Question: Write a balanced nuclear equation for positron

> Describe the relationship between the length of hydrocarbon chains and the melting points of the compounds.

> Why do linear alkanes have higher melting and boiling points than branched-chain alkanes?

> Describe London dispersion forces.

> The following is the structure of the pain reliever ibuprofen, found in Advil. Circle and label the functional groups of the ibuprofen molecule. OH Ibuprofen

> Folic acid is a vitamin required by the body for nucleic acid synthesis. The structure of folic acid is given below. Circle and identify as many functional groups as possible. H,NN N CH,NH- -NH–CHCH,CH,COOH OH ČOOH Folic acid

> Classify each of the carbon atoms in the following structures as primary, secondary, tertiary, or quaternary. a. CH3CH2C(CH3)2CH2CH3 b. CH3CH2CH2CH2CH(CH3) CH(CH3) CH3 c. d.

> What is the major structural feature that distinguishes between saturated and unsaturated hydrocarbons?

> Of the classes of compounds listed in Question 10.35, which are saturated? Which are unsaturated? Question 10.35: Give the general formula for each of the following: a. An alkane b. An alkyne c. An alkene d. A cycloalkane e. A cycloalkene

> Convert the following condensed formulas into structural formulas: a. CH3CH(CH3) CH(CH3) CH(CH3) CH2CH3 b. CH3C(CH3)2CH(CH2CH3) CH2CH2CH3

> Using the octet rule, explain why carbon forms four bonds in a stable compound.

> How do soaps assist in the removal of oil and grease from clothing?

> Convert the following line formulas into condensed formulas: b. а. d. с.

> Convert the following structural formulas into line formulas: a. b. c. H. H H-C-H Н-С-Н H H H H ннн H-C-H H Н-С—Н H H H H-C-H H нн H-C=C-C-C=Ċ-C=Ċ-Ċ-C=Ċ-H нн H H H H-C-H H-C-H H H. нн H HÇ=C-C-Ç=C-H H H Н-С—Н H

> Condense each of the following structural formulas: H H Н-С—Н H-C-H H ннн H H а. Н—С—С С-С—С—Н b. Н—С—С С-Н ннннн H Н-С—Н H H. Н-С—Н H нннн ннн I III нн Н-С—Н H H H H нн Н-С—н H H

> What results would the student expect if the sample in Question 10.1 were an inorganic compound? What results would the student expect if it were an organic compound? Question 10.1: A student is presented with a sample of an unknown substance and asked

> Describe what is meant by the term nuclide.

> Is the roentgen unit used in the measurement of alpha particle radiation? Why or why not?

> Which of the compounds in Question 10.12 would be soluble in water? Question 10.12: Based on intermolecular forces or ionic interactions, rank the following compounds from highest to lowest melting points: a. H2O2 CH4 KCl b. C6H14 C18H38 NaCl

> Based on intermolecular forces or ionic interactions, rank the following compounds from highest to lowest melting points: a. H2O2 CH4 KCl b. C6H14 C18H38 NaCl

> Why would a Geiger counter be preferred to film for assessing the immediate danger resulting from a spill of some solution containing a radioisotope?

> Give all the possible monochlorinated products for the following reaction: Name the products, using IUPAC nomenclature. Light CH,CH(CH,)CH,CH, + Cl, ?

> Calculate the number of mol corresponding to: a. 15.0 g NH3 b. 16.0 g O2

> For gasoline, isooctane, 2,2,4-trimethylpentane, is the standard of excellence. Write a balanced equation for the complete combustion of isooctane.

> Why are ionic substances more likely to be water-soluble?

> Suggest a protocol for radioactive waste disposal.

> Would the use of concrete rather than wood paneling help to protect workers in other parts of the clinic? Why?

> Would wearing a lab apron lined with thin sheets of lead have a positive effect? Why?

> Would wearing gloves have any significant effect? Why?

> Why do high-altitude jet flights increase a person’s exposure to background radiation?

> Radioactive molybdenum-99 is used to produce the tracer isotope, technetium-99m. Write a nuclear equation for the formation of molybdenum-99 from stable molybdenum- 98 bombarded with neutrons.

> Describe an application of each of the following isotopes: a. iodine-131 b. thallium-201

> Describe how medically useful isotopes may be prepared.

> Calculate the number of ATP molecules produced by the complete b-oxidation of eicosanoic acid.

> Describe how radioactive tracers are used in the diagnosis of disease.

> What type of nuclear reaction fuels our solar system?

> In what way are beta particles and positrons similar?

> Why are cadmium rods used in a fission reactor?

> What are the major disadvantages of a fission reactor for electrical energy production?

> Which type of nuclear process combines small nuclei to release energy?

> What property of carbon enables us to assess the age of a painting?

> The hydronium ion concentration in the blood of three different patients was: Patient.. [H3O1] A.. 5.0 x 10-8 B. 3.1 x10-8 C.. 3.2 x 10-8

> A patient receives 9.0 ng of a radioisotope with a half-life of 12 h. How much will remain in the body after 2.0 days, assuming that radioactive decay is the only path for removal of the isotope from the body?

> Would you predict lithium-9 to be stable? Explain your reasoning.

> Note the major accomplishment of each of the following: a. Thomson b. Rutherford c. Geiger d. Bohr

> Would you predict cobalt-59 to be stable? Explain your reasoning.

> Phosphorus-31, known to bioaccumulate in the liver, decays by beta emission. Write a balanced nuclear equation for this process.

> Cobalt-60 has a half-life of 5.3 years. How many half-lives occur after 21.2 years?

> Explain why the binding energy of a nucleus is expected to be large.

> Element 106 was named seaborgium (Sg) in honor of Glenn T. Seaborg, a pioneer in the discovery of lanthanide and actinide elements. Seaborgium-263 decays by alpha emission. Write a balanced nuclear equation for this process.

> Write a balanced nuclear equation for alpha decay of bismuth-212.

> Element 109 was synthesized by bombarding bismuth-209 with iron-58. Write the equation for this process if one product is a neutron.

> Complete the following nuclear equation: ? −−−→ (90 ^ 214) Th + (2 ^4) HE

> Complete the following nuclear equation: (78 ^ 190) Pt −−−→ a + ?

> a. Write the sequence of steps that would be followed for one round of b-oxidation of hexanoic acid. b. Calculate the number of ATP molecules produced by complete b-oxidation of hexanoic acid.

> Complete the following nuclear equation: (92 ^ 238) U + (7 ^14) N−−−−→?6(0 ^1) n

> Write a nuclear equation to represent radium-226 decaying to radon-222 plus an alpha particle.

> Samarium-147 is one of many rare earth isotopes that undergo alpha decay. Write a balanced nuclear equation for this process.

> How many protons and neutrons are contained in each of the three isotopes of carbon?

> How many protons and neutrons are contained in the nucleus of uranium-235?

> Write the nuclear symbol for carbon-14.

> Rank the four major types of radiation in order of size, speed, and penetrating power.

> What is the major difference between beta and gamma radiation?

> Write the nuclear symbol for a beta particle.

> We can control the rate of chemical reactions. Can we control the rate of natural radiation?

> Observed increases in global temperatures are caused by elevated levels of carbon dioxide. Is this statement a theory or a scientific law? Explain your reasoning.

> What are the major differences between alpha particles and gamma radiation?

> What is the composition of a positron?

> What is alpha decay?

> How does the energy of gamma radiation compare with that of other regions of the electromagnetic spectrum?

> A buffer solution is prepared in such a way that the concentration of propanoic acid is 2.00 3 1021 M and the concentration of sodium propanoate is 4.00 3 1021 M. If the buffer equilibrium is described by Ka = 1.34 × 10-5 use the Henderso

> Barium-131 is a radioisotope used to study bone formation. A patient ingested barium-131. How much time will elapse until only one-fourth of the barium-131 remains, assuming that none of the isotope is eliminated from the body through normal processes? T

> Calculate the pH of a buffer system containing 1.0 M NH3 and 1.0 M NH4Cl. (Ka of NH4+, the acid in this system, is 5.6 × 10-10.)

> What is the pH of the solution described in Question 8.101? Question 8.101: What is [H3O+] for a buffer solution that is 0.200 M in acid and 0.500 M in the corresponding salt if the weak acid Ka = 5.80 × 10-7?

> What is meant by the term lethal dose of radiation?

> The half-life of strontium-87 is 2.8 h. What percentage of this isotope will remain after 8 h and 24 minutes (min)?

> What are the roles of DNA, RNA, and protein in information flow in biological systems?

> Write the equilibrium constant expression for the reaction described in Question 7.96. Question 7.96: N2 (g) + O2 (g)↽−−−−⇀2NO(g)

> Will an increase in pressure increase, decrease, or have no effect on the concentration of NO(g) in the reaction: N2 (g) + O2 (g)↽−−−−⇀2NO(g)

> Which of the following are capable of forming a buffer solution? a. HBr and MgCl2 b. H2CO3 and NaHCO3

> Write out each step of the dissociation of chromic acid, H2CrO4.

> Use the equilibrium constant expression you wrote in Question 7.87 and the equilibrium constant you calculated in Question 7.88 to determine the equilibrium concentration of H2S if: Question 7.87: Write the equilibrium constant expression for the react

> Using the equilibrium constant expression in Question 7.87, calculate the equilibrium constant if: Question 7.87: Write the equilibrium constant expression for the reaction: 2H2 (g) 1 S2 (g)↽−−&a

> Chromic acid, H2CrO4, is a polyprotic acid. How many protons can it donate?

> Rewrite the equation in Question 8.82 as a net, balanced ionic equation. Question 8.82: Write an equation to represent the neutralization of an aqueous solution of HCl with an aqueous solution of KOH.

> Write an equation to represent the neutralization of an aqueous solution of HCl with an aqueous solution of KOH.

> What are the products of a neutralization reaction?

> Calculate formula mass and the molar mass of each of the following formula units: a. S8 b. (NH4)2SO4 c. CO2

> Two nitrogen atoms in a nitrogen molecule are held together more strongly than the two chlorine atoms in a chlorine molecule. Explain this fact by comparing their respective Lewis structures.

> The hydroxide ion concentration in a sample of urine was determined to be of 1.0 × 10-8 M (at 250C). Calculate the hydronium ion concentration of this aqueous solution.

> In a neutralization reaction, how many mol of NaOH are needed to react with 3 mol of HCl?

> Calculate the pH of a solution that has [OH-] = 6.7 × 10-9 M.

> Calculate the pH of a solution that has [H3O+] = 6.6 × 10-5 M.

> Distinguish between the rate constant and the equilibrium constant for a reaction.

> Can a dilute solution of a strong acid ever have a higher pH than a more concentrated solution of a weak acid? Why or why not?

> Write the rate law for the reaction: H2S(aq) + Cl2 (aq)↽−−−−⇀S(s) + 2HCl(aq) Represent the order as n, n', and so forth.

> A 6.00-mL portion of an 8.00 M stock solution is to be diluted to 0.400 M. What will be the final volume after dilution?

> A 50.0-mL sample of a 0.250 M sucrose solution was diluted to 5.00 × 102 mL. What is the molar concentration of the resulting solution?

> Identify the conjugate acid-base pairs for the reversible reactions in Question 8.4. Question 8.4: Write an equation for the reversible reactions of each of the following with water. a. H3PO4 b. CH3NH2

> Explain the differences between leading strand and lagging strand replication.

> Calculate [H3O+] for a solution of hydrochloric acid for which: a. pH = 2.00 b. pH = 3.00