Chemical clock

In an iodine clock reaction, colour changes after a time delay.

A chemical clock (or clock reaction) is a complex mixture of reacting chemical compounds in which the onset of an observable property (discoloration or coloration) occurs after a predictable induction time due to the presence of clock species at a detectable amount.[1] In cases where one of the reagents has a visible color, crossing a concentration threshold can lead to an abrupt color change after a reproducible time lapse.

Types

Clock reactions may be classified into three or four types:[2]

Substrate-depletive clock reaction

The simplest clock reaction featuring two reactions:[2]

A → C (rate k1)
B + C → products (rate k2, fast)

When substrate (B) is present, the clock species (C) is quickly consumed in the second reaction. Only when substrate is all used up or depleted, species C can build up in amount causing the color to change. An example for this clock reaction is the sulfite/iodate reaction or iodine clock reaction, also known as Landolt's reaction.

Sometimes, a clock reaction involves the production of intermediate species in three consecutive reactions.

P + Q → R
R + Q → C
P + C → 2R

Given that Q is in excess, when substrate (P) is depleted, C builds up resulting in the change in color.

Autocatalysis-driven clock reaction

The basis of the reaction is similar to substrate-depletive clock reaction, except for the fact that rate k2 is very slow leading to the co-existing of substrates and clock species, so there is no need for substrate to be depleted to observe the change in color. The example for this clock is pentathionate/iodate reaction.[2][3]

Pseudoclock behavior

The reactions in this category behave like a clock reaction, however they are irreproducible, unpredictable and hard to control. Examples are chlorite/thiosulfate and iodide/chlorite reactions.[2]

Crazy clock reaction

The reaction is irreproducible in each run due to the initial inhomogeneity of the mixture which result from variation in stirring rate, overall volume as well as geometry of the reactors. Repeating the reaction in the statistically meaningful manners leads to the reproducible cumulative probability distribution curve. The example for this clock is iodate/arsenous acid reaction.[4]

One reaction may fall into more than one classification above depending on the circumstance. For example, iodate−arsenous acid reaction can be substrate-depletive clock reaction, autocatalysis-driven clock reaction and crazy clock reaction.

Examples

One class of example is the iodine clock reactions, in which an iodine species is mixed with redox reagents in the presence of starch. After a delay, a dark blue color suddenly appears due to the formation of a triiodide-starch complex.

Additional reagents can be added to some chemical clocks to build a chemical oscillator. For example, the Briggs–Rauscher reaction is derived from an iodine clock reaction by adding perchloric acid, malonic acid and manganese sulfate.[5]

See also

  • Circadian clock
  • Chemical oscillator

References

  1. ^ Wright, Stephen W. (2002-01-01). "Tick Tock, a Vitamin C Clock". Journal of Chemical Education. 79 (1): 40A. doi:10.1021/ed079p40.
  2. ^ a b c d Horváth, Attila K.; Nagypál, István (23 February 2015). "Classification of Clock Reactions". ChemPhysChem. 16 (3): 588–594. doi:10.1002/cphc.201402806. PMID 25425415.
  3. ^ Xu, L.; Horváth, A.K. (2014). "A Possible Candidate To Be Classified as an Autocatalysis-Driven Clock Reaction: Kinetics of the Pentathionate-Iodate Reaction". Journal of Physical Chemistry. 118 (32): 6171–6180. Bibcode:2014JPCA..118.6171X. doi:10.1021/jp5057573. PMID 25068832.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  4. ^ Valkai, L.; Csekő, G.; Horváth, A.K. (2015). "Initial inhomogeneity-induced crazy-clock behavior in the iodate-arsenous acid reaction in a buffered medium under stirred batch conditions". Phys Chem Chem Phys. 17 (34): 22187–22194. Bibcode:2015PCCP...1722187V. doi:10.1039/c5cp02572a. PMID 26239390.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  5. ^ Briggs, Thomas S.; Rauscher, Warren C. (1973-07-01). "An oscillating iodine clock". Journal of Chemical Education. 50 (7): 496. Bibcode:1973JChEd..50..496B. doi:10.1021/ed050p496. ISSN 0021-9584.

Media files used on this page

Iodine clock - persulphate.ogv
Author/Creator: TheSmuel, Licence: CC BY-SA 3.0
Video of iodine clock reaction. Potassium persulphate is used to oxidize iodide ions to iodine, in the presence of starch and a small amount of thiosulphate ions. When the thiosulphate is exhausted (by reaction with the iodine produced), the dark blue iodine-starch complex is formed. The time taken for the blue colour to appear varies with rate of reaction and can be used to study the reaction kinetics.
For the purposes of this video, the reaction is catalysed by Fe2+ ions to drastically shorten the time for the colour change to occur.