what are the functional groups in organic chemistry?

please list the must know ones in a bond-like template.

Experiment - Claisen Condensation Reactions:

In this experiment, we performed a Claisen condensation reaction of ethyl phenylacetate using potassium tert-butoxide to form ethyl 3-oxo-2,4-diphenylbutanoate and ethanol without using a solvent. This allowed us to reduce waste, have reagents that have a relatively low toxicity level, and made the reaction much more convenient.

Question 2: If this reaction were run in a solution (as opposed to solvent-free) it would require several hours of refluxing and provide a much smaller yield. Why is this the case?

I cannot seem to find an answer to this question. The only thing that I can find is that the reaction is reversible when a solvent is used (which I'm assuming means that the reaction is not reversible when there is no solvent). If this is correct, why is the reaction reversible when a solvent is used, and not reversible when a solvent is not used?

A source for the answer would be appreciated if possible.

Thank you for the help in advance!

Develop a hypothesis to explain why the protein is folded in its native state

A 2.46 g sample of a substance suspected of being pure gold is warmed to 72.7 ∘C and submerged into 15.0 g of water initially at 24.7 ∘C. The final temperature of the mixture is 26.6 ∘C.

Part A:

What is the specific heat capacity of the unknown substance?

Part B:

Could the substance be pure gold?

1. Name and draw two biocompatible hydrophilic polymers. Briefly describe their applications. Circle the functional groups that interact with water. What type(s) of interaction is (are) involved?

2. Draw the following tripeptides in their predominant form at pH 7. Determine the net charge of the predominant form of the peptides at pH 1, pH 7, and pH 12. a. Phe-Thr-Lys b. Trp-Arg-Asp

If you began with 5.5 mL of 0.20 M NaHCO₃, how many mL of 0.10M HCl would you need to add to get a pH 7 buffer? Given that carbonic acid, H₂CO₃, has a pK_a1 = 6.37 and a pK_a2 = 10.33

Which of the following bases should be used to prepare a buffer with a pH of 4.5?

ammonia, K_b = 1.8 × 10^-5

hydroxylamine, K_b = 1.1 × 10^-8

codeine, K_b = 1.6 × 10^-6

pyridine, K_b = 1.7 × 10^-9

anyline, K_b = 3.8 × 10^-10

The heat of combustion of benzoic acid (C6H5COOH) is -3226 kJ/mol. When 0.919 g of benzoic acid was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose from 22.25 °C to 26.27 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

A Vi = 10-3 m3 chamber of a gas bottle contains some argon gas (atomic weight = 0.040 kg/mole) at a pressure of 104 Pa and a temperature of 34� C. 1)What is the number density of atoms in this chamber? N/V =

Draw sigma only molecular orbital diagram for CH4 assuming square planar geometry.

Use the following data to work through problems 4-6.

• 50.0 mL of each solution was used in each experiment.
• Each solution had a molarity of 2.00 M.
• The density of the solutions once mixed are 1.03 g/mL.
• The following table is data collected from an actual experiment.

1. Calculate the amount of heat energy, q_surroundings, produced in each reaction. Use 03 g/mL for the density of all solutions. Use the specific heat of water, 4.184 J/(g•°C), for each of the three reactions. q_surroundings = C_s ´ m ´ ∆T

2. Calculate the enthalpy change, ∆H_reaction, per mole of reactant for each of the three reactions in units of kJ/mole.

                                    ∆H_reaction = ∆H_system

3. Calculate a percent error between the accepted values for ∆H_reaction(use values calculated in question 1 as accepted values) and the “experimental” values you calculated in question 5 for each reaction.

                        % Error = Experimental – Accepted x 100

                                                Accepted

A 1.268 g sample of a metal carbonate, MCO33, was treated 100.00 mL of 0.1083 M H22SO44, yielding CO22 gas and an aqueous solution of the metal sulfate. The solution was boiled to remove all of the dissolved CO22 and then was titrated with 0.1241 M NaOH. A 71.02 mL volume of the NaOH solution was required to neutralize the excess H22SO44.

Start by writing a balanced chemical equation for this reaction.

What's the identity of the metal?

Give the elemental symbol

How many grams of CO2 gas were produced?

1) The correct arrangement of the following complex ions in terms of increasing crystal field splitting energy (D) is:

[CrI₆]^3-            [CrF₄]^-            [Cr(en)₃]³⁺            [W(en)₃]³⁺

a) Smallest [CrI₆]^3- < [Cr(en)₃]³⁺ < [CrF₄]^- < [W(en)₃]³⁺ Largest

b) Smallest [CrI₆]^3- < [W(en)₃]³⁺ < [CrF₄]^- < [Cr(en)₃]³⁺ Largest   

c) Smallest [CrF₄]^- < [CrI₆]^3- < [Cr(en)₃]³⁺ < [W(en)₃]³⁺ Largest

d) Smallest [CrF₄]^- < [W(en)₃]³⁺ < [CrI₆]^3- < [Cr(en)₃]³⁺ Largest

e) Smallest [W(en)₃]³⁺ < [Cr(en)₃]³⁺ < [CrF₄]^- < [CrI₆]^3- Largest

2) Determine the number of unpaired electrons for each of the following coordination complexes:

Arrange these complexes in order of increasing number of unpaired electrons (in the answers below an = sign is used if two complexes have the same number of electrons).

a) Fewest [Pt(CN)₄]^2– < [Ni(H₂O)₆]²⁺ < Cr(CO)₆ < [CoCl₆]^2– Greatest

b) Fewest [Pt(CN)₄]^2– = Cr(CO)₆ < [CoCl₆]^2– < [Ni(H₂O)₆]²⁺ Greatest

c) Fewest [Pt(CN)₄]^2– < Cr(CO)₆ < [CoCl₆]^2– < [Ni(H₂O)₆]²⁺   Greatest

d) Fewest [Pt(CN)₄]^2– < Cr(CO)₆ < [Ni(H₂O)₆]²⁺ < [CoCl₆]^2– Greatest

e) Fewest [Pt(CN)₄]^2– = Cr(CO)₆ < [Ni(H₂O)₆]²⁺ < [CoCl₆]^2– Greatest

The pH of solution containing 1 mol Cu(OH)2 in 1L water is 7.66.

Has all the Cu(OH)2 dissolve in water? Ksp=4.8 × 10^-20.