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chemistry principles and practice
Chemistry Principles And Practice 3rd Edition Daniel L. Reger, Scott R. Goode, David W. Ball - Solutions
Discuss the factors that cause the chemistry of the elements in the second period to be different from that of the elements in the same group in later periods.
Why do elements of the second period form stronger bonds than elements of the third period? Give a specific example of a structural contrast between elemental forms from a single group that can be explained by this difference.
Compare the electronegativities and ionization energies of metals and nonmetals.
Why does sulfur form expanded valence shell compounds such as SF6, whereas oxygen does not?
Three different bonding modes occur for hydrogen.Describe them and give a specific example of each.
Describe the bonding of the hydrogen in(a) KH (b) HCl (c) H2
Why does H2 have such a low boiling point (-253 °C)?
List the symbols of the three isotopes of hydrogen and the approximate abundance of each.
Why is helium rather than hydrogen currently used as the gas in blimps?
What is the main difference between saturated and unsaturated cooking oils?
What is the inert pair effect? How does it affect the chemistry of Group 3A?
Explain why the +1 oxidation state is more stable for thallium than for aluminum.
Classify the Group 3A elements as nonmetals, metals, or metalloids.
What unusual structural feature is found in the elemental forms of boron?
Explain why aluminum, a reactive metal, can be used in airplanes and on the exteriors of houses, where it is exposed to the oxygen in the air.
Explain why Group 4A elements, especially carbon and silicon,are ideally suited to making four electron-pair bonds.
State three commercial uses for graphite.
What is meant by the term adsorption, and why does activated charcoal have high adsorption qualities?
How is silicon purified for use in the electronics industry?
How does doping silicon with phosphorus change its conducting properties?
What mineral is mined for the production of lead? Describe the process for obtaining the metal from this mineral.
Describe the Haber process for the synthesis of ammonia. Be sure to comment on the positive and negative effects that Le Chatelier’s principle has on the production of ammonia by this process.
Even though phosphates are found widely in most soils, fertilizers are used to supply additional phosphates.What is the problem with the “natural phosphates,” and how is this problem overcome in commercial fertilizers?
Briefly outline the important physical and chemical properties of the two main allotropes of oxygen.
Classify as acidic, basic, or amphoteric the oxides of the metals, the nonmetals, and the metalloids.
Why are elements in Group 8A expected to be monomeric and relatively nonreactive?
What realization led Bartlett to prepare the first compound of a noble gas?
What is the main source of radon in homes?
Of the following pairs of elements, which element is more likely to be able to form a double bond with carbon?(a) Nitrogen or phosphorus (b) Oxygen or sulfur
Of the following pairs of elements, which element is more likely to be able to form a double bond with oxygen?(a) Carbon or silicon (b) Oxygen or sulfur
From the elements nitrogen, silicon, and gallium, pick the ones with the most and the least metallic properties.Explain your choices.
From the elements silicon, germanium, and tin, pick the ones with the most and the least metallic properties.Explain your choices.
Write the equation for the reaction of NaH and water.What mass of NaH is needed to prepare 1.00 L hydrogen gas at 25 °C and 1.00 atm pressure?
Write the equation for the reaction of zinc metal with hydrochloric acid. What mass of zinc metal is needed to prepare 1.00 L hydrogen gas at 25 °C and 1.00 atm pressure,assuming excess HCl?
Give two important industrial preparations for H2.
What is the most important industrial use of H2? Write the equation for this use.
Write the equation for the water-gas shift reaction.
Write a series of equations that shows how coal plus water can be converted to methanol. Be careful to balance all equations.
Draw the structure of B2H6, and describe the bonding in this molecule. What is the hybridization at the boron atoms?
Describe the bonding in BCl3. What is the hybridization at the boron atom? Is the boron really electron deficient?
What is a three-center, two-electron bond?
How does a three-center, two-electron bond differ from a normal two-center, two-electron bond?
Describe the Hall process for the production of aluminum from the mineral bauxite. How is energy saved by recycling aluminum rather than preparing it by the Hall process?
What is the thermite reaction, and why can it be used to weld steel?
Describe the composition of a ruby.
How is ϒ-alumina used to purify water?
Draw the structure of Al2Cl6. Compare the bonding in Al2Cl6 and B2H6.
The oxide Ga2O3 is amphoteric. Write an equation for its reactions, if any, with HCl and NaOH.
Draw the structure of silica, SiO2, and compare it with the structure of CO2. Why are the structures so different?
Describe an n-type semiconductor based on silicon.
What is the hybridization of silicon in SiCl4? Is this compound polar or nonpolar?
What is the hybridization of silicon in silicates?
What are the structures of the most common allotropic forms of nitrogen and phosphorus? Explain why they are so different.
Write the Lewis structure of P4.
Nitrogen is the substance isolated in second-largest quantity in the chemical industry. How is it isolated?
What is meant by the fixation of nitrogen with hydrogen?
Write the Lewis structures of NO2 and N2O3. What is the hybridization of the nitrogen atoms in each compound?
Write the Lewis structures of N2O and N2O4. What is the hybridization of the nitrogen atoms in each?
Write an equation for each of the following reactions.(a) Reaction between magnesium and nitrogen(b) Preparation of P4O10(c) Reaction of nitrogen dioxide with water
Write an equation for each of the following reactions.(a) Preparation of dinitrogen oxide(b) Reaction of hydrazine with oxygen(c) Reaction between P4O10 and water
Discuss the structure of (NO2)x in both the gas and solid phases.
Write two reactions that show how NO gas can catalytically decompose large amounts of ozone, O3.
How is nitric acid prepared by the Ostwald process?
The largest use of nitric acid is in the production of ammonium nitrate. Write the equation for this process.
Indicate which elements form binary compounds with oxygen.
Describe two allotropic forms of sulfur.
Write equations for the industrial preparation of sulfuric acid from sulfur.
Identify the three main types of reactions that sulfuric acid undergoes.
Draw the Lewis structures and assign the shapes of XeF2and XeO3. Is either of these compounds polar?
Draw the Lewis structures and assign the shapes of XeF4 and XeO4. Is either of these compounds polar?
Write the equation for the oxidation of ammonia to nitrogen monoxide (the first step in the Ostwald process).What mass of ammonia is needed to produce 25 kg nitrogen monoxide?
Write the equation for the preparation of ammonium nitrate from NH3. What mass of ammonia is needed to produce 5.22 kg ammonium nitrate?
Compare the boiling points of NH3 and PH3, and explain the difference.
Given that the H–P–H angles in phosphine are about 90 degrees, what orbitals on the phosphorus are used to make the H–P bonds?
Oxygen can be prepared in the laboratory by heating KClO3 in the presence of MnO2. Write the equation; then determine the mass of KClO3 needed to produce 0.50 L O2 gas at 27 °C and 755 torr pressure.
Write the equation for the roasting of lead sulfide. What volume of SO2 gas measured at standard temperature and pressure is produced from the roasting of 1.0 × 102 g lead sulfide?
As outlined in this chapter, hydrazine is used to remove oxygen from water used in boilers of electrical generating plants. If the water contains 2.0 × 10-8 g O2 per gram of water, what mass of hydrazine is needed to remove the oxygen in 10 tons of water?
What is the most important crystal force that holds each of the following substances together?(a) Pb (b) SiO2 (c) P4 (d) Buckyballs
Write the Lewis structure and use valence shell electronpair repulsion theory to predict the shape of XeF4O2.
Draw all possible resonance forms of H2SO4 and HNO3.Explain why resonance forms that do not show formal charges can be written for H2SO4 but not HNO3.
Write the Lewis structure and molecular orbital diagram for NO. What bond order and number of unpaired electrons does each predict for NO?
Write nuclear equations for the following radioactive decays:(a) Beta decay of radium-228(b) Alpha decay of polonium-210(c) Electron capture by lanthanum-137 Strategy The numbers of nucleons (protons plus neutrons) are conserved. If we know the starting nuclide and the particle emitted or captured,
Predict the kind of decay expected, and write the nuclear equation for each of the following radioactive nuclides.Strategy If the atomic number is greater than 83, alpha emission is observed. If the atomic number is lower, compare the mass number with the atomic mass shown in the periodic table; if
Determine the numbers of alpha and beta decays needed to change 238U into 206Pb.Strategy The mass number decreases by 4 for each alpha particle emitted, whereas a beta decay does not change the mass number. The atomic number decreases by 2 for each alpha particle emitted and increases by 1 for each
The nuclide 31Si is a radioactive isotope that disintegrates by beta decay.A sample of silicon-31 is found to produce 251 disintegrations/s . Exactly 3.00 hours later, the same sample produces 113 disintegrations/s . What is the half-life of 31Si?Strategy The relative rate of decay is proportional
An artifact found in an ancient Egyptian tomb produced 11.8 disintegrations of14C per minute per gram of carbon in the sample. Estimate the age of this sample,assuming that its original radioactivity was 15.3 disintegrations per minute per gram of carbon.Strategy Equation 21.3 relates the rate of
The mass spectrum of a rock sample shows that it contains 4.40 μg 238U and 1.21 μg 206Pb. Assuming that all of the lead was produced from radioactive decay of uranium-238, how old is the rock? The half-life of 238U is 4.5 × 109 years.Strategy We need to calculate the original mass of uranium,
Calculate the mass defect of 4He. The atomic mass of the atom is 4.002602 atomic mass units (u) .Strategy Use the information in Table 21.3, to calculate the atomic masses of the nucleons; then calculate the mass defect by the difference from its atomic mass of 4.002602 u.Table 21.3
What is the energy change when 1 mol 4He is made from fundamental particles?Strategy Use the results of the calculation of Example 21.9 and Equation 21.5:Remember to express the mass defect in kilograms and the speed of light in meters per second.Example 21.9Calculate the mass defect of 4He. The
Write the nuclear equation that forms tin-117 by a positron emission.
Predict the kind of decay expected, and write the nuclear equation for the radioactive isotope
The decay of 241Am in smoke detectors terminates in 209Bi. Find the number of alpha and beta decays that occurred in this transformation.
A sample that contains 4.50 × 1014 atoms of a radioactive isotope decays at a rate of 503 disintegrations/min. What is the half-life (in years) of this isotope?
The radioactive decay of a sample containing 41Ar produces 555 disintegrations/min. The rate decreases to 314 disintegrations/min exactly 90.0 minutes later. Calculate the half-life of 41Ar.
What is the age of a bone found by an archaeologist if its 14C activity was 2.9 disintegrations per minute per gram of carbon?
The ratio of 40Ar/40K can also be used for the dating of minerals, because 40Ar is a stable nuclide.Analysis of a rock showed that the atom ratio of 40Ar/40K was 0.44. What is the age of the sample?
Write the balanced nuclear reaction for the bombardment of 56Fe with protons to form 56Co.
Calculate the mass defect for 16O. The mass of the atom is 15.99502 u.
The mass defect for 16O is 0.1369 u. Express the nuclear binding energy for this nucleus in kilojoules per mole.
What is the binding energy per nucleon (in MeV) for 16O, which has a mass defect of 0.1369 u?
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