Polynitrogen & High Nitrogen Chemistry:
A New World of Challenges
March 25, 2004
Cal State University, Fullerton
Ashwani Vij
Research Scientist
AFRL/PRSP
Air Force Research Laboratory
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Polynitrogen and High Nitrogen Chemistry: A New World of Challenges
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5d. PROJECT NUMBER
Ashwani Vij
DARP
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A205
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Air Force Research Laboratory (AFMC),AFRL/PRS,5 Pollux
Drive,Edwards AFB,CA,93524-7048
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The original document contains color images.
14. ABSTRACT
Polynitrogen compounds contain only nitrogen atoms and are expected to have unusual properties. Most
important among these are High endothermicity šGreenŠ propellant šcombustionŠ product is only
gaseous N2 High density High Isp values when compared to other monopropropellants or bipropellants
High detonation velocity
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ABSTRACT
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84
Standard Form 298 (Rev. 8-98)
Prescribed by ANSI Std Z39-18
Why Polynitrogen Compounds ?
•
Polynitrogen compounds contain only nitrogen atoms and
are expected to have unusual properties. Most important
among these are:
•
High endothermicity
•
“Green” propellant
“combustion” product is only gaseous N 2
March 25, 2004
•
High density
•
High Isp values when compared to other
monopropropellants or bipropellants
•
High detonation velocity
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2
Predicted Specific Impulse (s) Values
for Neutral Polynitrogen Compounds
500
Monopropellants
Specific Impulse (s)
450
400
350
Bipropellants
Blended
Monopropellants
300
Standard Propellants
AFRL In Development
AFRL In Research
250
200
Po
Hy
NT
Pe
Nit
Nit
rox
dra
rat
rat
O/M
lyn
e
eb
i
itro
zin
de
MH
ble
len
e
/MM
ge
n
d
d2
n
H
1
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3
Polynitrogen Program Objectives
Discover, synthesize, characterize, and scale-up
novel, highly energetic polynitrogen compounds
Technical Approach:
• Exploit synergism between theory and synthesis
w Use computational expertise to identify the most promising candidates and
predict their properties
w Use experimental expertise to design synthesis approaches, prepare novel
compounds, and characterize products
+
N5 cation
March 25, 2004
−
N5 anion
+
−
N10 (C 3)
N7 anion
N11 cation
• ^^'^X
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Challenge of
Polynitrogen HEDM Synthesis
•
All the energy must come from endothermicity, and sensitivity typically
increases with endothermicity
•
Basis for high energy content is the large differences in bond energies
Carbon bond enthalpies
C−C
85 kcal/mol
C=C
143 kcal/mol
C≡C
194 kcal/mol
(−HC=CH)n− +34
85 + 143
HC ≡CH
194
Nitrogen bond enthalpies
N− N
38 kcal/mol
N= N
N≡ N
100 kcal/mol
226 kcal/mol
(− N= N)n− -88
38 + 100
stable polymers,
unstable monomers
N ≡N
226
unstable polymers,
stable monomer
This is the reason why N-N polymers
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Research Philosophy and
Technical Approach
Initially we preferred catenated over cyclic or polycyclic
compounds
A
+
o^
• Although polycyclic compounds are more energetic due to strain energy,
and some of them have large barriers to decomposition (tetrahedral N 4),
synthetic routes for their preparation are much more difficult
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Polynitrogen for Dummies
What has Thermodynamics and Kinetics
got to do with it ??
Kinetics
Thermodynamics
It is an uphill battle !!
Low Barrier towards
catastrophic
downfall
Pumping in energy into a
polynitrogen species is like
pushing a boulder uphill
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Polynitrogen for Dummies
•
Metastability requires a delicate balancing act !!
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Polynitrogen for Dummies
Avoid a domino effect !!!
Assembling a polynitrogen chain is like assembling metastable dominos with
perfect spacing, without prematurely triggering an unwanted collapse
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Recipe for Synthesizing Neutral
Polynitrogen Compounds
•
Combine a polynitrogen cation with a polynitrogen anion to
form a neutral polynitrogen compound.
N x+
+
Ny
-
N x+y
ONLY TWO STABLE POLYNITOGEN IONS KNOWN TO EXIST
IN BULK
Cation
Anion
+
March 25, 2004
-
N5+ cation
N3- anion
(discovered in 1999, AFRL, Christe)
(discovered in 1890, Curtius)
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Selection of Suitable Starting
Materials for N5 + Synthesis
• Requirements:
Ø Starting fragments must have relatively weak bonds
Ø Must have formal positive charge (first IP of N2 = 359 kcal/mol)
Ø Coupling reaction must be endothermic
Ø Suitable solvent must be used as a heat sink and for stabilization
• Ideal candidate system:
F
N
N
AsF6−
March 25, 2004
+
H
+
N
N
N
-HF
N
N
N
N
AsF6
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+
−
N
11
Synthesis of the N 2F+SbF6− Precursor
• Reduction of N2F4 to N2F2
·
Graphite + AsF5
C12 AsF5
·
2 C12+AsF6− + trans-N2F2
C12 AsF5 + N 2F4
• trans-cis isomerization of N 2F 2:
trans-N2F2 + AsF5
+
−
N2F AsF6 + Na F
T/P
HF
+
N2F AsF6
−
NaAsF6 + cis-N2F2
• Formation of N2F+SbF6−:
cis-N2F2 + SbF5
HF
+
N2F SbF6
−
Aim: Can we cut any steps and decrease the synthesis time?
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trans-cis Isomerization of N 2F2
ü Improved process (only ~10% SbF 5 needed as a catalyst)
room temperature
trans-N2F2 +
N2F+Sb2F11-
SbF5
+
cis-N2F2
4 days
ü Other process:
trans-N2F 2
AlF 3, 45 °C
cis-N2F2
15 hours
ü Catalyst is not consumed and can be reused
ü Gives pure cis-N 2F2 in high yield.
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Actual Synthesis of N5 +AsF6 −
• Reaction system worked as planned:
+
N2F AsF6
−
HF
+
−
+ HN3 → N5 AsF 6 + HF
-78° C
Ø High yield
Ø Only byproducts were 20-40% H 2N3+AsF6−
Ø 2 mmol (0.5 g) scale
• Properties of N5+AsF6 −:
Ø White solid
Ø Sparingly soluble in HF
Ø Marginally stable at 22°C
Ø Highly energetic
Ø Reacts violently with water and organics
Ø Calculated ∆Hf (298°C) = 351 kcal/mol
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Characterization of N 5+AsF 6−
• 14N and 15N NMR spectroscopy
• Low-temperature Raman and IR spectroscopy of normal
and isotopically labeled N 5+
• Normal coordinate analysis
• Mass spectrometry
• Calculations:
Ø Electronic structure and geometry
Ø Vibrational spectra, including isotopic shifts
Ø NMR chemical shifts
Ø Heat of formation
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Vacuum Line Synthesis
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Safer replacements for HN 3
in the N 5+ synthesis
• HN3 is very shock sensitive and frequently explodes in the presence of
fluorinating agents (possible formation of FN 3)
• HN3 can be replaced by insensitive, commercially available (CH3)3SiN3
(TMS azide)
+
−
N2F MF6 + (CH3)3SiN3
SO2
+
−
N5 MF6 + (CH3)3SiF
(M = As, Sb)
• HF solutions of HN 3 generated from NaN 3 and HF are another
alternative to handling HN3 directly
• Use of FEP-double U-tube apparatus to generate HN3 in situ.
AVIOD
METAL VALVES AND CONNECTORS
• N 5+ formation has been demonstrated for both systems in high yield,
and N5SbF6 is now routinely prepared on a 5 g scale
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. 1,..
.
..:
t-
^m^
I
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,
18
Background in Nitrogen Chemistry
Ø HN(SO2F)2 and HN(SO2CF3)2 : Bis(fluorosulfonyl) and
bis(trifluoromethylsulfonayl)imides and their derivatives (Electrophiles)
Ø Synthesis and reactivity of Perfluorovinylamines: RfN-CF=CF2 (fire
retardants, surfactants etc.)
Ø Phosphonitrilic compounds: N3 P3 monomers/prepolymers
Ø Triazenes, Mono- and Dicarbaphosphazenes: N3 CxP3-x and P-C-N
polymers
Ø Sappharenes, Sulfur/Selenium-Nitrogen macrocyclic ring systems.
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Oxidizing Power of N5 +
• The electron affinity of N5+ was determined by examining its ability to
oxidize the following substrates:
First IP of
substrate (eV)
N5+SbF6− + NO
NO +SbF6− + 2.5 N2
9.26
N5+SbF6− + NO 2
NO2+SbF6− + 2.5 N2
9.75
N5+SbF6− + Br 2
Br2+SbF6− + 2.5 N2
10.52
N5+SbF6− + Cl 2
Cl2+SbF6− + 2.5 N2
11.48
N5+SbF6− + O 2
O2+SbF6− + 2.5 N2
12.07
Xe2+SbF6− + 2.5 N2
12.13
N5+SbF6− + 2 Xe
• N 5+ is a weaker oxidizer than PtF 6, which can oxidize O 2 to O 2+.
+
also a weaker oxidizer than O 2 , which can oxidize Xe to Xe2
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+
It is
20
Electron Affinity of N 5+
• Electron affinity (EA) of N 5+ needed for stability predictions of new N 5+
salts using Born-Haber cycles
• EA of an oxidizer equals the IP of the substrate for gas-phase reactions;
when solids are involved, lattice energy changes must be included
N5+ SbF6-(s)
+
UL
N5 SbF6
+119
N5+(g)
+ SbF6-(g)
ElAff
N5 +(g)
N5 (g)
Br2(g)
∆Hr ≤ 0
Br 2+SbF6-(s)
+
N5(g)
0
+
0
+ SbF 6-(g)
Br 2(g)
1.IP
Br2
+
+242
UL
Br2 +SbF6 -
-125
0
Br 2+(g)
• The EA of N5+ falls between 236 and 255 kcal/mol (10.24 – 11.05 eV); it is
a powerful one-electron oxidizer that neither fluorinates nor oxygenates
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The Taming of N 5+SbF 6−
• Desired a more stable N5+ salt
• Prepared N5+SbF6−:
+
HF
−
N2F SbF 6 + HN3 → N5+SbF6− + HF
-78°C to RT
• Properties of N5+SbF6−:
Ø White solid
Ø Stable to 70°C
Ø Obtained in high purity
Ø Does not explode at 150 kg•cm (impact sensitivity test)
Ø Exhibits all the still missing vibrational bands with the predicted frequencies
Ø Soluble in SO2, SO2ClF, and HF
Ø Are preparing it routinely on a 5 g scale
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Raman Spectrum of N 5+SbF6−
ZHKf
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2nn
too
1D00
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Infrared Spectrum of N 5+SbF 6−
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Vibrational Assignments for N 5+
Observed
Calculated
IR
Raman
B3LYP/
6-311+G(2d)
2268
2268
2236
2229
ν1 (A1)
2205
2205
2282
2175
ν7 (B1)
1167
1032
872
850
818
ν2 (A1)
672
678
644
ν3 (A1)
478
502
475
ν5 (A2)
424
405
ν6 (B1)
414
436
399
ν9 (B2)
204
193
181
ν4 (A1)
1090
1055
873
Fermi
Resonance
425
412
March 25, 2004
CCSD(T)/
6-311+G(2d)
Assignment
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ν3 (A1) + ν9 (B2)
ν8 (B2)
25
Geometry of the N 5+ Cation
112º
N
167º
1.11Å
Calculated Structure
N
(+)
(+)
(-)
..N
(-)
N
N
N..
(+)
N
..
N
..
N
..
(+)
..
1.30 Å
..
N
..
V-Shaped Geometry
Resonance Structure
1.302 Å
111.2º
168.1º
1.107Å
Experimental Structure
Vij, Wilson, Vij, Tham, Sheehy & Christe,
J. Am. Chem. Soc., 2001,123, 6308-6313
N2 makes contacts at 2.723 and 2.768 Å
N4 contacts are at 2.887 and 2.814 Å
C&E News, 2000, 78, 41
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Synthesis of New, More Energetic
N5+ Salts
•
Salts with Energetic Counterions – N5+N3−
ØDesired Metathesis:
N5SbF6 + CsN3
SO2
-64°C
N5N3 + CsSbF6
ØObtained Products
CsSbF6 + 4 N2 +
ØBorn-Haber Cycle Shows that Stabilization of N 5+N3− Requires a
Minimum Lattice Energy of 183 ± 20 kcal/mol, but Estimated U L for N5+N3−
Is only 130 kcal/mol
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Unexpected complexation of SO2 with
the azide ion in CsN3
Structure shows novel
SO2N3 as well as
SO3N3 groups
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Synthesis of New, More Energetic
N5+ Salts
•
Salts with Energetic Counterions – N5+NO 3−
ØDesired Metathesis:
SO2
N5SbF6 + CsNO3
N5NO 3 + CsSbF6
-64 to 20°C
ØDid Not Proceed because CsNO 3 Is Less Soluble in SO 2 than CsSbF6
ØUL Required for Stabilization Is 154 kcal/mol; Estimate for N 5NO3
Is 129 kcal/mol
•
Salts with Energetic Counterions – N5+ClO 4−
ØDesired Metathesis Resulted in:
N5SbF6 + CsClO4
HF
-78°C
NO +ClO4− + CsSbF6 + N 2
ØUL Required for Stabilization Is 138 kcal/mol; Estimate for N 5ClO4
Is 125 kcal/mol
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Synthesis of more energetic N5+ salts, and
estimated energy content of N 5+N3−
•
Heat of Formation of N 5+N 3−
Ø∆Hf (298) of N 5+(g) = 351 kcal/mol
(Calculated Value)
Ø∆Hf (298) of N 3−(g) = 43.2 kcal/mol
(NBS Tables)
ØLattice Energy of N5+N3− ≈ 130 ± 20 kcal/mol
(Christe Estimate)
So ∆H f (298) of N 5+N 3− = 351 + 43 – 130 = 264 ± 25
kcal/mol
•
Energy Density of N 5+N 3−(s) = 2.36 kcal/g
•
Comparison with Other Molecular Systems (kcal/g):
O3
C(N 3)3+N(NO 2) 2−
HN 3
N 5+N3−
H 2/O 2
0.71
1.42
1.63
2.36
3.21
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Synthesis of new N 5+ salts
N5B(CF3)4
•
N 5SbF 6 successfully converted to N 5B(CF3)4 by metathesis in SO 2
solution
N5SbF 6 + KB(CF3)4
•
SO2
-64°C
N5B(CF3)4 + KSbF6
N 5B(CF3)4 Is a white solid, stable at room temperature
Ø Characterized by mass balance
Ø Characterized by vibrational spectroscopy
Ø Characterized by
14N, 11B,
and
13C
NMR
Ø Indefinitely stable in HF solution at room temperature with no
decomposition products nor any unidentified species
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(In)Compatability of N5 +
Conclusion……Attempts to couple N 5+ with
energetic anions may result in explosive
reactions !!!
March 25, 2004
N5+N3-
N5+ClO4-
N5+NO3-
N5+N(NO2 )2-
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Syntheses of new N5 + salts
(N5)2 SnF6 and N5 SnF5
•
Salt with higher N 5+ content (2:1 Cation/Anion Ratio)
2 N 5SbF6 + Cs2SnF 6
•
HF
-78°C
(N5)2SnF6 + 2 CsSbF6
(N 5)2SnF6 marginally stable, but Friction Sensitive with explosive
decomposition
ØWhite solid with double the N 5+ content of N 5SbF6
ØImportant step toward synthesis of salts with “touching” Polynitrogen ions
Intensity
(N 5)2SnF6
_L_Jl
]}:
ztoa
Frequency, cm-1
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Thermal Generation of N 5SnF 5
from (N5)2SnF 6
• Thermolysis of (N5)2SnF6 above room temperature
(N5)2SnF6
•
> 20°C
N5SnF5 + "N5F"
Properties of N5SnF 5
Ø White solid
Ø Stable up to 50-60ºC
Ø Characterized by vibrational and multi-Nuclear Magnetic Resonance
spectroscopy
Ø Contains Sn2F102- and Sn4 F204- anions
•
“N 5F” Unstable
Ø Only decomposition products observed by FTIR and noncondensible
measurements: N 2, trans-N2F2 and NF3
Ø J. Phys. Chem. 2003, .
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w
119
^±p
Sn NMR Spectrum of N5 SnF5
[Sn 4F20 ]
2-
Fax
Fax
Fbr
Feq
Feq
Fax
Fax
Fax
Fbr
Fax
. t.
F eq
F eq
F ax
Feq
Feq
Fax
F br
F eq
Feq
Fbr
Fax
[Sn2 F10 ]
4-
Fbr
Feq
Fbr
F eq
Feq
Feq
F ax
F ax
F ax
Simulated
.1
r^'*5[ir^'«Swr*'^«iE7''TE»*'*«iC^
M._k
Experimental
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Attempted Preparation of the N 7O+
Cation
• Another promising Polynitrogen target ion Is N7 O+ cation.
Ø
Reaction of NOF2SbF6 with HN 3 studied in HF at –78 °C
Ø
N3NOF+SbF6- isolated as white solid stable up to ~ -20 °C
Ø
N3NOF+ exists as both a z- and e-isomer
NOF2+SbF6 - + HN3
- HF
O
N N
F
N3NOF+SbF6- + HN 3
O
N
N
SbF6-
E-isomer
- HF
N
F
Z-isomer
N
N
N
O
x
N3
N
N3
SbF6-
Ø Characterized by vibrational and multi-nuclear resonance
spectroscopy and calculations
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The NOF2+ Cation Case
Due to their similar space requirements and electronic
configurations, oxygen and fluorine ligands in oxofluorides
are frequently disordered, particularly when the central atom
lies on an intramolecular rotation axis.
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The NOF2+ Cation Case….
The Structure of NOF 2+AsF 6-
ü The crystals grown from HF
ü Monoclinic space group P21/n
ü Cell constants: a = 7.513(2) Å , b =
%
8.083(2) Å, c = 10.314(2) Å; β =
107.46(2)º
Y
What is wrong with this structure ??
N-O = 1.190(4) Å
…long!
N-F = 1.245(4), 1.246(4) Å
…short
Angle O-N-F = 122º
…wider
Angle F-N-F = 116º
…narrower
March 25, 2004
ü Z=4
ü R = 0.0372
ü Refined oxygen occupancy
in NOF 2+
cation is 55%
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The disordered NOF2+ cation case….
Extracting the “true” geometry
Bond Length (Å)
1.3
Plot of N-O and N-F distances versus %F occupancy
1.2835
1.25
1.2
.0
y=0
1.15
1.1
RN-O
135
+ 1.1
017x
1. Sums of partial occupancies
for O/F at any site is restricted to
ONE.
1.1135
0
20
40
60
80
% F Occupancy
2. The total O occupancy equals
100
ONE and total F occupancies
equals TWO.
Plot of F-N-O and F-N-F versus %F occupancy
130
Bond Angle (degrees)
Rules for refining occupancies
RN-F
125
126.0
∠ F-N-F
120
y=
∠ F-N-O
115
-0.3
618
Refined Occupancies
x+
144
.12
110
107.9
F/O = 77 and 78%
O/F = 45%
105
50
March 25, 2004
60
70
80
90
100
%F Distribution
Occupancy
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Results of Geometric “Extraction”
Calculated
Experimental
B3YLP/ CCSD(T)/
631+G(2d)*, VTZ
“Apparent”
“Extraction” Method
N-O (Å)
1.129
1.137
1.190(4)
1.114
N-F (Å)
1.312
1.305
1.245(4), 1.246(4)
1.284
O-N-F (º)
125.8
125.6
122.0(3), 122.1(3)
126.0
F-N-F (º)
108.4
108.8
115.9(3)
107.9
3.17, 7.33
3.03, 6.68
R (wR2) (%)
-----
* Gillespie, R. J. et al., Inorg. Chem., 1998, 37, 6884
The analysis demonstrates that the crystal structure of F 2NO+AsF6 -, extracted from an
oxygen/fluorine disordered structure, is in very good agreement with the theoretical predictions
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Factors influencing the stability of
Polynitrogen compounds
? Thermodynamic Factors
1. Electron Affinity of the Cation
?A fixed value, if we aim for a N 5+ salt , i.e., 10.5-11.5 eV
2. First Ionization Potential of the Anion
?The azide ion has a very low value of about 2.1 eV, which is the main
+
-
reason for the instability of N5 N3
?New polynitrogen anions are needed with higher first IP values. N5 - and N7 anions are most promising candidates
3. Lattice Energy of the Crystal
?UL fixed by the molar volumes of cation and anion. Born -Haber cycle
calculations for the lattice energy estimated for N 5+N3- are 50 kcal/mole
lower than the requirement for the stabilization of an ionic salt
? Kinetic Factors
?Low activation energy towards decomposition!
These energy values determine the stability of the individual ions
March 25, 2004
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Polynitrogen Anions
Identification and Synthesis of
Polynitrogen Anions
March 25, 2004
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New Polynitrogen Anions as
Counterparts for N 5+
Heptanitrogen anion (N7-)
•
Theoreticians predict reasonable stability
•
No reports have been published on attempts to prepare
this anion. Work is in progess!
R
H
R Si N
R
H
R
R Si N
R
Cl
M N3
March 25, 2004
Cl TMSN
3
N
R
N3
R Si N
R
N3
+M F
-R3SiF
N3
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New Polynitrogen Anions as
Counterparts for N 5+
Pentazole anion (N5-)
• Theoretical calculations show that this
anion has a 28 kcal/mole activation energy
barrier for decomposition and its
decomposition to N 3- and N2 is only 11
kcal/mol exothermic
N 5Energy
• Free pentazole has not been isolated or
characterized to date. Only aryl substituted
pentazoles can be isolated and stabilized at
low temperatures. These compounds
rapidly decompose above 273K to form aryl
azides and N 2 gas
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28 kcal
11 kcal
N 3- + N 2
44
Identifying Potential Polynitrogen Precursors
This ion has been suggested
as a useful precursor to new
polynitrogen molecules...
... but calculations predict it to be
unstable.
+
NN
C
March 25, 2004
3.21
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Synthetic Challenge – How do we make
These New Anions??
Synthesis of Substituted Pentazoles
Sources for the Pentazole Anion (N 5-)
Silyl Diazonium Salts
Aryl Diazonium Salts
R
R Si N2+
R
+N3R
N
R = electron
releasing group
I. Ugi, Angew
Chem., 1961,
73, 172
+N3-
N
R Si N
N
R
N
Unknown
March 25, 2004
N2+
R
N
R
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N
N
N
N
46
Formation and Stability of Silyl
Diazonium Salts
•
Attempts to synthesize silyl diazonium salts
+
N2F SbF6
-
+ Me3SiSiMe3
-Me3SiF
Me3SiN2+SbF6-
OR
R3SiNH2
•
+ NO+ BF4-
-H2O
R3SiN2+ BF 4-
R3SiN2+ salts are unstable and spontaneously lose
N2
R3SiN2
+
X-
-N2
R3Si+ X-
Theoretical calculations support this experimental observation
March 25, 2004
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Use of Aryl Diazonium Salts –
A Better Bet!
N 2+
R
X
-
+ N3 -
N
R
N
N
N + M+ XN
M+ N5- + R
•
R must be an electron releasing group, i.e., -NMe2, -OH, -OCH 3,
-OC6H5,-O -, etc.
•
Some of these substituted arylpentazoles have been known for about
four decades but no success had been achieved to cleave the N 5
ring from the aryl group
X
Aryl Pentazoles can rapidly lose N 2 at room temperature
N
R
N
N
March 25, 2004
N
N
-N2
R
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N N
N
48
Synthesis of Aryldiazonium Salts
Aqueous Media
R
NH2
NaNO2/HCl
R
< 0 °C
N2+Cl-
NaBF4
R
N2+BF4-
R = H, OH, OCH3, OC 6H5 , OC 6 H4 N2+, N(CH 3 )2
mo
March 25, 2004
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Synthesis of Aryldiazonium Salts…Nonaqueous synthesis
Non-aqueous Media
isoamyl nitrite
R
Ø
NH2
CF3COOH
CH2 Cl2
R
Colas and Goeldner reported that the
p-phenoxydiazonium trifluoroacetate to
be a double salt. However, our results
show no such behavior. In the case of
a double salt, the –OH group can get
protonated which prohibits pentazole
formation!
N2+CF3COO-
N2+CF3COO-. CF3COOH
HO
Colas and Goeldner, Eur. J. Org. Chem. 1999, 1357-1366
March 25, 2004
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Single or Double Diazonium Salt ?
Consequences of Lone Pair Occupation!
We DO NOT find any trifluoroacetic acid double salt. In fact,
such a double salt would kill the pentazole formation
P-1
N2+CF 3COO-. CF3COOH
??
HO
2 ion pairs within the asymmetric unit
March 25, 2004
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Pentazole Formation…
Role of the Substituent Electronic Effects
Me 2N
NH2
i. xs NaNO 2/HCl
~0
°C, ii. NaN
N
H
Me 2N
3
N
N
NO3
N
N
- N2
H
Me 2N
N3
NO3
NaNO2
+
HCl
3 HONO (aq)
March 25, 2004
<0
°C
NaCl
+
HONO
H3O+ + NO3- + 2NO
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52
Identification of Arylpentazoles
Pentazoles can be characterized by low temperature NMR
spectral studies using 15N labeled samples.
N4 N3
•
1H
NMR:
AB-type spectrum with Ha and H b
at 8.0 and 7.0 ppm
•
14N
NMR:
N 1 at ~ -80 ppm
•
15N
NMR:
N 2/N 5 at ~ -27 ppm and N 3/N 4 at ~4
ppm
N5
N1
N2
Ha
Ha
Hb
Hb
R
Note: Qualitative evidence for the presence of a pentazole
ring: N2 gas evolution in solution
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Cleavage of the Aryl-Pentazole Bond
with Retention of the Pentazole Ring
•
Chemical Methods
Ø Ozonolysis does not work! (Ugi, Radziszewski)
V. Benin, P. Kszynski and G. J. Radziszewski, J. Org. Chem., 2002, 67, 1354
Ø Nucleophilic substitution using strong
nucleophiles such as the OH -, OR-, F- etc.
•
Collisional Fragmentation (ElectroSpray Ion Mass
Spectroscopy – ESIMS)
N N
N
Ø Electrospray is very gentle and produces high
concentration of the parent anion which can be mass
selected
Ø Collisional fragmentation of the mass selected anions
with variable collisional energies allow tailoring of
fragmentation
Ø Negative ion detection eliminates interference from
neutral or positively charged species
March 25, 2004
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N
N
Weakest
bond
Nu
R
54
ESIMS of para-Phenoxypentazole
Observed peaks in the MSMS of 162
N
N N
N
N
N
N
N
Low Collison
Voltage
-N 2
-CO
O-
ES
MSMS
O-
N
-N2
High Collison
Voltage
Om/z = 134
m/z = 78
m/z = 106
N N
-C6H4O
N
m/z = 162
N
N
m/z = 70
March 25, 2004
N
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-N2
N3 m/z = 42
55
15 N
N Labeling of the Pentazole Ring
N N
bN
aN
N N
N
bN
aN
R
R
Na
Nb
*N
N
N
R
N N
N
N
Na
N
Net
Structure
R
N N
N
Na
R
March 25, 2004
Nb
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N N
N
Na
Nb
R
56
Is the Peak at m/z 70 indeed due to the
Pentazole Anion?
15N
Observed peaks in the MSMS of 163
Labeled Pentazole
2/5 N
N4 N3
5N
N1
3/4 N
Low Collison
Voltage
N2
ES
MSMS
m/z = 163
15N
N C
-N 2*
N
-CO
O-
m/z = 135/134
O
Om/z = 106
m/z = 78
Labeling experiment shows that CO is
lost in the last step
High Collison
Voltage
statistically distributed
over N2, N 3, N4 & N5
March 25, 2004
or -N2*
N
or -N2
-N 2
Unlabeled
O-
N1
-C6H4O
N
N
N
N
N
m/z = 71
Definitive proof for the pentazole anion
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ESI-MS-MS fragmentation of 4pentazolylphenolate anion at low and high
collision voltages.
V
-10 V
-50 V
1 5N
Labeled
-75 V
Irel
Negat ive ion, f ull- range CI D mass
spect ra of t he mass select ed, 15N
labeled (m/
(m/ z 163) and unlabeled
(m/ z 162) peaks due t o [OC6 H4 N 5 ]–
recorded at collision volt ages of
–75, - 50, and –10 Volt s. All
spect ra are mult i- channel spect ra
and t he t ypical mass resolut ion and
noise level are shown f or t he m/ z
70 and 71 peaks in t he insert s.
-75 V
Unlabeled
C&E News, 2002, 80, 8
m/z
March 25, 2004
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Crystal structure of 4-Hydroxyphenylazide
The thermal decomposition of 4hydroxyphenylpentazole (4-HPP)
results in the loss of N 2 gas and the
formation of 4-hydroxyphenylazide.
The “two” hydrogen atoms present
on the p-oxygen atom are
disordered.
March 25, 2004
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Pentazoles with Heterocyclic
Substituents
•
Tetrazolyl system is unstable above -70 °C and the
pentazole ring rapidly decomposes to liberate N2 gas.
N
N
N
NH2
N
i. NaNO2/HCl
N
ii. -70 °C, LiN3 *
N
H
•
N
N
N
N
N
N
-N2
N
N
N
N
N
N3
N
A. Hammerl and T. M. Klapoetke, Inorg . Chem. 2002, 41, 906-912
In comparison, the pentazole ring derived from 2-amino-4,5dicyanoimidazole shows higher thermal stability (-30 °C)
C
N
NH2
C
N
March 25, 2004
N
H
i. NaNO 2/HCl
N
C
ii. -30 °C, NaN3*
N
N
N
N
N
N
C
N
Na
N
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-N2
C
N
N3
N
C
N
N
Na
60
15 N
NMR of 2-pentazolyl-4,5-dicyanoimidazole
2,5
3,4
N
2
C
N
1
N
N
3
N
C
N
15 N
March 25, 2004
N
N
N
5
4
NMR recorded in a mixture of methanol and acetonitrile at -30 °C,
nitromethane used as an external reference (0 ppm)
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Crystal structure of 2-Diazo-4,5dicyanoimidazole
N-N = 1.096 ?
C-N = 1.334, 1.336 ?
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Does the Pentazolate Anion Exist in
Solution ?
S5
3 is
N
N
2
C
N
N
1
N
N
N
3,4
N
N
2,5
C
N
N
N
5
N
N
3
4
,^iM«» ^ImilfiiLWMlii HiHifillltfrtiihilLiMiry
T
IC
^
1
I
-]
-'-I——
-iB
\
-iJD
1
-at
r—— ^,-1-^—^T
-m
-35
ITpx
#iLUi
Ø
15N
ion.
«HHW
NMR shows a peak at -10 ppm (-30 °C), which slowly decomposes to form N 2 and azide
Ø This peak is also observed upon adding a base to the solution of arylpentazoles at -30 °C.
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High Nitrogen Chemistry
Synthesis, Mechanistic Studies and Structural
Characterization of Binary Metal Azides
March 25, 2004
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Reactions of Group 15 halides with
Trimethylsilylazide
Crystalline binary metal azides were obtained upon reacting
the corresponding metal fluorides with TMSN 3. These
compounds were reported as either liquids or tacky solids by
Klapoetke et al.
MF3
+
Me3SiN3
-Me3SiF
M(N3)3
These solids could be sublimed under vacuum to yield
colorless diffraction quality crystals with no incidents of
explosion or thermal decomposition
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Structure of As(N3 )3
One of the azide groups N7-N8-N9
destroys the C3 symmetry
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Crystal Structure of Sb(N 3)3
All azide groups oriented in a
propeller-like fashion
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Crystal Structure of Sb(N 3)3
View down the three-fold axis, all azide groups equivalent
Example of perfect C 3 symmetry
March 25, 2004
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Crystal Structure of Sb(N 3)3
Sb
N
“Star of David” Perspective
March 25, 2004
“Isle of Man” Perspective
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Reactivity of hexachloroantimonate (VI)
with Trimethylsilylazide
[Ph4M][SbCl6]
+
Me3SiN 3
-Me3SiCl
CH3CN
o
60 C
[Ph4M][SbCl6-x(N 3)x]
M = P, As; x = 2-6
üThe substitution of all the six chlorine atoms in SbCl 6by the azide groups could not be accomplished in a single
step, as reported in literature. The stepwise substitution
gives a good insight into the substitution mechanism.
ü Total substitution was achieved after four “refreshment”
cycles of the reagents. During the intermediate cycles,
the azide content gradually increased from two to five.
March 25, 2004
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Episode I…Generation of the starting
material
Ph 4MCl
+
SbCl5
1,2-DCE
[Ph4M][SbCl6]
M = P, As
Cl
Cl
Cl
Sb
Cl
Cl
Cl
March 25, 2004
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71
Episode II….cis- or trans- disubstitution
with azide groups?
N3
Cl
Cl
Cl
Cl
N3
Cl
Sb
Sb
Cl
Cl
Cl
N3
N3
cis-isomer
trans-isomer
%
%
March 25, 2004
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Episode III…Substitution of 3 rd chlorine…
fac- or mer- isomer ???
Cl
N3
Cl
Cl
Cl
N3
N3
Sb
Sb
Cl
Cl
N3
N3
N3
•
\
•
mer-SbCl 3(N 3)3
March 25, 2004
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fac-SbCl3(N3)3
73
Episode IV…Capturing the “transition
state” during the fourth substitution!
Cl
N3
Cl
Sb
N3
N3
i
N3
Cis- vs. trans- substitution
Cl
N3
Sb
N3
N3
Cl
March 25, 2004
N3
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Chloropentaazidoantimonate(VI) Anion
Cl
N3
Sb
N3
N3
N3
N3
The Structure of Ph 4PSbCl(N 3)5
ü The crystals grown from CH3 CN
ü Triclinic space group P-1
ü Cell constants: a = 11.134(3) Å , b =
11.663(3) Å, c = 13.754(4) Å; α =
104.314(5)º; β = 97.914(5)º; γ =
115.807(4)º
ü Z=2
ü R = 0.0762
ü All azide distances “normal” except
N10-N11-N12
March 25, 2004
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Episode VI…Complete substitution of
chlorine atoms
No crystal structure obtained
yet. However, IR and Raman
spectroscopy shows that Sb-Cl
bonds are absent i.e., complete
substitution by the azide
groups.
March 25, 2004
N3
N3
Sb
N3
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N3
N3
N3
76
Solvent effect in halide substitution
reaction with TMSN3
Using tetrahydrofuran (THF) in place of acetonitrile (AN)
results in the formation of the Sb2OCl62- anion. This
probably results from the ring opening oxidation of THF.
[Ph 4P][SbCl6 ]
March 25, 2004
+
Me 3SiN 3
THF
2[Ph4 P]+ .[Sb 2OCl 6] 2-.SbCl3
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Summary – Polynitrogen Anions
Ø
Synthesized aryl pentazoles: hydroxy group at the paraposition on the aryl ring gives the best results as observed
during this study.
Ø
Demonstrated selective cleavage of C-N bond by ESIMS with
retention of pentazole ring. Results confirmed studying 15N
labeled pentazoles.
Ø
First experimental detection of pentazolate anion.
Ø
Synthesis of pentazoles with a heterocylic substitutents
Ø
Addition of OH- ions to a solution of pentazole suggest C-N
bond cleavage.
Ø
Offers potential pathway for bulk synthesis of N 5- salts
March 25, 2004
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Summary- Polynitrogen Cations
Ø
Use of AlF 3 as an efficient catalyst for the trans-cis isomerization
of N2F2, which is a precursor for the synthesis of N5AsF6 and
N5SbF6.
Ø
Successfully demonstrated conversion of N5SbF 6 into other salts,
such as N5B(CF3)4 and N5SnF5
Ø
Prepared and characterized (N5)2SnF6, thereby doubling the N5+
content of N5SbF6
Ø
Obtained experimental and computational evidence for instability
of N5N3, N5NO3, N5N(NO 2)2 and N5ClO4
Ø
Ø
Ø
Prepared and characterized the N3NOF+ cation
Attempted the preparation of N2(N3)3 + cation
Attempted the preparation of N(N3)4+ cation
March 25, 2004
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Conclusions
Ø
Ø
AlF3 is the best catalyst for the isomerization of trans-N2F2
Ø
Only one fluorine atom in N(O)F 2+ has been replaced with an
azide ion to form the N3N(O)F+ cation
Ø
Ø
Ø
The N2(N3)3+ cation could not be stabilized and isolated
Ø
2-Pentazolyl-4,5-imidazole appears to undergo chemical C-N
bond cleavage. Results are under investigation!
N5+ cation can be stabilized with anions such as B(CF 3)4-, SnF5-,
SnF62-, SbF 6- and Sb2F112- but NOT with N3-, NO3-, ClO 4- and
N(NO2)-
The N(N3)4+ cation could not be stabilized and isolated
Pentazoles with substituents other than the aryl group can be
prepared and stabilized at low temperatures.
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AFRL/USC/UC Coworkers and
Collaborators
Air Force Research Laboratory, Edwards
Dr. Karl Christe, Dr. William Wilson, Ms. Vandana Vij
University of Southern California
Dr. Ralf Haiges
University of California, Riverside
Dr. Fook Tham
University of California, Santa Barbara
Dr. James Pavlovich
March 25, 2004
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Acknowledgments
Dr. Robert Corley, Tech
Dr. Timothy Haddad, NMR
Dr. Rusty Blanski, NMR
Dr. James Pavlovich, UCSB-MS
Dr. Fook Tham, UCR-X-ray
March 25, 2004
Mr. Michael Huggins
Dr. Ronald Channell
Mr. Wayne Kalliomaa
Dr. Don Woodbury
Dr. Arthur Morrish
Dr. Michael Berman
Dr. David Campbell
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BACKUP
March 25, 2004
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General approach for treating disorder
Bond Length
(Arbitrary Units)
Plot of O-X and X-F distances versus %F occupancy
b
1/3(RO-X + 2RX-F)
RX-F
a
½(RO-X + RX-F)
RO-X
0
25
50
75
100
% F Occupancy
Plot of F-X-O and F-X-F angles versus %F occupancy
∠ F-X-O
Bond Angle
(degrees)
360/3º
c
∠ F-X-F
50
60
70
80
90
• For a linear C • v structure,
FXO, midpoint is at 50%
occupancy (plot a)
• For a trigonal C2v species
F2XO, equilibrium point is
weighted for the two types of
atoms i.e., 2F and 1O (plot b)
• Plot c shows equilibrium
bond angles for equal
occupancies for two Fs (2/3)
and O (1/3) i.e., 120 º. Also
angle F-X-O = (1/2)(360angle F-X-F)
100
%F Occupancy
March 25, 2004
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