5)
Snuf
f 10
.5
9.8
51.0
3.8
- r(
Na2
fsad
ien
)VO
-7,
(6)
Brow
n 10.8
8.4
47.7
4.0
8.0
1.73
[(N
a2f
sadi
en)V
O( OH-7, (
I)
Dir
ty
8.9
8.2
46.0
3.2
9.0
Dia
mag
neti
c
yell
ow
(10.56)
(8.7)
(49.8)
(4.35)
(10.97)
(9.05) (51.7)
(4.09)
(10.3)
(8.2
) (47.24)
(3.34)
(9.05)
yell
ow
(9.7)
(8.0)
(45.7)
(3.4
) (8.76)
u 1.67
1.68
1.70
a)
The
com
poun
ds d
id n
ot m
elt
up
to 30O0C.
b)
emp
iric
al f
orm
ula
of
(I) C
2&1UN5014
c)
emp
iric
al f
orm
ula
of
(2)
c~~H~,vN~o,~s
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0x0-CATION COMPLEXES. XI11 151
Molar conductance v a l u e s . The molar conductance value of t h e
complex (2) i n l3:SO i s 45.7 ohm-’ cm2 mol-I i n d i c a t i n g t h a t t h e
complex i s a 1:l e l e c t r o l j j e 1 3 .
on t h e o t n e r hand, a r e non-conducting i n t h e same so lvent (Arq = 5.8 - 8.2 ohm” c m 2 mol-I range).
conductance values of t h e rest of t h e compounds could not be recorded.
I t is i n t e r e s t i n g t o r o t e t h a t t h e value o f A , ( i n I X S O s o l u t i o n ) of
t h e complex (1) - i n c r e a s e s on prolonged s tandine , which a f t e r about 3
days a t t a i n s a value of 58.5 ohm-’ a n 2 mol‘ . sed bv t h e fol lowing equat ion, which shows t h e f o n ? t i o n of a 1:2
e l e c t r o l y t e in s o l u t i o n :
U02(H4L)(N03)2 + LT:SO = rUO2(H4L)(WSO)X-7*+ + 2 NO;
- r w h e r e H4L s tands f o r H4fsadien-7
The complexes (l), ( z ) , (5) and (2).
Due t o s o l u b i l i t y problems t h e molar
1 T h i s nay be r a t i o n a l i -
E l e c t r o n i c spectra. The e l e c t r o n i c s p e c t r a of t h e oxovan.-dim( IV)
and 0x0-vanadium(V) complexes a r e re?orted in Table 2. The ox+
vanadium(1V) complexes, (3 ) t o ($) snow one prominent maximimum at about
15500-16000 cm-’.
ap?ear i n t h e s9ec t ra a t
I n addi t ion , a few shoulders ( o r weak-broad bands)
11000-13000 cm” and 17600-18800 cm-’.
Although t h e e l e c t r o n i c s p e c t r a of t h e oxo-vanadium( I V ) conplexes
are discussed in many place^^^^^, t h e ass iennent of observed,
e l e c t r o n i c absorpt ion bands f o r 0x0-vanadium( N) complexes h a s been a
m a t t e r of controversy, Kost of t h e d iscuns ions ere made i n terms of
CbV and a few i n t e r n s of CZv symmetry.
t r a n s i t i o n s 21-e expected for t h e d’ oxo-vanadium(IV)20.
of t h e symmetry from C4,, t o Ca o r Cs h a s t h e e f f e c t of removing t h e
degeneracy in the d - o r b i t a l s and t h u s f o u r t r a n s i t i o n s are predicted.
I n symmety t h r e e e l e c t r o n i c
The lowering
It has been observed i n t h e p r e s e n t i n v e s t i g a t i o n t h a t a l l the
bands a r e not w e l l resolved i n t o t h e i r components. The broad band
observed about 15500-16000 cm” is e a s i l y i d e n t i f i e d , and may be
a t t r i b u t e d t o 4 *B, i n CkV symmetry 16’20.
range 17600-18800 an” may be due t o
The high i n t e n s i t y of t h i s band may be due t o inf luence of some charge-
The shoulder in t h e
4 2A, t r a n s i t i o n ( i n C4v).
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152 DEY ET AL.
TABLE - 2 .
E l e c t r o n i c abscjrption s p e c t r a l d a t a of oxovanadium complexes with
Hqfsadien.
complex/Ligand Solvent $,, in Cm-I
H4fsa dien Nu j o l mull 27397( s h ) ; 24390; 22727; 21 276.
26500 sh * 24937 23000t shj ’ 1 8 W f sh) , 16000, IlbCO(w).
26315 sh ) , 24390, 1‘7857 w) , 155OO( w) , 13908 I b r , v ) , 12500(w).
25641 25000( s h ) , 188001 sh), 17300, 15500(w, br) , I ’ l ~ ( w > .
25641 23255( sh) 19000( s h l , l8000[ sh) , 15OOO(sh., 12500 w,br).
sh = shoulder ; w = w e a k ; b r , w = broad and weak.
16 t r a n s f e r or i n t r a - l i g i n d t r a n s i t i o n . The low-energy band observed
around 11000-13000 cm” may be assigned t o ‘?j2 j % t r a n s i t i o n s .
t h e p r e s e n t oxc-vanadium( IV) complexes of t h e l igand H4f sadien a r e
square p:iramidal i n s t r u c t u r e l i k e t h o s e of oxo-vanadium(N) complexes
o f / -diketones, t h e y shoula then r e a d i l y add a donor l i g a n d t o t h e
metal a t t h e vacant axi.1 coord ina t ion p o s i t i o n and thereby produce a
marked s h i f t t h e d-d t r a n s i t i o n bands. The e l e c t r o n i c s p e c t r a of t h e
p r e s e n t complexes have been found t o be so lvent independent r c o m p a r a b l e
s p e c t r a were obta ined when measured rn pyr id ine and INSO as seen i n
n u j o l mull (Table 2)-7,
of t h e present complexes (2) t o (g) may be due t o s t e r i c hindrance of
If
This so lvent independent e l e c t r o n i c s p e c t r a
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0x0-CATION COMPLEXES. XI11
O H H O I
o= c 0 I c = o
153
FIG. L
t h e t r i a n i n e fragment of t h e che la te ring, whizh might put a b a r r i e r
t o c l o s e ap?roach of t h e donor solvent o r e l s e t h e complex may have a
t r igonal -b ipyr imida l s t r u c t u r e which, unl ike t h e square-pyramidal
geometry, h inders complex-base i n t e r a c t i o n . A l t e r n a t i v e l y , it nay
so happer, t h a t i n t h e s e complexes t h e secondary amide (-1JH) func t ion
might from a weak bond with t h e vanadium atom ( s e e Fig. 4) and t h u s
Drevent t h e incoming donor l igand from forming a bond.
16
The absorp t ion bands observed f o r t h e present 0x0-vanedium(V)
However, t h e band around c m p l e x (2) are very d i f f i c u l t t o ass ign .
17000-18000 an’’ may be due t o ligand-to-metal charge t r a n s f e r
t r a n s i t i o n . It i s q u i t e i n t e r e s t i n s t o note t h a t t h i s diamagnetic
0x0-vanadium(V) canplex (z) may be converted t o t h e paramagnetic
oxc-vanadiun(N) complex (5) simply by gr inding it b!ith sodium
b i s u l p h i t e in a l i t t l e water . The s p e c t r a l p a t t e r n and Sand p o s i t i o n s
(in t h e range 350-450 nm) of t h e free l igand Hqfsadien d i f f e r
apprec iab ly from those observed f o r t h e 0x0-cation complexes of
u r a n i m and vanadium.
21
Infrared spec t ra . The genera l t r e n d of the i n f r a r e d s p e c t r a
of t h e present oxo-cation complexes a r e comparable with t h o s e
publ i shed previously with s i m i l a r tvpes of ligand1’2’22-24. A l l t h e
0x0-cation complexes under discuss ion show broad-medium bands in t h e
reg ion 3600-3000 an-’, which a r e ass ignable t o OH s t r e t c h i n g v i b r a t i o n s
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154 DEY ET AL.
TABLE 3.
Infrared spec t ra l data of dioxo-uraziunl( V I ) , 0x0-vanadium( N & V) . Complexes with S c k i f f bases.
Complex/Ligand Band ( cm" )
- rH4f sa dien-7
[(H2fsa dien)U0&7, ($1
r ( H 2 f sa dien)V0-7H20, (5)
3660-3350( br,rn), 3?ibO(w), 3140-28800
3640-3240(br, band not w e l l resolved) ; 3200-2960 br,w); 2410-2300(w,br w i t h two peaks!; 1645( s), 1595( s); 1545(m, with a sh a t 1520); 1450(br, m ) ; 1355(m); 1305(w ; 1275(vw), 125O(s with sh a t I Z O O ] ; 1155(s); 11OO(vwj; 1080(vw); 920(br,m with sh a t 875); 830 vw); 79O(vw); 665(s 650 w ; 6 2 0 1 ~ ) ; 58O(vw) ; ~ ~ O ( V W ] i 425tm1.
3640-2800[br. not well resolved):
900 br, rn with &I ?t 875(vw); 790(sh); 765tm); 650(w); 62O(w); 420(br,w).
3640-2800(br); 2300(m); 1645, 1600 & 1555 3 str. bands not well resolved); 1450 {str. bands with sh a t 1460). 1390(w); 1305(w); 127O(w); 123O(sj;
3600-3200(br, not wel l resolved); 3030(w ; 291O(w); 2840(w); 1640(rn); 1600(w{ ; 1570-1500 ( o r , m not well resolved wi th several peaks) ; 1440(br, m with sh e t 1468); 1400(br, w); 129O(w); 1245(m)* 1200 vw); 1150(m); 1080(vw); 1035(vwj; 975tbr.m); 695, 850 and 810 ( th ree w bands ; 760(m); 735(w); 695(w); 670( w) ; 600( ; 565( vw) ; 540( vw) ; 42O( vw)
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0x0-CATION COMPLEXES. X I 1 1
TABLE 3 (Contd.)
155
Pomplex/Ligand Band (cm-’)
3640-3000( br ) ; 2400( vw) ; 2300(vw) ; 167&1580(br, not well resolved with severa l peaks); 1550(m); 14&O(br,rn)- 1350( br,w) ; 1305( vw) ; 1230( s) ; 11 5 O t s) ; 1080(w ; 1025(vw); 945(br,w) ; 875(rn) ; BlO(vw]; 760(s); 650(v).
3600-3000 (br, band not well resolved); 2915 (br,,.r); 2380-2290 ( b r , m with two peaks a t 2350, 2330); 1700-1500(m, with two Deaks a t 1600. 1560): 1480-1410(br. m peaks 2 t 1455 i 4 3 5 ) ; - i x p ~ ( b r , w); ‘
128O(w); 1115 sj; 958(vw); 930(m); w ) ; 840(wj; 765(m); 632(w); 610(w);
364O-3000( br) ; 2900( br,w) ; 2380-2280( S , s p l i t i n to two peaks -t 2345 and 2330); 1700-1500 ( b r m w i t h t h r e e peaks a t 1600 and 15551; 156C(sh); 1470-1410(br, m with two peaks a t 7430, 1460); 3410- 1210(br, w with --Vera1 peaks); 1000(br, m w i t h a sh a t 1170). 935(s
420 (vw); 375(m).
670 w ; 840(m); 760(sj; 635(s{j 610{~{ ; 570, 530, 470,
s = strong; IP = medium; w = weak; vw = very weak;
b r = broad; sh = shoulder; vs = very strong.
due t o the presence of water molecule( s) and o r hydroxyl groups
[complexes
group(s) [complexes (2). (z) , (11, (5) and (5) -7 25926.
s t r e t c h i n the complexes (2) t o (2) observed as medium-weak broadlor
sharp peak i n the region 3300-3100 cm
complexes is observed around 1645-1630 crn” (which i s 1025 cm” lower
than t h a t observed i n t h e free l igand) and lend support for the
coordination of h i n e nitrogen 25-28.
group ( 6 as(COO) was observed a t 1720-1680 ern-', suggesting a mononu-
c l e r r formulation of t he complexes. The phenolic (c-o) generally
appears around 1500 cm” in the free Schiff base and 1540 cm” when
attached t o a s ing le metal ion ( n o n b r i d ~ F n g ) ~ ’ ~ ’ ~ & ~ ~ .
($), (2),7 and a l s o due t o the presence of f r e e COOH
The N-H
The (c=N) in the -1 25,26 ,
A band due t o the f r e e carboxyl
On the o ther
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156 DEY ET A L .
OH
CHz-N OH @
‘ 0
O H 0
‘ 0’ H2C,
CH2- N
H OH
F I G . 5
hand, t h e br idging phenol ic 6 (c-o) a?pears a t 1560 cm”. Hence, t h e
h i g h e r energy s h i f t of t h e band h a s been used f o r a d iagnos is of t h e
f o r n a t i o n of phenol ic oxygen br idge. On t h e b a s i s of t h i s we can
safely say t h a t present oxo-cation complexes a l p mononuclear in
n a t u r e with a free COOH group. The i n f r a r e d s p e c t r a of t h e complexes
(2) and (z) , show an in tense absorp t ion i n t h e 888-923 cm” region
a t t r i b u t a b l e t o t h e $ as ( U 0 2 ) mode31s32. The 4 ,(UO2) v i b r a t i o n s in
t h e s e complexes a r e expected t o be weaker in i n t e n s i t y ; t h e i r presence
could not be e s t a b l i s h e d unequivocally s i n c e t h e l i g a n a a b s a h h t h i s
region.
1380 an”, where t h e f r e e NO; ion i s known t o absorb.
be conclEded t h a t t h e two NO;
this complex (1) shows absorpt ion peak a t about 1470 cm” and 1240 an-’,
which a r e ass ignable t o t h e 4, ( N O s t r e t c h i n g ) and J b ( N O 2 assymetr ic
s t r e t c h i n g ) v i b r a t i o n , respectively3F36; it i s presumed t h a t in t h e s e
complexes the n i t r a t e ions a r e coordinated with t h e metal i on a s
un identa te l igands. It is t h u s p l e u s i b l e t h a t t h e dioxouranium(V1) ion
i n the coEplex (1) may a t t a i n e i g h t c o o r d i n a t i ~ n ~ ~ (Fig. 5).
a t e n t a t i v e suggestion.
The complex (A) does not show any absorpt ion band n e a r about
It may, thereforw,
i o n s a r e bonded t o t h e UO;’ ion. Since
T h i s i s
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1.
2.
3.
4.
5.
6.
7.
8.
0.
10.
11.
12.
0x0-CATIOK COMPLEXES. XI11 157
The in’rared. bands f o r \i(v=o) of t h e complexes (2) t o ($) ape
observed i n t h e range 95&?60 an”, which i n a l l p r o b a b i l i t y support
monomeric V=O u n i t in these c h e l s t e ~ ~ ~ . 1 lower t h a n t h e value observed (996 cm- ) for d(,=,) in VO(aczcJ2. The
s l i g h t decrezse in V=O s t r e t c h e s of t h e present vanadyl c h e l a t e s nzy
be due t o t h e s t ronger l igand f i e l d s of t h e S h i f f base H,+fsedien.
The V=O s t r e t c h i n g frequency in t h e 0x0-vanadium(Y) comglex (21, observed a t 935 an”, which i s s l i g h t l y lower t h a n t h o s e observed
f o r u;aloeous 0x0-vanadium( N) complexes. 9 u t t h e d i f f e r e n c e in
oxida t ion s t a t e s of t h e meta: i n t h e s e two types of compound prevents
any meaningful i n t e r p r e t a t ion.
ACKNOWLEDGEMENT
These values ape s l i g h t l y
We thank t h e C S I , New Delhi 2nd t h e CSIR, Kew Delhi f o r f i n a n c i a l
a s s i s t a n c e . We a r e a l s o g r a t e f u l t o t h e Univers i ty of Kalyani f o r
research grant. Analy t ica l s e r v i c e from RSIC, C D R I , Lucknor i s a l s o
acknowled,oed, ! L K . N. is thankfu l t o CSIR f o r a junior resesrch fel lowship.
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Received: 4 February 1991 Accepted: 1 August 1991
R e f e r e e I : K . Edgar R e f e r e e 11: A . Pidcock
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