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All Textbook Solutions for Chemistry by OpenStax (2015-05-04)

Write a balanced equation for the reaction of elemental strontium with each of the following: (a) oxygen (b) hydrogen bromide (c) hydrogen (d) phosphorus (e) water How many moles of ionic species are present in 1.0 L of a solution marked 1.0 M mercury(I) nitrate?What is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of mercury, if the fish contains 30 parts per million of mercury by weight? (Assume that all the mercury from the fish ends up as mercury (II) chloride in the body and that a fatal dose is 0.20 g of HgCl2.) How many pounds of fish is this?The elements sodium, aluminum, and chlorine are in the same period.. (a) Which has the greatest electronegativity?. (b) Which of the atoms is smallest?. (c) Write the Lewis structure for the simplest covalent compound that can form between aluminum and chlorine. (d) Will the oxide of each element be acidic, basic, or amphoteric?Does metallic tin react with HCl?What is tin pest, also Known as tin disease?Compare the nature of the bonds in PbCl2 to that of the bonds in PbCl4.Is the reaction of rubidium with water more or less Vigorous than that of sodium? How does the rate of reaction of magnesium compare?Write an equation for the reduction of cesium chloride by elemental calcium at high temperature.Why is it necessary to keep the chlorine and sodium, resulting from the electrolysis of sodium chloride, separate during the production of sodium metal?Give balanced equations for the overall reaction in the electrolysis of molten lithium chloride and for the reactions occurring at the electrodes. You may wish to review the Chapter on electrochemistry for relevant examples.The electrolysis of molten sodium chloride or of aqueous sodium chloride produces chlorine. Calculate the mass of chlorine produced from 3.00 kg sodium Chloride in each case. You may wish to review the chapter on Electrochemistry for relevant examples.What mass, in grams, of hydrogen gas forms during the complete reaction of 10.01 g of calcium with water?How many grams of oxygen gas are necessary to react completely with 3.011021 atoms of magnesium to yield magnesium oxide?Magnesium is an active metal; it bums in the form of powder, ribbons, and filaments to provide flashes of brilliant light. Why is it possible to use magnesium in construction?Why is it possible for an active metal like aluminum to be useful as a structural metal?Describe the production of metallic aluminum by electrolytic reduction.What is the common are of tin and how is tin separated from it?A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric acid, and metastannic acid, H2SnO3, is precipitated. She heats the precipitate to drive off the water, which leaves 0.4909 g of tin(IV) oxide. What was the percentage of [in in the original sample?Consider the production of 100 kg of sodium metal using a current of 50,000 A, assuming a 100% yield.. (a) How long will it take to produce the 100 kg of sodium metal?. (b)VVhatv01ume of chlorine at 25 C and 1.00 atm forms?What mass of magnesium forms when 100,000 A is passed through a MgCl2 melt for 1.00 h if the yield of magnesium is 85% 0f the theoretical yield?Give the hybridization of the metalloid and the molecular geometry for each of the following compounds or ions. You may wish to review the chapters on chemical bonding and advanced covalent bonding for relevant examples. (a) GEH4. (b) SbF3. (c) Te(OH)6. (d) H2Te. (e) GeF2. (f) TeCl4. (g) SiF62-. (h) SbCl5,. (i) TEF6 Write a Lewis structure for each of the following molecules or ions. You may wish to review the chapter on chemical bonding. (a) H3BPH3. (b) BF4-. (c) BBr3. (d) B(CH3)3. (e) B(OH)3 Describe the hybridization of boron and the molecular structure about the boron in each of the following: (a) H3BPH3. (b) BF4-. (c) BBr3. (d) B(CH3)3. (e) B(OH)3 Using only the periodic table, write the complete electron configuration for silicon, including any empty orbitals in the valence shell. You may wish to review the chapter on electronic structure.Write a Lewis structure for each of the following molecules and ions: (a) (CH3)3SiH (b) SiO44- (C) Si2H6 (d) Si(OH)4 (e) SiF62-Describe the hybridization of silicon and the molecular structure of the following molecules and ions: (a) (CH3)3SiH. (b) SIO44-. (c) Si2H6. (d) Si(OH)4. (e) SiF62-Describe the hybridization and the bonding of a silicon atom in elemental silicon.Classify each of the following molecules as polar or nonpolar. You may wish to review the chapter on chemical bonding. (a) SiH4. (b) Si2H6. (c) SiCl3H. (d) SiF4. (e) SiCl2F2 Silicon reacts with sulfur at elevated temperatures. If 0.0923 g of silicon reacts with sulfur to give 0.3030 g of silicon sul?de, determine the empirical formula of silicon sulfide.Name each of the fallowing compounds: (a) TeO2 (b) Sb2S3 (C) GeF4 (d) SiH4 (e) GeH4 Write a balanced equation for the reaction of elemental boron with each of the following (most of these reactions require high temperature): (a) F2. (b) O2. (C) S. (d) Se. (e) Br2 Why is boron limited to a maximum coordination number of four in its compounds?Write a formula for each of the following compounds: (a) silicon dioxide (b) silicon tetraiodide (c) silane (d) silicon carbide (6) magnesium silicide From the data given in Appendix I, determine the standard enthalpy change and the standard free energy change for each of the following reactions: (a) BF3(g)+3H2O(l)B(OH)3(s)+3HF(g) (b) BCl3(g)+3H2O(l)B(OH)3+3HCl(g) (c) B2H6(g)+6H2O(l)2B(OH)3(s)+6H2(g)A hydride of silicon prepared by the reaction of Mg2Si with acid exerted a pressure of 306 torr at 26 C in a bulb with a volume of 57.0 mL. If the mass of the hydride was 0.0861 g, what is its molecular mass? What is the molecular formula for the hydride?Suppose you discovered a diamond completely encased in a silicate rock. How would you chemically free the diamond without harming it?Carbon forms a number of allotropes, two of which are graphite and diamond. Silicon has a diamond structure. Why is there of allotrope of silicon with a graphite structure?Nitrogen in the atmosphere exists as very stable diatomic molecules. Why does phosphorus form less stable P4 molecules instead of P2 molecules?Write balanced chemical equations for the reaction of the following acid anhydrides with water: (a) SO3 (b) N2O3 (c) Cl2O7 (d) P4O10 (e) NO2 Determine the oxidation number of each element in each of the following compounds: (a) HCN (b) OF2 (c) ASCl3 Determine the oxidation state of sulfur in each of the following: (a) SO3 (b) SO2 (C) SO32-Arrange the following in order of increasing electronegativity: F; Cl; O; and S.Why does white phosphorus consist of tetrahedral P4 molecules while nitrogen consists of diatomic N2 molecules?Why does hydrogen- not exhibit an oxidation state of 1- when bonded to nonmetals?The reaction of calcium hydride, CaH2, with water can be characterized as a Lewis acid-base reaction: CaH2(s)+2H2O(l)Ca(OH)2(aq)+2H2(g) Identify the Lewis acid and the Lewis base among the reactants. The reaction is also an oxidation-reduction reaction. Identify the oxidizing agent, the reducing agent, and the changes in oxidation number that occur in the reaction.In drawing Lewis structures, we learn that a hydrogen atom forms only one bond in a covalent compound. Why?What mass of CaH2 is necessary to react with water to provide enough hydrogen gas to fill a balloon at 20 C and 0.8 arm pressure with a volume of 4.5 L? The balanced equation is: CaH2(s)+2H2O(l)Ca(OH)2(aq)+2H2(g)What mass of hydrogen gas results from the reaction of 8.5 g of KH with water?. KH+H2OKOH+H2 Carbon forms the CO32- ion, yet silicon does not form an analogous SiO3-2 ion. Why?Complete and balance the following chemical equations: (a) hardening of plaster containing slaked lime. Ca(OH)2+CO2 (b) removal of sulfur dioxide from the ?ue gas of power plants. CaO+SO2 (c) the reaction of baking powder that produces carbon dioxide gas and causes bread to rise. NaHCO3+NaH2PO4 Heating a sample of Na2CO3xH2O weighing 4.640 g until the removal of the water of hydration leaves 1.720 g of anhydrous Na2CO3. What is the formula of the hydrated compound?Write the Lewis structures for each of the following: (a) NH2- (b) N2F4 (c) NH2- (d) NF3 (e) N3-For each of the following, indicate the hybridization of the nitrogen atom (for N3-. the central nitrogen). (a) N2F4 (b) NH2- (C) NF3 (d) N3-Explain how ammonia can function both as a Bronsted base and as a Lewis base.Determine the oxidation state of nitrogen in each of the following. You may wish to review the chapter on chemical bonding for relevant examples. (a) NCl3. (b) ClNO. (c) N2O5. (d) N2O3. (e) NO2-. (f) N2O4. (g) N2O. (h) NO3-. (i) HNO2. (j) HNO3 For each of the following draw the Lewis structure, predict the ONO bond angle, and give the hybridization of the nitrogen. You may wish to review the chapters on chemical bonding and advanced theories of covalent bonding for relevant examples. (a) NO2. (b) NO2-. (c) NO2+How many grams of gaseous ammonia will the reaction of 3.0 g hydrogen gas and 3.0 g of nitrogen gas produce?Although PF5 and ASF5 are stable, nitrogen does not form NF5 molecules. Explain this difference among members of the same group.The equivalence point for the titration of a 25.00-mL sample of CSOH solution with 0.1062 M HNO3 is at 35.27 mL. What is the concentration of the CsOH solution?Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry. (a) PH3. (b) PH4+. (c) P2H4. (d) PO43-. (e) PF5 Describe the molecular structure of each of the following molecules or ions listed. You may Wish to review the chapter on chemical bonding and molecular geometry. (a) PH3. (b) PH4+. (c) P2H4. (d) PO43-Complete and balance each of the following chemical equations. (In some cases, there may be more than one correct answer.) (a) P4+Al (b) P4+Na (c) P4+F2 (d) P4+Cl2 (e) P4+O2 (f) P4O6+O2 Describe the hybridization of phosphorus in each of the following compounds: P4O10, P4O6, PH4l (an ionic compound), PBr3, H3PO4, H3PO3, PH3, and P2H4. You may wish to review the chapter on advanced theories of covalent bonding.What volume of 0.200 M NaOH is necessary to neutralize the solution produced by dissolving 2.00 g of PCl3 is an excess of water? Note that when H3PO3 i5 titrated under these conditions, only one proton of the acid molecule reacts.How much POCl3 can form from 25.0 g of PCl5 and the appropriate amount of H2O?How many tons of Ca3(PO4)2 are necessary to prepare 5.0 tons of phosphorus if the yield is 90%?Write equations showing the stepwise ionization of phosphorous acid.Draw the Lewis structures and describe the geometry for the following: (a) PF4+ (b) FF5 (c) PF6- (d) POF3 Why does phosphorous acid form only two series of salts, even though the molecule contains three hydrogen atoms?Assign an oxidation state to phosphorus in each of the following: (a) NaH2PO3 (b) PF5 (c) P4O6 (d) K3PO4 (e) Na3P (f) Na4P2O7 Phosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of phosphorus(V) oxide, an acidic oxide, with water. Phosphorus(V) oxide is prepared by the combustion of phosphorus. (a) Write the empirical formula of phosphorus(V) oxide. (b) What is the molecular formula of phosphorus(V) oxide if the molar mass is about 280. (c) Write balanced equations for the production of phosphorus(V) oxide and phosphoric acid. (d) Determine the mass of phosphorus required to make 1.00104 kg of phosphoric acid, assuming a yield of 98.35%.Predict the product of burning francium in air.Using equations, describe the reaction of water with potassium and with potassium oxide.Write balanced chemical equations for the following reactions: (a) zinc metal heated in a stream of oxygen gas (b) zinc carbonate heated until loss of mass stops (c) zinc carbonate added to a solution 0f acetic acid, CH3CO2H (d) zinc added to a solution of hydro-bromic acid Write balanced chemical equations for the following reactions: (a) cadmium burned in air. (b) elemental cadmium added to a solution of hydrochloric acid. (c) cadmium hydroxide added to a solution of acetic acid, CH3CO2H Illustrate the amphoteric nature of aluminum hydroxide by citing suitable equations.Write balanced chemical equations for the following reactions: (a) metallic aluminum burned in air (b) elemental aluminum heated in an atmosphere of Chlorine (c) aluminum heated in hydrogen bromide gas (d) aluminum hydroxide added to a solution of nitric acid Write balanced chemical equations for the following reactions: (a) sodium oxide added to water (b) cesium carbonate added to an excess of an aqueous solution of HF (c) aluminum oxide added to an aqueous solution of HClO4 (d) a solution of sodium carbonate added to solution of barium nitrate (e) titanium metal produced from the reaction of titanium tetrachloride with elemental sodium What volume of 0.250 M H2SO4 solution is required to neutralize a solution that contains 5.00 g of CaCO3?Which is the stronger acid, HClO4 or HBrO4? Why?Write a balanced chemical equation for the reaction of an excess of oxygen with each of the following.. Remember that oxygen is a strong oxidizing agent and tends to oxidize an element to its maximum oxidation state. (a) Mg. (b) Rb. (c) Ga. (d) C2H2. (e) CO Which is the stronger acid, H2SO4 or H2SeO4? Why? You may wish to review the Chapter on acid-base equilibria.Explain why hydrogen sulfide is a gas at room temperature, whereas water, which has a lower molecular mass, is a liquid.Give the hybridization and oxidation state for sulfur in SO2, in SO3, and in H2SO4.Which is the stronger acid, NaHSO3 or NaHSO4?Determine the oxidation state of sulfur in SF6, SO2F2, and KHS.Which is a stronger acid, sulfurous acid or sulfuric acid? Why?Oxygen forms double bonds in O2, but sulfur forms single bonds in S8. Why?Give the Lewis structure of each of the following: (a) SF4 (b) K2SO4 (c) SO2Cl2 (d) H2SO3 (e) SO3 Write two balanced chemical equations in which sulfuric acid acts as an oxidizing agent.Explain why sulfuric acid, H2SO4, which is a covalent molecule, dissolves in water and produces a solution that contains ions.How many grams of Epsom salts (MgSO47H2O) will form from 5.0 kg of magnesium?What does it mean to say that mercury (II) halides are weak electrolytes?Why is SnCl4 not classified as a salt?The following reactions are all similar to those of the industrial chemicals. Complete and balance the equations for these reactions: (a) reaction of a weak base and a strong acid. NH3+HClO4 (b) preparation of a soluble silver salt for silver plating. Ag2CO3+HNO3 (c) preparation of strontium hydroxide by electrolysis of a solution of strontium chloride SrCl2(aq)+H2O(l)electrolysis Which is the stronger acid, HClO3 or HBrO3? Why?What is the hybridization of iodine in IF3 and IF5?Predict the molecular geometries and draw Lewis structures for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry. (a) IF5. (b) I3-. (c) PCl5. (d) SeF4. (e) ClF3 Which halogen has the highest ionization energy? Is this what you would predict based on what you have learned about periodic properties?Name each of the following compounds: (a) BrF3. (b) NaBrO3. (c) PBr5. (d) NaClO4. (e) KClO Explain why, at room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.What is the oxidation state of the halogen in each of the following?. (a) H5IO6. (b) IO4-. (c) ClO2. (d) ICl3. (e) F2 Physiological saline concentration—that is, the sodium chloride concentration in our bodies—is approximately 0.16 M . A saline solution fur contact lenses is prepared to match the physiological concentration. If you purchase 25 mL of contact lens saline solution, how many grams of sodium chloride have you bought?Give the hybridization of xenon in each of the following. You may wish to review the chapter on the advanced theories of covalent bonding. (a) XeF2. (b) XeF4. (c) XeO3. (d) XeO4. (e) XeOF4 What is the molecular structure of each of the following molecules? You may wish to review the chapter on chemical bonding and molecular geometry. (a) XeF2. (b) XeF4. (c) XeO3. (d) XeO4. (e) XeOF4 Indicate whether each of the following molecules is polar or nonpolar. You may wish to review the chapter on chemical bonding and molecular geometry. (a) XeF2. (b) XeF4. (c) XeO3. (d) XeO4. (e) XeOF4 What is the oxidation state of the noble gas in each of the following? You may wish to review the chapter on chemical bonding and molecular geometry. (a) XeO2F2. (b) KrF2. (c) XeF3+. (d) XeO64-. (e) XeO3 A mixture of xenon and ?uorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 ml of xenon (at STP) and hydrogen ?uoride, which was collected in waiter, giving a solution of hydro?uoric acid. The hydro?uoric acid solution was titrated, and 68.43 mL of 0.3172 M sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced Chemical equations for the reactions involving xenon.Basic solutions of Na4XeO6, are powerful oxidants. What mass of Mn(NO3)26H2O reacts with 125.0 mL of a 0.1717 M basic solution of Na4XeO6 that contains an excess of sodium hydroxide if the products include Xe and solution of sodium permanganate?Write the electron configurations far each of the following elements: (a) Sc. (b) Ti. (c) Cr. (d) Fe. (e) Ru Write the electron con?gurations for each of the following elements and its ions: (a) Ti. (b) Ti2+. (c) Ti3+. (d) Ti4+Write the electron configurations for each of the following elements and its 3+ ions: (a) La (b) Sm (c) Lu Why are the lanthanoid elements not found in nature in their elemental forms?Which of the following elements is most likely to be used to prepare La by the reduction of La2O3: Al, C, or Fe? Why?Which of the following is the strongest oxidizing agent: VO43, CrO42-, or MnO4-?Which of the following elements is most likely to form an oxide with the formula MO3: Zr, Nb, or Mo?The following reactions all occur in a blast furnace. Which of these are redox reactions? (a) 3Fe2O3(s)+CO(g)2Fe3O4(s)+CO2(g) (b) Fe3O4(s)+CO(g)3FeO(s)+CO2(g) (c) FeO(s)+CO(g)Fe(l)+CO2(g) (d) C(s)+O2(g)CO2(g) (e) C(s)+CO2(g)2CO(g) (f) CaCO3(s)CaO(s)+CO2(g) (g) CaO(s)+SiO2(s)CaSiO3(l)Why is the formation of slag useful during the smelting of iron?Would you expect an aqueous manganese (VII) oxide solution to have a pH greater or less than 7.0? Justify your answer.Iron (II) can be oxidized to iron (III) by dichromate ion, which is reduced to chromium (III) in acid solution. A 2.5000-g sample of iron ore is dissolved and the iron converted into iron(II). Exactly 19.17? ml. of 0.0100 M Na2Cr2O7 is required in the titration. What percentage of the ore sample was iron?How many cubic feet of air at a pressure of 760 torr and 0 C is required per ton of Fe2O3 to convert that Fe2O3 into iron in a blast furnace? For this exercise, assume air is 19% oxygen by volume.Find the potentials of the following electrochemical cell: Cd|Cd2+,M=0.10Ni2+,M=0.50|Ni A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with excess silver nitrate. The resulting precipitate, filtered and dried, weighs 3.03707 g. What was the percent by mass of chloride ion in the original compound? What is the identity of the salt?The standard reduction potential for the reaction [Co( H 2 O)6]3+(aq)+e[CO( H 2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co( NH 3 )6]3+(aq)+e[Co( NH 3 )6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions,. [Co( H 2 O)6]2+ and or [Co( NH 3 )6]2+, can be oxidized to the corresponding Cobalt (III) complex by oxygen.Predict the products of each of the following reactions. (Note: In addition to using the information in this chapter, also use the knowledge you have accumulated at this stage of your study, including information on the prediction of reaction products.) (a) MnCO3(s)+HI(aq) (b) CoO(s)+O2(g) (c) La(s)+O2(g) (d) V(s)+VCl4(s) (e) Co(s)+xsF2(g) (f) CrO3(s)+CsOH(aq)Predict the products of each of the following reactions. (Note: In addition to using the information in this chapter, also use the knowledge you have accumulated at this stage of your study, including information on the reaction of reaction products.) (a) Fe(s)+H2SO4(aq) (b) FeCl3(s)+NaOH(aq) (c) Mn(OH)2(s)+HBr(aq) (d) Cr(s)+O2(g) (e) Mn2O3(s)+HCl(aq) (f) Ti(s)+xsF2(g)Describe the electrolytic process for refining copper.Predict the products of the following reactions and balance the equations. (a) Zn is added to a solution of Cr2(SO4)3 in acid. (b) FeCl2 is added to a solution containing an excess of Cr2O72- in hydrochloric acid. (c) Cr2+ is added to Cr2O72- in acid solution. (d) Mn is heated with CrO3. (e) CrO is added to 2HNO3 in water. (f) FeCl3 is added to an aqueous solution of NaOH.What is the gas produced when iron(II) sulfide is treated with a non-oxidizing acid?Predict the products of each of the following reactions and then balance the chemical equations. (a) Fe is heated in an atmosphere of steam. (b) NaOH is added to a solution of Fe(NO3)3. (c) FeSO4 is added to an acidic solution of KMnO4. (d) Fe is added to a dilute solution of H2SO4. (e) A solution of Fe(NO3)2 and HNO3 is allowed to stand in air. (f) FeCO3 is added to a solution of HClO4. (g) Fe is heated in air.Balance the following equations by oxidation-reduction methods; note that three elements change oxidation state.. Co(NO3)2(s)Co2O3(s)+NO2(g)+O2(g)Dilute sodium cyanide solution is slowly dripped into a slowly stirred silver nitrate solution. A white precipitate forms temporarily but dissolves as the addition of sodium cyanide continues. Use chemical equations to explain this observation. Silver cyanide is similar to silver chloride- in its solubility.Predict which will be more stable, [CrO4]2- or [WO4]2-, and explain.Give the oxidation state of the metal for each of the following oxides of [Hint: first transition series. (Hint: Oxides of formula M3O4 are examples of mixed valence compounds in which the metal ion is present in more than one oxidation state. It is possible to write these compound formulas in the equivalent format MO-M2O 3, to permit estimation of the metal’s two oxidation states.) (a) SC2O3. (b) TiO2. (C) V2O5. (d) CrO3. (e) MnO2. (f) Fe3O4. (g) CO3O4. (h) NiO. (i) CU2O Indicate the coordination number for the central metal atom in each of the following coordination compounds: (a) [Pt(H2O)2Br2]. (b) [Pt(NH3)(py)(Cl)(Br)] (py = pyridine, C5H5N). (c) [Zn(NH3)2Cl]. (d) [Zn(NH3)(py)(Cl)(Br)]. (e) [Ni(H2O)4Cl2]. (f) [Fe(en)2(CN)2]+ (en = ethylenediamine, C2H8N2)Give the coordination numbers and write the formulas for each of the following, including all isomers where appropriate: (a) tetrahydroxozincate(ll) ion (tetrahedral). (b) hexacyanopalladate(IV) ion. (c) dichlomaurate(I) ion (note that aurum is Latin for "gold"). (d) diamminedichloroplatinum(Il). (e) potassium diamminetetrachlorochromate(III). (f) hexaamminecobalt(III) hexacyanochromate(III). (g) dibromobis(ethylenediamine) cobalt(III) nitrate Give the coordination number for each metal ion in the following compounds: (a) [Co(CO3)3]3- (note that CO32- is bidentate in this complex). (b) [Cu(NH3)4]2+. (c) [Co(NH3)4Br2]2(SO4)3. (d) [Pt(NH3)4][PtCl4]. (e) [Cr(en)3](NO3)3. (f) [Pd(NH3)2Br2] (square planar). (g) K3[Cu(Cl)5]. (h) [Zn(NH3)2Cl2]Sketch the structures of the following complexes. Indicate any cis, trans, and optical isomers.. (a) [Pt(H2O)2Br2] (square planar). (b) [Pt(NH3)(py)(Cl)(Br)] (square planar, py = pyridine, C5H5N). (c) [Zn(NH3)3Cl]+(tetrahedral). (d) [Pt(NH3)3Cl]+ (square planar). (e) [Ni(H2O)4Cl2]. (f) [Co(C2O4)2Cl2]3- (note that C2O42- is the bidentate oxalate ion, -O2CCO3-)Draw diagrams for any Cis, trans, and optical isomers that could exist for the following (en is ethylenediamine): (a) [CO(en)2(NO2)Cl]+. (b) [Co(en)2Cl2]+. (c) [Pt(NH3)2Cl4]. (d) [Cr(en)3]3+. (e) [Pt(NH3)2Cl2]Name each of the compounds or ions given in Exercise 19.28, including the oxidation state of the metal.Name each of the compounds or ions given in Exercise 19.30.Specify whether the following complexes have isomers.. (a) tetrahedral [Ni(CO)2(Cl)2]. (b) trigonal bipyramidal [Mn(CO)4NO]. (c) [Pt(en)2Cl2]Cl2 Predict whether the carbonate ligand CO32- will coordinate to a metal center as a monodentate, bidentate, or tridentate ligand.Draw the geometric, linkage, and ionization isomers for [COCl5CN][CN].Determine the number of unpaired electrons expected for [Fe(NO2)6]3- and for [FeF6]3- in terms of crystal field theory.Draw the Crystal field diagrams for [Fe(NO2)6]4- and [FeF6]3-. State whether each complex is high spin or low spin, paramagnetic or diamagnetic, and compare ?oct to P for each complex.Give the oxidation state of the metal, number of d electrons, and the number of unpaired electrons predicted for [CO(NH3)6]Cl3.The solid anhydrous solid CoCl2 is blue in color. Because it readily absorbs water from the air, it is used as a humidity indicator to monitor if equipment (such as a cell phone) has been exposed to excessive levels of moisture. Predict what product is formed by this reaction, and how many unpaired electrons this complex will have.Is it possible for a complex of a metal in the transition series to have six unpaired electrons? Explain.How many unpaired electrons are present in each of the following?. (a) [COF6]3- (high spin). (b) [Mn(CN)6]3- (low spin). (c) [Mn(CN)6]4- (low spin). (d) [MnCl6]4- (high spin). (e) [RhCl6]3- (low spin)Explain how the diphosphate ion, [O3P-O-PO3]4-, can function as a water softener that prevents the precipitation of Fe2+ as an insoluble iron salt.For complexes of the same metal ion with no change in oxidation number, the stability increases as the number of electrons in the t2g orbitals increases. Which complex in each of the following pairs of complexes is more stable? (a) [Fe(H2O)6]2+ or [Fe(CN)6]4-. (b) [Co(NH3)6]3+ or [CoF6]3-. (c) [Mn(CN)6]4- or [MnCl6]4-Trimethylphosphine, P(CH3)3, can act as a ligand by donating the lone pair of electrons on the phosphorus atom. If trimethylphosphine is added to a solution of nickel(Il) chloride in acetone, a blue compound that has a molecular mass of approximately 270 g and contains 21.5% Ni, 26.0% Cl, and 52.5% P(CH3)3 can be isolated. This blue compound does not have any isomeric forms. What are the geometry and molecular formula of the blue compound?Would you expect the complex [Co(en)3]Cl3 to have any unpaired electrons? Any isomers?Would you expect the Mg3[Cr(CN)5]2 to be diamagnetic or paramagnetic? Explain your reasoning.Would you expect salts of the gold(I) ion, Au+, to be colored? Explain.[CuCl4]2- is green. [Cu(H2O)6]2+ is blue. Which absorbs higher-energy photons? Which is predicted to have a larger crystal field splitting?Write the chemical formula and Lewis structure of the following each of which contains five carbon atoms: (a) an alkane. (b) an alkene. (c) an alkyne What is the difference between the hybridization of carbon atoms' valence orbitals in saturated and unsaturated hydrocarbons?On a microscopic level, how does the reaction of bromine with a saturated hydrocarbon differ from its reaction with an unsaturated hydrocarbon? How are they similar?On a microscopic level, how does the reaction of bromine with an alkene differ from its reaction with an alkyne? How are they similar?Explain why unbranched alkenes can form geometric isomers while unbranched alkanes cannot. Does this explanation involve the macroscopic domain or the microscopic domain?Explain why these two molecules are not isomers:Explain why these two molecules are not isomers:How does the carbon-atom hybridization change when polyethylene is prepared from ethylene?Write the Lewis structure and molecular formula for each of the following hydrocarbons: (a) hexane (b) 3-methylpentane (c) cis -3-hexene (d) 4-methyl-1-pentene (e) 3-hexyne (f) 4-methyl-2-pentyne Write the chemical formula, condensed formula, and Lewis structure for each of the following hydrocarbons: (a) heptane (b) 3-methylhexane (c) trans -3-heptene (d) 4-methyl-1-hexene (e) 2-heptyne (f) 3, 4-dimethyl-1-pentyne Give the complete IUPAC name for each of the following compounds: (a) CH3CH2CBr2CH3 (b) (CH3)3CCl (c) (d) CH3CH2CCHCH3CH2CCH (e) (f) (g) (CH3)2CHCH2CH=CH2 Give the complete IUPAC name for each of the following compounds: (a) (CH3)2CHF. (b) CH3CHClCHClCH3 (C) (d) CH3CH2CH = CHCH3 (e) (f) (CH3)3CCH2CCH Butane is used as a fuel in disposable lighters. Write the Lewis structure for each isomer of butane.Write Lewis structures and name the five structural isomers of hexane.Write Lewis structures for the Cis -trans isomers of CH3CH = CHCl.Write structures for the three isomers of the aromatic hydrocarbon xylene, C6H4(CH3)2.Isooctane is the common name of the isomer of C8H18 used as the standard of 100 for the gasoline octane rating: (a) What is the IUPAC name for the compound? (b) Name the other isomers that contain a five-carbon chain with three methyl substituents.Write Lewis structures and IUPAC names for the alkyne isomers of C4H6.Write Lewis structures and IUPAC names for all isomers of C4H9Cl.Name and write the structures of all isomers of the propyl and butyl alkyl groups.Write the structures for all the isomers of the -C5H11 alkyl group.Write Lewis structures and describe the molecular geometry at each carbon atom in the following compounds: (a) cis -3-hexene (b) cis -1-chloro-2-bromoethene (c) 2-pentyne (d) trans -6-ethyl-7-methyl-2-octene Benzene is one of the compounds used as an octane enhancer in unleaded gasoline. It is manufactured by the catalytic conversion of acetylene to benzene: 3C2H2C6H6 Draw Lewis structures for these compounds, with resonance structures as appropriate, and determine the hybridization of the carbon atoms in each.Teflon is prepared by the polymerization of tetra?uoroethylene. Write the equation that describes the polymerization using Lewis symbols.Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures. (a) 1 mol of 1-butyne reacts with 2 mol of iodine. (b) Pentane is burned in air.Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures. (a) 2-butene reacts with chlorine. (b) benzene burns in air.What mass of 2-bromopropane could be prepared from 25.5 g of propane? Assume a 100% yield of product.Acetylene is a very weak acid; however, it will react with moist silver(I) oxide and form water and a compound composed of silver and carbon. Addition of a solution of HCl to a 0.2352-g sample of the compound of silver and carbon produced acetylene and 0.2822 g of AgCl. (a) What is the empirical formula of the compound of silver and carbon? (b) The production of acetylene on addition of HCl to the compound of silver and carbon suggests that the carbon is present as the acetylide ion, C22-. Write the formula of the compound showing the acetyl ide ion.Ethylene can be produced by the pyrolysis of ethane: C2H6C2H4+H2 How many kilograms of ethylene is produced by the pyrolysis of 1.00103 kg of ethane, assuming a 100.0% yield?Why do the compounds hexane, hexanol, and hexane have such similar names?Write condensed formulas and provide IUPAC names for the following compounds: (a) ethyl alcohol (in beverages). (b) methyl alcohol (used as a solvent, for example, in shellac). (c) ethylene glycol (antifreeze). (d) isopropyl alcohol (used in rubbing alcohol). (e) glycerine Give the complete IUPAC name for each of the following compounds:Give the complete IUPAC name and the common name for each of the following compounds:Write the condensed structures of both isomers with the formula C2H6O. Label the functional group of each isomer.Write the condensed structures of all isomers with the formula C2H5O2. Label the functional group (or groups) of each isomer.Draw the condensed formulas for each of the following compounds: (a) dipropyl ether. (b) 2, 2-dimethyl-3-hexanol. (c) 2-ethoxybutane MTBE, Methyl tert -butyl ether, CH3OC(CH3)3, is used as an oxygen source in oxygenated gasolines. MTBE is manufactured by reacting 2-methy1propeue with methanol. (a) Using Lewis structures, write the Chemical equation representing the reaction. (b) What volume of methanol, density 0.7915 g/mL, is required to produce exactly 1000 kg of MTBE, assuming a 100% yield?Write two complete balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures. (a) propanol is convened to dipropyl ether. (b) propene is treated with water in dilute acid.Write two complete balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures. (a) 2-butene is treated with water in dilute acid (b) ethanol is dehydrated to yield ethene Order the following molecules from least to most oxidized, based on the marked carbon atom:Predict the products of oxidizing the molecules shown in this problem. In each case, identify the product that will result from the minimal increase in oxidation state for the highlighted carbon atom:Predict the products of reducing the following molecules. In each case, identify the product that will result from the minimal decrease in oxidation state for the highlighted carbon atom:Explain why it is not possible to possible a ketone that contains only two carbon atoms.How does hybridization of the substituted carbon atom change when an alcohol is converted into an aldehyde? An aldehyde to a carboxylic acid?Fatty acids are carboxylic acids that have long hydrocarbon chains attached to a carboxylate group. How does a saturated fatty acid differ from an unsaturated fatty acid? How are they similar?Write a condensed structural formula, such as CH3CH3, and describe the molecular geometry at each carbon atom. (a) propane. (b) 1-butanol. (c) ethyl propyl ether. (d) cis -4-bromo-2-heptene. (e) 2, 2, 3-trimethylhexane. (f) formaldehyde Write a condensed structural formula, such as CH3CH3, and describe the molecular geometry at each carbon atom. (a) 2-propanol. (b) acetone. (c) dimethyl ether. (d) acetic acid. (e) 3-methyl-1-hexene The foul odor of rancid butter is caused by butyric acid, CH3CH2CH2CO2H. (a) Draw the Lewis structure and determine the oxidation number and hybridization for each carbon atom in the molecule. (b) The esters formed from butyric acid are pleasant-smelling compounds found in fruits and used in perfumes. Draw the Lewis structure for the ester formed from the reaction of butyric acid with 2-propanol.Write the two-resonance structures for the acetate ion.Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures: (a) ethanol reacts with propionic acid. (b) benzoic acid, C6H5CO2H, is added to a solution of sodium hydroxide Write two complete balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures. (a) 1-butanol reacts with acetic acid (b) propionic acid is poured onto solid calcium carbonate Yields in organic reactions are sometimes low. What is the percent yield of a process that produces 13.0 g of ethyl acetate from 10.0 g of CH3CO2H?Alcohols A, B and C all have the composition C4H 100. Molecules of alcohol A contain a branched carbon chain and can be oxidized to an aldehyde; molecules of alcohol B contain a linear carbon chain and can be oxidized to a ketone; and molecules of alcohol C can be oxidized to neither an aldehyde nor a ketone. Write the Lewis structures of these molecules.Write the Lewis structures of both isomers with the formula C2H7N.What is the molecular structure about the nitrogen atom in trimethyl amine and in the trimethyl ammonium ion, (CH3)3NH+? What is the hybridization of the nitrogen atom in trimethyl amine and in the trimethyl ammonium ion?Write the two resonance structures for the pyridinium ion, C5H5NH+.Draw Lewis structures for pyridine and its conjugate acid, the pyridinium ion, C5H5NH+. What are the geometries and hybridizations about the nitrogen atoms in pyridine and in the pyridinium ion?Write the Lewis structures of all isomers with the formula C3H7ON that contain an amide linkage.Write two complete balanced equations for the following reaction, one using condensed formulas and one using Lewis structures. Methyl amine is added to a solution of HCl.Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures. Ethylammonium chloride is added to a solution of sodium hydroxide.Identify any carbon atoms that change hybridization and the change in hybridization during the reactions in Exercise 20.26.Identify any carbon atoms that change hybridization and the change in hybridization during the reactions in Exercise 20.39.Identify any carbon atoms that change hybridization and the change in hybridization during the reactions in Exercise 20.51.Write the following isotopes in hyphenated form (e.g., carbon-14). (a) N1124a (b) A1329l (c) K3673r (d) I77194r Write the following isotopes in nuclide notation (E.g., " C614 ")? (a) oxygen-14. (b) copper-70. (c) tantalum-175. (d) francium-217 For the following isotopes that have missing information, fill in the missing information to complete the notation (a) X1434 (b) PX36 (c) MX57n (d) X56121 For each of the isotopes in Exercise 21.1, determine the numbers of protons, neutrons, and electrons in a neutral atom of the isotope.Write the nuclide notation, including charge if applicable, for atoms with the following characteristics: (a) 25 protons, 20 neutrons, 24 electrons. (b) 45 protons, 24 neutrons, 43 electrons. (c) 53 protons, 89 neutrons, 54 electrons. (d) 97 protons, 146 neutrons, 97 electrons Calculate the density of the M1224g nucleus in g/L, assuming that it has that it has the typical nuclear diameter of 11013 cm and is spherical in shape.What are the two principal differences between nuclear reactions and ordinary chemical changes?The mass of the atom N1123a is 22.9893 arm.. (a) Calculate its binding energy per atom in millions of electron volts. (b) Calculate its binding energy per nucleon.Which of the following nuclei lie within the band of stability shown in Figure 21.2? (a) chlorine-37 (b) calcium-4O (c) 204Bi (d) 56Fe (e) 206pb (f) 211pb (g) 222Rn (h) carbon-14 Which of the following nuclei lie within the band of stability shown in Figure 21.2? (a) argon-40 (b) oxygen-16 (c) 12Ba (d) 58Ni (e) 205Tl (f) 210Tl (g) 226Ra (h) magnesium-24 Write a brief description or definition of each of the following: (a) nucleon. (b) particle. (c) particle. (d) positron. (e) ray. (f) nuclide. (g) mass number. (h) atomic number Which of the various particles ( particles, particles, and so on) that may be produced in a nuclear reaction are actually nuclei?Complete each of the following equations by adding the missing species: (a) A1327l+H24e?+n01 (b) P94239u+?C96242m+n101 (c) N714+H24e?+H11 (d) U92235?+C55135s+4n01 Complete each 0f the following equations: (a) L37i+?2H24e (b) C614N714+? (c) A1327l+H24e?+n01 (d) C96250m?+S3898r+4n01 Write a balanced equation for each of the following nuclear reactions: (a) the production of 17O from 14N by a particle bombardment. (b) the production of 14C from 14N by neutron bombardment. (c) the production of 233Th from 232Th by neutron bombardment. (d) the production of 239U from 238U by H12 bombardment Technetium-99 is prepared from 98Mo. Molybdenum-SS combines with a neutron to give molybdenum-99, an unstable isotope that emits a particle to yield an excited form of technetium-99, represented as 99Tc*. This excited nucleus relaxes to the ground state, represented as 99Tc, by emitting a ray. The ground state of 99Tc then emits a particle. Write the equations for each of these nuclear reactions.The mass of the atom F919 is 18.99840 amu.. (a) Calculate its binding energy per atom in millions of electron volts. (b) Calculate its binding energy per nucleon.For the reaction C614N714+?, if 100.0 g of carbon reacts, what volume of nitrogen gas (N2) is produced at 273K and 1 atm?What are the types of radiation emitted by the nuclei of radioactive elements?That changes occur to the atomic number and mass of a nucleus during each of the following decay scenarios?. (a) an particle is emitted. (b) a particle is emitted. (c) radiation is emitted. (d) a positron is emitted. (e) an electron is captured What is the change in the nucleus that results from the following decay scenarios?. (a) emission of a particle. (b) emission of a + particle. (c) capture of an electron Many nuclides with atomic numbers greater than 83 decay by processes such as electron emission. Explain the observation that the emissions from these unstable nuclides also normally include particles.Why is electron capture accompanied by the emission of an X-ray?Explain, in terms of Figure 21.2, how unstable heavy nuclides (atomic number > 83) may decompose to form nuclides of greater stability (a) if they are below the band of stability and (b) if they are above the band of stability.Which of the following nuclei is most likely to decay by positron emission? Explain your choice.. (a) chromium-53. (b) manganese-51. (c) iron-59 The following nuclei do not lie in the band of stability. How would they be expected to decay? Explain your answer.. (a) P1534 (b) U92239 (c) C2038a (d) H13 (e) P94245u The following nuclei do not lie in the band of stability. How would they be expected to decay?. (a) P1528 (b) U92235 (c) C2037a (d) L39i (e) C96245m Predict by what mode(s) of spontaneous radioactive decay each of the following unstable isotopes might proceed: (a) H26e (b) Z3060n (c) P91235a (d) N94241p (e) 18F (f) 129Ba (g) 237Pu Write a nuclear reaction for each step in the formation of P84218o from U98238 which proceeds by a series of decay reactions involving the step-wise emission of ,,,,, particles, in that order.Write a nuclear reaction for each step in the formation of P82208b from T90228h, which proceeds by a series of decay reactions involving the step-wise emission of a, ,,,,,, particles, in that order.Define the term half-life and illustrate it with an example.A 1.00106 -g sample of nobelium, N102254o, has a half-life of 55 seconds after it is formed. What is the percentage of N102254o remaining at the following times? (a) 5.0 min after it forms. (b) 1.0 h after it forms 239Pu is a nuclear waste byproduct with a half-life of 24,000 y. What fraction of the 239Pu present today will be present in 1000 y?The isotope 208Tl undergoes decay with a half-life of 3.1 min.. (a) What isotope is produced by the decay?. (b) How long will it take for 99.0% of a sample of pure 208Tl to decay?. (c) What percentage of a sample of pure 208Tl remains un-decayed after 1.0 h?If 1.000 g of R88226a produces 0.0001 mL of the gas R86222n at STP (standard temperature and pressure) in 24 h, what is the half-life of 226Ra in years?The isotope S3890r one of the extremely hazardous species in the residues from nuclear power generation. The strontium in a 0.500-g sample diminishes to 0.393 g in 10.0 y. Calculate the half-life.Technetium-99 is often used for assessing heart, liver, and lung damage because certain technetium compounds are absorbed by damaged tissues. It has a half-life of 6.0 h. Calculate the rate constant for the decay of T4399c.What is the age of mummified primate skin that contains 8.25% of the original quantity of 14C?A sample of rock was found to contain 8.23 mg of rubidium-87 and 0.47 mg of strontium-87.. (a) Calculate the age of the rock if the half-life of the decay of rubidium by emission is 4.71010 y. (b) If some S3887r was initially present in the rock, would the rock be younger, older, or the same age as the age calculated in (a)? Explain your answer.A laboratory investigation shows that a sample of uranium ore contains 5.37 mg of U92238 and 2.52 mg of P82206b. Calculate the age of the ore. The half-life of U92238 is 4.5109 yr.Plutonium was detected in trace amounts in natural uranium deposits by Glenn Seaborg and his associates in 1941. They proposed that the source of this 239Pu was the capture of neutrons by 238U nuclei. Why is this plutonium not likely to have been trapped at the time the solar system formed 4.7109 years ago?A B47e atom (mass = 7.0169 amu) decays into a L37i atom (mass = 7.0160 amu) by electron capture. How much energy (in millions of electron volts, MEV) is produced by this reaction?A B58 atom (mass = 8.0246 amu) decays into B48 atom (mass = 8.0053 amu) by loss of a + panrticle (mass = 0.00055 amu) or by electron capture. How much energy (in millions of electron volts) is produced by this reaction?Isotopes such as 26Al (half-life: 7.2105 years) are believed to have been present in our solar system as it Formed, but have since decayed and are now called extinct nuclides. (a) 26Al decays by + emission or electron capture. Write the equations for these two nuclear transformations. (b) The earth was formed about .4.7109 (4.7 billion) years ago. How old was the earth when 99.999999% of the 26Al originally present had decayed?Write a balanced equation for each of the following nuclear reactions: (a) bismuth-212 decays into polonium-212. (b) beryllium-8 and a positron are produced by the decay of an unstable nucleus. (c) neptunium-239 forms from the reaction of uranium-238 with a neutron and then spontaneously converts into plutonium-239. (d) strontium-90 decays into yttrium-90 Write a balanced equation for each of the following nuclear reactions: (a) mercury-180 decays into platinum-176. (b) zirconium-90 and an electron are produced by the decay of an unstable nucleus. (c) thorium-232 decays and produces an alpha panicle and a radium-228 nucleus, which decays into actinium-228 by beta decay. (d) neon-19 decays into fluorine-19 Write the balanced nuclear equation for the production of the following transuranium elements: (a) berkelium-244, made by the reaction of Am-241 and He-4. (b) fermiurn-254, made by the reaction of Pu-239 with a large number of neutrons. (c) lawrencium-257, made by the reaction of Cf-250 and B-11. (d) dubnium-260, made by the reaction of Cf-249 and N-15 How does nuclear fission differ from nuclear fusion? Why are both of these processes exothermic?Both fusion and fission are nuclear reactions. Why is a very high temperature required for fusion, but not for ?ssion?Cite the conditions necessary for a nuclear chain reaction to take place. Explain how it can be controlled to produce energy, but not produce an explosion.Describe the components of a nuclear reactor.In usual practice, both a moderator and control rods are necessary to operate a nuclear chain reaction safely for the purpose of energy production. Cite the function of each and explain why both are necessary.Describe how the potential energy of uranium is convened into electrical energy in a nuclear power plant.The mass of a hydrogen atom (11H) is 1.007825 arm; that of a tritium atom (13H) is 3.01605 amu; and that of an a particle is 4.00150 amu. How much energy in kilojoules per mole of 24He produced is released by the following fusion reaction: 11H+13H24He How can a radioactive nuclide be used to show that the equilibrium: AgCl(s)Ag+(aq)+Cl(aq) is a dynamic equilibrium?Technetium-99m has a half-life of 6.01 hours. If a patient injected with technetium-99m is safe to leave the hospital once 75% of the dose has decayed, when is the patient allowed to leave?Iodine that enters the body is stored in the thyroid gland from which it is released to control growth and metabolism. The thyroid can be imaged if iodine-131 is injected into the body. In larger doses, I-133 is also used as a means of treating cancer of the thyroid. I-131 has a half-life of 3.70 days and decays by emission. (a) Write an equation for the decay. (b) How long will it take for 95.0% of a dose of I-131 to decay?If a hospital were storing radioisotopes, what is the minimum containment needed to protect against: (a) cobalt-60 (a strong emitter used for irradiation). (b) molybdenum-99 (a beta emitter used to produce technetium-99 for imaging)Based on what is known about Radon-222’s primary decay method, why is inhalation so dangerous?Given specimens uranium-232 (t1/2=68.9y) and uranium-233 (t1/2=159,200y) of equal mass, which one would have greater activity and why?A scientist is studying a 2.234 g sample of thorium-229 (t1/2=7340y) in a laboratory. (a) What is its activity in Bq?. (b) What is its activity in Ci?Given specimens neon-24 (t1/2=3.38min) and bismuth-211 (t1/2=2.14min) of equal mass, which one would have greater activity and why?

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