Abstract:A physical organic chemistry experiment
is described for second-year
college students. Students performed nucleophilic aromatic substitution
(NAS) reactions on 5,10,15,20-tetrakis(2,3,4,5,6-pentafluorophenyl)porphyrin
(TPPF20) using three different nucleophiles. Substitution
occurs preferentially at the 4-position (para) because
it is thermodynamically favored, and the 2- and 6- (ortho) positions are kinetically disfavored because of steric interactions
with the porphyrin ring. The activation energy depends … Show more
“…The subsequent analysis in the context of competing reaction pathways is not reported in the chemistry education literature. A literature search reveals experimental determination of transition state energies that focus on a single reaction pathway or infer thermochemical properties from quantum-chemical calculations. − To the best of our knowledge, this is the first undergraduate laboratory procedure that emphasizes product distributions when reactions are conducted under kinetic vs thermodynamic control by microwave-assisted techniques. Moreover, activation parameters (ΔΔ H ⧧ (≈ Δ E a ), ΔΔ S ⧧ , and ΔΔ G ⧧ ) are directly accessible by analysis of product ratios determined under kinetic control.…”
The effects of kinetic vs thermodynamic control on endo/exo stereoisomer ratios can be observed in a simple Diels−Alder reaction between Nphenylmaleimide and furan. The use of microwave-promoted synthesis affords the cycloadducts in yields ranging from 65−100%, employing reaction times of 1−10 min at temperatures of 55−130 °C. Short reaction times enable screening of numerous reaction conditions (time and temperature) within a single lab period, where endo:exo product ratios follow the primary facets of kinetic and thermodynamic control. Analysis of product ratios obtained under kinetic control allows for the evaluation of activation parameters (ΔΔH ⧧ (≈ ΔE a ), ΔΔS ⧧ , and ΔΔG ⧧ ) by means of the Arrhenius and Eyring equations. Values of ΔΔH ⧧ , ΔΔS ⧧ , and ΔΔG ⧧ were found to be 6.4 ± 0.3 kJ mol −1 , 16.5 ± 0.9 J mol −1 K −1 , and 1.5 ± 0.4 kJ mol −1 (ΔΔ: exo − endo), respectively. Experimentally determined activation parameters correlate well with quantum-chemical calculations. Several key teaching points are also addressed, including frontier molecular orbital analysis, reversibility of the Diels−Alder reaction, column chromatography, and the use of 1 H nuclear magnetic resonance spectroscopy to assess both stereoisomeric yield and purity.
“…The subsequent analysis in the context of competing reaction pathways is not reported in the chemistry education literature. A literature search reveals experimental determination of transition state energies that focus on a single reaction pathway or infer thermochemical properties from quantum-chemical calculations. − To the best of our knowledge, this is the first undergraduate laboratory procedure that emphasizes product distributions when reactions are conducted under kinetic vs thermodynamic control by microwave-assisted techniques. Moreover, activation parameters (ΔΔ H ⧧ (≈ Δ E a ), ΔΔ S ⧧ , and ΔΔ G ⧧ ) are directly accessible by analysis of product ratios determined under kinetic control.…”
The effects of kinetic vs thermodynamic control on endo/exo stereoisomer ratios can be observed in a simple Diels−Alder reaction between Nphenylmaleimide and furan. The use of microwave-promoted synthesis affords the cycloadducts in yields ranging from 65−100%, employing reaction times of 1−10 min at temperatures of 55−130 °C. Short reaction times enable screening of numerous reaction conditions (time and temperature) within a single lab period, where endo:exo product ratios follow the primary facets of kinetic and thermodynamic control. Analysis of product ratios obtained under kinetic control allows for the evaluation of activation parameters (ΔΔH ⧧ (≈ ΔE a ), ΔΔS ⧧ , and ΔΔG ⧧ ) by means of the Arrhenius and Eyring equations. Values of ΔΔH ⧧ , ΔΔS ⧧ , and ΔΔG ⧧ were found to be 6.4 ± 0.3 kJ mol −1 , 16.5 ± 0.9 J mol −1 K −1 , and 1.5 ± 0.4 kJ mol −1 (ΔΔ: exo − endo), respectively. Experimentally determined activation parameters correlate well with quantum-chemical calculations. Several key teaching points are also addressed, including frontier molecular orbital analysis, reversibility of the Diels−Alder reaction, column chromatography, and the use of 1 H nuclear magnetic resonance spectroscopy to assess both stereoisomeric yield and purity.
“…Latimer et al compared microwave-induced organic reaction enhancement to that of more traditional synthetic procedures toward S N Ar reaction . Rizvi et al determined the activation energy of S N Ar on porphyrins . Goodrich et al employed S N Ar reaction as one of the reactions in the synthesis of a fluorescent acridone …”
Section: Introductionmentioning
confidence: 99%
“…Even though aryl halides are generally inert to nucleophilic substitution, aryl halides that contain electron withdrawing groups such as a nitro group ortho or para to the halogen undergo nucleophilic aromatic substitution. Variations of S N Ar experiments have been developed for chemistry education in the past, each with distinct value. − For example, Santos et al developed a problem-solving and collaborative-learning approach to the synthesis of aryl-substituted 2,4-dinitrophenylamines to facilitate higher retention and encourage students to interpret and draw conclusions from data themselves . Avila et al redesigned the synthesis of 2-ethylbenzoic acid into a five-step microscale experiment .…”
Section: Introducing
the Experimentsmentioning
confidence: 99%
“…39 Rizvi et al determined the activation energy of S N Ar on porphyrins. 40 Goodrich et al employed S N Ar reaction as one of the reactions in the synthesis of a fluorescent acridone. 41 Ambrose University, 42 a liberal arts university with smaller class sizes, is committed to the incorporation of green chemistry practices into chemistry laboratories with safer chemicals and processes.…”
This paper revisits the tie-dyeing
process through a bioinspired
and safer alternative to nucleophilic aromatic substitution (SNAr) reactions for an introductory organic chemistry laboratory.
The simple and straightforward experiment provides students with an
opportunity to gain practical experience in conducting a chemical
reaction in a real-world context while applying concepts of design
for biodegradability and reusability. The water-soluble reactive dye
that replaces the use of a conventional SNAr substrate
does not require any heavy metals, toxic substances, or mordants but
utilizes a much less toxic and safer sodium carbonate to generate
the cellulosate nucleophile. This reaction generates no waste, and
the end-product, the tie-dyed T-shirt, is reusable and biodegradable.
Through this experiment, students can see connections between chemistry
and environmental health while gaining a practical insight into dyeing
chemistry, making use of a systems thinking approach. This experiment
serves not only to employ safer alternatives to hazardous chemicals
in the undergraduate organic chemistry laboratory but also to educate
students to recognize the relevance and importance of applying green
chemistry wherever it is possible, emphasizing life cycle thinking
and stewardship.
“…This helps students understand (a) the relationship between temperature and reaction rate and (b) why spontaneous processes (such as combustion) often require an initial input of energy to get started. Many undergraduate-level laboratory experiments have been devised to determine the activation energy of chemical reactions using tools such as spectroscopy, , chromatography, calorimetry, , and even “levitating” magnetic beads to monitor solution density . These experiments are creative and well-designed and yield consistent results, but often they require the use of expensive equipment or clever mathematical manipulations that may be unnecessarily confusing for high school students and first-year college students.…”
A highly visual, inexpensive, straightforward
laboratory experiment
for the determination of the activation energy of a demulsification
process is presented. The experiment uses low-density polyethylene
(LDPE) beads to clearly mark the interface between an NaCl(aq) solution
and isopropanol. The NaCl(aq)–isopropanol system is shaken
to produce an emulsion, and the rate of demulsification is subsequently
observed at different temperatures. The Arrhenius equation is then
used to relate the rate and temperature data to an energy of activation
for the demulsification process. A total of 36 undergraduate laboratory
groups in first-year chemistry courses performed this experiment.
The students’ data consistently yielded linear Arrhenius plots
with an average R
2 value of 0.928 ±
0.035. The activation energy of the demulsification process described
in this work was found to be 34.3 ± 2.5 kJ/mol. The reproducibility
of the results, the simplicity of the data collection, and the low
cost of the materials make this laboratory exercise easily adaptable
to a variety of grade levels, from middle school students to first-year
college students.
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