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chemistry principles and practice

Questions and Answers of Chemistry Principles And Practice

A nuclide that lies above the band of stability shown in Figure 21.1 has too large a neutron-to-proton ratio to be stable. Which of the natural decay processes for such a nuclide will move it toward
Does the neutron-to-proton ratio increase, decrease, or remain unchanged when each of the following radioactive decays occurs?(a) Beta decay (b) Positron decay(c) Gamma decay (d) Alpha decay
A nuclide that lies below the band of stability shown in Figure 21.1 has too small a neutron-to-proton ratio to be stable. Which of the natural decay processes for such a nuclide will move it toward
Why are the high-energy photons that accompany an electron capture decay called x rays rather than gamma rays?
Most alpha and beta decays are accompanied by the emission of gamma rays as well. Why?
What property of the products of radioactive decay is used to detect and measure the presence of the radiation?
Would carbon-14 dating be useful for determining whether a sample of paper was 20 or 50 years old?
Why are charged particles with very high energies needed to cause nuclear reactions with the heavier elements?
Why are low-energy neutrons able to react with nearly all nuclides?
What are the roles of the moderator and the control rods in a nuclear reactor?
Explain why most fission products formed in a nuclear reactor decay by beta emission rather than undergoing another kind of nuclear decay.
A person’s exposure to radiation can depend greatly on occupation. List several occupations that may result in an exposure to radiation greater than the average exposure of the U.S. population.
Nuclear fuel rods are fabricated in a standard manufacturing facility, but after the same rods are removed from the reactor, they are hazardous to approach. Explain.
Write the fusion reaction that occurs in the Sun. Why are researchers trying to use fusion as a power source?What are the advantages and disadvantages compared with nuclear fission?
Fill in the missing entries in the table below.
Fill in the missing entries in the table below.
Calculate the neutron-to-proton ratio (to two decimal places) for each of the following stable isotopes.
Calculate the neutron-to-proton ratio (to two decimal places) for each of the following stable isotopes.
Which of the following isotopes lie(s) within the band of nuclear stability shown in Figure 21.1 ?Figure 21.1
Which of the following isotopes lie(s) within the band of nuclear stability shown in Figure 21.1 ?Figure 21.1
Write the balanced nuclear equation for each of the following nuclear decays. Show the mass and atomic numbers for each of the particles in the equation.(a) Alpha decay of bismuth-201(b) Positron
Write the balanced nuclear equation for each of the following nuclear decays. Show the mass and atomic numbers for each of the particles in the equation.(a) Beta decay of carbon-14(b) Alpha decay of
Identify the missing particles by balancing the mass and atomic numbers in each of the following nuclear decay equations.
Identify the missing particles by balancing the mass and atomic numbers in each of the following nuclear decay equations.
Identify the missing particles by balancing the mass and atomic numbers in each of the following nuclear decay equations.
Identify the missing particles by balancing the mass and atomic numbers in each of the following nuclear decay equations.
Radioactive decay always moves the nuclide toward the band of stability. Based on the mode of decay for each of the following radioactive nuclides, state whether it lies above or below the band of
Radioactive decay always moves the nuclide toward the band of stability. Based on the mode of decay for each of the following radioactive nuclides, state whether it lies above or below the band of
For each of the following radioactive nuclides, predict the mode of decay from its location in the periodic table and by comparing the mass number with the atomic mass of the element in the periodic
Predict the probable mode of decay for each of the following radioactive isotopes, and write an equation to show the products of decay.(a) 54Mn (b) 241Am (c) 110Ag (d) 197Hg
For each of the following radioactive nuclides, predict the mode of decay from its location in the periodic table and by comparing the mass number with the atomic mass of the element in the periodic
Write a nuclear equation for the type of decay each of these unstable isotopes is most likely to undergo.(a) 19Ne (b) 230Th (c) 92Br (d) 212Po
The decay of 238Pu terminates in 206Pb. Determine the number of alpha and beta decays that occurred in this transformation.
A decay series begins with 235U, finally producing the stable isotope 207Pb. Find the numbers of alpha and beta decays that occurred in this transformation.
A sample that contains 3.75 × 1013 atoms of a beta emitter has a disintegration rate of 382 disintegrations/min.What is the half-life (in years) for this isotope?
By mass spectral analysis, a sample of strontium is known to contain 2.64 × 1010 atoms of 90Sr as the only radioactive element. The absolute disintegration rate of this sample is measured as 1238
The radioactive decay of a sample containing 121Te produced 865 disintegrations/min. Exactly 7.00 days later, the rate of decay was found to be 650 disintegrations/min.Calculate the half-life, in
A tree was cut down and used to make a statue 2300 years ago. What fraction of the 14C that was present originally remains today? t1/2 of 14C is 5730 years.)
In a living organism, the decay of 14C produces 15.3 disintegrations per minute per gram of carbon. The half life of 14C is 5730 years. What percentage of the atoms of carbon in the biosphere is 14C?
Complete and balance the following nuclear equations.
Complete and balance the following nuclear equations.
The molar mass of 31P is 30.9738 g/mol.(a) Use the masses of hydrogen-1 and the neutron given in Table 21.3 to calculate the mass defect of this nuclide in grams per mole.(b) Express the total
The atomic masses of three isotopes of phosphorus are
When 239Pu is used in a nuclear reactor, one of the fission events that occurs isThe atomic mass of each atom is given below its symbol in the equation.(a) Calculate the change in mass, expressed in
When 239Pu is used in a nuclear reactor, one of the fission events that occurs isThe atomic mass of each atom is given below its symbol in the equation.(a) Calculate the change in mass, expressed in
A product of the fission of 235U is 137Cs, which undergoes beta decay with a half-life of 30.17 years. What fraction of the 137Cs that was formed in the detonation of the first fission bombs in
Cadmium is used in the control rods of fission reactors because it absorbs neutrons efficiently. Most of the neutrons are absorbed by 113Cd to produce 114Cd and a gamma ray. The atomic masses of
The 146C activity of an artifact from a burial site was 8.6/min per gram carbon. The half-life of 146C is 5730 years, and the current 146C activity is 15.3 disintegrations per minute per gram of
128I decays by both beta and positron decay. What are the product nuclides from each of these decays?
One kilogram of high-grade coal produces about 2.8 × 104 kJ energy when it is burned. Fission of 1 mol 235U releases 1.9 × 1010 kJ.(a) Calculate the number of metric tons (1 metric ton = 1000 kg)
How many disintegrations per second occur in a basement that is 40 × 40 × 10 feet if the radiation level from radon is the maximum allowed, 4 × 10-12 Ci/L?
What is the equivalence point in the titration of 5.00 mL of 0.0110 M Ba(OH)2 with 0.0251 M HCl?
How many disintegrations per second occur in a basement that is 40 × 40 × 10 feet if the radiation level from radon is the maximum allowed, 4 × 10-12 Ci/L?
Natural potassium is 0.0117% radioactive 40K, which decays by positron emission with a half-life of 1.26 × 109 years. If an average banana has 6.00 × 10-1 g potassium in it, what is the
Compare and contrast Brønsted–Lowry and Arrhenius acids.
Can a compound be an Arrhenius base and not a Brønsted–Lowry base? Explain your answer.
Water is not the only solvent that undergoes autoionization. Write the equation for the autoionization of acetic acid.
Write two Brønsted–Lowry acid-base reactions and show how they represent proton-transfer reactions.
Define pH and explain why pH, rather than molarity, is used as a concentration measure of H3O+.
List the strong acids and bases. Why are they called “strong”?
Define a weak acid.
Compare and/or contrast strong and weak acids.
In acidic solvents, such as concentrated acetic acid, some of the acids considered strong (in water) behave as weak acids. Explain why HCl behaves as a weak acid and HClO4 behaves as a strong acid in
Is the conjugate base of a strong acid always a spectator ion? Explain.
What is the relationship between weak bases and their conjugate acids?
Define analytical concentration and give an example for HNO3 and for CH3COOH solutions.
Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
You are asked to design an experiment to determine the percentage of ionization of HCl in aqueous solution at 4 °C. You accurately dissolve 4.1349 g HCl in 1001.34 g water. Would you set up an
In Section 15.6, a base is stated to have a neutral or negative charge. Although positively charged bases exist, they are not Positive bases are rare because they tend to repel positively charged
If Kb for ammonia is 1.8 × 10-5, calculate Ka for its conjugate acid, NH4+. Note that NH3 is the conjugate acid of the amide ion, NH2+. Can Ka and Kb for the NH3| NH-2 pair be calculated from the
What are the expected trends in acidity of binary acids, going diagonally to the lower right (“southeast”) on the periodic chart from carbon? Is the same trend observed if the starting point is
Element 85, astatine (At), is a radioactive halogen that is not present in appreciable amounts in nature. The acid HAt can be prepared and compared with the other hydrogen halides. Explain why you
Define oxyacid and give examples from among the strong acids.
Define Lewis acids and bases, and compare with Brønsted–Lowry acids and bases.
Propose an experiment to determine whether a coordinate covalent bond is different from other covalent bonds. Usefor a concrete example.
Compare strong and weak acids and bases.(a) How are a strong acid and a weak acid similar? How are they different?(b) How are a strong base and a weak base similar? How are they different?
Write the formula and name of the conjugate acid of the following substances.(a) Hydrogen sulfate ion(b) Water(c) Ammonia(d) Pyridine
Write the formula and name for the conjugate base of the following substances.(a) Nitric acid(b) Hydrogen carbonate ion(c) Water(d) Hydrogen chloride
Write the formula and name for the conjugate base of the following substances.
Write the formula and name for the conjugate acid of the following substances.
For each of the following reactions, identify the Brønsted–Lowry acids and bases. What are the conjugate acid/base pairs?
Write the formula, and give the name of the conjugate acid of each of the following bases.
The following species react in aqueous solution. Predict the products, identify the acids and bases (and their conjugate species), and show the proton transfer in the acidbase reactions.
The following species react in aqueous solution. Predict the products, identify the acids and bases (and their conjugate species), and show the proton transfer in the acidbase reactions.(a) Ammonia
What are the products of each of the following acidbase reactions? Indicate the acid and its conjugate base, and the base and its conjugate acid.
Write an equation to describe the proton transfer that occurs when each of these acids is added to water.
Determine the hydrogen ion or hydroxide ion concentration in each of the following solutions, as appropriate.
Determine the hydrogen ion or hydroxide ion concentration in each of the following solutions, as appropriate.
The concentration of hydrogen ions in human blood is approximately 4.0 × 10-8 M. What is the hydroxide ion concentration in blood?
The hydroxide ion concentrations in wines actually range from 7.4 × 10-12 M to 1.6 × 10-10 M. What is the range of hydrogen ion concentrations in wine?
Fill in the following table, and indicate whether the solution is acidic, basic, or neutral.
Fill in the following table, and indicate whether the solution is acidic, basic, or neutral.
Fill in the following table, and indicate whether the solution is acidic, basic, or neutral.
Fill in the following table, and indicate whether the solution is acidic, basic, or neutral.
What are the concentrations of hydrogen ion and hydroxide ion in each of the following?(a) Vinegar(b) Stomach acid(c) Coffee(d) Milk
What are the concentrations of hydrogen ion and hydroxide ion in each of the following?(a) Lemon juice(b) Wine(c) Blood(d) Household ammonia
Calculate the pH and pOH of the following solutions.(a) 0.050 M HCl(b) 0.024 M KOH(c) 0.014 M HClO4(d) 1.05 M NaOH
Calculate the pH and pOH of the following solutions.(a) 0.51 M CsOH(b) 0.0040 M HI(c) 0.13 M LiOH(d) 0.66 M HClO4
Calculate the pH and pOH of the following solutions.(a) 0.94 M HBr(b) 0.042 M Sr(OH)2(c) 0.00033 M HCl(d) 0.88 M RbOH
Calculate the pH and pOH of the following solutions.(a) 0.0045 M Ba(OH)2(b) 0.080 M HI(c) 0.030 M Sr(OH)2(d) 12.3 M HNO3

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