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N.M. Shavaleev, M.K. Nazeeruddin / Journal of Molecular Structure 1081 (2015) 244–247
Br
Cl
Br
N
N
N
N
a
+ N
Br
N
Cl
Br
Cl
8
OCH3
OCH3
OH
O
P
O
P
c
b
9
10
d
PF6
P O
O
N
N
H3
Scheme 3. Synthesis of H3: (a) neat, room temperature; (b) (i) Mg, chlorodiphenylphosphine, THF, under Ar, room temperature to reflux; (b) (ii) hydrogen peroxide, CH2Cl2,
under air, 0 °C to room temperature; (c) BBr3, CH2Cl2, under Ar, 0 °C to room temperature; (d) (i) 8, K2CO3, DMF, under Ar, 60 °C; (d) (ii) KPF6, room temperature.
that are observed in the synthesis of H1 likely originate from
60
N-alkylation or the N4-to-N1 substitution rearrangement [13] of
H1
the 1,2,4-triazole; however, low temperature and the excess of
base favor the desired O-alkylation of the phenol.
50
40
30
20
10
0
H2
We modified the hosts with an imidazolium cation because it
has high-energy excited states and it is electrochemically-inert
[9] (it is often used to make ionic liquids). The m-substitution in
the ‘‘anisole’’ disrupts the conjugation, while a hexyloxy chain
makes the hosts hydrophobic, increases their solubility in organic
solvents, and minimizes interaction of the imidazolium cation with
the core of the host.
The hosts were purified by chromatography and by recrystalli-
zation. They were characterized by elemental analysis and by 1H
and 31P NMR spectroscopy. Their ESI+ mass-spectra display the
cation {MÀPF6}+. The purity of the ionic hosts is not likely to be a
limiting factor in solution-processed organic electronics devices
that use polymers or charged metal complexes, which themselves
cannot be vacuum-processed by sublimation [8].
ε
260
280
300
320
340
360
Wavelength [nm]
Fig. 1. Absorption spectra of H1 (1.36 Â 10À4 M) and H2 (9.98 Â 10À5 M) in
dichloromethane.
The hosts are white solids. They are soluble in polar organic sol-
vents and have absorption cut-off (optical gap) at short wavelength
(high energy) at 330 nm (30,300 cmÀ1) for H1 and at 355 nm
(28,200 cmÀ1) for H2 in dichloromethane (Fig. 1 and Table 1).
Replacement of the 1,2,4-triazole with the carbazole chromophore
[3,14] red-shifts the absorption spectrum from H1 to H2.
In cyclic voltammetry (CV), the ionic hosts undergo oxidation
and reduction processes that are irreversible at scan rates of 0.1–
1 V/s in acetonitrile on glassy-carbon electrode (Fig. 2 and Table 1).
The redox irreversibility in the CV experiment does not necessarily
mean that the host will not function in the device.
The oxidation process is localized on the ‘‘anisole’’ fragment of
H1 and on the ‘‘anisole-carbazole’’ of H2 [3,8]; the reduction—on
the 1,2,4-triazole of H1 [2] (it is accompanied by adsorption on
the electrode) and on the phosphineoxide of H2 [4–7]. Unlike the
previously reported hole-transport ionic host that exhibits reduc-
tion at 0.77 V but no oxidation to À2.7 V against ferrocene [8],
the new ionic hosts exhibit both the reduction and the oxidation
and, therefore, are probably ambipolar, that is, they may support
the transport of both the electrons (through the 1,2,4-triazole [2]
Table 1
Absorption and redox properties.
a
kabs/nm (
e
/103 MÀ1 cmÀ1
)
E
ox/Vb
E
red/Vb
H1
H2
272 (25)
1.44
1.28
<(À2.5)
À2.75
254 (58), 278 (57), 327 (3.8), 341 (2.6)
a
See Fig. 1. In dichloromethane at room temperature. At 250–500 nm. Errors:
2 nm; 5%.
See Fig. 2. Irreversible processes. At scan rates of 0.1–1 V/s in acetonitrile with
kabs
b
,
e,
0.1 M NBu4PF6 on glassy-carbon working electrode. Peak potentials are reported
relative to the ferrocene couple at 0.1 V/s.
and the phosphineoxide [4–7]) and the holes (through the ‘‘ani-
sole’’ and the carbazole [3,8]). In fact, the neutral analogs of H2
are known to be ambipolar hosts [5–7].
The redox gap (
D
ER = Eox À Ered; >3.94 V for H1; 4.03 V for H2)
and optical gap (>28,200 cmÀ1) of the new hosts are large enough
for blue-fluorescent emitters; however, these parameters may need