The Great Step Backwards: Polymer to Monomer

By Hyungjun Cho, member-at-large for the GCI

There is a movement to develop a new type of product life system called ‘the circular economy’ [3]. Part of this movement aims to manufacture products from recycled or raw materials, and after its useful lifetime, re-introduce the product (now considered waste) as recycled material. The motivation for the introduction of the circular economy is to minimize the need for virgin raw material, especially when it originates from non-renewable resources. This effort is being spearheaded by the Ellen MacArthur Foundation with major industry partners like Google, Unilever, Solvay, and Philips, among others [3]. A critical component to the function of the circular economy is developing the capability to turn waste into a desirable product.

There are several methods of recycling all the different types of materials we use in every day life. This blog will discuss a niche in the ‘plastic to monomer’ field. Evidently, in April of 2019, IUPAC named ‘plastic to monomer’ as part of the 10 chemical innovations that could have high impact in society [6]. Before discussing ‘plastic to monomer’, I must clarify the term ‘plastic’. Generally, plastic is made up of many polymer chains that are physically entangled with one another. A macroscopic analogy is when many electrical wires (think of Christmas tree lights) become entangled: the wires are stuck to each other and the rigidity of the ball of wire is greater than the rigidity of a single wire.

Much like the type of wire influences the tangled ball it forms, the chemical structure of the polymer influences the material properties of the plastic. Examples of properties of plastics include rigidity, elasticity, malleability, gas permeability, friction to skin, transparency, and many others. The polymers that are used for commercial plastic products have been studied and developed for decades to be able perform a specific function. For example, polyvinyl chloride and polystyrene were initially discovered in the 1800s [2,8]. Thus, it would be ideal if the currently used polymers can be de-polymerized back into monomers for recycling purposes. This would be a major move by the plastics industry to become environmentally friendly.

The conventional method to turn polymers into monomer is thermal decomposition. Samples of polymer can be heated to high temperature (typically 220-500 °C) to break some of the bonds that hold the monomers together [10]. When this occurs, radicals can form at the site of the broken bond, which can lead to de-polymerization [10]. The required temperature and how much monomer is formed is dependent on the chemical structure of the monomers that are formed. Thermal decomposition to recover monomer is suitable only for a few types of polymers, such as poly(α-methylstyrene), which has ceiling temperature of 66 °C to propagate depolymerization; the monomer recovery after thermal decomposition of poly(α-methylstyrene) is excellent at 95% [11]. However, for polymers like polyethylene (PE, the most produced polymer) and polypropylene (PP, 2^nd most produced polymer), the monomer recovery yield is poor (0.025-2%) [11]. In some cases such as polyvinylchloride (PVC, 3^rd most produced polymer), thermal decomposition is even more problematic because PVC will release harmful hydrochloric acid and vinylenes upon heating [11]. Thus, the monomer recovery is poor (1 %) and the process is highly corrosive.

Therefore, one of the key challenges to address for ‘polymer to monomer’ is to perform de-polymerization at a low temperature. There are 4 recent publications that explore this challenge [5,7,9,12]. In general, the authors synthesized polymers using reversible-deactivation radical polymerization (RDRP) techniques and explored the de-polymerization reactions they encountered. Below is a brief highlight from the publications from the Haddleton group [9] and the Gramlich group [5].

Scheme 1: De-polymerization of RAFT polymers with trithioester end-group [5]. Reproduced from ref. [5] with permission from The Royal Society of Chemistry.

Flanders et al. polymerized methacrylate monomers, including methylmethacrylate (MMA), using reversible addition-fragmentation chain-transfer (RAFT) polymerization with a trithioester chain-transfer agent (CTA) [5]. This type of polymerization places trithioester end-group at end of the polymer chain (Scheme 1). Typically, this end-group is used to re-start the polymerization at the trithioester end of the polymer. However, as we will see, it may have another function. The authors isolated the polymer, then re-dissolved the polymer in 1,4-dioxane at 70 °C (Scheme 1). This caused monomers to be released from the polymer chains at a temperature much less than the ceiling temperature of MMA, which is 227 °C [13]. Analysis of the polymer after partial de-polymerization demonstrated that the trithioester end-group was still attached to the polymer and the size dispersity (range of polymer ‘molecular weight’) was low, which suggested that the de-polymerization was moderated by the trithioester end-group. The authors observed 10-35% de-polymerization after heating at 70 °C for 12-60 hrs.

Scheme 2: ATRP of NIPAM in carbonated water, followed by de-polymerization [9]. Reproduced from ref. [9] with permission from The Royal Society of Chemistry.

Lloyd et al. used an alkylbromide initiator, Cu-based catalyst system to polymerize N-isopropylacrylamide (NIPAM) in Highland Spring carbonated water at 0 °C (Scheme 2) [9]. This type of polymerization places a halide at the end of the polymer chain. The authors monitored the monomer conversion into polymer using ¹H-NMR spectroscopy. They measured that ca. 99% of the monomer was converted into polymer chains within 10 min. Unexpectedly, in the next 50 min. the authors observed 50% de-polymerization. The authors attempted to optimize de-polymerization conditions by changing the pH, using dry ice in HPLC grade water instead of Highland Spring carbonated water, etc. which led to 34-71% de-polymerization after 0.5-24 hrs. Years later, the same group used a very similar polymerization condition to polymerize NIPAM [1]. This time, non-carbonated water was used as the solvent and they did not report any de-polymerization.

The reports on RDRP followed by de-polymerization highlighted here are not yet ready to make an impact to ‘plastic to monomer’. The authors admit that the mechanism of de-polymerization is unknown. However, these seem to be the first set of reports on de-polymerization occurring at low temperatures. Perhaps these publications could be the birth of the reversible-deactivation radical de-polymerization (RDRDe-P) field. This is especially intriguing because RDRP have already been studied for decades in academia and are being adopted by the polymer industry [4]. Companies like BASF, Solvay, DuPont, L’Oréal, Unilever, 3 M, Arkema, PPG Industries, etc. already claimed patents for technology and products based on RDRP [4]. Somewhat ironically, RDRP was also part of the IUPAC’s 10 chemical innovations for impact on society but not for its potential to recycle polymer [6].

The polymers of the future may not be made from monomers abundantly used today, but the polymers of the future may be degradable through a low energy process.

References

1.  Alsubaie, F.; Liarou, E.; Nikolaou, V.; Wilson, P.; Haddleton, D. M. Thermoresponsive Viscosity of Polyacrylamide Block Copolymers Synthesised via Aqueous Cu-RDRP. European Polymer Journal 2019, 114, 326–331.
2. Baumann, E. Ueber Einige Vinylverbindungen. Justus Liebigs Annalen der Chemie 1872, 163 (3), 308–322.
3. Circular Economy – UK, USA, Europe, Asia & South America – The Ellen MacArthur Foundation https://www.ellenmacarthurfoundation.org/ (accessed Jan 5, 2020).
4. Destarac, M. Industrial Development of Reversible-Deactivation Radical Polymerization: Is the Induction Period Over? Chem. 2018, 9 (40), 4947–4967.
5. Flanders, M. J.; Gramlich, W. M. Reversible-Addition Fragmentation Chain Transfer (RAFT) Mediated Depolymerization of Brush Polymers. Chem. 2018, 9 (17), 2328–2335.
6. Gomollón-Bel, F. Ten Chemical Innovations That Will Change Our World: IUPAC Identifies Emerging Technologies in Chemistry with Potential to Make Our Planet More Sustainable. Chemistry International 2019, 41 (2), 12–17.
7. Li, L.; Shu, X.; Zhu, J. Low Temperature Depolymerization from a Copper-Based Aqueous Vinyl Polymerization System. Polymer 2012, 53 (22), 5010–5015.
8. Liebig, J. Justus Liebig’s Annalen Der Chemie. Annalen der Chemie 1832, 1874-1978.
9. Lloyd, D. J.; Nikolaou, V.; Collins, J.; Waldron, C.; Anastasaki, A.; Bassett, S. P.; Howdle, S. M.; Blanazs, A.; Wilson, P.; Kempe, K.; et al. Controlled Aqueous Polymerization of Acrylamides and Acrylates and “in Situ” Depolymerization in the Presence of Dissolved CO2. Commun. 2016, 52 (39), 6533–6536.
10. Microwave-Assisted Polymer Synthesis. Springer eBooks 2016
11. Moldoveanu, Șerban. Analytical Pyrolysis of Synthetic Organic Polymers; Techniques and instrumentation in analytical chemistry; Elsevier: Amsterdam ; Oxford, 2005.
12. Sano, Y.; Konishi, T.; Sawamoto, M.; Ouchi, M. Controlled Radical Depolymerization of Chlorine-Capped PMMA via Reversible Activation of the Terminal Group by Ruthenium Catalyst. European Polymer Journal 2019, 120, 109181.
13. SFPE Handbook of Fire Protection Engineering, 5th ed.; Hurley, M. J., Gottuk, D. T., Jr, J. R. H., Harada, K., Kuligowski, E. D., Puchovsky, M., Torero, J. L., Jr, J. M. W., Wieczorek, C. J., Eds.; Springer-Verlag: New York, 2016.

Green Marketing in the Plastic Era: Honesty or Hype?

By Nina-Francesca Farac, Member-at-Large for the GCI

The impact of human activity on climate and the environment has moved beyond a mainstream headline. It has come to the point where we are considered the dominant influence on our ecosystems and geology, so much so that there is a buzzword for it: ‘Anthropocene’. Within the Anthropocene, our greatest challenge is lessening the effects of our immense footprint on Earth, mainly caused by consumption of fossil fuels and our obsession with plastics. Consequently, there has been a considerable spike in eco-friendly or ‘green’ marketing of numerous products labeled as ‘organic’, ‘biodegradable’, or ‘sustainable’ ranging from fuels, cars, skincare, all the way to clothing¹. One common advertising theme for several everyday products is post-consumer recycled materials and their incorporation into the design and production of such commodities.  But to what extent are the advertised claims legitimate and whether they allow for a circular economy (e.g. make, use, recover)? Here, we will cover the chemistry of popular sustainable alternatives to plastics and compare them to their non-sustainable counterparts to assess whether the ‘green’ hype is valid.

Recycling Plastics: Single-Use vs. Biodegradable vs. Compostable

Let’s start with why commonly used plastics, including single-use plastics, pose such an environmental liability. The reality of plastic recycling is that it is far less efficient in practice than one would hope. The types of plastics that can be recycled, the number of times they can be recycled and reused starts with the ubiquitous recycling symbols found on the bottom of plastic products². A common misconception is to equate the presence of this symbol to the ability of recycling a given type of plastic; however, this is not the case. The truth is just because there is a recycling sign doesn’t necessarily mean it gets recycled³. According to Resin Identification Codes (RICs), plastics are organized into 7 categories according to the temperature at which the material has been heated, and this numerical categorization is only indicative of the kind of plastic it is, and not necessarily its recyclability (Fig. 1).

Figure 1. Resin Identification Codes (RICs) designating the seven categories of plastics, the corresponding chemical structure of each polymer, and graphical illustrations of common plastic products of each type.

In other words, just because we place it in a blue bin doesn’t mean it gets recycled. In fact, an astonishing 91% of plastics are not recycled². You may be wondering, “how are recycling rates that low?” As with any commodity, recycling is ultimately determined by the market.  If there is a demand, recyclers and companies will pay for post-consumer recyclables; but, without market demand, recycling bares no profit and placing them in a blue bin doesn’t make a difference³. For example, out of the seven categories of plastics depicted in Figure 1, only PET has a high recycling value (i.e. the price of PET scrap is high) while other plastics are projected to see a drop in recycling rates (at least in North America)^4–6. In addition, certain types of everyday plastics are simply not recyclable, such as plastic bags, straws, and coffee cups (the latter is not possible unless the paper exterior is separated from the plastic interior)³; in effect, these items are tossed together in the “everything else” category #7 (Other) as non-recyclables and mainly contribute to plastic waste generation. Other limiting factors include the inability to recycle dirty plastic and how the quality of plastic is downgraded each time plastic is recycled⁷.

Since many everyday items are plastic-based and plastics are a staple of modern life, the most common sustainable alternative to single-use plastics are bioplastics, a.ka biodegradable plastics (Figure 2).

Figure 2. Types of biodegradable plastics in use today, their chemical structures, and their applications.

Consumer confusion often arises when the terms “biodegradable” and “compostable” are used interchangeably, although they do not convey the same concept. Biodegradable plastics are a class of polymers that can break down by the action of living organisms into natural byproducts such as water, biomass, gases (e.g. N₂, CO₂, H₂, CH₄), and inorganic salts within a reasonable amount of time⁸. The issue with this definition is that many plastic products eventually degrade; for instance, low density polyethylene (LDPE, category #4 – Fig. 1) has been shown to biodegrade slowly to carbon dioxide (0.35% in 2.5 years) and thus can be considered a biodegradable polymer according to the above description⁹. Because certain definitions of biodegradability do not state a time limit or timeframe within which degradation should occur, consumers can be easily misled, and companies can hide behind this ambiguity. It is assumed, however, that a biodegradable product has a degradation rate that is comparable to that of its application rate, i.e. the break down process is fast such that product accumulation in the environment does not occur.

To understand why certain polymers biodegrade and others do not, one has to consider the chemical structure of biodegradable polymers along with the mechanisms through which polymeric material are biodegraded. Structurally, many biodegradable polymers, both natural and synthetic, often contain amide, ester, or ether bonds¹⁰. Those deriving from biomass (i.e. agro-polymers) include polysaccharides (glycosidic bonds via condensation of a saccharide hemiacetal bond and an alcohol) and proteins (chains of amino acids linked via amide groups). The other major category is biopolyesters, which are typically derived from microorganisms or are synthetically made (Figure 3).

Figure 3. Categories of biodegradable polymers.

Mechanistically, biodegradation is defined as a process caused by biological activity, especially driven by enzymes, but it can occur simultaneously with – and sometimes even initiated by – abiotic process such as photodegradation and hydrolysis⁹. From the chemical perspective, biodegradation can occur in the presence of oxygen (aerobic, Equation 1.1) or in the absence of oxygen (anaeriobic, Equation 1.2), where C_polymer represents either a polymer or a fragment from an earlier degradation process⁹.

C_polymer + O₂→CO₂ + H₂O + C_residue + C_biomass (Aerobic biodegradation,1.1)

C_polymer→ CO₂ + CH₄ + H₂O + C_residue + C_biomass (Anaeriobic biodegradation,1.2)

Complete biodegradation is said to occur when no C_residue remains, and no oligomers or polymers are left to be further broken down⁹. As polymers represent major constituents in living cells that have a high turnover rate, i.e. they are constantly degraded in response to environmental changes and metabolic requirements, numerous microorganisms are capable of breaking down naturally occurring polymers as a result of millions of years of adaption. However, for many new synthetic polymers invented in the last 100 years (categories 1-6, Fig. 1) which find their way into the environment, such biodegradation mechanisms have yet to be developed. Other key factors affecting polymer biodegradation include copolymer composition and environmental factors such as pH, temperature, and water content⁹. This suggests that even if a product is made from bioplastics, it doesn’t necessarily mean it will fully decompose. If such products end up in landfills, for instance, the low oxygen content of such an environment impedes complete degradation. Furthermore, although bioplastics fall within category 7 (Fig.1), these plastics aren’t suitable for recycling and can even degrade the quality of plastic if added to a recycled mixture.

In contrast, compostable materials can break down into water, carbon dioxide, inorganic salts and biomass at the same rate as cellulose, or roughly 90 days^11,12. In addition, compostable plastics must disintegrate fully and be indistinguishable in the compost while leaving no toxic material behind. Although compostable plastics appear to have more environmental benefits, this material is equally limited by an inability to biodegrade in a landfill and being incompatible with mixed recycled plastics¹¹. When it comes to biodegradable and compostable plastics, these products make for sustainable alternatives only if they are destined for the appropriate composting facilities whereby the specific conditions for their complete biodegradation are met.

In short, today’s environmental pressures have urged the mainstream production of sustainable alternatives to an ever-growing plastic problem. Although socially responsible plastic products exist with the intention of lessening their environmental footprints, their legitimacy as sustainable alternatives lies in their proper disposal and complete integration into a given environment without any adverse or toxic effects. For a more concrete circular economy, products made of glass and metal can be recycled infinitely without losing product quality, have no need for additional virgin material in the recycling process, and do not generate waste during the process³. Ultimately, a future with a reduced plastic impact depends not only on closed-loop recycling habits, but also on consumer education and awareness about how these products are made and disposed of.

References

(1)        Schmuck, D.; Matthes, J.; Naderer, B. Misleading Consumers with Green Advertising? An Affect–Reason–Involvement Account of Greenwashing Effects in Environmental Advertising. J. Advert. 2018, 47 (2), 127–145.

(2)        Lu, C. The Truth about Recycling Plastics. Mitte. 2018. https://mitte.co/2018/07/18/truth-recycling-plastic/

(3)        Sedaghat, L. 7 Things You Didn’t Know About Plastic (and Recycling). https://blog.nationalgeographic.org/2018/04/04/7-things-you-didnt-know-about-plastic-and-recycling/

(4)        Toto, D. The Value of Plastics. https://www.recyclingtoday.com/article/recyclingtoday-1011-plastics-value/

(5)        Dell, J. U.S. Plastic Recycling Rate Projected to Drop to 4.4% in 2018 https://www.waste360.com/plastics/us-plastic-recycling-rate-projected-drop-44-2018.

(6)        A Circular Economy For Plastics In Canada: A bold vision for less waste and more value. http://circulareconomyleaders.ca/downloads/A_Circular_Economy_for_Plastics_in_Canada.pdf

(7)        Hopewell, J.; Dvorak, R.; Kosior, E. Plastics Recycling: Challenges and Opportunities. Philos. Trans. R. Soc. B Biol. Sci. 2009, 364 (1526), 2115–2126.

(8)        Gross, R. A.; Kalra, B. Biodegradable Polymers for the Environment. Science (80-. ). 2002, 297 (5582), 803–807.

(9)        Bastiolo, C. Handbook of Biodegradable Polymers; 2005. Rapra Technology Limited.

(10)      Vroman, I.; Tighzert, L. Biodegradable Polymers. Materials (Basel). 2009, 2 (2), 307–344.

(11)      https://pelacase.com/blogs/news/5-things-you-probably-didnt-know-about-compostable-plastics

(12)     https://www.food.ee/blog/compostable-vs-recyclable-vs-biodegradable/

Boat Antifouling Technology: the problems and the green chemistry solutions!

By Alana Rangaswamy (Vice-President, Dalhousie University Green Chemistry Initiative)

The iconic Halifax Ferry is one of many boats to traverse the Harbour every day.

One great part of attending Dalhousie University is living steps away from the ocean. Much of Halifax’s history and development is due to its access to water, both as a naval base and port of call. With the massive amount of boat traffic seen daily by the harbour, marine industries strive to maximize the efficiency of travel. And one major way to do that is preventing small creatures from hitching a ride on your boat, causing drag and lowering the efficiency of your vessel. Enter antifoulants: coatings that kill organisms or otherwise block their ability to stick onto your ship. Antifouling is a necessary technology, but introducing biocidal agents into a marine environment, unsurprisingly, poses many environmental challenges. Let’s take a look at two commonly used antifoulants, their issues, and how scientists have tried to fix them:

Tributyltin 

You may have heard of tributyltin (TBT) as a biocidal agent. TBT is an excellent poison – effectively nonpolar due to its alkyl groups, it’s able to accumulate in organisms, rapidly killing them due to the high toxicity of Sn^III. This property makes TBT an extremely effective antifouling agent, however, it easily leaches from boat hull paint into the ocean where it persists due to its high stability. Fortunately, the dangers TBT have been recognized worldwide and use as a biocidal agent has been banned as of 2008¹. Canada jumped on the bandwagon slightly earlier, with the last TBT-containing paint product registered in 1999.² With this restriction, the industry is searching for alternatives that are as effective as TBT, without the environmental drawbacks.

Copper

Copper as a bulk metal is naturally antiseptic, promoting the formation of reactive hydroxyl radical species which lead to cell death in living systems.³ Copper has been used on boat hulls since the 1700s, and now usually shows up in paints as its metal oxide⁴ or as a suspension of copper powder.⁵ Although copper is less bioavailable than TBT, it persists and continually forms unstable radical species (and can, therefore. wreak ecological havoc) in a marine environment. Since copper is widely considered the new “gold” standard in antifouling, the sheer amount of it present on (and leaching off of) boat hulls today points to a long-term impact.

New Antifouling Tech

Green chemistry and engineering are all about designing cleaner systems that work as well as, or better than, the existing standard. TBT and copper are high bars to clear, but scientists are up to the challenge. As early as 1996, the environmentally benign Sea-Nine antifouling compound had received the Designing Greener Chemistry Award as part of the US EPA’s Presidential Green Chemistry Challenge.⁶ Sea-Nine is a derivative of isothiazolinone, a 5-membered heterocycle containing nitrogen and sulfur atoms. The compound is acutely toxic to marine organisms at the surface of boats, but biodegrades rapidly in marine environments through a ring-opening mechanism to form non-toxic by-products. Sea-Nine (and its derivatives) is currently present in commercial boat hull paints,⁷ however, degradation times may vary based on geographical location and local environment⁸ so our job isn’t done yet.

There are many newer studies in the works. For instance, investigation has been done into using natural products as antifouling agents. Natural products are secondary metabolites produced by microorganisms as a defence mechanism in response to stress. As such, they often have antimicrobial properties, while being naturally biodegradable. For example, 1-hydroxymyristic acid, a simple alpha-hydroxy fatty acid, was isolated from the marine bacterium Shwanella oneidensis. When panels were coated with paint containing the fatty acid, and subsequently immersed in a marine environment, no growth of foulants was observed even after 1.5 years.⁹ Other studies have added hydrophobic coatings which disrupt the binding interactions between the microorganism and the vessel’s hull, and promote detachment due to the natural flow of the water over the hull.¹⁰ Some research has diverted away from chemical modifiers altogether, using microtextures, which remove the flat surfaces required for spores to settle,¹⁰ to deter growth. UV-LEDs¹¹ which are mutagenic and cytotoxic at a small scale, have also been used to reduce growth of foulants.

The long history and many methods developed to prevent boat hull fouling demonstrates that this is an important and challenging problem. But many results are promising, and green chemists and engineers are well on their way to solving it.

References:

1. http://wwf.panda.org/?145704/tributyltin-canned
2. Health Canada – Consumer Product Safety Registrar

http://pr-rp.hc-sc.gc.ca/ls-re/result-eng.php?p_search_label=antifouling+paint&searchfield1=ACT&operator1=CONTAIN&criteria1=tin&logicfield1=AND&searchfield2=NONE&operator2=CONTAIN&criteria2=&logicfield2=AND&searchfield3=NONE&operator3=CONTAIN&criteria3=&logicfield3=AND&searchfield4=NONE&operator4=CONTAIN&criteria4=&logicfield4=AND&p_operatordate=%3D&p_criteriadate=&p_status_reg=REGISTERED&p_status_hist=HISTORICAL&p_searchexpdate=EXP

3. Grass, G., Rensing, C., and Solioz, M. Metallic copper as an antimicrobial surface. Environ. Microbiol. 2011, 77, 1541-1547. DOI: 10.1128/AEM.02766-10.
4. https://www.chemistryworld.com/news/antifouling-coatings-cling-to-copper/3010011.article
5. http://coppercoat.com/coppercoat-info/antifoul-how-it-works/
6. https://www.epa.gov/greenchemistry/presidential-green-chemistry-challenge-1996-designing-greener-chemicals-award
7. https://www.epaint.com/product/sn-1-antifouling-paint/
8. Chen, L. and Lam, J. C. W. SeaNine 211 as an antifouling biocide: a coastal pollutant of emerging concern. Environ. Sci., 2017, 61, 68-79. DOI: 10.1016/j.jes.2017.03.040.
9. Qian, P-Y., Xu, Y. and Fusetani, N. Natural products as antifouling compounds: recent progress and future perspectives. Biofouling, 2009, 26, 223-234. DOI: 10.1080/08927010903470815.
10. Salta, M. et al. Designing biomimetic antifouling surfaces. Trans. R. Soc. A, 2010, 368, 4729-4757. DOI:10.1098/rsta.2010.0195
11. https://www.pcimag.com/articles/104484-marine-fouling-prevention-solution-to-use-uv-led-technology

 

 

 

Canada Becomes a Leader in Carbon Capture

By Karlee Bamford, Treasurer for the GCI

The attention of international media has been captured by the remarkable success in CO₂ sequestration achieved by the Canadian company Carbon Engineering, located in Squamish, British Columbia. Sustainability-related, world-saving initiatives often have an easier sell in the media than, say, incremental advances reported by researchers on equally sustainable academic pursuits (rough, eh?). In this instance the craze over Carbon Engineering’s advances has been amplified by the news of their recent partnerships with household-name energy and oil giants, such as Chevron, BHP, and Occidental Petroleum, in the form of a CAD $68 million investment.  So, what is this incredible advance?

From the success of their pilot plant and the data they’ve accumulated thus far, Carbon Engineering implementation of their technology has achieved capture of The technology in question can be split into two major advances. Referred to as direct air capture, or DAC, the first process developed by Carbon Engineering involves the transfer of gaseous CO₂ from ambient air to an absorber fluid, a strongly basic solution of sodium or potassium hydroxide. The transfer process is achieved using an air-liquid contactor, designed and described by the company in 2012,⁴ that involves an array of fans, pumps, cheap PVC piping and structure, and fluid distributors. These components are fundamentally no different than those commonly found in cooling towers used as heat exchangers for water cooling. However, the orthogonal geometry (Figure 1) of air (atmospheric, ~ 400 ppm CO₂) and fluid (the absorber) flow differs significantly, making repurposing of existing cooling tower designs for DAC an inefficient and expensive strategy for CO₂ capture.

Figure 1. Commercial realization of air-fluid contactor designed by Carbon Engineering. M = Na or K. Image obtained from CanTech Letter and modified.5

The CO₂ taken up by the alkaline absorber fluid is converted to carbonate (CO₃^2-) salts and can be precipitated from the aqueous solution by treatment with calcium hydroxide to give calcium carbonate pellets. The captured CO₂ can thus be stored as calcium carbonate or can be cleanly regenerated as pure CO₂ gas, with elimination of a CaO , at high temperatures (650 °C) for commercial resale. The byproduct CaO may even repurposed by conversion back to Ca(OH)₂ in a lime slaker, using water.¹ Carbon Engineering has been piloting this process at their facility in Squamish since 2015, according to their website, after having tested a smaller prototype from 2010 and published the performance results in 2013.⁶ At the time of Carbon Engineering’s founding and until as recently as 2018, no commercial-scale air capture systems had been developed, which was a direct result of the anticipated inefficiency of CO₂ capture using conventional cooling tower designs.⁴ Undeterred, Carbon Engineering has proven otherwise with their innovative use of cross-flow geometry.

The second break-through technology from Carbon Engineering is their patented Air To Fuels^TM process, which they’ve been piloting since 2017. Taking the stored CO₂ from their DAC process, Carbon Engineering has successfully produced a clean, sulfur-free, source of hydrocarbon fuel that requires no further modification for consumer consumption. The process involves passing the regenerated CO₂ gas through a reactor containing hydrogen (H₂) gas to generate synthesis gas (syn-gas), a mixture of CO and . The syn-gas is then passed through a Fischer-Tropsch reactor where the synthetic hydrocarbon fuel is thermally generated over a heterogenous base-metal catalyst (e.g. iron, cobalt, nickel).⁷

The technologies have been developed by the research groups of founder and U of T alumnus Prof. David Keith. Prof. Keith is currently faculty at Harvard University in the School of Engineering and Applied Sciences. To date, the company has filed 13 patents and produced numerous publications describing their innovations. According to media reports,⁸ recent multimillion-dollar investments will allow their and the company has already signed a memorandum of understanding with Squamish First Nations about their intentions.⁹

One of the most attractive aspects of the DAC and Air to Fuels^TM technology is location. Plants could, hypothetically, be built anywhere, as CO₂ is well mixed in the atmosphere and Carbon Engineering’s technology does not require that CO₂ capture occur at the point of CO₂ generation as in, for example, CO₂-scrubbers used in exhaust systems.

However, with the excitement surrounding Carbon Engineering’s projected ability to capture CO₂ at low cost and high volume, controversy has inevitably been close to follow. The interest from large oil corporations in this technology may not be as principled in sustainability as it appears but driven in part by their need for large volumes of CO₂ for so-called green fracking (hydraulic fracturing). Supporting further oil extraction in this way goes completely counter to the need for elimination of emissions that the 2018 Intergovernmental Panel on Climate Change (IPCC) report clearly indicates must accompany advances in carbon capture and storage.¹⁰ Still, perhaps the positives outweigh the negatives in this instance. This very week, Environment and Climate Change Canada reported that Canada is warming at twice the rate of the rest of the globe.¹¹ The need for efficient technologies to address climate change has never been more immediate. Fortunately, Carbon Engineering is not alone: at least two other companies with commercial plans for CO₂ capture have started in Switzerland (Climeworks)¹² and the USA (Global Thermostat).¹³ Whether the Canadian solution is adapted worldwide will depend not only upon Carbon Engineering, but also upon how these alternative approaches evolve.  For once, it is probably best not to pick a team to cheer for but, instead, hope that each country’s company develop a complimentary capture strategy to address the international dilemma that is climate change.

References:

1. Keith, D. W.; Holmes, G.; St. Angelo, D.; Heidel, K., Joule 2018, 2, 1573-1594.
2. American Physical Society. Direct Air Capture of CO₂ with Chemicals: A Technology Assessment for the APS Panel on Public Affairs. June 1, 2011 https://www.aps.org/policy/reports/assessments/upload/dac2011.pdf ; accessed April 24, 2019.
3. Carbon Engineering, https://carbonengineering.com/ .
4. Holmes, G.; Keith, D. W., Trans. R. Soc. A 2012, 370, 4380-403.
5. Artist’s rendition of a commercial scale Carbon Engineering contactor, CanTech Letter. https://www.cantechletter.com/2016/10/squamish-b-c-s-carbon-engineering-begins-scale-co2-capture-new-deal/ ; accessed April 4, 2019.
6. Holmes, K. Nold, T. Walsh, K. Heidel, M. A. Henderson, J. Ritchie, P. Klavins, A. Singh and D. W. Keith, Energy Procedia, 2013, 37, 6079-6095.
7. Heidel, Keton et al. Method and system for synthesizing fuel from dilute carbon dioxide source. WO2018112654A1, 2017.
8. BBC News, Matt McGrath. Climate change: ‘Magic bullet’ carbon solution takes big step. April 3, 2019 https://www.bbc.com/news/science-environment-47638586 ; accesed April 3, 2019.
9. CBC News, Angela Sterritt. In fight to combat climate change, Squamish Nation joins forces to capture carbon. November 29, 2018. https://www.cbc.ca/news/canada/british-columbia/in-fight-to-combat-climate-change-squamish-nation-joins-forces-to-capture-carbon-1.4924017 ; accesesd April 4, 2019.
10. Intergovernmental Panel on Climate Change 2018 Summary for Policy Makers, Global Warming of 1.5 °C. https://www.ipcc.ch/site/assets/uploads/sites/2/2018/07/SR15_SPM_version_stand_alone_LR.pdf ; accessed April 4, 2019.
11. Environment and Climate Change Canada, Canada’s Changing Climate Report, April 1, 2019. https://www.nrcan.gc.ca/environment/impacts-adaptation/21177 ; accesed April 4, 2019.
12. Climeworks, http://www.climeworks.com/
13. Global Thermostat, https://globalthermostat.com/

How green is your bromination reaction?

By Diya Zhu: Symposium Coordinator for the GCI

Electrophilic bromination is a common type of reaction in undergraduate organic laboratories. In these experiments, we rarely use Br₂ as a bromine source. Why? This dense brownish-red liquid is a pain in the butt for a few reasons. First of all, it fumes. Once you open the bottle, orange fumes start migrating everywhere. Without efficient ventilation, soon you will smell an offensive and suffocating odor. Second, bromine is corrosive to human tissue as a liquid and its vapours irritate the eyes and throat. Moreover, with inhalation, bromine vapours are very toxic. Third, bromine is very dense, with a density of 3.1 g/cm³, which makes it very difficult to measure and transfer.

Figure 1. A bottle containing bromine.1

Instead, N-bromosuccinimide (NBS) is often used as a brominating and oxidizing agent in various electrophilic addition, radical addition, and electrophilic substitution reactions. Pure NBS is a white crystalline solid with a melting point of 175-180 ^oC. Even though it’s a solid and easier to handle, you still need to be careful when working with NBS. Due to the higher electronegativity of nitrogen, the Br atom is partially positively charged and thus electrophilic, ready to be attacked by a nucleophile (eg. an alkene).

Figure 2. N-bromosuccinimide (NBS)

NBS will form bromonium ions with alkenes, and when an alcohol or water is added, it will attack the bromonium ion, which will generate bromohydrins. Importantly, the nucleophilic attack only happens on the face opposite the bromonium ion.

Figure 3. Alkene reaction with NBS showing the bromonium ion and attack of water to form a racemic mixture.

Usually, when undergraduate students preform this experiment, we also emphasized the importance of Green Chemistry. Green chemistry and its 12 principles help to improve conventional reactions. For example, increasing the efficiency of synthetic methods, reducing the steps of synthesis, and minimizing toxic reagents and solvents. In the formation of bromohydrins, compared to using Br₂, NBS is less hazardous.  Also, water or alcohol can be used as the solvent which eliminates the use of organic solvents, especially chlorinated solvents.

However, the use of NBS also creates by-products. For example, succinimide and the very strong hydrobromic acid. It also has a reduced atom economy, since only one Br atom of 8 atoms in a NBS molecule is used in bromination.

With all of this taken into consideration, can it be concluded that NBS is a greener alternative to Br₂? What do you think, and which reagent will you be reaching for in your next bromination experiment?

References:

1. https://en.wikipedia.org/wiki/Bromine

The Future of Sustainability in the Younger Generations’ Hands

By Alex Waked, Co-chair for the GCI

In the last couple decades, there has been an increasing focus on developing sustainable practices in society to reduce our environmental impact. Probably the most notable effort in this endeavour is the signing of the Paris Agreement within the United Nations Framework Convention on Climate Change, in which 194 states and the European Union have set goals to reduce the global carbon footprint to reasonable levels.

As we progress forward, there will be a need to propagate this mindset to the coming generations. Fortunately, I don’t think there will be too much difficulty in achieving this. A growing number of schools have been instituting environmental- and sustainability-related courses in their curricula. In my opinion, this strategy has been the most effective in conveying the importance of being conscious of any consequences of our actions and learning how to improve.

In the last few years, many of the chemistry courses at the University of Toronto have incorporated green chemistry and safety modules in both the laboratory and theory sections of the courses. The number of factors that we now consider when designing experiments is much larger than in the past. For instance, are the molecules we’re synthesizing going to be very toxic? Can they be safely disposed of? Do we use harmful substances or solvents during the experiment? How much chemical waste is produced?

Figure 1. Graphic of the 12 Principles of Green Chemistry, which currently play an important role in designing safe and environmentally benign chemical processes.1

These are all questions that have traditionally been overlooked in the past. However, the description of the 12 Principles of Green Chemistry by Anastas and Warner in 1998² was a huge and essential step forward in the current direction we’re heading of thinking about chemistry from a sustainability and safety perspective. Many student-led groups and schools are now taking initiative in this endeavour.

The earlier and more the students are taught about these topics, the greater the chance it will have of the students developing genuine interests in them. In June of this year, the University of Toronto Schools held their first Sustainability Fair, in which grade 8-9 students participated in a science fair-like event where they worked on sustainability-related projects.

Figure 2. Examples of posters at the University of Toronto Schools’ Sustainability Fair in June 2018.3

The GCI was invited to participate in listening to the students’ presentations describing their projects and to give any advice and encouragement to them; three of us, myself included, attended it. I would say there were at least 40 projects in total. These are just a few examples of some the projects:

• Calculating how much water was saved by reducing shower time over a 2-week period
• Collecting and recycling e-waste (any old electrical parts) that would traditionally be thrown away in the garbage
• Calculating the reduction of carbon footprint by biking to work or school instead of driving

There were two things that really stood out to us: one being the range of topics (water reduction, carbon footprint reduction, recycling plastics and electronic waste, and minimizing food waste), and two being the genuine enthusiasm and interest of the students in their projects.

These are the students that will develop into people that will have important leadership roles in society in the future. The prospect of this is what excites me and gives me confidence that the future generations will continue to propel society forward in terms of being even more environmentally conscious and actually walk the walk, and not only talk the talk!

References:

1. The Green Chemistry Initiative website. Accessed September 13, 2018. <http://greenchemuoft.ca/resources.php&gt;
2. Anastas, P. T.; Warner, J. C. Green Chemistry: Theory and Practice, Oxford University Press: New York, 1998, p. 30.
3. Obtained with permission of the University of Toronto Schools.

 

ACS Summer School on Green Chemistry and Sustainable Energy 2018

By Kevin Szkop and Rachel Hems

The Colorado School of Mines in Golden, CO is a wonderful campus with cutting-edge facilities and a great place to spend a week with 60 young scientists interested in green chemistry. This is where the ACS Summer School on Green Chemistry and Sustainable Energy was held from July 10 – 17. The group consisted of chemists and chemical engineers from North and South America, all with unique perspectives, experiences, and attitudes towards sustainability. Below is a photo of our awesome class!

The 2018 ACS Summer School on Green Chemistry and Sustainable Energy class

The program consisted of technical and professional development sessions. A highlight was a life cycle assessment group project and presentation, led by Prof. Philip Jessop from Queen’s University. During Professor Jessop’s lectures, we learned how to think about the “greenness” of a process, and how this often-nebulous concept is best used as a comparative tool. While every process likely has downfalls, using the green chemistry principles and metrics allowed us to think critically about which process has the least downfalls, and how to address these in our work. The assignment included a group project, during which groups of students had to evaluate the merits and drawbacks of 5 synthetic routes to the same product. In this context, we learned that it is not only the reagents that go into a flask, but everything that happens behind the scenes, including shipping of reagents, the type of waste generated, amount of energy consumed, and much, much more. As a synthetic chemist (Kevin), it really made me think about solvent consumption and work up techniques in my own work!

In addition to learning about green chemistry and sustainable energy, there were some great professional development lectures and activities. Dr. Nancy Jenson, the program manager for the Petroleum Research Fund at the ACS, gave an engaging talk on tips for writing research proposals and common mistakes that are made. While she gave examples from her experience at the Petroleum Research Fund, there were many lessons that could be applied to any type of proposal writing.

Another great professional development lecture was given by Joerg Schlatterer from the American Chemical Society. He gave an overview of the ACS’s many resources for young chemists, such as the Chem IDP website for career planning, workshops for prospective faculty organized by the Graduate & Postdoctoral Scholars Office, and the new Catalyzing Career Networking program at ACS National Meetings. As part of the career planning case study, we took some time to make some SMART goals for ourselves for the next two years. I (Rachel) found it’s really helpful to have others share their goals and give suggestions for yours to make them the SMARTest they can be!

Rafting down Clear Creek

Of course, we also had time to have fun! On the Saturday (also Rachel’s birthday!) we went white water rafting on Clear Creek. The river is mountain fed, so it was very cold, but it was a beautiful warm and sunny day! We had a great time rafting down the river, with a quick stop to jump in for a swim. It was a great way to spend my birthday! Throughout the week-long summer school, there was a decent amount of free time to enjoy the sunshine and the sights around Golden. Some of the fun things we got to do were swim in and raft down the river that goes through ‘downtown’ Golden, an early morning hike up the South Table Mountain, tour the Coors Brewery, and get to know all the other awesome chemists!

Kevin and Rachel enjoying the Golden nightlife after a long day of learning!

We highly recommend attending this summer school. It is a great opportunity to learn and to meet great people who care about sustainable chemistry! Read more about past GCI members that have attended the ACS Summer School in 2014 and  2017.

More information on the summer school and how to apply can be found online here.

The plastic problem – accumulation before alternatives

By Karlee Bamford, Treasurer for the GCI

Plastics undoubtedly play a central role in our daily lives and played a pivotal role in the development of consumer societies across the globe for over a century. Concurrent with newfound materials and newfound possibilities, unprecedented environmental problems have emerged as a result of our reliance on plastics. The accumulation of plastics in allocated disposal sites (e.g. landfills) and in otherwise uninhabited spaces (e.g. beaches, open ocean) present threats to human health, water security, and food supply. These challenges now impact communities globally, irrespective of their actual contribution to the generation of plastic waste, and affect individuals of all economic backgrounds.

Figure 1. Examples of waste plastic accumulation in landfills and the environment. Images source: Pixabay.

Given the scale and significance of these challenges, is there anything that chemists can do to resolve this panhuman problem? A recent blog post from the Green Chemistry Initiative (https://greenchemuoft.wordpress.com/category/author/molly-sung/) highlighted the advances that have been made in synthetic and materials chemistry towards plant-derived and biodegradable plastics as alternatives to traditional petroleum-derived plastics. While this is undoubtedly a crucial area of research as humanity has become permanently dependent on plastics, the design of next generation plastics that are inherently sustainable will not mitigate the overwhelming impacts of existing plastic waste. Arguably, attenuating the problem of plastic waste is more important than finding alternatives to traditional plastics. Indeed, the decomposition time for products made from the top four families of commodity plastics (PP, PE, PVC, PET), produced on a 224.6 million tonne-scale alone in 2017,¹ is estimated at 1 to 600 years in marine environments² and considerably longer in landfills due to lack of moisture.⁴

Figure 2. Examples of the top five most-produced commodity polymers and their production scale in 2017.1,3

Traditional plastic-recycling methods are not equipped to resolve the issue of waste plastic accumulation either. Recycling can be broken down into three distinct varieties: primary, secondary, and tertiary.⁵ Primary recycling, which is equivalent to repurposing or reusing, is used limitedly for products such as plastic bottles, typically made of PET, which be directly reused following the necessary sterilization. Secondary recycling involves mechanical processing of plastics into new materials and frequently results in reduction of the plastics overall quality or durability due to the thermal or chemical processes involved. Primary and secondary recycling account for the majority of recycling efforts, however, as a consequence of poor consumer compliance (e.g. <10 % in the US and 30-40 % in the EU)⁶ and the deteriorating value of plastics with repeated secondary recycling, all plastics eventually become waste. The last and most underutilized form of recycling is tertiary recycling, the degradation or depolymerization of plastics into useful chemicals or materials. In the last year alone, numerous high profile editorial and review articles have appeared in Science^7,8,9 and Nature^6,10 emphasizing the incredible potential of chemical (tertiary) recycling as means of reducing plastic waste and as a new, sustainable chemical feedstock for the polymer (plastics) industry.

The challenge of chemical recycling is immediately evident: plastics have been expertly designed to be highly durable and chemically resistant, and thus, plastics cannot be easily transformed chemically. Ideally, polymers used in plastics could be depolymerized to monomer for subsequent repolymerization. For condensation polymers, such as polyethylene terephthalate (PET), the reverse of the polymerization reaction is the addition of a small molecule to the polymer to reform monomer. While completely reversible on paper or in theory, such depolymerization strategies have had limited success for PET.

Reacting the polymeric PET material with protic reagents (e.g. amines, alcohols) followed by hydrolysis to give monomers that can be repolymerized, if of sufficient purity (Figure 3), requires high temperature (250-300 °C) and high pressure (0.1-4 MPa) conditions unless additives, such as strong acids and bases or metal salts, are used.¹¹ The action of many additives is not well understood, thus precluding rational improvement of the system. Hydrolysis of PET itself, especially at neutral pH, is the most challenging approach to PET chemical recycling as water is a relatively poor nucleophile. Hence stronger nucleophiles, such as ethylene glycol, are preferred.

Figure 3. Depolymerization of PET by glycolysis.

One practical problem in the chemical recycling of any plastic is its insolubility. Phase transfer catalysts –  species capable of transferring from one phase to another – have been used to address the insolubility of PET¹² and have permitted the direct hydrolysis of PET at operating temperatures as low as 80 °C, as in the work of Karayannidis and coworkers (Figure 4). The phases in these systems are the insoluble PET polymer (the organic phase) and the basic solution (the aqueous phase) surrounding it.¹³

Figure 4. Phase transfer catalyzed hydrolysis of PET (catalyst shown in blue).

Addition polymers, such as polypropylene (PP) or polyethylene (PE), cannot be depolymerized to monomer form using the above strategies as their polymerization does not involve the loss of small molecules. Until very recently, the best end-of-life purpose for the majority of plastics has been energy recovery through incineration. The work of Huang and coworkers on the chemical degradation of PE plastics is a break-through for the field of plastic recycling. While previous studies have reported that thermolysis of PE yields poorly defined mixtures of hydrocarbons, these authors have found a remarkable, highly targeted method for converting PE to a narrow distribution of fuels (3 to 30 carbons in length) using a dehydrogenative metathesis strategy (Figure 5).¹⁴ The homogeneous iridium catalysts employed were previously reported in the literature for alkane dehydrogenation (step 1) and hydrogenation (step 3), but no such polymer substrates had apparently been attempted for main-chain dehydrogenation. Similarly, the authors used a previously-established rhenium oxide/aluminium oxide catalyst for olefin metathesis (step 2).

Figure 5. The transition-metal catalyzed degradation of PE to liquid fuels reported by Huang and Guan (catalysts shown in blue).14

The chemical recycling of PET by phase transfer catalysis and of PE by dehydrogenative-metathesis have very little in common with one another on a technical level. What unites these two strategies is the desire to transform the problematic, highly abundant and inexpensive resource that is waste plastic into useful commodities. Perhaps more importantly, these two examples both take revolutionary approaches to old problems through inspiration from fundamental research and parallels found in small molecule catalysis. Rethinking the plastic problem into a challenge for catalysis, rather than solely a call for clever materials design, is critical if we wish to reduce the threats that waste plastics pose to our health and our environment.

References:

1. Tavazzi, L., et al., The Excellence of the Plastics Supply Chain in Relaunching Manufacturing in Italy and Europe, The European House, Ambrosetti, 2013 (as cited in Bühler‐Vidal, J. O. The Business of Polyethylene. In Handbook of Industrial Polyethylene and Technology; Spalding, M. A.; Chatterjee, A. M., Eds.; John Wiley & Sons: Hoboken, NJ, 2017; p. 1305).
2. Mote Marine Laboratory Biodegradation Timeline; 1993. Available from: https://www.mass.gov/files/documents/2016/08/pq/pocket-guide-2003.pdf ; accessed July 10, 2018.
3. Image sources: Image sources: (Plastic recycling symbols) http://naturalsociety.com/recycling-symbols-numbers-plastic-bottles-meaning/ ; (PP) https://www.screwfix.com/p/stranded-polypropylene-rope-blue-6mm-x-30m/98570 ; (LLDPE) https://www.polymersolutions.com/blog/differences-between-ldpe-and-hdpe/ ; (HDPE) https://chemglass.com/bottles-high-density-polyethylene-hdpe-wide-mouths ; (PVC) https://omnexus.specialchem.com/selection-guide/polyvinyl-chloride-pvc-plastic ; (PET) https://ecosumo.wordpress.com/2009/06/04/what-does-the-recycle-symbol-mean-part-2/
4. Andrady, A. L. Journal of Macromolecular Science, Part C: Polymer Reviews, 1994, 34(1), 25-76.
5. Hopewell, J.; Dvorak, R.; Kosior, E. Trans. R. Soc. B, 2009, 364, 2115–2126.
6. Rahimi, A.; García, J. M. Nature Reviews Chemistry, 2017, 1, 0046.
7. MacArthur, E. Science, 2017, 358 (6365), 843.
8. García, J. M.; Robertson, M. L. Science, 2017, 358(6365), 870-872.
9. Sardon, H.; Dove, A. P. Science, 2018, 360(6387), 380-381.
10. The Future of Plastic. Nature Communications, 2018, 9, 2157.
11. Venkatachalam, S.; Nayak, S. G.; Labde, J. V.; Gharal, P. R.; Rao, K.; Kelkar, A. K. Degradation and Recyclability of Poly (Ethylene Terephthalate). In Polyester; Saleh, H. E. M., Ed.; InTech: London, 2004; p. 78.
12. Glatzer, H. J.; Doraiswamy, L. K. Eng. Sci. 2000, 55(21), 5149-5160.
13. Kosmidis, V. A.; Achilias, D. S.; Karayannidis, G. P. Mater. Eng. 2001, 286(10), 640-647.
14. Jia, X.; Qin, C.; Friedberger, T.; Guan, Z.; Huang, Z. Science Advances 2016, 2(6), e1501591.

Leading by Example in the Lab

By Ian Mallov, Co-Chair for the GCI

Ask a scientist what their greatest satisfaction is from research.  Most will probably tell you something along the lines of “the pursuit and discovery of new knowledge.”

Some will mention the parallel satisfaction of originating inventions or techniques that are broadly applicable, and seeing that work applied for the benefit of society.

Much of the challenge of moving towards a truly sustainable culture is in applying what we’ve already shown to be effective on small scales.

Two years ago, the Green Chemistry Initiative’s 2014 Workshop team developed ten recommendations entitled “Simple Techniques to Make Everyday Lab Work Greener.”  Led by co-founder Laura Hoch, with important contributions from Cookie Cho and Dr. Andy Dicks, we publicized these during the workshop.  So what has happened to these recommendations since?  They’ve been developed – are researchers in our department incorporating them into their work habits?  Are we ourselves applying what we already know to be effective?

I was pleasantly surprised to find out that a number of our researchers were in fact using these greener lab techniques.  In an effort to make their use even more widespread, I’d like to highlight some examples of researchers in our department who are leading by example.

Further, next week our “Simple Techniques to Make Everyday Lab Work Greener” poster will be posted around the department!

---

 

Scientist: Karlee Bamford, Stephan lab

Technique: Recycling solvents from rotovap to use for cleaning vials and glassware

Why it’s greener: Saves solvent, reduces waste generated, and reduces energy used in production and disposal of additional solvent

Issues to Consider: Use in synthesis and purification often requires solvents to be more pure than those collected from rotovap

---

Scientist: Aleksandra Holownia, Yudin lab

Technique: Setting GC to stand-by mode when not in use

Why it’s greener: The GC uses much less helium gas (a rapidly diminishing resource) and reduces the temperature of the oven, saving energy

Issues to Consider: Does take a few minutes to start up again

---

Scientist: Karl Demmans, Morris lab

Technique: Using 2-methyl THF as a reaction solvent instead of THF

Why it’s greener: 2-methyl THF is derived from the aldehyde furfural, sourced from renewable crops.  THF, on the other hand, is derived from fossil fuels.  While crop-sourcing does not automatically make it “greener,” consensus in the case 2-methyl THF is that it is indeed less energy- and resource-intensive to produce than THF.

Issues to Consider: Unlike THF, it is immiscible with water.  Slightly less polar than THF

---

Scientist: James LaFortune, Stephan lab

Technique: Isopropanol/dry ice instead of acetone/dry ice for cold baths

Why it’s greener: An Isopropanol/dry ice bath maintains a temperature of -77 ^oC, almost exactly the same as acetone/dry ice’s -78 ^oC.   However, isopropanol is much less volatile (bp: 83 ^oC) than acetone (bp: 56 ^oC); practically, this allows for the recovery and reuse of the isopropanol after several hours or overnight, while acetone evaporates.

                                                                          Issues to Consider: Must actually recover and reuse the isopropanol!

---

Scientist: Samantha Smith, Morris lab

Technique: Closing the fume hood sash when not in use.

Why it’s greener: Modern, variable-flow fume hoods – used in the Davenport wing of our building – regulate the strength of their vacuum for safety based on how far open the fume hood is.  When wide open, the fume hood uses much more energy than when closed (see Just Shut It campaign!)

Issues to Consider: Is your fume hood variable-flow?

 

---

Scientist: Brian de la Franier, Thompson lab

Technique: Using a closed-loop cooling system for refluxes and distillations.

Why it’s greener: Uses much less water.  While some of our undergraduate labs have built-in closed-loop cooling systems, Brian simply got a small fish tank pump from a pet store and uses a Styrofoam box with ice to keep his water cold – a very easy DIY solution!

Issues to Consider: Does water saved compensate for the extra energy for the ice/pump?  Consider the energy used to purify and deliver the extra water and we can safely say yes.

---

Scientist: Alex Waked, Stephan lab

Technique: Reusing rubber septa used to seal Schlenk flasks

Why it’s greener: Saves materials and money

Issues to Consider: There is a limit to their reusability.  At some point, if a septum has been perforated by too many needle holes it is no longer an effective seal.  Must also ensure septa are kept clean.

---

Scientist: Molly Sung, Morris lab

Technique: Reusing gas chromatography vial caps by replacing their septa

Why it’s greener: Saves materials and money

Issues to Consider: Somewhat time-consuming to remove and replace rubber septa for each cap

 

---

Iceland is Greener Than You Think

By Peter Mirtchev, Member-at-Large for the GCI

This past summer I had the opportunity to travel to Iceland as part of the Global Renewable Energy Education Network’s (GREEN) 10-day program in Renewable Energy & Sustainability. GREEN organizes educational adventure workshops in a number of unique locations including Iceland, Costa Rica, and Peru. The trips are focused on a central theme such as Renewable Energy or Water Resource Management, and are open to undergraduate and graduate students from around the world through a competitive application process. The registration fees cover all expenses except the flight and even though the cost might be steep for a student budget, there are plenty of funding opportunities to explore through your university’s financial office. Feel free to email the GCI if you’re interested and want to know more!

Iceland is as interesting to learn about as it is beautiful to explore. And that’s a lot.

Iceland is an amazing place. The country is completely isolated on a volcanic island in the mid-Atlantic and has a population of just over 300,000 or about the same as a few large sports stadiums packed together. As such, it tends to lead the world in per capita categories; for example Iceland has the most tractors per acre of arable land, but the second least amount of actual arable land of all countries that practice agriculture. More relevantly, Iceland is a global leader in renewable energy, supplying approximately 80% of its total energy demand from renewable sources. The country has abundant geothermal and hydroelectric resources that are used for heating and electricity generation respectively. In fact, the only fossil fuel burned in Iceland is the gasoline used to power everyone’s cars!

A geothermal plant in Iceland.

As part of the program, our group got guided tours of two geothermal and hydroelectric power plants and two days of energy lectures from professors at Reykjavik University’s School of Energy. We were also invited to a reception by Iceland’s President, Olafur Grimsson, where we discussed global renewable energy policy and how we might be able to implement some of the lessons learned in Iceland when we return to our home countries. At the end of the program, we developed innovative Capstone Projects and got feedback on their feasibility. And that was only the educational aspect of the program! When not working, we took advantage of Iceland’s stunning natural beauty, doing everything from soaking in hot springs to hiking on glaciers.

I’d like to conclude by saying that I only became aware of this fascinating program by being part of the GCI. As we’ve become more established and started getting more recognition outside of U of T, we’ve received many new opportunities for our members to get involved in outside initiatives. This has helped us expand our knowledge of sustainability, and helped us professionally by introducing us to many new contacts. To students, this is hugely helpful and I encourage anyone with an interest in sustainability to get involved in any initiative that tries to lessen our impact on our planet.

And try to go to Iceland. You won’t regret it.