Production of Synthetic Nuclear Melt Glass

Joshua J. Molgaard; John D. Auxier II; Andrew V. Giminaro; Colton J. Oldham; Jonathan Gill; Howard L. Hall

doi:10.3791/53473

JoVE Journal > Engineering

Ingenieurwesen

Production of Synthetic Nuclear Melt Glass

Published: January 04, 2016

doi:

10.3791/53473

Joshua J. Molgaard¹, John D. Auxier II^2,3, Andrew V. Giminaro^2,3, Colton J. Oldham², Jonathan Gill², Howard L. Hall^2,3,4

¹Department of Physics and Nuclear Engineering,United States Military Academy, ²Department of Nuclear Engineering,University of Tennessee, ³Radiochemistry Center of Excellence (RCoE),University of Tennessee, ⁴Institute for Nuclear Security,University of Tennessee

Summary

A protocol for the production of synthetic nuclear melt glass, similar to trinitite, is presented.

Abstract

Realistic surrogate nuclear debris is needed within the nuclear forensics community to test and validate post-detonation analysis techniques. Here we outline a novel process for producing bulk surface debris using a high temperature furnace. The material developed in this study is physically and chemically similar to trinitite (the melt glass produced by the first nuclear test). This synthetic nuclear melt glass is assumed to be similar to the vitrified material produced near the epicenter (ground zero) of any surface nuclear detonation in a desert environment. The process outlined here can be applied to produce other types of nuclear melt glass including that likely to be formed in an urban environment. This can be accomplished by simply modifying the precursor matrix to which this production process is applied. The melt glass produced in this study has been analyzed and compared to trinitite, revealing a comparable crystalline morphology, physical structure, void fraction, and chemical composition.

Introduction

Concerns over the potential malicious use of nuclear weapons by terrorists or rogue nations have highlighted the importance of nuclear forensics analysis for the purpose of attribution.¹ Rapid post-detonation analysis techniques are desirable to shorten the attribution timeline as much as possible. The development and validation of such techniques requires realistic nuclear debris samples for testing. Nuclear testing no longer occurs in the United States and nuclear surface debris from the testing era is not readily available (with the exception of trinitite – the melt glass produced by the first nuclear test at the trinity site) and therefore realistic surrogate debris is needed.

The primary goal of the method described here is the production of realistic surrogate nuclear debris similar to trinitite. Synthetic nuclear melt glass samples which are readily available to the academic community can be used to test existing analysis techniques and to develop new methods such as thermo-chromatography for rapid post-detonation analysis.² With this goal in mind the current study is focused on producing samples which mimic trinitite but do not contain any sensitive weapon design information. The fuel and tamper components within these samples are completely generic and the comparison to trinitite is based on chemistry, morphology, and physical characteristics. The similarities between trinitite and the synthetic nuclear melt glass produced in this study have been previously discussed.³

The purpose of this article is to outline the details of the production process used at the University of Tennessee (UT). This production process was developed with two key parameters in mind: 1) the composition of material incorporated into nuclear melt glass, and 2) the melting temperature of the material. Methods exist for estimating the melting temperature of glass forming networks⁴ and these techniques have been employed here, along with additional experimentation to determine the optimal processing temperature for the trinitite matrix.⁵

Alternative methods for surrogate debris production have been published recently. The use of high power lasers has the advantage of creating sufficiently high temperatures to cause elemental fractionation within the target matrix.⁶ Porous chromatographic substrates have been used to produce small particles similar to fallout particles using condensed phase methods⁷. The latter method is most useful for producing particulate debris (nuclear fallout) and has been demonstrated with natural metals. The advantages of the method presented here are 1) simplicity, 2) reproducibility, and 3) scalability (sample sizes can range from tiny beads to large chunks of melt glass). Also, this method is expandable both in terms of production output and variety of explosive scenarios covered, and it has already been demonstrated using radioactive materials. A sample has been successfully activated at the High Flux Isotope Reactor (HFIR) at Oak Ridge National Laboratory (ORNL). Natural uranium compounds were added to the matrix prior to melting and fission products were produced in situ by neutron irradiation.

Methods within the glass making industry and those employed for the purpose of radioactive waste immobilization⁸ have been consulted in the development of the method presented here. The unique effects of radiation in glasses are of inherent interest⁹ and will constitute an important area of study as this method is further developed.

The method described below is appropriate for any application where a bulk melt glass sample is desired. These samples most closely resemble the material found near the epicenter of a nuclear explosion. Samples of various sizes can be produced, however, methods employing plasma torches or lasers will be more useful for simulating fine particulate debris. Also, commercial HTFs do not reach temperatures high enough to cause elemental fractionation for a wide range of elements. This method should be employed when physical and morphological characteristics are of primary importance.

Protocol

Caution: The process outlined here includes the use of radioactive material (e.g., Uranium Nitrate Hexahydrate) and several corrosive substances. Appropriate protective clothing and equipment should be used (including a lab coat, gloves, eye protection, and a fume hood) during sample preparation. In addition, laboratory areas used for this work should be monitored regularly for radioactive contamination.

Note: The chemical compounds needed are listed in Table 1. This formulation was developed by examining previously reported compositional data for trinitite.¹⁰ The mass fractions reported here were determined by averaging the mass fractions for several different trinitite samples.¹⁰ The "missing" mass (the fractions to not sum to unity) exists to allow for some flexibility when adding fuel, tamper, and other constituents. Our independent analysis of several trinitite samples suggests that quartz is the only mineral phase surviving in trinitite.⁵ Therefore, quartz is the only mineral included in our Standard Trinitite Formulation (STF). Although relic grains of other minerals have been reported in trinitite,¹¹ these tend to be the exception, rather than the rule. In general, quartz is the only mineral found in the melt glass.^10,12 Also, quartz sand is a common component of asphalt and concrete which will be important in the formation of urban nuclear melt glass.

Averaged Trinitite Data		Standard Trinitite Formulation (STF)
Compound	Mass Fraction	Compound	Mass Fraction
SiO₂	6.42×10^-1	SiO₂	6.42×10^-1
Al₂O₃	1.43×10^-1	Al₂O₃	1.43×10^-1
CaO	9.64×10^-2	CaO	9.64×10^-2
FeO	1.97×10^-2	FeO	1.97×10^-2
MgO	1.15×10^-2	MgO	1.15×10^-2
Na₂O	1.25×10^-2	Na₂O	1.25×10^-2
K₂O	5.13×10^-2	KOH	6.12×10^-2
MnO	5.05×10^-4	MnO	5.05×10^-4
TiO₂	4.27×10^-3	TiO₂	4.27×10^-3
Total	9.81×10^-1	Total	9.91×10^-1

Table 1. List of chemical compounds.

1. Preparation of the STF

Note: Equipment needed includes a microbalance, metal spatulas, a ceramic mortar and pestle, a chemical fume hood, latex gloves, a lab coat, and eye protection.

Mixing of non-radioactive components
1. Acquire at least 65 g of quartz sand (SiO₂), 15 g of Al₂O₃ powder, 10 g of CaO powder, 2 g of FeO powder, 2 g of MgO powder, 2 g of Na₂O powder, 7 g of KOH pellets, 1 g of MnO powder and 1 g of TiO₂ powder (compounds listed in Table 1).
2. Use a microbalance and small spatula to precisely measure the mass fractions of each compound as listed in Table 1. For best results prepare 100 g of the non-radioactive precursor matrix at one time.
3. Use a mortar and pestle to pulverize (to ~10-20 µm size granules) and thoroughly mix the compounds, forming a homogenous powder mixture containing 64.2 g of SiO₂, 14.2 g of Al₂O₃, 9.64 g of CaO, 1.97 g of FeO, 1.15 g of MgO, 1.25 g of Na₂O. 6.12 g of KOH, 0.0505 g of MnO, and 0.427 g of TiO₂.
4. Agitate the mixture, using a ball mixer, shortly before the next step is taken.
Mixing of STF with Uranium Nitrate Hexahydrate (UNH)
1. Acquire at least 1 g of UNH.
2. Inside a fume hood, pulverize a few UNH crystals (using a mortar and pestle) to form a fine powder of 1-2 µm granules.
3. Add 33.75 µg of UNH per gram of the non-radioactive precursor matrix (this ratio is appropriate for simulating a simple weapon with a yield of 1 kiloton).¹³
4. Thoroughly mix the powder mixture, including the UNH, using a mortar and pestle. Complete final mixing shortly before the melting step.

2. Production of 1-gram Melt Glass Sample

Note: Equipment needed includes an HTF rated at 1,600 °C or higher, high purity graphite crucibles, long stainless steel crucible tongs, heat resistant gloves, and eye protection. Heat resistant gloves and eye protection should be worn when introducing or removing samples from the furnace. Tinted safety goggles (or sun glasses) are useful as they reduce the glare from the furnace.

Production of a non-radioactive sample
1. Fill a thick ceramic dish (such as a mortar) with ~100 g of pure quartz sand and maintain at RT near the location of the furnace where the samples will be melted.
2. Preheat the HTF to 1,500 °C.
3. Carefully measure 1.00 g of the non-radioactive powder mixture and place the powder in a high purity graphite crucible.
4. Carefully place the crucible in the heated HTF (using a long pair of steel crucible tongs) and melt the mixture for 30 min.
5. Remove the sample (again using the tongs) and pour the molten sample into the mortar filled with sand.
6. Allow the glass bead to cool for 1-2 min before handling.
7. Polish the bead to remove residual sand (if necessary).
Production of a radioactive sample
1. Repeat steps 2.1.1 and 2.1.2 above.
2. Carefully measure 1.00 gram of the radioactive powder mixture (including UNH) and place the powder in a high purity graphite crucible using a separate spatula and microbalance to avoid cross contamination.
3. Repeat steps 2.1.4 – 2.1.6 above.
4. Monitor the area around the furnace (using a hand-held radiation detector and/or swipe assays) to check for radioactive contamination.

3. Sample Activation

Note: The equations that follow were derived assuming the use of weapons grade (enriched) uranium metal. The quantities of UNH or Uranium Oxide will need to be scaled according to the mass fraction of elemental uranium and the level of ²³⁵U enrichment.

Activation of a Melt Glass Sample with Uranium Fue
1. Calculate the mass fraction of uranium metal required for the sample using the equation below¹³ (where m_U represents the uranium mass fraction and Y represents the weapon yield):
2. Optional: Calculate the mass fraction of tamper (e.g., natural uranium, lead, tungsten) using the equation below:¹³
3. Calculate the target number of fissions in the sample using the following equation¹³ where M_s represents the mass of the sample in grams and N_f represents the number of fissions produced in the sample during irradiation:
4. Calculate the required irradiation time using the equation below¹³ where m₂₃₅ represents the ²³⁵U mass fraction (enrichment level) and t_irr is the irradiation time in seconds:
5. Irradiate the sample for t_irr seconds at a thermal neutron flux of 4.0 x 10¹⁴ n/cm²/sec. For example, a 60 sec irradiation in Pneumatic Tube 1 (PT-1) at HFIR (with a thermal to resonance ratio of 35) will produce approximately 1.1 x 10¹¹ fissions in a sample containing 870 µg of UNH (equivalent to 410 µg of natural uranium, or 3.0 µg of ²³⁵U). This has been accomplished for one 0.433 g glass bead designed to simulate a melt glass sample produced by a weapon with a 0.1 kiloton yield. This sample has been thoroughly analyzed by Cook et al.¹⁴
6. Follow applicable safety protocols for handling the radioactive sample post-irradiation.
Activation of a Melt Glass Sample with Plutonium Fuel (Planning Factors)
1. Calculate the mass fraction of plutonium metal required for the sample using the equation below¹³ where m_Pu represents the plutonium mass fraction and Y represents the weapon yield:
2. Repeat Steps 3.1.2 and 3.1.3 above.
3. Determine the irradiation time required to obtain the desired number of fissions in the melt glass sample. This time will depend on the composition and grade of the plutonium as well as the neutron energy spectrum.

Note: Great care should be taken when dealing with plutonium and additional analysis will be required. As of this writing, only uranium has been used in the synthetic melt glass samples produced at UT and irradiated at HFIR.

Representative Results

The non-radioactive samples produced in this study have been compared to trinitite and Figures 1-3 show that the physical properties and morphology are indeed similar. Figure 1 provides photographs that reveal the similarities in color and texture which are observed at the macroscopic level. Figure 2 shows Scanning Electron Microscope (SEM) Secondary Electron (SE) images which reveal similar features at the micron level. SEM analysis was performed using a SEM and SEM software. Numerous voids are observed in both trinitite and synthetic samples. The defects and heterogeneity are similar in both as well. Figure 3 provides a comparison of Powder X-Ray Diffraction (P-XRD) spectra for trinitite and synthetic samples. P-XRD analysis was performed on trinitite and synthetic melt glass samples using a X-ray diffractometer with a 3D detector. The x-ray source was a Cu anode set at 40 mA and 45 kV. A slit window of 1/4° 2θ was used along with a 1/8° 2θ anti-scatter diffraction grating. All samples were measured using a silicon (001) no-background sample holder and were set to spin at 4 revolutions/sec. All spectra were acquired from 10° 2θ to 100° 2θ. Quartz is the only mineral present in both cases, and the peak intensities are similar, suggesting a comparable degree of amorphousness³. These results are consistent with previous studies of trinitite^15,16,12,17and other types of nuclear melt glass.^18,19

Figure 1. Macroscopic comparison of trinitite and synthetic nuclear melt glass. (A) Photograph showing the top surface of a trinitite sample, (B) Photograph showing the top surface of a synthetic nuclear melt glass sample produced at UT, (C) Photograph showing the internal structure (cross sectional view) of a trinitite sample, (D) Photograph showing the internal structure of a synthetic nuclear melt glass sample. Please click here to view a larger version of this figure.

Figure 2. Microscopic comparison of trinitite and synthetic nuclear melt glass. SEM images showing the details of the microstructure of trinitite (top images) and synthetic nuclear melt glass (bottom images). Please click here to view a larger version of this figure.

Figure 3. Crystalline morphology of trinitite and synthetic nuclear melt glass. P-XRD spectra of trinitite (blue line) and synthetic nuclear melt glass (red line). The vertical, dashed green lines represent the locations of peaks typically associated with quartz. Please click here to view a larger version of this figure.

Discussion

Note regarding steps 1.2.2 and 1.2.3: The exact amount of UNH will vary depending on the scenario being simulated. The planning formulas developed by Giminaro et al. can be used to choose the appropriate mass of uranium for a given sample¹³ as discussed in the "Sample Activation" section of this paper. Also, Uranium Oxide (UO₂ or U₃O₈) may be used in place of UNH, if available, and the mass fraction of ²³⁵U in the compound (whether UNH or Uranium Oxide) must be considered. For the experiments discussed here the UNH was mixed homogeneously within the precursor matrix. It is anticipated that the melting process will affect the distribution of uranium and other elements within the glass. Qualitatively, the glass appears to be heterogeneous. However, fission track mapping post-irradiation was not conducted to fully analyze the distribution of uranium and fission products within the glass. This is a potential topic for a future study.

Quartz is the only mineral included in the precursor powder matrix because it is the only mineral expected to survive the melting process.^3,10,12 The quantity of quartz remaining in the melted samples serves as a monitor to optimize the melting temperature and time in the furnace⁵. It is assumed that a method which produces the appropriate degree of amorphousness in a sample initially containing quartz will produce a similarly amorphous sample when other minerals are included in the precursor.

One radioactive sample produced in this study was activated by neutron irradiation at HFIR. The uranium fuel content and irradiation times can be calculated based on uranium significant quantities reported by the International Atomic Energy Agency²⁰ as well as early calculations by Glasstone and Dolan²¹ regarding the relationship between weapon yield and the mass of melt glass produced by a nuclear detonation. These concepts are consolidated in the analysis of Giminaro et al.¹³. Analysis of the one activated sample was conducted by Cook et al.¹⁴

The novel method outlined here can be used to produce synthetic "trinitite" samples and then can be extended to other scenarios of forensic interest (e.g., urban nuclear melt glass). Previous efforts to produce surrogate nuclear debris have focused on the chemical and radioactive properties of the glass.²² The focus of the work presented here is the production of a surrogate with accurate physical, chemical, and morphological features. This method is unique in that it makes use of rapid heating in a furnace followed by rapid cooling at RT. There is no ramp-up or ramp-down phase and no mixing during the melting process. The resulting defects (e.g., cracks and voids) and heterogeneities are desirable (as a close match to trinitite). In addition, the protocol outlined here is relatively simple (compared to methods using plasmas or lasers⁶) and yet the results are reasonably accurate and reproducible³.

The HTF used in this study is designed to perform best when a gradual "ramp up" and "ramp down" period is employed during heating. However, for this method a gradual cool down phase is not desirable as recrystallization may occur, destroying the amorphous nature of the sample. For this reason samples produced in this study were introduced after the furnace was brought up to peak temperature and then removed and cooled rapidly outside of the furnace. This required that the furnace door be opened twice while the furnace was at peak temperature (which is not recommended by the manufacturer). This process tends to stress the heating elements and may adversely affect their longevity. This risk was acceptable for our purposes. However, the sample introduction process should be carefully considered and potentially modified, depending on the particular equipment used and the desired end product. Other limitations of this method are discussed in the following paragraphs.

The use of graphic crucibles introduces some carbon contamination into the synthetic melt glass samples (due to the tendency for graphite to volatilize at high temperatures). This contamination may be removed by polishing, post-synthesis, or the samples may be broken and only the "clean" half retained for analysis. The carbon contamination is usually localized near the bottom of the glass bead. Using graphite crucibles in open air also leads to an uncontrollable (and thus unknown) reduction/oxidation state. Iron will likely be oxidized and Fe/C alloys may be produced. For this reason other types of crucibles have been tested including platinum and zirconium oxide, however, graphite remains the best option in spite of the potential carbon contamination and Fe/C coupling issues. Silica and platinum bonding make the platinum crucibles impractical. Zirconium oxide cracks during the quenching process. Further study may reveal a better choice, but as of this writing graphite is the most economical and experimentally practical choice. There are various ways to control the environment within the furnace (e.g., filling a tube furnace with argon) and these should be explored in the future. For the experiments discussed here the environment within the furnace was not manipulated and yet the key characteristics of the glass samples produced were appropriate for their purpose. It should be noted that the environment existing near ground zero during a nuclear detonation is not well understood.

Irradiating samples in the Pneumatic Tube system at HFIR introduces some error in the radioactive properties of the surrogates. This error arises due to the distinct difference between nuclear weapon and reactor neutron energy spectra. The fission product spectrum will thus be characteristic of a reactor (produced by a thermal neutron spectrum) rather than a weapon (produced by a fast neutron spectrum). In addition, the ratio of fission to activation products will be inaccurate when both are produced by irradiation in situ. Studies are ongoing to better understand and possibly counteract this effect.²³ Altering the chemistry of the precursor matrix may be necessary.

The method outlined here will produce a nuclear melt glass surrogate which is accurate in terms of color, texture, porosity, microstructure, mineral morphology, compositional heterogeneity, and degree of amorphousness. There are essentially three key steps to successfully replicate the results presented here: 1) carefully prepare the STF powder according to specifications, 2) safely and quickly heat the powder to a high temperature (well above the melting point of the matrix), and 3) cool rapidly (quench) to avoid recrystallization. It is important to note, however, that identical procedures will not produce identical samples and this is perfectly acceptable as the same is true for real nuclear melt glass (trinitite samples exhibit a high degree of variability as well).³

The most critical steps in the protocol are steps 1.1.1 through 2.1.6. Following these steps will lead to the production of a non-radioactive sample with the desired properties. A radioactive sample may be produced by following essentially the same steps with additional caution due to the hazard associated with radioactive materials.

This method will be used in the future to produce urban nuclear debris surrogates¹³ and may be expanded further. The potential also exists to employ this method in the study of radioactive waste immobilization which is important to the future of the nuclear power industry.

Offenlegungen

The authors have nothing to disclose.

Acknowledgements

Portions of this study have been previously published in the Journal of Radioanalytical and Nuclear Chemistry.^3,13 A patent is pending for this method.

Materials

High Temperature Furnace (HTF)	Carbolite	HTF 18	1800C HTF used to melt samples
High Temperature Drop Furnace	CM Inc.	1706 BL	1700C Drop Furnace used to melt samples
Graphite Crucibles	SCP Science	040-060-041	27 mL high purity graphite crucibles (10 pack)
Crucible Tongs	Grainger	5ZPV0	26 in, stainless steele tongs for handling crucibles
Heat Resistent Gloves	Grainger	8814-09	Gloves used to protect hands from heat during sample intro/removal
Mortar & Pestle	Fisherbrand	S337631	300 mL, Ceramic mortar and pestle for powdering and mixing
Micro Balance	Grainger	8NJG2	220g Cap, high precision scale for measuring powder mass
Spatulas	Fisherbrand	14374	Metal spatulas for measure small quantities of powder
SiO₂	Sigma-Aldrich	274739-5KG	Quartz Sand CAS Number: 14808-60-7
Al₂O₃	Sigma-Aldrich	11028-1KG	Aluminum Oxide Powder CAS Number: 1344-28-1
CaO	Sigma-Aldrich	12047-2.5KG	Calcium Oxide Powder CAS Number: 1305-78-8
FeO	Sigma-Aldrich	400866-25G	Iron Oxide Powder CAS Number: 1345-25-1
MgO	Sigma-Aldrich	342793-250G	Magnesium Oxide Powder CAS Number: 1309-48-4
Na₂O	Sigma-Aldrich	36712-25G	Sodium Oxide Powder CAS Number: 1313-59-3
KOH	Sigma-Aldrich	278904-250G	Potasium Hydroxide Pellets CAS Number: 12030-88-5
MnO	Sigma-Aldrich	377201-500G	Manganese Oxide Powder CAS Number: 1344-43-0
TiO₂	Sigma-Aldrich	791326-5G	Titanium Oxide Beads CAS Number: 12188-41-9

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Molgaard, J. J., Auxier II, J. D., Giminaro, A. V., Oldham, C. J., Gill, J., Hall, H. L. Production of Synthetic Nuclear Melt Glass. J. Vis. Exp. (107), e53473, doi:10.3791/53473 (2016).