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Here the Lewis acidic CO2 molecule binds to the Lewis basic carbene center to form the product carboxylate on the right. This reaction can be reversed by heating or by reducing the CO2 pressure, or the carboxylate intermediate can be further reduced to methanol.2 More recently, bifunctional “frustrated” Lewis acid–base pairs (see “Getting a Grip on CO2”) have been exploited to the same end:3 Acids and bases are the yin yang of chemistry—opposite yet interconnected forces behind chemical bonding and reactions. In the Lewis definition, an acid is an electron pair acceptor and a base an electron pair donor. When brought together, the female acid and male base tend to combine to form an acid-base bair, neutralizing each other. Most common molecules are thus either Lewis acidic or basic, but not both. Getting A Grip on CO2 Frustrated Lewis pairs are cleverly designed molecules that break this rule.4 These molecules contain acidic and basic elements linked together in a way that prevents the two from internally neutralizing one another. These frustrated systems can promote normally difficult reactions, such as the heterolytic splitting of H2. CO2 as a molecule is Lewis acidic—the C center is electron-deficient and likes to behave as an electron pair donor, as in its reactions with amines described in the sidebar “Aqueous Amines for CO2 Separation” in the liquids panel report. The O centers are weakly Lewis basic, becoming more so when CO2 combines with a base. This internal yin yang can be exploited in reactions with frustrated Lewis pairs. As shown in the image, a properly designed frustrated pair (purple, basic phosphorus, and light blue, acidic boron) can put a pincer grip on CO2, grabbing both the more acidic carbon (green) and somewhat basic oxygen (red).3 Because both the shape of the pincer and the strengths of the acidic and basic ends can be tuned, frustrated pairs hold promise for reversible CO2 capture. 46PDF Image | 2020 Carbon Capture
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