Cyclopropane behaves as a stronger bronsted acid as compared to cyclohexane- explain?
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A stronger Bronsted-Lowry acid is, by definition, the stronger proton donor. The ideal bond angle between carbon atoms is 109.5 degrees. In cycloproprane, the bond angle is 60 degrees, and for the sp3 hybridized carbon, this is not ideal. As this is so far from the ideal, cyclopropane is said to have high ring strain, which causes instability. Thus a higher likelihood of donating a proton. Cyclohexane, has a bond angle very close to 109.5, thus it has significantly lower ring strain (the lowest of any cyclic alkane), and is more stable. So, it is less likely to donate a proton.
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