a. Draw and name all of the isomeric products obtained from the monobromination of propane with Br2/ light. If halogenation were a completely random reaction and had an equal probability of occurring at any of the C—H bonds in a molecule, what percentage of each of these monobromo products would be expected? b. Answer part (a) using 2-methylpropane as the starting material.
> For each of the elements Ca, K, Cu, Zn, Br, and Kr, provide the following information: a. Which are metals? b. Which are representative metals? c. Which are inert or noble gases?
> Which group of the periodic table is known as the noble gases? List their names.
> Rank the following in order of increasing bond length: single bond, double bond, triple bond
> Use LeChatelier’s principle to predict the effects, if any, of each of the following changes on the equilibrium system, described below, in a closed container. C(s) + 2H2 (g) ↽−−−−⇀ CH4 (g) + 18 kcal a. C is added. b. H2 is added. c. CH4 is removed. d.
> Calculate the pH of a solution that is: a. 1.0 × 10-1 M in HCl b. 1.0 × 10-5 M in HNO3
> Express each of the following in units of psi: a. 12.5 cm Hg b. 46.0 torr c. 254 mm Hg d. 0.48 atm
> A 0.0500-mol sample of a nutrient substance is burned in a bomb calorimeter containing 2.00 × 102 g H2O. If the formula weight of this nutrient substance is 114 g/mol, what is the fuel value (in nutritional Cal) if the temperature of the water increased
> A 0.325-mol sample of ammonium nitrate was dissolved in water producing a 4.00 × 102 g solution. The temperature decreased from 25.08C to 15.70C. If the specific heat of the resulting solution is 1.00 cal/g · 0C, calculate the quantity of energy absorbed
> What is plane-polarized light?
> a. Why is DNA polymerase said to be template-directed? b. Why is DNA replication a self-correcting process?
> Why don’t proteins turn around in biological membranes like revolving doors?
> What enzymatic reactions of gluconeogenesis bypass the irreversible steps of glycolysis?
> Why are there several alternative mRNA sequences that could encode the same peptide?
> Explain the feedforward activation mechanism that results in the activation of pyruvate kinase.
> Explain the role of allosteric enzymes in control of glycolysis.
> Contrast ionic and covalent compounds with respect to their relative melting points.
> Except for the functional groups attached to the rings, the nitrogenous bases are largely flat, hydrophobic molecules. Explain why the arrangement of the purines and pyrimidines found in DNA molecules is very stable.
> A balloon, filled with an ideal gas, has a volume of 5.00 L at 500F. At what temperature (0F) would the balloon’s volume double?
> Which of the following structures have incorrect IUPAC names? If incorrect, give the correct IUPAC name. a. CH,C=CCH,CH(CH), 2-Methyl-4-hexyne b. CH,CH2, CH,CH, CH,CH, н H. 3-Ethyl-3-hexene c. CH,CH(CH,)CH,C=CCH,CH(CH,) CH,CH, с. 2-Edhy-7-methyl-4-о
> What is the function of the enzyme primase?
> Describe the stages of protein digestion, including the location of each.
> Saturated fatty acids have higher melting points than monounsaturated fatty acids. Polyunsaturated fatty acids have even lower melting points. Develop a hypothesis to explain this observation.
> Discuss the digestion of dietary carbohydrates, lipids, and proteins.
> a. What is the ultimate goal of genetic engineering? b. What ethical issues does this goal raise?
> How do the sulfa drugs selectively kill bacteria while causing no harm to humans?
> How is it possible for sickle cell trait to confer a survival benefit on the person who possesses it?
> List the functions of each of the coenzymes. What classes of enzymes would require these coenzymes?
> a. What properties are associated with molecular solids? b. Provide two examples of molecular solids.
> How many protons, neutrons, and electrons are present in a single atom of: a. phosphorus-30 b. sulfur-32 c. chlorine-35
> Why was the Benedict’s reagent useful for determining the amount of glucose in the urine?
> Describe the classification of the R groups of the amino acids, and provide an example of each class.
> Can you think of any disadvantage associated with the use of isotopes described in Question 9.13? Explain. Question 9.13: Describe the advantage of using isotopes with short half-lives for tracer applications in a medical laboratory.
> How does extremely low pH cause proteins to coagulate?
> Explain the difference between the d- and l-designation and the (1) and (2) designation.
> Why would you predict that a carboxylic acid would be more polar and have a higher boiling point than an alcohol of comparable molar mass?
> Write an equation representing the reaction catalyzed by each of the enzymes listed in Practice Problem 19.1e through i at the end of Example 19.1. (Hint: You may need to refer to the index of this book to learn more about the substrates and the reaction
> How is LDL taken into cells?
> How can structural analogs serve as enzyme inhibitors?
> What is the benefit for an enzyme such as triacylglycerol lipase to be regulated by covalent modification, in this case phosphorylation?
> Calculate the [HCO3-]/[H2CO3] that corresponds to a pH of 7.4. The Ka for carbonic acid is 4.2 × 10-7.
> What is the difference between lactose intolerance and galactosemia?
> Explain why genetic mutations that result in the replacement of one amino acid with another can lead to the formation of a protein that cannot carry out its biological function.
> Describe the series of experiments that characterized the electron.
> What are the principal uses of methanol, ethanol, and isopropyl alcohol?
> Write the structure of each of the following peptides: a. Lys-trp-pro b. Gln-ser-his c. Arg-met-asp
> Write an equation to show a reaction that would produce each of the following amines: a. 1-Pentanamine b. N, N-Dimethylethanamine c. N-Ethyl propanamine
> A typical concentration of magnesium ion in certain types of intravenous solutions is 3 meq/L. Represent this concentration in mol/L.
> What is the function of lactic acid in food products? Of what significance is lactic acid in muscle metabolism?
> Is the solution osmolarity that you calculated in Question 6.11 isotonic with blood plasma? Why or why not? Question 6.11: Refer to the intravenous solution in Figure 6.7 and calculate the osmolarity of its contents. Figure 6.7: Composition and conce
> Predict which compound in each of the following pairs should have the higher melting and boiling points (Hint: Write the Lewis structure and determine whether the compound is ionic, polar covalent, or nonpolar covalent.): a. C2H6 and CH4 c. F2 and Br2 b
> Why do the hydrocarbon tails of membrane phospholipids provide a barrier between the inside and outside of the cell?
> How does the structure of amylose differ from that of amylopectin and glycogen?
> State Hund’s rule. Determine whether the following orbital diagrams violate Hund’s rule. а. 1s 2s 2p b. 1s 2s 2p C. 1s 2s 2p
> List the functions of several a-globulins.
> By comparing two solutions: 0.50 M sodium chloride (an ionic compound) and 0.50 M sucrose (a covalent compound). Each solution is separated from water by a semipermeable membrane. Which solution has the higher osmotic pressure?
> Distinguish among the three types of glycosphingolipids, cerebrosides, sulfatides, and gangliosides.
> Describe the purpose of a titration.
> Indicate whether the side chains of each of the amino acids listed in Question 18.1 is polar, nonpolar, basic, or acidic. Question 18.1: Write the one-letter and three-letter abbreviations, and draw the structure of each of the following amino acids. a
> What is the function of each of the four types of plasma lipoproteins?
> What is a heteropolysaccharide?
> How do antibodies protect us against infection?
> Give the Lewis structure for each of the following compounds: a. HNO3 b. CCl4 c. PBr3 d. CH3CH2OH
> How are the structural differences between triglycerides and phospholipids reflected in their different biological functions?
> An instrument for cancer treatment containing a cobalt-60 source was manufactured in 1988. In 1995, it was removed from service and, in error, was buried in a landfill with the source still in place. What percentage of its initial radioactivity will rema
> Do you think that a diet higher in omega-3 fatty acids would be an effective treatment for the symptoms of arthritis? Defend your answer.
> How would you produce a Fischer Projection beginning with a three-dimensional model of a sugar?
> Explain the bond angles of ethyne in terms of the valenceshell electron-pair repulsion (VSEPR) theory.
> Explain the bond angles of ethene in terms of the valenceshell electron-pair repulsion (VSEPR) theory.
> List the biological functions of lipids.
> Using Lewis structures and VSEPR, predict whether each of the following molecules is polar: a. CO2 b. SCl2 c. BrCl d. BCl3
> Express each of the following in units of atm: a. 10.0 torr b. 61.0 cm Hg c. 275 mm Hg d. 124 psi
> The reaction: 2NO(g) + O2 (g)−−−−→2NO2 (g) is one step in the process of forming atmospheric smog. a. How many g of NO2 can be produced by the reaction of excess O2 with 50.0 g of NO? b. If the actual yield of NO2 is 50.0 g, what is the % yield?
> Explain the mechanism by which glutamate and NO may function to promote development of memories and learning.
> For the equilibrium situation involving acetic acid, CH3COOH (aq) + H2O(l) −↽−−−−−−⇀− CH3COO-(aq) + H3O+(aq), explain the equilibrium shift occurring for the following changes: a. A strong base is added to the solution. b. More acetic acid is added to th
> Explain how the molar concentration of carbonic acid in the blood would be changed during a situation of alkalosis.
> For the reaction 47 kcal + 2SO3 (g)↽−−−−⇀2SO2 (g) + O2 (g) predict the effect on the position of the equilibrium (will it shift to the left or to the right, or will there be no change?) for each of the following changes. a. The temperature is increased.
> Where do a-amylase and b-amylase carry out their enzymatic functions?
> Titration of 17.85 mL of HNO3 solution requires 16.00 mL of 0.1600 M KOH solution. What is the molarity of the HNO3 solution?
> What metabolic defect causes galactosemia?
> How can Le Chatelier’s principle help us to increase yields of chemical reactions?
> Which of the following alcohols can be oxidized to a carboxylic acid? Name the carboxylic acid produced. For those alcohols that cannot be oxidized to a carboxylic acid, name the final product. a. Ethanol b. 2-Propanol c. 1-Propanol d. 3-Pentanol
> Describe the rules for determining the common names of carboxylic acids.
> Define the terms primary, secondary, and tertiary alcohol, and draw a general structure for each.
> For each pair of compounds, predict which would have the higher boiling point. Explain your reasoning. a. Propanamine or propanol b. Propane or ethanamine c. Methanamine or water d. Propyl methylamine or pentane
> Describe the role of disulfide bonds in the synthesis and structure of insulin.
> Calculate the osmotic pressure of 0.50 M C6H12O6 (nonelectrolyte).
> Describe the relationship between acyl group transfer and the process of protein synthesis.
> Design the synthesis of each of the following esters from organic alcohols. a. Methyl butanoate (apples) b. Octyl ethanoate (oranges)
> In your own words, describe the steps used to name a compound, using IUPAC nomenclature.
> Calculate the pH of a 1.0 × 10-5 M solution of NaOH.
> The element lithium has two naturally occurring isotopes. One of these has a mass of 6.0151 amu and a natural abundance of 7.49%. A second isotope has a mass of 7.0160 amu and a natural abundance of 92.51%. Calculate the atomic mass of lithium.
> Describe an experiment that would enable you to determine the mass (g) of solids suspended in a 1-L sample of seawater.
> Explain the significance of thioester formation in the metabolic pathways involved in fatty acid and carbohydrate breakdown.
> Cu2+(aq) can be reduced in an electrolytic cell to prepare high purity copper metal. a. Does this reduction take place at the positive or negative electrode of the electrolytic cell? Why? b. In this electrode termed the cathode or the anode? c. Write the
> Write the net ionic equation for the reaction of Pb(NO3)2(aq) with K2S(aq).
> Describe an application of reasoning involving the scientific method that has occurred in your day-to-day life.
> The tsetse fly Glossina morsitans is a large biting fly found in regions of Africa. They carry sleeping sickness, a deadly disease caused by a parasitic protozoan. The pheromone secreted by the tsetse fly contains four straight-chain alkanes: 2-methylhep
> Define each of the following radiation units: a. rad b. rem c. gray
> Describe the IUPAC rules for naming cycloalkanes.
> Calculate both [H3O+] and [OH+] for a solution for which: a. pH = 5.50 b. pH = 7.00
