Post-lab 3

Make sure you label everything as labeled as asked and make sure you explain everything is asked step by step.

7. Now circle the lewis acid and lewis base sites on the following compounds. Some compounds may have both or just one. Note you can use LA for lewis acid and LB for lewis base as labels. S-H H.

The synthesis of an azo dye is shown below. Please answer the following questions. NH2 1) Na2CO3 2) NaNO2, HCI B N-Ñ A Š3H ŠO3 Step 1 Step 2 ŠO3 2 1 1. Why you need to add Na2CO3 in step 1? (multiple answers) Oa)To decrease the solubility of compound 1 - "salting out" ob) To deprotonate compound 1, increase solubility in water Oc) To increase the reaction yield Od)To slow down the reaction rate Oe)To neutralize the HCI

4. For the following question please consider the four chemicals shown below. Me H2N s, NH2 acetaldehyde Chemical 1 methanamine Chemical 2 S-methyl ethanethioate Chemical 3 ethanamine Chemical 4 Chemical 4 will readily react with two other chemicals above. a. What are those two chemicals? b. Provide a chemical structure of formed products along with a probable mechanism using the arrow formalism. c. At which of the following pH's (out of 1,7,14) do you expect each reaction to occur? Why?

Select the stronger base and then draw its conjugate acid below. CICH₂CH₂O or CH3CH₂O- • You do not have to consider stereochemistry. • You do not have to explicitly draw H atoms. • You do not have to include lone pairs in your answer. Ⓡ OO. n[1] ? ChemDoodle

Please don't provide handwritten solution ....

.A justification for the rankings based on the factors that influence the relative stability of the different conjugate bases. I need to answer these for C3H5ClO2, ClCH2CO2, and CH3COOH. (Acetic acid, 3-chloropropanic, and chloroacetic acid). Pleaseeee help I will definitely rate

Draw the structure of the conjugate base of the acid given below. (Note that the acidic H in consideration is bold and underlined.)

Draw the structure of the product of the reaction between the compound shown below and H2SO4.

I'm stuck on step 3. Please help, thank you

Answer questions a-c about the Bronsted acid-base reaction below using the identifying letters A-D below each structure. A table of pK, values for various organic and inorganic acids can be found in the references section. CH₂ -NH3 A ethylammonium + CH₂ B ethoxide CH₂ "NH₂ + CH₂ C ethylamine a) The weaker base is b) Its conjugate acid is c) The species that predominate at equilibrium are (two letters, e.g. AC) OH D ethanol

From each pair, select the stronger base. Then draw the conjugate acid of the strong base below. CH3CH20 or CH3CEC • You do not have to consider stereochemistry. You do not have to explicitly draw H atoms. • You do not have to include lone pairs in your answer. C opy aste

In the following acid-base reactions, 1. draw Lewis structures of the reactants and the products. 2. determine which species are acting as electrophiles (acids) and which are acting as nucleophiles (bases). 3. use the curved-arrow formalism to show the movement of electron pairs in these reactions, as well as the imaginary movement in the resonance hybrids of the products. 4. indicate which reactions are best termed Brønsted-Lowry acid-base reactions. (c) -BH₁₂ BH3 + CH3-O-CH3 → CH3-O-CH3 (d) 유 0- CH3-C H + -OH CH₁₂-C-H OH

Draw the major organic products of Hofmann elimination from the following amine. CH3 NHCHCH2CH2CH2CH3 You do not have to consider stereochemistry. • You do not have to explicitly draw H atoms. • Do not include lone pairs in your answer. They will not be considered in the grading. • Draw one structure per sketcher. Add additional sketchers using the drop-down menu in the bottom right corner. Separate multiple products using the + sign from the drop-down menu.

Please only answer if you are sure of the answer The choices are - Only Hydroxide - Only bicarbonate -Hydroxide or Bicarbonate -Neither hydroxide nor bicarbonate

3. The ranking of the acids in terms of increasing acid strength. 4. The ranking of the conjugate bases in terms of increasing base strength. 5.A justification for the rankings based on the factors that influence the relative stability of the different conjugate bases. I need to answer these for C3H5ClO2, ClCH2CO2, and CH3COOH. (Acetic acid, 3-chloropropanic, and chloroacetic acid). Pleaseeee help I will definitely rate

Reversed phase HPLC refers to the condition of stationary phase and a mobile phase of separation. Select the best condition A. A hydrophilic stationary phase is combined with a non-polar mobile phase. B. A hydrophilic stationary phase is combined with a polar mobile phase C. A hydrophobic stationary phase is combined with a polar mobile phase. D. A hydrophobic stationary phase is combined with a non-polar mobile phase. describe the statement

On... what is an is. 4-ethyl-2-.. is c-k polar.. [Review Topics] [References] Answer questions a-c about the Bronsted acid-base reaction below using the identifying letters A-D below each structure. A table of pK values for various organic and inorganic acids can be found in the references section. CH3 CH3 OH но HO HO, acetic acid bicarbonate acetate carbonic acid a) The weaker base is b) Its conjugate acid is c) The species that predominate at equilibrium are (two letters, e.g. AC)| Submit Answer Retry Entire Group 8 more group attempts remaining

Examine the molecules below. Which site is most basic? Which H is most acidic? Highlight this site. Highlight this H. H :S- H. :O:

6.. a) The structure of penicillin G is shown below. Circle the most acidic proton in the structure and give an approximate pKa value for that proton in the box povided. ortx Penicillin G + b) Based on your answer to part (a), calculate the equilibrium constant for the reaction of penicillin G with ammonia. Be sure to show your work for partial credit! NH3 Penicillin G Penicillin G O₂N Approximate pka = 0 pka = SH NH4 Keq c) The pka value of protonated penicillin G is approximately 6. Based on this information, calculate the pKa value ofthe thiol shown below, given that the equilibrium constant for the reaction is approximately 1. OH = 1 O₂N + Deprotonated Penicillin G Kea = Protonated Penicillin G pK₂ = 6

3. Give the pK₂ values for the following compounds and then rank them in terms of increasing acidity. Explain why the values change so dramatically (each pk- unit is an order of magnitude) from one member of the series to the next. H₂C=CH2 H₂C-CH₂ HC=CH

The two following molecules are very common reagents for organic synthesis. They botn have a basic nitrogen, but their pka's are very different (see values given in question 1). The goal of this problem is to understand why. N-H A 1) Please draw below the conjugated acid of A and B respectively: H base conjugated acid base conjugated acid pka of this acid/base pair: - 5 pka of this acid/base pair: ~ 0 2) Both molecules exhibit resonance forms (see below). Draw curved arrows to go from one resonance structure to the next (molecule A: 1->2; molecule B 1->2->3–>4->5). A 1 1 2 4 5

9.19, please

Curved arrows are used to illustrate the flow of electrons. In this reaction, a pi bond acts as a Bronsted base. Using the provided starting structures, draw the curved electron- pushing arrows for the acid-base reaction. Be sure to account for all bond-breaking and bond-making steps. Then draw the organic product of the reaction. + Include all lone pairs in the structures. Ignore inorganic byproducts and counterions. I I HH :CI. co THE I Select to Edit Arrows

7. Draw the conjugate acid for the aromatic compound and predict if the pKa will be closer to 10 or 5? need t Stronger 8. In general second-order resonance structures are not as important as first-order resonance structures. This is not usually the case with amides. Use the second-order resonance structure given below to explain why amides are very weak bases. NH₂ CH3 NH₂ Stronger NH₂ (+) 9. Indicate if each of the molecules is a stronger, weaker or similar base to aniline and provide an explanation. Oxygens make compounds Weaker (electronegative+y), brod While methyl groups make them stronger (electron donating groups). (Label as similar, stronger or weaker) HN-CH3 NH₂ Fir • Amides are weaker electron donors and have a negative woloua Charge if a hydrogen is removed. pKa =4.6 NH₂ p Ka will be closer to five. Weaker NO₂ quocib NH₂ mums lydig bas orH₂qdorb word d CH3 NO2 slax Stronger Stronger DAT NH Weaker O Similar NH

How is nucleophilicity (nucleophile strength) related to basicity?

Dr. Goode uses a rather specific three-steps procedure (described below) to cook up a spicy sugar derivative. Why does she make use of such a protocol? Describe the purpose of each steps. 1) acetone, cat. H 2) 2,5-dimethylbenzyl bromide, NaH 3) H30", r.t. он NH, "NH2 'Buo 'Buo "O'Bu O'Bu

Need help answering these two Qs and an explanation after solving asap. thank you.

help

[5] On the back of the quiz, derive the acid form of the Henderson-Hasselbalch Equation (above) as was done in class.

Chemistry Seeking help with this honest problem